Download Which notation represents an atom of sodium

1. subatomic particles (p,n & e) 2. atomic mass/number & periodic table 3 ground v. excited states
4. valence e-/ dot diagrams
5. electron configuration - short
6. atomic model
7. creation
of light
-- bohr, wave mechanical, rutherford
Name: ___________________________
a
1) ____ Which subatomic particle is negatively charged?
a)
b)
c)
d)
electron
neutron
positron
proton
c What is the mass number of a carbon atom that contains six protons, eight neutrons, and six electrons?
2) ____
a) 6
b) 8
c) 14
d) 20
d An atom in the ground state has a stable valence electron configuration. This atom could be an atom of
3) ____
a) Al
b) Cl
8 valence electron (noble
c) Na
gases, group 18)
d) Ne
b Which electron configuration represents an atom in an excited state?
4) ____
a) 2–7
b) 2–6–2
c) 2–8–1
d) 2–8–8–2
c What information is necessary to determine the atomic mass of the element chlorine?
5) ____
a) the atomic mass of each artificially produced isotope of chlorine, only
b) the relative abundance of each naturally occurring isotope of chlorine, only
c) the atomic mass and the relative abundance of each naturally occurring isotope of chlorine
d)
the atomic mass and the relative abundance of each naturally occurring and artificially produced isotope of chlorine
Base your answers to questions 6 through 8 on the information
to the right.
6) State, in terms of the number of subatomic particles, one
similarity and one difference between the atoms of these
isotopes of sulfur.
They all contain 16 protons
Similarity: ______________________________________
They have different # of neutrons
Difference: _____________________________________
7) In the space provided, draw a
Lewis electron-dot diagram for an
atom of sulfur-33.
8) atomic mass = (mass)(%) + (mass)(%)+
# of valence electrons
8) In the space provided, calculate the atomic mass of sulfur. = 30.249 + 0.243
+ 1.457
32.06 u
+
a In an atom of argon-40, the number of protons
9) ____
a) equals the number of electrons
b) equals the number of neutrons
c) is less than the number of electrons
d) is greater than the number of electrons
=
Regents Review - Atomic Structure
Created: February 2010
1-3
0.00719
Name: ___________________________
a An electron in a sodium atom moves from the third shell to the fourth shell. This change is a result of the atom
10) ____
a)
b)
c)
d)
absorbing energy
releasing energy
gaining an electron
losing an electron
Base your answers to questions 11 and 12 on the information below.
In 1897, J. J. Thomson demonstrated in an experiment that cathode rays were deflected by an electric field. This
suggested that cathode rays were composed of negatively charged particles found in all atoms. Thomson concluded that
the atom was a positively charged sphere of almost uniform density in which negatively charged particles were
embedded. The total negative charge in the atom was balanced by the positive charge, making the atom electrically
neutral. In the early 1900s, Ernest Rutherford bombarded a very thin sheet of gold foil with alpha particles. After
interpreting the results of the gold foil experiment, Rutherford proposed a more sophisticated model of the atom.
11) State one conclusion from Rutherford’s experiment that contradicts one conclusion made by Thomson.
Rutherford experiment determined that an atom is mostly
empty space.
12) State one aspect of the modern model of the atom that agrees with a conclusion made by Thomson.
The atom has a positive nucleus.
b Which electron configuration represents an excited state for a potassium atom?
13) ____
a) 2-8-7-1
b) 2-8-7-2
c) 2-8-8-1
d) 2-8-8-2
Given the bright-line spectra of three
elements and the spectrum of a
mixture formed from at least two of
these elements:
a Which elements are
14) ____
present in this mixture?
a) E and D, only
b) E and G, only
c) D and G, only
d) D, E, and G
15) Describe the electrons in an atom of carbon in the ground state. Your response must include:
• the charge of an electron
• the location of electrons based on the wave-mechanical model
• the total number of electrons in a carbon atom
An electron has a negative charge, and is located in areas of
probability
outside the nucleus, there are 6 electrons in carbon
b Which two particles have opposite charges?
16) ____
a) an electron and a neutron
b) an electron and a proton
c) a proton and a neutron
d) a proton and a positron
Regents Review - Atomic Structure
2-3
Created: February 2010
Name: ___________________________
a Which statement describes how an atom in the ground state becomes excited?
17) ____
a)
b)
c)
d)
The atom absorbs energy, and one or more electrons move to a higher electron shell.
The atom absorbs energy, and one or more electrons move to a lower electron shell.
The atom releases energy, and one or more electrons move to a higher electron shell.
The atom releases energy, and one or more electrons move to a lower electron shell.
d Which symbol represents an atom in the ground state with the most stable valence electron configuration?
18) ____
a) B
b) O
Noble gases have stable octet, 8 valence ec) Li
d) Ne
b Each diagram to the right represents the nucleus of a
19) ____
different atom. Which diagrams represent nuclei of the same
element?
same # of protons = same element
a) D and E, only
b) D, E, and Q
different # of neutrons = isotope
c) Q and R, only
different # of electrons = ion
d) Q, R, and E
Base your answers to questions 20 through 23 on the information to the right.
The atomic and ionic radii for sodium and chlorine are shown in the table
below.
20) Write the ground state electron configuration for the ion that has a radius of
181 picometers. ion of Chlorine = 18e
2
2
6
2
6
or
2-8-8
1s 2s 2p 3s 3p
___________________________________
21) Convert the radius of an Na+ ion to meters. _____________________
102.x10-12 = 1.2 x 10-10
22) Explain, in terms of atomic structure, why the radius of an Na atom is
larger than the radius of an Na+ion.
Na has 3 energy level while Na+ has only
2 energy levels
Base your answers to questions 23 and 23 on the information below.
The nucleus of one boron atom has five protons and four neutrons.
5
23) Determine the total number of electrons in the boron atom. ___________________
+
5
24) Determine the total charge of the boron nucleus. ________________
number of protons
neutrons don't have
a charge
Regents Review - Atomic Structure
3-3
Created: February 2010
1. Gram formula mass = mass of 1 mole = atomic mass in grams
2. mass = gfm
4. particles = 6.02x1023 6. conservation of mass
Name: ______________________
3. volume = 22.4L/mol
5. % composition
7. mass <--> mole
d
1) ____ A 1.0-mole sample of krypton gas has a mass of
a)
b)
c)
d)
19 g
36 g
39 g
84 g
1 mole = 6.02x1023 atoms of Krypton = atomic mass in grams
moles ratio
Given the balanced equation representing a reaction:
28 moles
2) Determine the total number of moles of oxygen that react completely with 8.0 moles of C2H6.____________
3) Determine the mass of
5.20 moles of C2H6 .
Show your work.
mass = moles x gfm
= 5.20 moles x 30 g/mol
= 156 g
Base your answers to questions 4 through 8 on the information below.
Arsenic is often obtained by heating the ore arsenopyrite, FeAsS. The decomposition of FeAsS is represented by the
balanced equation below.
125
=
67.5 + X
In the solid phase, arsenic occurs in two forms. One form, yellow arsenic, has a density of 1.97 g/cm3 at STP. The other
form, gray arsenic, has a density of 5.78 g/cm3 at STP. When arsenic is heated rapidly in air, arsenic(III) oxide is formed.
Although arsenic is toxic, it is needed by the human body in very small amounts. The body of a healthy human adult
contains approximately 5 milligrams of arsenic.
0.005 g
4) Convert the mass of arsenic found in the body of a healthy human adult to grams. _________________
1000 mg = 1 g
5) When heated, a 125.0-kilogram sample of arsenopyrite yields 67.5 kilograms of FeS. Determine the total mass of
conservation of mass
arsenic produced in this reaction.
total mass of reactants = total mass of products
125.0 g = 67.5g + X
X = 57.5 g
As2O3
6) Write the formula for the compound produced when arsenic is heated rapidly in air. _____________________
(III) --> As+3
stock system
7) Explain, in terms of the arrangement of atoms, why the two forms of arsenic have different densities at STP.
gray arsenic has particles that are more closely packed together
creating a high density
8) Calculate the percent composition by mass of arsenic in arsenopyrite. Your response must include both a correct
numerical setup and the calculated result.
% comp by mass = mass of part x100 % comp = 74.9 g/mol x100
mass of whole
162.7 g/mol
= 46% of FeAsS is As
a The gram-formula mass of NO2 is defined as the mass of
9) ____
a) one mole of NO2
b) one molecule of NO2
c) two moles of NO
d) two molecules of NO
Regents Review – Moles
1-2
Created: February 2010
Name: ______________________
c The particles in which sample of LiCl(s) have the same average kinetic energy as the particles in a 2.0-mole
10) ____
sample of H2O(l) at 25°C?
a) 1.0 mol at 75°C
b) 2.0 mol at 50.°C
c) 3.0 mol at 25°C
d) 4.0 mol at 0°C
temperature = average kinetic energy
11) Based on data collected during a laboratory investigation,
a student determined an experimental value of 322 joules
per gram for the heat of fusion of H2O. Calculate the
student’s percent error. Your response must include a
correct numerical setup and the calculated result.
% error = dif. from accepted
accepted
x 100
= 12 J/g x 100
334 J/g
= 3.59%
don't forget about this
equation
Base your answers to questions 12 through 14 on the information below.
A method used by ancient Egyptians to obtain copper metal from copper(I) sulfide ore was heating the ore in the presence
of air. Later, copper was mixed with tin to produce a useful alloy called bronze.
12) Calculate the density of a 129.5-gram sample of bronze that has a volume of 14.8 cubic centimeters. Your response
remember 1 mole = 22.4L
must include a correct numerical setup and the calculated result.
this is even easier
Density = mass/volume
= 129.5 g / 14.8 cm3
8.75 g/cm3
1084oC
13) Convert the melting point of the metal obtained from copper(I) sulfide ore to degrees Celsius. ______________
0 K = -273oC
14) A 133.8-gram sample of bronze was 10.3% tin by mass. Determine the total mass of tin in the sample.
Mass of part = % composition x total mass
= 10.3 % x 133.8 g
= 13.78 g of tin in the sample
= 13.8 g
b
15) ____ Which rigid cylinder contains the same number of gas molecules at STP as a 2.0-liter rigid cylinder containing
H2(g) at STP?
a) 1.0-L cylinder of O2(g)
gases: same volume = same moles = same # of particles
b) 2.0-L cylinder of CH4(g)
c) 1.5-L cylinder of NH3(g)
d) 4.0-L cylinder of He(g)
200g
X
+
88
=
Given the balanced equation representing a reaction:
c What is the total mass of CaO(s) that reacts completely with 88 grams of CO2(g) to produce 200. grams of
16) ____
CaCO3(s)?
a) 56 g
conservation of mass
b) 88 g
c) 112 g
d) 288 g
Regents Review – Moles
2-2
Created: February 2010
Name: _____________________________
b
1) ____
Which substance can be decomposed by chemical means?
a)
b)
c)
d)
aluminum
octane
silicon
xenon
2
Which equation represents an exothermic reaction at 298 K?
2) ____
d Changes in activation energy during a chemical reaction are represented by a
3) ____
a) cooling curve
b) heating curve
c) ionization energy diagram
d) potential energy diagram
Given the equation representing a reaction:
b
Which statement describes this reaction at equilibrium?
4) ____
a) The concentration of N2O4(g) must equal the concentration of NO2(g).
b) The concentration of N2O4(g) and the concentration of NO2(g) must be constant.
c) The rate of the forward reaction is greater than the rate of the reverse reaction.
d) The rate of the reverse reaction is greater than the rate of the forward reaction.
Given the balanced equation representing a reaction:
d
Which type of chemical reaction is represented by this equation?
5) ____
a) double replacement
b) single replacement
c) substitution
d) synthesis
Given the balanced equation representing a reaction:
c
Decreasing the concentration of Na2S2O3(aq) decreases the rate of reaction because the
6) ____
a) activation energy decreases
b) activation energy increases
c) frequency of effective collisions decreases
d) frequency of effective collisions increases
Given the equation representing a reaction at equilibrium:
b Which change favors the reverse reaction?
7) ____
a) decreasing the concentration of HI(g)
b) decreasing the temperature
c) increasing the concentration of I2(g)
d) increasing the pressure
Regents Review – Reactions
1-4
Created: February 2010
Name: _____________________________
a
8) ____ Which reaction occurs spontaneously?
a)
b)
c)
d)
Cl2(g) + 2NaBr(aq) ÆBr2(l) + 2NaCl(aq)
Cl2(g) + 2NaF(aq) ÆF2(g) + 2NaCl(aq)
I2(s) + 2NaBr(aq) ÆBr2(l) + 2NaI(aq)
I2(s) + 2NaF(aq) ÆF2(g) + 2NaI(aq)
b
9) ____
Which substance can not be decomposed by a chemical change?
a) ammonia
b) copper
c) propanol
d) water
a
10) ____ The activation energy of a chemical reaction can be decreased by the addition of
a) a catalyst
b) an indicator
c) electrical energy
d) thermal energy
c Why can an increase in temperature lead to more effective collisions between reactant particles and an
11) ____
increase in the rate of a chemical reaction?
a) The activation energy of the reaction increases.
b) The activation energy of the reaction decreases.
c) The number of molecules with sufficient energy to react increases.
d) The number of molecules with sufficient energy to react decreases.
1
12) ____ Which equation represents a decomposition reaction?
Given the balanced particle-diagram equation:
c
Which statement describes the type of change and the
13) ____
chemical properties of the product and reactants?
a) The equation represents a physical change, with the product and reactants having different chemical properties.
b) The equation represents a physical change, with the product and reactants having identical chemical properties.
c) The equation represents a chemical change, with the product and reactants having different chemical properties.
d) The equation represents a chemical change, with the product and reactants having identical chemical properties.
c
What is the oxidation state of nitrogen in the compound NH4Br?
14) ____
a) –1
b) +2
c) –3
d) +4
15) Identify the element in Period 3 of the Periodic Table that reacts
Na _____________
with oxygen to form an ionic compound represented by the formula X2O. ______
16) On the potential energy diagram provided draw an arrow to represent
the activation energy of the forward reaction.
a
In which type of reaction do two or more substances combine to
17) ____
produce a single substance?
a) synthesis
b) decomposition
c) single replacement
d) double replacement
Regents Review – Reactions
2-4
Created: February 2010
Name: _____________________________
Base your answers to questions 18 through 20 on the information below.
A 1.0-gram strip of zinc is reacted with hydrochloric acid in a test tube. The unbalanced equation below represents the
reaction.
18) Balance the equation for the reaction of zinc and hydrochloric acid, using the smallest whole-number coefficients.
2 HCl(aq) Æ ____ H2(g) + ____ ZnCl2(aq)
____ Zn(s) + ____
19) Explain, using information from Reference Table F, why the symbol (aq) is used to describe the product ZnCl2.
ZnCl2 is soluble in water
20) Explain, in terms of collision theory, why using 1.0 gram of powdered zinc, instead of the 1.0-gram strip of zinc, would
have increased the rate of the reaction.
1.0 gram of powder has more surface area for effective collisons
d In which type of reaction do two lighter nuclei combine to form one heavier nucleus?
21) ____
a) combustion
b) reduction
c) nuclear fission
d) nuclear fusion
b
For which compound is the process of dissolving in water exothermic?
22) ____
a) NaCl
b) NaOH
c) NH4Cl
d) NH4NO3
b
23) ____
Which quantities must be equal for a chemical reaction at equilibrium?
a) the activation energies of the forward and reverse reactions
b) the rates of the forward and reverse reactions
c) the concentrations of the reactants and products
d) the potential energies of the reactants and products
Given the balanced equation representing a reaction:
c
Which statement describes the energy changes in this reaction?
24) ____
a) Energy is absorbed as bonds are formed, only.
b) Energy is released as bonds are broken, only.
c) Energy is absorbed as bonds are broken, and energy is released as bonds are formed.
d) Energy is absorbed as bonds are formed, and energy is released as bonds are broken.
Given the balanced equation representing a phase change:
b
Which statement describes this change?
25) ____
a) It is endothermic, and entropy decreases.
b) It is endothermic, and entropy increases.
c) It is exothermic, and entropy decreases.
d) It is exothermic, and entropy increases.
Regents Review – Reactions
3-4
Created: February 2010
Name: _____________________________
a
26) ____
In a biochemical reaction, an enzyme acts as a catalyst, causing the
a)
b)
c)
d)
activation energy of the reaction to decrease
potential energy of the reactants to decrease
kinetic energy of the reactants to increase
heat of reaction to increase
Base your answers to questions 27 through 30 on the information
below.
An experiment is performed to determine how concentration affects the
rate of reaction. In each of four trials, equal volumes of solution A and
solution B are mixed while temperature and pressure are held constant.
The concentration of solution B is held constant, but the concentration of
solution A is varied. The concentration of solution A and the time for the
reaction to go to completion for each trial are recorded in the data table
below.
27) Describe the relationship between the concentration of solution A and the time for the reaction to go to completion.
As the concentration of solution A decreases, the reaction time increases
28) On the grid provided, mark an appropriate scale on the axis labeled “Reaction Time (s).”
29) On the same grid, plot the data from the data table. Circle and connect the points.
30) Identify one factor, other than the concentration of the solutions, that can affect the rate of this reaction.
temperature, catalyst
Regents Review – Reactions
4-4
Created: February 2010
1. phases of matter
6. heat transfer
2. vapor pressure
3. specific heat
4. STP
5. kinetic molecular theory
7. heat/cooling curve 8. heat of fusion & vaporization 9. combined gas law
Name:_________________________________
a Standard pressure is equal to
1) ____
a)
b)
c)
d)
1 atm
1 kPa
273 atm
273 kPa
Ref. table cover
c A large sample of solid calcium sulfate is crushed into smaller pieces for testing. Which two physical properties
2) ____
are the same for both the large sample and one of the smaller pieces?
a) mass and density
b) mass and volume
c) solubility and density
d) solubility and volume
kinetic molecular theory
c According to the kinetic molecular theory, the molecules of an ideal gas
3) ____
model of how gases behave
a) have a strong attraction for each other
assumptions about gases
b) have significant volume
c) move in random, constant, straight-line motion
p. 24-26 from book
d) are closely packed in a regular repeating pattern
b At 65°C, which compound has a vapor pressure of 58 kilopascals?
4) ____
a) ethanoic acid
reference table H
b) ethanol
c) propanone
d) water
b A person with a body temperature of 37°C holds an ice cube with a temperature of 0°C in a room where the air
5) ____
temperature is 20.°C. The direction of heat flow is
heat travels from source
a) from the person to the ice, only
to sink (high to low)
b) from the person to the ice and air, and from the air to the ice
c) from the ice to the person, only
d) from the ice to the person and air, and from the air to the person
d At standard pressure, which element has a freezing point below standard temperature?
6) ____
a) In
freezing point = melting point
b) Ir
c) Hf
"liquid at 0oC "
d) Hg
The graph below represents the relationship between temperature and time as heat
is added to a sample of H2O.
c Which statement correctly describes the energy of the particles of the
7) ____
sample during interval BC?
a) Potential energy decreases and average kinetic energy increases.
b) Potential energy increases and average kinetic energy increases.
c) Potential energy increases and average kinetic energy remains the same.
d) Potential energy remains the same and average kinetic energy increases.
4 At STP, which 2.0-gram sample of matter uniformly fills a 340-milliliter closed container?
8) ____
(1) Br2(l)
(2) Fe(NO3)2(s)
uniformly filling a container, must be a gas
(3) KCl(aq)
(4) Xe(g)
c Under which conditions of temperature and pressure would a real gas behave most like an ideal gas?
9) ____
a) 200. K and 50.0 kPa
Kinetic molecular theory
b) 200. K and 200.0 kPa
act most ideal at high temp. and low pressure
c) 600. K and 50.0 kPa
act least ideal at low temp. and high pressure
d) 600. K and 200.0 kPa
Regents Review – Matter
1-5
Created: February 2010
Name:_________________________________
Base your answers to questions 10 through 12 on the information below.
A sample of helium gas is in a closed system with a movable piston. The volume of the gas sample is changed when both
the temperature and the pressure of the sample are increased. The table below shows the initial temperature, pressure,
and volume of the gas sample, as well as the final temperature and pressure of the sample.
10) In the space provided, show a correct numerical setup for
calculating the final volume of the helium gas sample.
P1V1
T1
=
P2V2
T2
(2.0)(500mL)
200 K
=
(7.0)(V2)
300 K
ref table T
V = 214 mL
o
27 C
11) Convert the final temperature of the helium gas sample to degrees Celsius. _______________________
12) Compare the total number of gas particles in the sample under the initial conditions to the total number of gas
particles in the sample under the final conditions.
they are the same
closed
container
Base your answers to questions 13 through 16 on the information below.
13) On the grid provided, mark an appropriate scale on the axis labeled “Boiling Point (K).”
14) On the same grid, plot the data from the data
table. Circle and connect the points.
15) Based on the data in the table, state the
relationship between the boiling point at 1
atmosphere and molar mass for these four
substances.
As the molar mass increases,
the boiling point
increases.
16) State, in terms of intermolecular forces, why
the boiling point of propane at 1 atmosphere
is lower than the boiling point of butane at 1 atmosphere.
Propane has weaker intermolecular attractions causing it to have
a lower boiling point than butane.
Regents Review – Matter
2-5
Created: February 2010
Name:_________________________________
Base your answers to questions 17 and 18 on the information below.
At a pressure of 101.3 kilopascals and a temperature of 373 K, heat is removed from a sample of water vapor, causing
the sample to change from the gaseous phase to the liquid phase. This phase change is represented by the equation
below.
entropy - randomness of
particles
17) Explain, in terms of particle arrangement, why entropy decreases during this phase change.
The entropy decrease because water has more organized particles than
a gas.
18) Determine the total amount of heat released by 5.00 grams of water vapor during this phase change.
q = mHv
q = 5.00g x 2259 J/g
q = 11295 J
melting/freezing - heat of fusion
vaporization/condensation - heat of vaporization
Reference table cover
Base your answers to questions 19 through 21 on the information below.
A soft-drink bottling plant makes a colorless, slightly acidic carbonated beverage called soda water. During production of
the beverage, CO2(g) is dissolved in water at a pressure greater than 1 atmosphere. The bottle containing the solution is
capped to maintain that pressure above the solution. As soon as the bottle is opened, fizzing occurs due to CO2(g) being
released from the solution.
19) Explain why CO2(g) is released when a bottle of soda water is opened. try to visualize the situation
When the cap is released, the CO2 is released because the pressure
is decreased.
reference table K & L
Carbonic acid
20) Write the chemical name of the acid in soda water. ________________________
21) State the relationship between the solubility of CO2(g) in water and the temperature of the aqueous solution.
As the temperature increases, the solubility will decrease.
b Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion?
22) ____
a) solution
solids - increase temp = inc solubility
b) compound
gases - increase temp = dec. solubility
c) homogeneous mixture
d) heterogeneous mixture
gas - dec. pressure = dec. solubility
d Particles are arranged in a crystal structure in a sample of
23) ____
a) H2(g)
b) Br2(l)
c) Ar(g)
d) Ag(s)
b Matter is classified as a
24) ____
a) substance, only
b) substance or as a mixture of substances
c) homogenous mixture, only
d) homogenous mixture or as a heterogeneous mixture
Regents Review – Matter
3-5
Created: February 2010
Name:_________________________________
a A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different
25) ____
a)
b)
c)
d)
boiling points
densities
particle sizes
solubilities
forcing a liquid to change to a gas
liquids of different boiling points can
be separated by distillation
c Which term is defined as a measure of the average kinetic energy of the particles in a sample of matter?
26) ____
a) activation energy
b) potential energy
c) temperature
d) entropy
c Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas?
27) ____
a) 100 K and 0.25 atm
high temp. & low pressure
b) 100 K and 25 atm
creates the most space for particles
c) 400 K and 0.25 atm
d) 400 K and 25 atm
b
According to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas?
28) ____
a) The force of attraction between the gas particles is strong.
b) The motion of the gas particles is random and straight-line.
c) The collisions between the gas particles cannot result in a transfer of energy between the particles.
d) The separation between the gas particles is smaller than the size of the gas particles themselves.
c Which statement describes the transfer of heat energy that occurs when an ice cube is added to an insulated
29) ____
container with 100 milliliters of water at 25°C?
source to sink
a) Both the ice cube and the water lose heat energy.
b) Both the ice cube and the water gain heat energy.
c) The ice cube gains heat energy and the water loses heat energy.
d) The ice cube loses heat energy and the water gains heat energy.
c Which quantity of heat is equal to 200. joules?
30) ____
a) 20.0 kJ
b) 2.00 kJ
1000 joules in a kilojoule
c) 0.200 kJ
d) 0.0200 kJ
4 Which graph represents the relationship between pressure and volume for a sample of an ideal gas at constant
31) ____
temperature?
compressing a syringe
c The entropy of a sample of H2O increases as the sample changes from a
32) ____
a) gas to a liquid
solids - lowest entropy
b) gas to a solid
gases - highest entropy
c) liquid to a gas
d) liquid to a solid
a Which statement describes the particles of an ideal gas based on the kinetic molecular theory?
33) ____
a) The gas particles are relatively far apart and have negligible volume.
p. 24-26 in book
b) The gas particles are in constant, nonlinear motion.
c) The gas particles have attractive forces between them.
d) The gas particles have collisions without transferring energy.
Regents Review – Matter
4-5
Created: February 2010
Name:_________________________________
c Under which conditions of temperature and pressure would a 1-liter sample of a real gas behave most like an ideal gas?
34) ____
a)
b)
c)
d)
100 K and 0.1 atm
100 K and 10 atm
500 K and 0.1 atm
500 K and 10 atm
high temp - low pressure
d Which type of energy is associated with the random motion of the particles in a sample of gas?
35) ____
a) chemical energy
b) electromagnetic energy
c) nuclear energy
d) thermal energy
= heat
d At STP, a 7.49-gram sample of an element has a volume of 1.65 cubic centimeters. The sample is most likely
36) ____
a) Ta
b) Tc
= mass/ volume
density
c) Te
7.49/1.65 = 4.54 g/cm3 reference table S
d) Ti
b What occurs when a 35-gram aluminum cube at 100.°C is placed in 90. grams of water at 25°C in an insulated cup?
37) ____
a) Heat is transferred from the aluminum to the water, and the temperature of the water decreases.
b) Heat is transferred from the aluminum to the water, and the temperature of the water increases.
c) Heat is transferred from the water to the aluminum, and the temperature of the water decreases.
d) Heat is transferred from the water to the aluminum, and the temperature of the water increases.
a Which temperature is equal to 120. K?
38) ____
a) 153°C
0oC = 273K
b) 120.°C
c) 293°C
X = 120K
d) 393°C
d A rigid cylinder contains a sample of gas at STP. What is the pressure of this gas after the sample is heated to
39) ____
410 K?
@ STP temp. = 273K
a) 1.0 atm
pressure = 1.0 atm
b) 0.50 atm
c) 0.67 atm
d) 1.5 atm
inc. heat = inc. pressure
Base your answers to questions 40 through 42 on the information below.
A phase change for carbon dioxide that occurs spontaneously at 20.°C and 1.0 atmosphere is represented by the
balanced equation below.
sublimation
40) Write the name of this phase change. _________________________
41) Describe what happens to the potential energy of the CO2 molecules as this phase change occurs.
the potential energy will increase
42) In the space provided, use the key to draw at least five molecules in the box to represent CO2 after this phase change
is completed.
mixture - two or more
substances
not combined - can be
separated
heterogeneous and
homogeneous
compound - two or
more elements chemically combined
in a definite ratio
Regents Review – Matter
5-5
Created: February 2010
1. metals, nonmetals & metalloids
2. groups and periods
3.
atomic radius
Name: _______________________
d
1) ____
Which element has the greatest density at STP? 4. atoms v. ions
5. ionization energy
a) barium
Table S
b) beryllium
6. electronegativity
c) magnesium
7. Reference tables - periodic table & table S
d) radium
c Which element is a metalloid?
2) ____
a) Al
B, Si, Ge, As, Sb, Te
b) Ar
c) As
d) Au
c An element that is malleable and a good conductor of heat and electricity could have an atomic number of
3) ____
a) 16
definition of a metal
b) 18
c) 29
d) 35
a An atom of an element has a total of 12 electrons. An ion of the same element has a total of 10 electrons.
4) ____
Which statement describes the charge and radius of the ion?
are you positive
a) The ion is positively charged and its radius is smaller than the radius of the atom.
b) The ion is positively charged and its radius is larger than the radius of the atom.
you lost the
c) The ion is negatively charged and its radius is smaller than the radius of the atom.
smaller cat
d) The ion is negatively charged and its radius is larger than the radius of the atom.
d Magnesium and calcium have similar chemical properties because a magnesium atom and a calcium atom
5) ____
have the same
a) atomic number
groups have the same # of valence eb) mass number
c) total number of electron shells
d) total number of valence electrons
c Which statement describes a chemical property of bromine?
6) ____
a) Bromine is soluble in water.
b) Bromine has a reddish-brown color.
c) Bromine combines with aluminum to produce AlBr3.
d) Bromine changes from a liquid to a gas at 332 K and 1 atm.
physical properties
d An atom of aluminum in the ground state and an atom of gallium in the ground state have the same
7) ____
a) mass
same group
b) electronegativity
c) total number of protons
d) total number of valence electrons
b Which element has the greatest density at STP?
8) ____
a) scandium
b) selenium
c) silicon
d) sodium
ESRT
d A sample of an element is malleable and can conduct electricity. This element could be
9) ____
a) H
b) He
c) S
d) Sn
Regents Review_ Periodic Table
1-2
Created: February 2010
Name: _______________________
b Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to
10) ____
bottom on the Periodic Table?
ionization energy dec.
a) a decrease in atomic radius
down a
electronegativiy dec.
b) a decrease in electronegativity
group
c) an increase in first ionization energy
atomic radius inc.
d) an increase in nonmetallic behavior
d Which element is a liquid at 758 K and standard pressure?
11) ____
a) gold 1338
if temp. is higher than
b) silver 1235
melting point --> liquid
2045 c) platinum
577
d) thallium
metallic character inc.
across a period
ionization energy inc.
electronegativity inc.
atomic radius dec.
metallic character dec.
a An element that has a low first ionization energy and good conductivity of heat and electricity is classified as a
12) ____
a) metal
def of metal
b) metalloid
c) nonmetal
d) noble gas
c The chemical properties of calcium are most similar to the chemical properties of
13) ____
a) Ar
b) K
same group
c) Mg
d) Sc
b Which element is a liquid at STP?
14) ____
a) argon
b) bromine
group 17 shows all three phases of matter
c) chlorine
d) sulfur
b Which statement describes a chemical property of aluminum?
15) ____
a) Aluminum is malleable.
physical properties
b) Aluminum reacts with sulfuric acid.
c) Aluminum conducts an electric current.
d) Aluminum has a density of 2.698 g/cm3 at STP.
a Which element has an atom in the ground state with a total of three valence electrons?
16) ____
a) aluminum
b) lithium
group 13
c) phosphorus
d) scandium
b As atomic number increases within Group 15 on the Periodic Table, atomic radius
17) ____
a) decreases, only
b) increases, only
down a group each element
c) decreases, then increases
d) increases, then decreases
has additional energy levels
making them larger
Regents Review_ Periodic Table
2-2
Created: February 2010
1. bonds between atoms
2. Ionic v. covalent
Name: ______________________ 3. polar v. nonpolar molecules
a Which formula represents a nonpolar molecule?
1) ____
a)
b)
c)
d)
CH4
HCl
H2O
NH3
4. ions forming bonds
5. Molecular v. empirical formula
6. Diatomic molecules
7. intermolecular attractions
8. dot diagrams
symmetrical = nonpolar
asymmetrical = polar
c The compound XCl is classified as ionic if X represents the element
2) ____
a) H
b) I
ionic bonds form neutral compounds
c) Rb
Which group has a +1 charge?
X+?Cl-1 --> X+1Cl-1
d) Br
c The chemical bonding in sodium phosphate, Na3PO4, is classified as
3) ____
a) ionic, only
Metal + polyatomic ion
b) metallic, only
covalent
ionic
c) both covalent and ionic
d) both covalent and metallic
d Which element is composed of molecules that each contain a multiple covalent bond?
4) ____
a) chlorine
N2 N N N N
b) fluorine
c) hydrogen
d) nitrogen
c What is the empirical formula for a compound with the molecular formula C6H12Cl2O2?
5) ____
a) CHClO
b) CH2ClO
empirical formula = simplest whole number ratio
c) C3H6ClO
d) C6H12Cl2O2
b Which two particle diagrams represent mixtures of
6) ____
diatomic elements?
seven that make a seven
a) A and B
b) A and C
plus hydrogen
c) B and C
N2, O2, F2,
d) B and D
Cl2, Br2, I2 & H2
c Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)?
7) ____
a) They have different molecular structures, only.
b) They have different properties, only.
c) They have different molecular structures and different properties.
d) They have the same molecular structure and the same properties.
allotropes
same element two
different structures
a
Which type of substance can conduct electricity in the liquid phase but not in the solid phase?
8) ____
ionic has free moving ions in the
a) ionic compound
b) molecular compound
liquid phase and when dissolved
c) metallic element
d) nonmetallic element
9)
a Why is a molecule of CO2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar?
____
a)
b)
c)
d)
The shape of the CO2 molecule is symmetrical.
The shape of the CO2 molecule is asymmetrical.
The CO2 molecule has a deficiency of electrons.
The CO2 molecule has an excess of electrons.
Regents Review _ Bonding
1-3
Created: February 2010
Name: ______________________
a Which formula represents a molecular compound?
10) ____
a)
b)
c)
d)
HI
KI
KCl
LiCl
molecular compounds are covalently bonded
a The relatively high boiling point of water is due to water having
11) ____
a) hydrogen bonding
stronger intermolecular attractions
b) metallic bonding
causes higher melting and boiling points
c) nonpolar covalent bonding
d) strong ionic bonding
2 A compound has the empirical formula CH2O and a gram-formula mass of 60. grams per mole. What is the
12) ____
molecular formula of this compound?
empirical formula = 30
60/30 = 2
d Which formula represents strontium phosphate?
13) ____
a) SrPO4
PO4-3
Sr+2
b) Sr3PO8
+6 +
-6 = 0
c) Sr2(PO4)3
d) Sr3(PO4)
Sr (PO )
dot diagrams for ionic bonds
have []
4 Which Lewis electron-dot diagram represents calcium oxide?
14) ____
3
4 2
15) ____
d Which formula represents a nonpolar molecule?
a) HCl
b) H2O
c) NH3
d) CH4
b Which element has an atom with the greatest tendency to attract electrons in a chemical bond?
16) ____
a) carbon
b) chlorine
c) silicon
electronegativity
d) sulfur
c The nitrogen atoms in a molecule of N2 share a total of
17) ____
a) one pair of electrons
b) one pair of protons
each bond shares a pair of electrons total 6ec) three pairs of electrons
d) three pairs of protons
a An ionic compound is formed when there is a reaction between the elements
18) ____
a) strontium and chlorine
b) hydrogen and chlorine
ionic bond --> metal + nonmetal
c) nitrogen and oxygen
d) sulfur and oxygen
a Which compound has both ionic and covalent bonding?
19) ____
a) CaCO3
metal + polyatomic ion
b) CH2Cl2
c) CH3OH
d) C6H12O6
Regents Review _ Bonding
2-3
Created: February 2010
Name: ______________________
b The liquids hexane and water are placed in a test tube. The test tube is stoppered, shaken, and placed in a test tube rack.
20) ____
The liquids separate into two distinct layers because hexane and water have different
a) formula masses
b) molecular polarities
"like dissolves like" -c) pH values
d) specific heats
21) _c
___ Hydrogen bonding is a type of
a) strong covalent bond
b) weak ionic bond
c) strong intermolecular force
d) weak intermolecular force
polar dissolve polar
polar covalent bond -- unequal sharing
nonpolar covalent bond -- diatomics, equally
sharing electrons
** greater difference the bond will be more polar
c Which formula represents copper(I) oxide?
22) ____
a) CuO
b) CuO2
c) Cu2O
d) Cu2O2
Cu+1 O-2
+2
+ -2
= 0
Cu2O
c Which element, represented by X, reacts with fluorine to produce the compound XF2?
23) ____
a) aluminum
X+? F-1
b) argon
+1
-1(2)
+2
-2 = 0
c) magnesium
d) sodium
MgF
+2 --> group 2 metal
2
Base your answers to questions 24 through 26 on the information below.
At STP, iodine, I2, is a crystal, and fluorine, F2, is a gas. Iodine is soluble in ethanol, forming a tincture of iodine. A typical
tincture of iodine is 2% iodine by mass.
24) Compare the strength of the intermolecular forces in a sample of I2 at STP to the strength of the intermolecular forces
both nonpolar - Vanderwaals force increases with
in a sample of F2 at STP.
F2 has weaker intermolecular forces
molecule size - I2 is larger than F2
25) In the space provided, draw a Lewis electron-dot diagram for a molecule of I2.
25)
26) Determine the total mass of I2 in 25 grams of this typical tincture of iodine.
26)
mass = total mass x %
= 25 g x 2%
= 0.5 g
Iodine is 2% of the
total mass
Base your answers to questions 27 through 29 on the information below.
Carbon has three naturally occurring isotopes, C-12, C-13, and C-14. Diamond and graphite are familiar forms of solid
carbon. Diamond is one of the hardest substances known, while graphite is a very soft substance. Diamond has a rigid
network of bonded atoms. Graphite has atoms bonded in thin layers that are held together by weak forces. Recent
experiments have produced new forms of solid carbon called fullerenes. One fullerene, C60, is a spherical, cagelike
molecule of carbon.
27) Determine both the total number of protons and the total number of neutrons in an atom of the naturally occurring
carbon isotope with the largest mass number. C-14
8 neutrons
Neutrons: _______________
6 protons
Protons _______________
covalent
28) Identify the type of bonding in a fullerene molecule. ______________________
29) State, in terms of the arrangement of atoms, the difference in hardness between diamond and graphite.
Diamond has stronger forces of attraction between atoms.
Regents Review _ Bonding
3-3
Created: February 2010
1. intermolecular attractions and boiling point
2. Polar and nonpolar solutions and miscibility
3. freezing and boiling points and conc. of solution 4. Molarity equation
5. concentration calc. (ppm)
6. solubility
chart
Table
F
7.
solubility
curves
Table
G
Name: ____________________________
b Compared to the freezing point and boiling point of water at 1 atmosphere, a solution of a salt and water at 1
1) ____
atmosphere has a
a) lower freezing point and a lower boiling point
b) lower freezing point and a higher boiling point
c) higher freezing point and a lower boiling point
d) higher freezing point and a higher boiling point
inc. concentration causes the
freezing point decreases,
and boiling point increases
d How do the boiling point and freezing point of a solution of water and calcium chloride at standard pressure
2) ____
compare to the boiling point and freezing point of water at standard pressure?
a) Both the freezing point and boiling point of the solution are higher.
b) Both the freezing point and boiling point of the solution are lower.
c) The freezing point of the solution is higher and the boiling point of the solution is lower.
d) The freezing point of the solution is lower and the boiling point of the solution is higher.
c Which substance is an electrolyte?
3) ____
a) CCl4
b) C2H6
electrolyte - conducts electricity b/c it has
c) HCl
free moving ions - ionic
d) H2O
a What is the total mass of solute in 1000. grams of a solution having a concentration of 5 parts per million?
4) ____
a) 0.005 g
b) 0.05 g
reference table - back cover
c) 0.5 g
d) 5 g
a
Which compound is least soluble in water at 60.°C?
5) ____
a) KClO3
b) KNO3
reference table - G
c) NaCl
d) NH4Cl
b
6) ____
Which sample of HCl(aq) contains the greatest number of moles of solute particles?
a) 1.0 L of 2.0 M HCl(aq)
largest volume with the
b) 2.0 L of 2.0 M HCl(aq)
c) 3.0 L of 0.50 M HCl(aq)
greatest concentration
d) 4.0 L of 0.50 M HCl(aq)
d What is the mass of NH4Cl that must dissolve in 200. grams of water at 50.°C to make a saturated solution?
7) ____
a) 26 g
b) 42 g
c) 84 g
reference table G
d) 104 g
c Which solution has the highest boiling point at standard pressure?
8) ____
2 ions
a) 0.10 M KCl(aq)
b) 0.10 M K2SO4(aq) 3 ions
greater number of impurities = higher boiling poit
4 ions
c) 0.10 M K3PO4(aq)
K3PO4 --> 3K+ + PO4-3
d) 0.10 M KNO3(aq) 2 ions
a What is the molarity of 1.5 liters of an aqueous solution that contains 52 grams of lithium fluoride, LiF, (gram9) ____
formula mass = 26 grams/mole)? 2 step problem
a) 1.3 M
moles = 2 moles/1.5L
b) 2.0 M
molarity = moles/liter
c) 3.0 M
= 1.3 M
d) 0.75 M
Regents Review – Solutions
moles = mass/gfm
= 52 g / 26 g/mole
1-2 = 2 moles
Created: February 2010
Name: ____________________________
Base your answers to questions 10 through 14 on the information to the below. Bond energy is the amount of energy
required to break a chemical bond. The table below gives a formula and the carbon-nitrogen bond energy for selected
nitrogen compounds.
10) Describe, in terms of electrons, the type of bonding between
the carbon atom and the nitrogen atom in a molecule of
methanamine.
C-N bond
3 pair
2 pair
Carbon and nitrogen share electrons
creating a covalent bond
11) Identify the noble gas that has atoms in the ground state with
the same electron configuration as the nitrogen in a molecule
Ne - neon
of isocyanic acid. _______________________
N - 7 electrons + 3e-
1 pair
= 10 electrons
neon
12) State the relationship between the number of electrons in a carbon-nitrogen bond and carbon-nitrogen bond energy.
As the number of electrons in the carbon-nitrogen bond
decreases, the bond energy decreases
13) Explain, in terms of charge distribution, why a molecule of hydrogen cyanide is polar.
"Saturday Night Party"
hydrogen cyanide has asymetrical charge distribution
14) A 3.2-gram sample of air contains 0.000 74 gram of hydrogen cyanide. Determine the concentration, in parts per
reference back cover
million, of the hydrogen cyanide in this sample.
ppm = 0.00074 g of Hydrogen cyanide/3.2 g of air
x 1,000,000
= 231 or 230
15) Based on Table G, determine the total mass of NH3 that must be dissolved in 200. grams of water to produce a
110 g
saturated solution at 20.°C.______________________
Base your answers to questions16 and 17 on the information below.
The dissolving of solid lithium bromide in water is represented by the balanced equation below.
16) Calculate the total mass of LiBr(s) required
to make 500.0 grams of an aqueous solution
of LiBr that has a concentration of 388 parts
per million. Your response must include
both a correct numerical setup and the
calculated result.
388 ppm = x/500
x 1,000,000
0.194 g
17) Based on Table F, identify one ion that reacts with Br ions in an aqueous solution to form an insoluble compound.
Ag+, Pb2+, Hg22+
_____________________________
a precipitate will form
Regents Review – Solutions
2-2
Created: February 2010
1. LEO goes GER
2. oxidation states
3. half reactions
4. Electrochemical cells - voltaic and electrolytic 4. AN OX, RED CAT 5. table
Name:_______________________________
Given the balanced equation representing a reaction:
c During this reaction, the oxidation number of Fe changes from
1) ____
a) +2 to 0 as electrons are transferred
b) +2 to 0 as protons are transferred
c) +3 to 0 as electrons are transferred
d) +3 to 0 as protons are transferred
Base your answers to questions 2 through 4 on the information below.
A voltaic cell with magnesium and copper electrodes is shown in the
diagram below. The copper electrode has a mass of 15.0 grams. When the
switch is closed, the reaction in the cell begins. The balanced ionic equation
for the reaction in the cell is shown below the cell diagram. After several
hours, the copper electrode is removed, rinsed with water, and dried. At this
time, the mass of the copper electrode is greater than 15.0 grams.
2) State the direction of electron flow through the wire between the
electrodes when the switch is closed. Mg is oxidized
electrons will travel from Mg to Cu
3) State the purpose of the salt bridge in this cell.
keep the solutions neutral
4) Explain, in terms of copper ions and copper atoms, why the mass of the copper electrode increases as the cell
operates. Your response must include information about both copper ions and copper atoms.
Copper electrode increases because copper ions are attracted to
the electrode where they gain electrons and form copper atoms
Base your answers to questions 6 through 8 on the information below.
In a laboratory investigation, a student constructs a voltaic cell with iron and copper electrodes. Another student
constructs a voltaic cell with zinc and iron electrodes. Testing the cells during operation enables the students to write the
balanced ionic equations below.
5) State evidence from the balanced equation for the cell with iron and copper electrodes that indicates the reaction in
the cell is an oxidation-reduction reaction.
Cu gains electrons (reductions) and Fe loses electrons (oxidation)
electrons
6) Identify the particles transferred between Fe2+ and Zn during the reaction in the cell with zinc and iron electrodes. ____________
7) Write a balanced half-reaction equation for the reduction that takes place in the cell with zinc and iron electrodes.
Fe+2
+ 2e-
-->
Fe
8) State the relative activity of the three metals used in these two voltaic cells.
Zn is the most active then Fe and Cu is the least active
Regent Review – Redox Reaction
1-2
Created: February 2010
Name:_______________________________
d Which substance can be broken down by chemical means?
9) ____
a)
b)
c)
d)
magnesium
manganese
mercury
methanol
d The diagram below represents an operating electrochemical cell
10) ____
and the balanced ionic equation for the reaction occurring in the cell.
Which statement identifies the part of the cell that conducts electrons
and describes the direction of electron flow as the cell operates?
a) Electrons flow through the salt bridge from the Ni(s) to the Zn(s).
b) Electrons flow through the salt bridge from the Zn(s) to the Ni(s).
c) Electrons flow through the wire from the Ni(s) to the Zn(s).
d) Electrons flow through the wire from the Zn(s) to the Ni(s).
Base your answers to questions 11 through 13 on the information below.
In a laboratory investigation, magnesium reacts with hydrochloric acid to produce hydrogen gas and magnesium chloride.
This reaction is represented by the unbalanced equation below.
11) State, in terms of the relative activity of elements, why this reaction is spontaneous.
Mg is more reactive than H2
12) Balance the equation, using the smallest whole-number coefficients.
2
13) Write a balanced half-reaction equation for the oxidation that occurs.
Mg0
-->
Mg+2
+
2e-
Base your answers to questions 14 through 16 on the
information below.
The diagram below shows a system in which water is
being decomposed into oxygen gas and hydrogen gas.
Litmus is used as an indicator in the water. The litmus
turns red in test tube 1 and blue in test tube 2.
The oxidation and reduction occurring in the test tubes
are represented by the balanced equations below.
14) Identify the information in the diagram that indicates this system is an electrolytic cell.
an electrical source is required to cause the reaction
-2 --> 0 _______
15) Determine the change in oxidation number of oxygen during the reaction in test tube 1. _______________
16) Explain, in terms of the products formed in test tube 2, why litmus turns blue in test tube 2.
OH- ions are produced in test tube 2 which is a base
causing litmus to turn blue
Regent Review – Redox Reaction
2-2
Created: February 2010
1. arrhenius definition of an acid and base
2. Bronsted-Lowry definition
3. neutralization equation
3. reactant/products of neutralization 4. indicators 5. pH scale and strength 6. naming acids & bases
Name: _________________________________
a Which word equation represents a neutralization reaction?
1) ____
a) base + acid Æsalt + water
definition
b) base + salt Æwater + acid
c) salt + acid Æbase + water
d) salt + water Æacid + base
d An aqueous solution of lithium hydroxide contains hydroxide ions as the only negative ion in the solution. Lithium
2) ____
hydroxide is classified as an
a) aldehyde
b) alcohol
definition
c) Arrhenius acid
d) Arrhenius base
a One alternate acid-base theory states that an acid is an
3) ____
+
a) H donor
b) H+ acceptor
Bronsted-Lowry
c) OH−donor
−
d) OH acceptor
B
A
A
D
b Which substance is always a product when an Arrhenius acid in an aqueous solution reacts with an Arrhenius
4) ____
base in an aqueous solution?
a) HBr
neutralization reaction
b) H2O
water and salt are product
c) KBr
d) KOH
d Which change in pH represents a hundredfold increase in the concentration of hydronium ions in a solution?
5) ____
a) pH 1 to pH 2
100X more acidic
b) pH 1 to pH 3
c) pH 2 to pH 1
10X scale
d) pH 3 to pH 1
b Which indicator would best distinguish between a solution with a pH of 3.5 and a solution with a pH of 5.5?
6) ____
a) bromthymol blue
b) bromcresol green
Reference table M
c) litmus
d) thymol blue
Given the equation:
b Which ion is represented by X?
7) ____
a) hydroxide
b) hydronium
c) hypochlorite
d) perchlorate
hydronium = H3O+
Base your answers to questions 8 and 9 on the information below.
In performing a titration, a student adds three drops of phenolphthalein to a flask containing 25.00 milliliters of HCl(aq).
Using a buret, the student slowly adds 0.150 M NaOH(aq) to the flask until one drop causes the indicator to turn light pink.
The student determines that a total volume of 20.20 milliliters of NaOH(aq) was used in this titration.
3
8) The concentration of the NaOH(aq) used in the titration is expressed to what number of significant figures? ______
9) Calculate the molarity of the HCl(aq) used in this titration. Your response must include both a correct numerical setup
and the calculated result.
Ma
X
Regents Review – Acids & Bases
Ma X Va = Mb X
25.00mL = 0.150M
X = 0.121 M
1-2
Vb
X 20.20mL
Created: February 2010
Name: _________________________________
b One acid-base theory defines a base as an
10) ____
a) H+donor
b) H+ acceptor
BAAD rule - Bronsted Lowry
c) H+ donor
+
BAAD -Bases Accept Acid Donate
d) H acceptor
11) A student completes a titration by adding 12.0 milliliters of NaOH(aq) of unknown concentration to 16.0 milliliters of
0.15 M HCl(aq). What is the molar concentration of the NaOH(aq)?
0.15M
Ma X Va = Mb X
X 16.00mL = Mb
Mb = 0.20 M
Vb
X 12.0mL
Base your answers to questions 12 through 14 on the information below.
A student used blue litmus paper and
phenolphthalein paper as indicators to test
the pH of distilled water and five aqueous
household solutions. Then the student
used a pH meter to measure the pH of the
distilled water and each solution. The
results of the student’s work are recorded
in the table below.
12) Identify the liquid tested that has the
lowest hydronium ion concentration.
household ammonia
____________________________
strongest base
13) Explain, in terms of the pH range for
color change on Reference Table M,
why litmus is not appropriate to
differentiate the acidity levels of tomato juice and vinegar.
both substances have pH values below that of the activation range of
litmus
14) Based on the measured pH values, identify the liquid tested that is 10 times more acidic than vinegar.
c The data collected from a laboratory titration are used to calculate the
15) ____
a) rate of a chemical reaction
b) heat of a chemical reaction
MaVa = MbVb
c) concentration of a solution
d) boiling point of a solution
pH = 2.3
c When one compound dissolves in water, the only positive ion produced in the solution is H3O(aq). This
16) ____
compound is classified as
a) a salt
b) a hydrocarbon
c) an Arrhenius acid
d) an Arrhenius base
d Which salt is produced when sulfuric acid and calcium hydroxide react completely?
17) ____
a) CaH2
H2SO4
b) CaO
CaOH
c) CaS
d) CaSO4
CaSO
+ HO
4
Regents Review – Acids & Bases
neutralization
2
2-2
Created: February 2010
1. Alkanes, Alkenes, Alkynes 2. bonding and molecular properties of hydrocarbons 3. sat. v. unsaturated
4. functional groups: alcohols, acids, halides, esters, ethers, ketones, amines, amides 5. isomers
6. organic
- polymerization, saponification, halogenation, combustion, esterification, fermentation
Name:reaction
_____________________________
b
1) ____
Which compound is a saturated hydrocarbon?
a) propanal
saturated hydrocarbons have all single bonds - alkanes
b) propane
unsaturated have at least one double or triple bond c) propene
d) propyne
alkenes, alkynes
b The isomers butane and methylpropane differ in their
2) ____
a) molecular formulas
isomers - different structure same
b) structural formulas
c) total number of atoms per molecule
molecular formula
d) total number of bonds per molecule
a Which particle has the greatest mass?
3) ____
a)
an alpha particle
not
b) a beta particle
organicc) a neutron
d) a positron
d A beta particle may be spontaneously emitted from
4) ____
a) a ground-state electron
b) a stable nucleus
c) an excited electron
after the 2nd carbon
d) an unstable nucleus
double bond
4
Which formula represents 2-butene?
5) ____
Base your answers to questions 6 through 8 on the information below.
During a bread-making process, glucose is converted to ethanol and carbon dioxide, causing the bread dough to rise.
Zymase, an enzyme produced by yeast, is a catalyst needed for this reaction.
6) Balance the equation provided for the reaction that causes bread dough to rise, using the smallest whole-number
coefficients.
2
2
7) In the space provided draw a structural formula for the
alcohol formed in this reaction.
7)
H
H
H - C - C -OH
8) State the effect of zymase on the activation energy
for this reaction. zymase is a catalyst
H
H
8) Zymase lowers the activation
energy.
c A straight-chain hydrocarbon that has only one double bond in each molecule has the general formula
9) ____
a) CnH2n−6
b) CnH2n−2
alkene - general formulas
c) CnH2n
reference table Q
d) CnH2n+2
Regents review – Organic Chemistry
1-1
Created: April 2008
polymerization - connecting small molecules
saponification - fat and base make soap
Name: _____________________________
esterification - acid and alcohol
d Which reaction results in the production of soap? halogenation - hydrocarbon and halogen
10) ____
combustion - hydrocarbon and oxygen produce
a) esterification
b) fermentation
carbon dioxide and energy
c) polymerization
fermentation - glucose and enzyme produce
d) saponification
CO2 and alcohol
a Ethanol and dimethyl ether have different chemical and physical properties because they have different
11) ____
a)
b)
c)
d)
functional groups
molecular masses
numbers of covalent bonds
percent compositions by mass
one is an alcohol and the other is an ether
isomers
1 Which formula represents an unsaturated hydrocarbon?
12) ____
Base your answers to questions 13 through 17 on the information below.
Biodiesel is an alternative fuel for vehicles that use petroleum diesel. Biodiesel is produced by reacting vegetable oil with
CH3OH. Methyl palmitate, C15H31COOCH3, a compound found in biodiesel, is made from soybean oil. One reaction of
methyl palmitate with oxygen is represented by the balanced equation below.
methanol
13) Write an IUPAC name for the compound that reacts with vegetable oil to produce biodiesel.___________________
14) Explain, in terms of both atoms and molecular structure, why there is no isomer of CH3OH.
The atoms can not be rearranged to created any different
molecular structure.
reference table R
ester
15) Identify the class of organic compounds to which methyl palmitate belongs. .___________________
combustion reaction
16) Identify the type of organic reaction represented by the balanced equation. .___________________
17) State evidence from the balanced equation that indicates the reaction is exothermic.
energy is a product
a What is the empirical formula of a compound that has a carbon-to-hydrogen ratio of 2 to 6?
18) ____
a) CH3
b) C2H6
c) C3H
d) C6H2
C4H9COOH
Given the formula for an organic compound:
d This compound is classified as an
19) ____
a) aldehyde
b) amine
c) ester
d) organic acid
Regents review – Organic Chemistry
2-2
Created: April 2008
Name: _____________________________
a Butanal and butanone have different chemical and physical properties primarily because of differences in their
20) ____
a)
b)
c)
d)
functional groups
molecular masses
molecular formulas
number of carbon atoms per molecule
functional groups determine the properties
of organic molecuels
Base your answers to questions 21 through 23 on the information below.
The formula below represents a hydrocarbon.
alkane,alkene, alkyne
alkane
21) Identify the homologous series to which this hydrocarbon belongs. ________________
22) Explain, in terms of carbon-carbon bonds, why this hydrocarbon is saturated.
all carbon atoms are bonded to another carbon atom
with a single bond
23) In the space provided, draw a structural formula for one isomer of this hydrocarbon.
Regents review – Organic Chemistry
3-3
Created: April 2008
1. transmutation
2. nuclear notation
3. emission particles 4. Fusion and Fission
5. Natural v. artificial transmutation
6. common uses of radioisotopes
Name: __________________________
4 Which particle has the least mass?
1) ____
mass
number of protons
d Which nuclide is used to investigate human thyroid gland disorders?
2) ____
a) carbon-14
b) potassium-37
c) cobalt-60
d) iodine-131
d
3) ____ A change in the nucleus of an atom that converts the atom from one element to another element is called
a) combustion
b) neutralization
definition
c) polymerization
d) transmutation
2
4) ____ Which particle is emitted from a hydrogen-3 nucleus when it undergoes radioactive decay?
reference table N
Base your answers to questions 5 through 7 on the information below.
Cobalt-60 is commonly used as a source of radiation for the prevention of food spoilage. Bombarding cobalt-59 nuclei with
neutrons produces the nuclide cobalt-60. A food irradiation facility replaces the cobalt-60, a source of gamma rays, when
the radioactivity level falls to of its initial level. The nuclide cesium-137 is also a source of radiation for the prevention of
food spoilage.
reference table N
beta particle
5) Identify one emission spontaneously released by a cobalt-60 nucleus. ___________________
6) Determine the total number of years that elapse before an
original cobalt-60 source in an irradiation facility must be replaced.
1-1/2-1/4-1/8 (3-half lives)
3 x 5.26y = 15.78 y
7) Complete the nuclear equation provided for the decay of cesium-137. Your response must include the symbol, atomic
number, and mass number of the missing particle.
top numbers must equal
137 Ba
56
bottom numbers must equal
b What is the half-life of a radioisotope if 25.0 grams of an original 200.-gram sample of the isotope remains
8) ____
unchanged after 11.46 days?
200 --> 100 --> 50 --> 25
a) 2.87 d
b) 3.82 d
11.46/3 = 3.82 d
c) 11.46 d
d) 34.38 d
Base your answers to questions 80 and 81 on the information below.
Scientists are investigating the production of energy using hydrogen-2 nuclei (deuterons) and hydrogen-3 nuclei (tritons).
The balanced equation below represents one nuclear reaction between two deuterons.
9) State, in terms of subatomic particles, how a deuteron differs from a triton.
deuteron has 1 neutron and a mass of 2
triton has 2 neutrons and a mass of 3
fusion
10) Identify the type of nuclear reaction represented by the equation._______________________
Regents Review _ Nuclear Energy
1-2
Created: February 2010
light nuclei combining to form
heavier nuclei
Name: __________________________
11) ____ Which nuclear emission has the greatest mass and the least penetrating power?
a)
b)
c)
d)
an alpha particle
a beta particle
a neutron
a positron
12) ____ Which radioisotope has an atom that emits a particle with a mass number of 0 and a charge of 1?
a) 3H beta
b) 16N beta
c) 19Ne positron
d) 239Pu alpha
13) ____ In which type of reaction do two lighter nuclei combine to form one heavier nucleus?
a) combustion
definition - fusion
b) reduction
c) nuclear fission
d) nuclear fusion
14) ____ Which radioisotope is used to treat thyroid disorders?
a) Co-60
b) I-131
c) C-14
d) U-238
15) Determine the total time that must elapse until only ¼ of an original sample of the radioisotope Rn-222 remains
7.74 days
unchanged. ______________
1 --> 1/2 --> 1/4 = 2 1/2 life periods
2 x 3.82 days = 7.74 days
Base your answers to questions 16 through 18 on the information below.
Hydrocarbons and fissionable nuclei are among the sources used for the production of energy in the United States. A
chemical reaction produces much less energy than a nuclear reaction per mole of reactant.
The balanced chemical equation below represents the reaction of one molecule of a hydrocarbon with two molecules of
oxygen.
The nuclear equation below represents one of the many possible reactions for one fissionable nucleus. In this equation, X
represents a missing product.
combustion
16) Identify the type of organic reaction represented by the chemical equation. ________________________
17) On the labeled axes provided, draw a potential energy diagram for the reaction of the hydrocarbon with oxygen.
exothermic
1 + 235 = 89 + X + 1
x= 146
0
X = 56
+ 92
= 36 + X + 0
18) Write an isotopic notation for the missing product represented by X in the nuclear equation.
Regents Review _ Nuclear Energy
2-2
146
Ba
56
Created: February 2010