Download Chemistry- CST Review

e) Na, Na+
g) I, I-
Chemistry- CST Review
Standard 1: Atomic and Molecular Structure
1. Complete this table.
Symbol
of
Element
Atomic
Number
Mass
Number
Number
of
Protons
9
55
Zn-64
Sb-3
Hg
51
122
201
14
25
30
Number
of
Neutrons
Number
of
Electrons
10
15
10
14
25
30
Atom,
Ion, or
Isotope
80
2. What is the size and mass of the nucleus in an atom?
3. How many electrons are available for bonding in the following
atoms?
a) barium
b) sodium
c) aluminum
d) oxygen
e) germanium
f) chlorine
g) argon
h) bismuth
4. Name the following groups: Group 1A, Group 2A, Group 7A, and
Group 8A.
f) S, S-2
h) Al, Al+3
8. Indicate which element in each pair has the greater
electronegativity/ionization energy, ability to attract electrons
for bonding.
a) lithium, boron
c) cesium, aluminum
b) magnesium, strontium
d) fluorine, chlorine
Standard 2- Chemical Bonds
1. Compare ionic and molecular (covalent) bonds. How are each
formed?
2. What type of compound (ionic or covalent) is each of the
following?
a) Cl2O
b) SrSO4
c) NH3
d) SnO2
e) N2H4
f) PI3
3. Draw Lewis dot structures for the following molecular
compounds.
a) difluorine monosulfide
b) water
c) carbon tetrachloride
5. Where are the transition metals? Write a general statement
identifying the locations of metals, nonmetals, and metalloids?
Standard 3- Conservation of Matter and Stoichiometry
6. Where on the periodic table would you find the elements with
large atomic numbers and large atomic masses?
1. Write a balanced chemical equation for each reaction below, and
then identify the type of reaction: synthesis, decomposition,
single replacement, double replacement, and combustion.
7. Indicate which element in each pair has the larger atomic
radius.
a) sodium, lithium
b) strontium, magnesium
c) carbon, oxygen
d) selenium, bromine
a)
b)
c)
d)
____ NaCl + ____ F2  ____ NaF + ____ Cl2
____ H2 + ____ O2  ____ H2O
____ Pb(OH)2 + ____ HCl  ____ H2O + ____ PbCl2
____ CH4 + ____ O2  ____ CO2 + ____ H2O
2. Define one mole?
3. What is the molar mass of NaCl, sodium chloride?
4. How many moles are in 15.45 g copper, Cu?
4. How many molecules are in 2 moles of H2O, water?
5. Convert 85.0 L Cl2, chlorine, gas to grams at STP. (Remember
22.4L at STP).
6.
CaCO3 + 2HCl → CO2 + H2O + CaCl2
a) How many moles of CaCO3, calcium carbonate, would be
needed to react completely with 3 moles of HCl, hydrochloric
acid?
b) How many grams of CO2, carbon dioxide, are produced when
10.0 g of CaCO3, calcium carbonate, reacts?
7.
2Ca + O2 → 2CaO
a) How many moles of O2, oxygen, are needed to produce 4.50
moles of CaO, calcium oxide?
b) How many grams of Ca, calcium, would be needed to make
14.5 g of CaO, calcium oxide?
Standard 4 – Gases and their Properties
1. What causes gas pressure in terms of kinetic theory?
2. If someone sprays perfume at the front of the room, will the
people in the back of the room eventually be able to smell it?
Why? Explain completely.
3. What values represent standard temperature and pressure
(STP)?
4. What is absolute zero? What happens at this temperature? Are
there any temperatures below absolute zero?
5. Convert the following.
a) 100 °C to K
c) -35 °C to K
e) 273 K to °C
b) 250 K to °C
d) 50 K to °C
6. How does changing the amount of gas, volume of gas, and
temperature affect the gas pressure?
For Q’s #9-14, name the gas law and show all your work.
7. The pressure on 2.00 L of anesthetic gas changes from 100 kPa
to 40 kPa. What will be the new volume if the temperature
remains constant?
8. If a sample of gas occupies 6.55 L at 300 °C, what will be its
volume at 25 °C if the pressure does not change?
9. A gas at 790 mm Hg and 25 °C occupies a container with an
initial volume of 1.20 L. By changing the volume, the pressure of
the gas increases to 1500 mm Hg as the temperature is raised to
125 °C. What is the new volume?
10. A 500 mL air sample at a temperature of -50 °C has a pressure
of 1.3 atm. What will be the new pressure if the temperature
is raised to 102 °C and the volume expands to 700 mL?
Standard 5- Acids and Bases
1. Classify the following properties as those belonging to an acid
or base or both.
a) bitter taste
b) sour taste
c) H+ ion donating
d) OH- ion donating
e) pH greater than 7
f) pH less than 7
g) H+ ion accepting
h) strong electrolyte (hint: an electrolyte dissolves into
ions in water and therefore conducts electricity)
i) weak electrolyte
j) feels slippery
2. What is the difference between a strong acid or base and a
weak acid or base?
3. Which substances are hydrogen ion donating, hydrogen ion
accepting, or neither.
a) HCl
b) CO2
c) KOH
d) H2O
Standard 6- Solutions
1. Define solute and solvent. Salt is dissolved in a glass of water.
Which is the solute? Which is the solvent?
2. Explain what you would do to quickly dissolve cube sugar in a cup
of coffee (Like changes in temperature and surface area,
breaking up the cube sugar).
3. What effect would increasing concentration (adding more
solute) have on the dissolving process? Lowering
concentration? Explain.
4. Calculate the molarity of each of the following solutions:
a) 0.60 mol of NaCl dissolved in 1.6 L of solution.
b) 25.2 g of potassium nitrate, KNO3, in enough water to make
150.0 mL of solution.
5. Calculate the number of grams of solute needed to prepare
each of the following solutions:
a) 4500.0 mL of a 2.0M solution of potassium hydroxide, KOH.
b) 2.0 liters of 3.0M nitric acid, HNO3, solution.
Standard 7- Chemical Thermodynamics
1. Compare exothermic and endothermic processes.
2. Is heat released or absorbed during these processes?
a) melting
b) freezing
c) boiling
d) condensing
3. How much heat is required to raise the temperature of 20.55 g
of mercury 50°C? The specific heat of mercury is 0.14 J/g °C.
4. Calculate how much heat 35.0 g of water absorbs when it is
heated from 20°C to 80°C. (Specific Heat of water = 4.180
J/gºC)
5. What is the specific heat of a 15.0 g substance that absorbs
350 J of heat when the temperature is raised 40 °C?
Standard 8- Reaction Rates
1. What is the rate of a reaction?
Standard 10- Organic Chemistry (Smells Unit)
2. What factors increase the rate (speed) of a reaction? (Like
concentration, pressure, and temperature)
3. What does a catalyst do to the reaction rate?
Standard 9- Equilibrium
2. Amino acids are building blocks for __________.
1. What is dynamic equilibrium?
2. Given the following system at dynamic equilibrium:
2SO2 (g) + O2 (g) ↔ 2SO3 (g) + heat
Determine the effect of each of the following changes on the
equilibrium position (shifts left or right) and on the amount of
O2 that would result (increase or decrease).
Reaction Shift
(left or right)
Increasing
temperature
Decreasing
pressure
Adding SO2
Removing SO3
Increasing
pressure
Adding SO3
Decreasing
temperature
Removing SO2
1. What following compounds contain simple repeating units?
a) nucleic acid
b) proteins
c) lipid
d) starch
e) water
f) salt
Amount of O2
(increase or
decrease)
3. How many bonds does the carbon atom form?
4. What atoms does carbon commonly form bonds with?
Standard 11- Nuclear Processes
1. What elements have radioactive isotopes?
2. What is the difference between a chemical and nuclear
reaction?
3. What is nuclear fission and nuclear fission?
4. Explain the three different types of nuclear decay: alpha
decay, beta decay, and gamma.
5. How danger is the radiation from alpha, beta, and gamma
particles?