Download Study Guide (Semester 2)

Name: _________________________ Date: ____________ Period: ________
Study Guide (Semester 2)
To be able to name a compound based on its formula (IUPAC).
Directions: Hook together the following ions to write the correct formula and place the
name of the resulting compound in the box
Fluorine
Oxygen
Lithium
Beryllium
Gallium
Ammonium
Directions: Name the following compounds:
1. FeCl3
______________________________
2. CdSe
______________________________
3. TiO2
______________________________
4. V2O5
______________________________
5. ZnBr2
______________________________
Directions: Name the following Molecules
1. CO
_________________________________
2. PCl5
_________________________________
3. N2O
_________________________________
4. P2O5
_________________________________
5. CS2
_________________________________
Phosphate
To be able to write the formula of a compound based on its name.
Directions: Write the formula:
1. Tin (IV) Chloride:
____________________________
2. Cobalt (III) Oxide:
____________________________
3. Vanadium (III) Chloride:
____________________________
4. Gold (I) Sulfide:
____________________________
5. Manganese (II) Sulfite:
____________________________
Directions: Write the Name:
1. Carbon Dioxide:
_____________________
2. Dinitrogen TetraOxide:
_____________________
3. Sulfur Hexachloride:
_____________________
4. Oxygen Difluoride:
_____________________
5. Phosphorus Tribromide:
_____________________
To know the common polyatomic ions and be able to use them in formulas and
names.
Directions: Write the formula.
1. Lead (II) Sulfite:
__________________________
2. Copper (I) Acetate:
__________________________
3. Ammonium phosphate:
__________________________
4. Aluminum Hydroxide:
__________________________
5. Magnesium Nitrate:
__________________________
Directions: Write the name.
1. Au(HCO3)3 :
_____________________________________
2. Be(NO3)2:
_____________________________________
3. Pb(OH)2:
_____________________________________
4. K(MnO4):
_____________________________________
5. Zn(SO4):
_____________________________________
To be able to write a skeleton chemical equation from words.
Directions: Write a complete balanced equation for each chemical reaction. Box your
answer.
1. Tin foil will oxidize when exposed to oxygen forming tin (II) oxide.
2. When solid potassium is added to water, hydrogen gas and aqueous potassium hydroxide
are produced.
3. Solid calcium hydrogen carbonate reacts with hydrochloric acid to produce aqueous
calcium chloride, water, and carbon dioxide gas.
4. Mercury (II) Bromide decomposes into its elements when treated with electricity.
To be able to differentiate between the five types of reactions.
Directions: Identify the following reactions as a synthesis, decomposition, combustion,
single-displacement, or a double displacement.
1. _________________________ 3Ag2SO4 (aq) + 2AlCl3  6AgCl (s) + Al2(SO4)3 (aq)
2. _________________________ C4H8 (g) + 6O2  4CO2 (g) + 4H2O (l)
3. _________________________ Zn (s) + 2AgNO3 (aq)  Zn(NO3)2 (aq) + 2Ag (s)
4. _________________________ 2KClO3 (s)  2KCl (s) 3O2 (g)
5. _________________________ 4Fe (s) + 3O2 (g)  2Fe2O3 (s)
To be able to properly balance chemical equations
Directions: Balance the equation and re-write the balance equation on the line given.
1. C + H2O  CO + H2
Balanced Equation: __________________________________________________
2. KClO3  KCl + O2
Balanced Equation: __________________________________________________
3. H3AsO4  As2O5 + H2O
Balanced Equation: __________________________________________________
4. KClO3  KClO4 + KCl
Balanced Equation: __________________________________________________
5. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4
Balanced Equation: __________________________________________________
Complete and Balance (where possible) the following reactions or label them No Reaction
(Use activation series of metals)
1.
Al(OH)3 +
Mg2+

___________________________
2.
LiOH
+
Fe2+

___________________________
3.
K+
+
H2 O

___________________________
4.
MgS
+
CaCl2
5.
Pt2+
+
O2


___________________________
___________________________
To understand the concept of the mole.
1.What is a mole? (Give a complete explanation)
______________________________________________________________________________
______________________________________________________________________________
______________________________________________________________________________
2. One Mole of any gas at STP will occupy ________________.
3. One Mole equals _______________________ particles.
To be able to calculate the molar mass of a compound.
4. Calculate the molar mass (AKA molecular mass) for the following:
a) : Mg(C2H3O2)2
b) Sodium Sulfite: Na2SO3
To be able to convert between moles, mass, and particles
5. Determine the number of particles for the following:
a) 3.2 moles CH4
b) 23.5 g BeCl2
6. Determine the mass for the following:
a) 8.2 moles NO2
b) 1.36 x 1024 molecules PCl4
To be able to solve stoichiometric calculations
Directions: Solve and label the following problems. Box your answer. (To receive credit,
work must be shown)
1. How many molecules of hydrogen are produced if 13.05 g of Zn reacts with excess
hydrochloric acid?
Equation: Zn + HCl  ZnCl2 + H2
2. If excess sulfuric acid reacts with 3.0 moles of sodium chloride, how many grams of
hydrogen chloride are produced?
Equation: NaCl + H2SO4  HCl + Na2SO4
3. If 24.2 g chlorine gas reacts with a solution containing 32.8 g of potassium bromide, how
many grams of bromine gas can be produced? (limiting reagent, honors only)
Equation: KBr + Cl2  KCl + Br2
4. How many grams of chlorine gas must be reacted with excess sodium iodide if 32.2g of
sodium chloride are needed?
Equation: NaI + Cl2  NaCl + I2
5. Aluminum metal reacts with chlorine gas to produce aluminum chloride, AlCl3.
a) Write a balance equation for the reaction.
______________________________________________________________________
b) If 12.3 g of aluminum is combined with 23.6 g of chlorine, show by calculation which
substance is the limiting reactant, and calculate the theoretical yield of aluminum chloride
for the reaction.
To be able to solve Gas Law Calculations and understand the behavior of gases.
1. What happens to the velocity of gas when
a. temperature increase?
b. temperature decrease?
c. when you reach absolute zero?
2. What is the value of absolute zero?
3. What does STP stand for?
a. what values does it have for pressure in the units of kPa, atm, and mmHg
b. what values does it have for temperature in the units of K and C°.
4. State Boyles Gas Law.
5. When temperature is held constant:
a. what happens to the volume of the gas if you double the pressure? (tip P1V1 = P2V2)
b. what relationship does volume and pressure have?
6. To increase pressure of a gas in a closed container, what would you have to do to the
following?
a. the number of moles
b. the temperature
c. the volume
7. What would happen to the volume of balloon if the temperature increased as a constant
pressure?
8. Name and list all the major gas laws.
9. Gas Law calculation:
a. At constant pressure, the volume of a gas increased from 60.0L to 130.0 when heated
from 85°C. What is the final temperature? (tip: Temp. must ALWAYS be in Kelvin for
gas law calculations)
b. At constant temperature, the volume of the gas increased from 5 L to 10 L, the
pressure was initially 100.0 kPa. What was the final pressure?
c. At constant volume, the pressure changed from 95.0 kPa to 105.0 kPa starting at 35°C.
What was the final temperature in Kelvins?
d. 55.5 mL of a gas is collected at 30°C and 85.3 kPa. What volume would the gas
occupy at STP? (tip: remember STP gives you 2 more given for the problem to use)
10. Ideal Gas Law
a. A gas has a volume of 35.4 L at a temperature of 30°C and a pressure of 88.5 kPa. If
Its an ideal gas, how many moles are there in the sample? (tip: R = 8.31 kPa L/ mol K)
b. You have 0.56 moles of NaCl at STP. What is the volume?
Name: _________________________ Date: ____________ Period: ________
Study Guide (Semester 1 Review)
To be able to differentiate between an element, a compound, and a mixture.
1) Fill in the chart and give 2 examples of each.
Matter
Mixtures
____________
Examples:
Pure Substance
____________
Examples:
____________
Examples:
____________
Examples:
____________
____________
____________
___________
____________
____________
____________
___________
2) For each sample of matter below, correctly classify it as a substance or a mixture.
1. Table Sugar
1. ___________________
2. Pure Sand
2. ___________________
3. Kool Aid
3. ___________________
4. Calcium
4. ___________________
5. Asphalt
5. ___________________
3) For each sample of matter below correctly classify as a homogenous mixture or a
heterogeneous mixture.
1. Salt Pepper
1. _______________________
2. Fruitopia Fruit Juice
2. _______________________
3. Oil Paint
3. _______________________
4. Air
4. _______________________
5. Brass
5. _______________________
To be able to differentiate between chemical and physical properties and chemical and
physical changes.
Read the following properties and changes. Decide if each one is physical (P) or chemical (C),
and whether it is a property (P), or a change (C). Thus, something that is a physical change
would be labeled PC.
Boiling point _____
Melting point _____
Color _____
Texture _____
Getting a haircut _____
Density _____
Acidity _____
Ice cube melting _____
Lighting a candle _____
Formation of acid rain _____
Dry ice “smoking” at a concert _____
Alka-seltzer tablets fizzing _____
Malleability _____
Flammability – the ability of an object to support combustion _____
Combustibility – the ability of an object to burn or ignite _____
To be able to determine the numbers of protons, electrons, and neutrons based on the
atomic number and atomic mass number.
Element
Symbol
Number of
Protons
Number of
Electrons
Number of
Neutrons
Lithium
Atomic
Number
Mass Number
4
26
56
47
108
2
2
Pd
105
For each isotope tell me how many electron, protons and neutrons.
a) Nitrogen – 14
b) Nitrogen – 15
Protons: ______
Protons: ______
Electrons: _____
Electrons: _____
Neutrons: _____
Neutrons: _____
To be able to describe the electron configuration for an atom.
1. Fill in the orbitals for the following elements, and state how many unpaired electron.
a) Copper (Cu): _________ unpaired electrons
b) Bromine (Br): __________ unpaired electrons
2. Write the complete electron configuration for the elements:
a) Chlorine (Cl)
b) Tin (Sn)
3. Write the short hand method (using the noble gas configuration) for the following elements.
a) Ruthenium (Ru)
b) Iodine (I)
c) Bromine (Br)
To be able to describe the characteristics of the representative elements and areas of the
periodic table.
1. Explain why electronegativity decreases as you go down the periodic table. (Must include
shielding effect, energy levels, and valence electrons in your response.)
2. Explain why electronegativity increase as you go from left to right on the periodic table.
3. Explain why the size of the atom decrease as you go from left to right in the periodic table.
4. Explain why the atom gets larger as you go down the periodic table.
To be able to explain how valence electrons are involved in bonding.
1. Define Valence Electrons.
______________________________________________________________________________
______________________________________________________________________________
______________________________________________________________________________
2. How do reactions occur, and what part of the atom interacts?
______________________________________________________________________________
______________________________________________________________________________
3. Reactions between atoms involve only their __________________________.
4. Define octet rule.
______________________________________________________________________________
______________________________________________________________________________
5. Elements become stable by achieving the same configuration of valence electrons as one of
the __________________________________.
6. How many valence electrons are in the following atoms.
a. Flourine: ____________________________
b. Carbon:
____________________________
c. Selenium: ____________________________
d. Gallium:
____________________________
7. The electron configuration of an element is 1s22s22p63s23p4. How many valence electrons
does it have?
_______________________
8. The noble gas configuration of an element is [Ar]4s23d104p5. How many valence electrons
does it have?
______________________
To be able to describe ionic and covalent bonding.
1. Define Covalent Bond.
______________________________________________________________________________
______________________________________________________________________________
2. Define Ionic Bond
______________________________________________________________________________
______________________________________________________________________________
3. Classify as Covalent (C) or Ionic(I).
________ Weak Interparticle force.
________
Strong Interparticle force.
________
Liquid or gas at room temperature
________
Solid at room temperature.
________
Less likely to dissolve in water.
________
Elements share electrons.
________
Dissolves in water.
________
Electrolyte
________
Transfer of electrons.
________
Ions
________
Molecules
________
The strong attractive force between ions of opposite charge.
________
The attraction of two atoms for a shared pair of electrons.
________
Non-metal + Non-metal
________
Non-metal + Metal
________
KCl
________
CH4
4. Use a table of electronegativity to find the electronegativity difference between each of
the following pairs of elements and to predict the kind of bond that will be formed.
a. Calcium and Fluorine
_____________________________
b. Carbon and Silicon
_____________________________
c. Beryllium and Sulfur
_____________________________
d. Hydrogen and Germanium
_____________________________
e. Zinc and Bromine
_____________________________
Nuclear Chemistry
1. Write the symbol, charge, and their properties for the following basic nuclear particles
a.
b.
c.
d.
Alpha
Beta
Positron
Gamma
3. Write equations for the following nuclear decay reactions.
a. Decay of polonium-218 by alpha (a) emission.
b. Decay of carbon-14 by beta (b-) emission.
Misc. Answer the following questions.
a. being warmed as a solid ___________
b. being warmed as a liquid __________
c. being warmed as a gas ____________
d. changing from a solid to a liquid _____
e. changing from a liquid to a gas ______
f. What is its boiling temperature? _________________
g. What is its melting temperature? _________________
h. Which resgions of the graph represents kinetic energy? ______________________
i. Which regions of the graph represents potential energy? _____________________