Download FINAL EXAM Review Sheet / Study Guide Honors Chemistry

Name: __________________________________ Period: ___ Date: ______
FINAL EXAM Review Sheet / Study Guide
Honors Chemistry


Exam contains information from all the chapters covered in the course
Review all Vocab, Notes Sheets, and Problems from those chapters
VOCAB
Below is a list of some of the important vocabulary terms from this course. You should study and know
the following terms for the exam. These terms might not be covered in the review questions, but they
are important for the exam!
Physical Property
Chemical Property
Element
Compound
Mixture
Heterogeneous
Homogeneous
Reactant
Product
Dissociation
Period
Group
Noble Gas
Anions
Cations
Shielding
Atomic Radius
Ionization Energy
Electronegativity
Octet Rule
Ionic Bond
Covalent Bond
Molecular Compound
Empirical Formula
Molecular Formula
Limiting Reagent
Excess Reagent
Solute
Solvent
Molarity
**STUDY COMMON CONVERSION FACTORS!!!!**
REVIEW QUESTIONS
Use your notes or worksheets to answer each of the following completely. You should study and know the
information / terms covered in these questions for the exam! SHOW ALL WORK!!
1) What is an isotope? Give an example.
2) Explain the difference between dissociation and dissolving. Use an example compound for each.
3) Write the full electron configurations for the following elements:
a) Copper
b) Iron
c) Iodine
1
4) Differentiate between polar and nonpolar covalent bonds. Give an example of each.
5) In lab, 8.47 g of potassium hydroxide are added to 425 mL of 2.10 M magnesium nitrate.
a) Write the balanced equation (with solubility indicated) for this reaction.
b) How many grams of the precipitate will form?
c) What is the concentration of each ion of the excess reagent that remains in solution after the
reaction is complete?
6) Differentiate between the Aufbau Principle, Hund's Rule, and Pauli Exclusion Principle.
7) A pitcher of lemonade contains a volume of 435 mL. If the percent by volume is 8.0%, what is the
volume of the solute in the lemonade?
2
8) Define each term AND identify the trends across a period and down a group for each.
a) Atomic Size
b) Electronegativity
c) Ionic Radius
d) Ionization Energy
9) Explain the role of shielding and nuclear charge in periodic trends.
10) Knowing the trend for ionization energy, explain why oxygen has a lower I.E. than nitrogen?
11) Write the number of significant figures for each of the following:
a) 423,000,000 g
c) 2.0000003 kg
b) 0.0000004008 m
d) 5090 cm3
12) If the temperature is 112 K, what is the temperature in °C?
13) What are valence electrons? Why are they important?
14) Identify the number of valence electrons AND the charge that forms for each.
a) Nitrogen
c) Aluminum
b) Calcium
d) Fluorine
3
15) In the lab, 0.236 kg of aluminum (initially at 342.0oC) are mixed with an unknown mass of water
(initially at 20.0oC). When thermal equilibrium is reached, the system has a temperature of
85.0oC. Find the mass of the water. The specific heat of the metal is 0.900 J/g°C.
16) Explain the law of conservation of mass. Give an example to support your response.
17) List the factors that affect the rate of dissolving for a solute.
18) A gas occupies 5.50 m3 at -53.0°C, exerting a pressure of 400.0 kPa. What volume (in liters)
would the gas occupy at 272.0°C if the pressure is increased to 5.91 atm.
19) Differentiate between physical and chemical changes. Give TWO examples of each.
20) Explain the VSEPR Theory.
21) A gamma ray has a frequency of 2.10 x 1022 Hz. What is the wavelength and energy associated
with these photons?
4
22) If the temperature of a gas decreases, what happens to the pressure of gas in a container?
23) If 5.6 kg of iron react with oxygen in the air, how many grams of iron (III) oxide will form?
24) When an atom gives off light after being heated, what happened to the electrons in that atom?
25) Differentiate between metals, nonmetals, and metalloids. Give TWO examples for each.
26) A student added 3.20 kg of sodium hydroxide to 750 mL of water. What is the molarity of the
solution that was created?
27) Differentiate between the Rutherford, Bohr, and Quantum Mechanical Models of the atom in
terms of positions of the electrons in an atom. Draw pictures to support your answer.
28) Differentiate between precision and accuracy.
5
29) Fill in the table for each of the following elements.
Element
Gold
Atomic #
Mass #
Protons
Neutrons
Electrons
P3-
Iridium
30) Perform the following conversions:
a) 4.9 years into seconds
b) 345.3 kg/L into mg/cm3
c) 887 m3 into L
31) How many grams of sodium metal are needed to produce 850.0 g of sodium chloride, if sodium
reacts with excess chlorine gas?
32) Ribose is a type of sugar consisting of 40% carbon, 6.7% hydrogen, and 53.3% oxygen. A mass
spectrometer was used to determine the molar mass of ribose to be 150 g/mol. Determine the
empirical and molecular formulas of this compound.
6
33) Write the name of each of the following compounds.
a) ________________________ AgNO3
g) ________________________ HBr
b) ________________________ SO3
h) ________________________ P4S5
c) ________________________ SnF4
i)
________________________ Mg(OH)2
d) ________________________ H2SO4
j)
________________________ CBr4
e) ________________________ K3N
k) ________________________ Pb(C2O4)2
f) ________________________ CuSO4
l)
________________________ C3H8
34) Write the formula of each of the following compounds.
a) ____________ Dinitrogen tetroxide
g) ____________ Aluminum oxide
b) ____________ Phosphoric acid
h) ____________ Gold (III) chloride
c) ____________ Iron (III) nitrate
i)
____________ Nitrous acid
d) ____________ Strontium perchlorate
j)
____________ Calcium phosphate
e) ____________ Tetraphosphorus decoxide
k) ____________ Diboron tetrabromide
f) ____________ Heptyne
l)
____________ Barium nitrate
35) Determine the volume of an object measuring 3.2 x 10 -3 m by 1.5 x 10-4 m by 2.4 x 10-2 m.
36) How does the energy of an electron change when the electron moves closer to the nucleus?
Farther away?
37) Describe how you would separate a mixture of coffee grounds, iron filings, water, and salt. Be
sure to name a physical property of each material that could be used to help separate it.
38) If the volume of air in a life raft increased, what must have happened to the temperature,
assuming the pressure was held constant? Explain.
7
39) Determine the number of moles of each of the following.
a) 43 g Ag
b) 782.45 L O2
c) 2.56 x 1024 atoms Al
40) Identify the following for the 3s atomic orbital: principal quantum number, shape, and number of
sublevels in this energy level.
41) Determine the percent composition for each of the following.
a) Ni2(SO4)3
b) Cu(OH)2
42) Differentiate between ionic and covalent bonds. Be sure to describe the properties in your
response and give an example for each.
8
43) Balance the following reactions and determine the type for each.
a) ____Fe(OH)2 + ____NaCl  ____FeCl2 + ____NaOH
Type of reaction _____________________
b) _____C6H12O6  _____C + _____H2O
Type of reaction _____________________
c) ____C4H10 + ____O2  ____H2O + ____CO2
Type of reaction _____________________
44) Determine the products for the following reactions, balance, and indicate the type of reaction.
a) _____Mg + _____O2 
Type of reaction _____________________
b) _____KI + _____Br2 
Type of reaction _____________________
c) _____NaI + _____Pb(NO3)2 
Type of reaction _____________________
45) Draw the dot structure and indicate the type of hybridization, number of pi bonds, and shape for
each: N2, CF4, O2.
46) Ethylene gas (C2H4) reacts with oxygen in the air. Write the balanced equation for this reaction,
draw the Lewis dot structures for the reactants and products, and determine the change in
enthalpy for the reaction.
9
47) Use the reaction to answer the following: Na2CO3 + Ca(OH)2  2 NaOH + CaCO3
a) If 167.3 grams of sodium carbonate react with 235.5 grams calcium hydroxide, how many
grams of calcium carbonate are formed?
b) What mass of the excess reagent remains?
c) What mass of sodium hydroxide would be formed?
d) If this reaction only gives a 73% yield of calcium carbonate in the lab, what is the actual yield
obtained by scientists?
48) What volume of oxygen is necessary to completely react with 324 liters of methane, CH4, at STP?
CH4 + 2 O2  CO2 + 2 H2O
49) Calculate the density of an unknown solid with a volume of 8.35 cm3 and a mass of 44.75 g. If the
density of gold is 19.3 g/cm3, is this solid pure gold? Explain.
50) Why is it important to learn and study chemistry?
10