Download Chemistry SOL Review Packet CH.1 The student will investigate and

Chemistry SOL Review Packet
CH.1 The student will investigate and understand that experiments in which
variables are measured, analyzed, and evaluated produce observations and
verifiable data.
a) designated laboratory techniques;
b) safe use of chemicals and equipment;
c) proper response to emergency situations;
d) manipulation of multiple variables, using repeated trials;
e) accurate recording, organization, and analysis of data through
repeated trials;
f) mathematical and procedural error analysis;
g) mathematical manipulations (SI units, scientific notation, linear
equations, graphing, ratio and
proportion, significant digits, dimensional analysis);
h) use of appropriate technology including computers, graphing
calculators, and probeware, for gathering data and communicating
results; and
i) construction and defense of a scientific viewpoint (the nature of
science).

design and perform controlled experiments to test predictions, including the
following key components: hypotheses, independent and dependent
variables, constants, controls, and repeated trials.

predict outcome(s) when a variable is changed.

read measurements and record data, reporting the significant digits of the
measuring equipment.

demonstrate precision (reproducibility) in measurement.

recognize accuracy in terms of closeness to the true value of a
measurement.

determine the mean of a set of measurements.

use data collected to calculate percent error and discover and eliminate
procedural errors.

use common SI prefixes and their values (milli-, centi-, kilo-) in
measurements and calculations.

demonstrate the use of scientific notation, using the correct number of
significant digits with powers of ten notation for the decimal place.

graph data utilizing the following:
independent variable (horizontal axis), dependent variable (vertical axis)
scale and units of a graph, regression line (best fit curve).

calculate mole ratios, percent composition, conversions, and average
atomic mass.

perform calculations according to significant digits rules.

convert measurements using dimensional analysis.

use graphing calculators to solve chemistry problems.

read a measurement from a graduated scale, stating measured digits plus
the estimated digit.

use appropriate technology for data collection and analysis, including
probeware interfaced to a graphing calculator and/or computer and
computer simulations.

summarize knowledge gained through gathering and appropriate
processing of data in a report that documents background, objective(s),
data collection, data analysis and conclusions.

explain the emergence of modern theories based on historical
development. For example, students should be able to explain the origin of
the atomic theory beginning with the Greek atomists and continuing
through the most modern quantum models.
In order to meet this standard, it is expected that students will

make connections between components of the nature of science and their
investigations and the greater body of scientific knowledge and research.

demonstrate safe laboratory practices, procedures, and techniques.

demonstrate the following basic lab techniques: filtering, using
chromatography, and lighting a gas burner.

understand Material Safety Data Sheet (MSDS) warnings, including
handling chemicals, lethal dose (LD), hazards, disposal, and chemical spill
cleanup.

identify the following basic lab equipment: beaker, Erlenmeyer flask,
graduated cylinder, test tube, test tube rack, test tube holder, ring stand,
wire gauze, clay triangle, crucible with lid, evaporating dish, watch glass,
wash bottle, and dropping pipette.

make the following measurements, using the specified equipment:
volume: graduated cylinder, volumetric flask, buret
mass: triple beam and electronic balances
temperature: thermometer and/or temperature probe
pressure: barometer and/or pressure probe.

identify, locate, and know how to use laboratory safety equipment,
including aprons, goggles, gloves, fire extinguishers, fire blanket, safety
shower, eye wash, broken glass container, and fume hood.
Chemistry SOL Review Packet
CH 1 Problems:
1. Review safety contract. Write precautions 27, 29, 33,39,40, and
42
5. Sue found several samples of the same substance in a riverbed.
She wanted to find the density of the substance to help identify it.
She gathered the following data:
2. Define: filtering, decanting, chromatography, and distillation.
Indicate which can be used to separate heterogeneous mixtures
and which can be used to separate homogeneous mixtures.
Mass (g)
3. Identify laboratory safety equipment in the classroom and their
locations. Be sure you understand how to use each one.
4. John performed an experiment in which he was concerned with
the effects of changing temperature on the volume of a gas. In his
experiment, he changed the temperature of a sealed balloon and
found the volume. The following table shows the data he collected:
Temperature Temperature Volume Vol/Temp
(°C)
(K)
(mL)
(mL/K)
1
-73.0
403
2
-1.0
546
3
0.0
546
4
1.0
545
5
10.0
601
6
100.0
748
a) Complete the above table.
b) If you wanted to graph this data which variable would go on
the x-axis? the y-axis?
c) In which trial is it likely that experimental error has been
made? Explain.
a)
b)
Trial #
c)
d)
e)
f)
g)
Volume
Density
(cm3)
(g/cm3)
Sample A 5.86
0.31
Sample B 6.24
0.36
Sample C 3.57
0.18
Sample D 1.19
0.06
Sample E 12.27
0.64
Sample F 8.49
0.44
Find the mean (average) value for the density of the
unknown substance.
According to the following density values, what is the
substance Sue has found?
a. Silver – 10.49 g/mL d. Gold - 19.32 g/mL
b. Titanium – 4.5 g/mL e. Lead – 11.3 g/mL
c. Copper – 8.92 g/mL
Which sample is it likely that a procedural error has been
made? Explain.
Discuss the precision and accuracy of Sue’s data.
Convert the mass of Sample E to kilograms. Express the
answer in scientific notation.
Convert the mass of Sample E to milligrams. Express the
answer in scientific notation.
Calculate the % error of Sue’s data.
Chemistry SOL Review Packet
CH 2 The student will investigate and understand that the placement of
elements on the periodic table is a function of their atomic structure. The
periodic table is a tool used for the investigations of
a) average atomic mass, mass number, and atomic number;
b) isotopes, half lives, and radioactive decay;
c) mass and charge characteristics of subatomic particles;
d) families or groups;
e) periods;
f) trends including atomic radii, electronegativity, shielding
effect, and ionization energy;
g) electron configurations, valence electrons, and oxidation
numbers;
h) chemical and physical properties; and
i) historical and quantum models.
In order to meet this standard, it is expected that students will

determine the atomic number, atomic mass, the number of protons,
and the number of electrons of any atom of a particular element
using a periodic table.

determine the number of neutrons in an isotope given its mass
number.

perform calculations to determine the “weighted” average atomic
mass.

perform calculations involving the half-life of a radioactive
substance.

differentiate between alpha, beta, and gamma radiation with respect
to penetrating power, shielding, and composition.

differentiate between the major atom components (proton, neutron
and electron) in terms of location, size, and charge.

distinguish between a group and a period.

identify key groups, periods, and regions of elements on the periodic
table.

identify and explain trends in the periodic table as they relate to
ionization energy, electronegativity, shielding effect, and relative
sizes.

compare an element’s reactivity to the reactivity of other elements in
the table.

relate the position of an element on the periodic table to its electron
configuration.

determine the number of valence electrons and possible oxidation
numbers from an element’s electron configuration.

write the electron configuration for the first 20 elements of the
periodic table.

distinguish between physical and chemical properties of metals and
nonmetals.

differentiate between pure substances and mixtures and between
homogeneous and heterogeneous mixtures.

identify key contributions of principal scientists including:
atomos, initial idea of atom – Democritus
first atomic theory of matter, solid sphere model – John Dalton
discovery of the electron using the cathode ray tube experiment,
plum pudding model – J. J. Thomson
discovery of the nucleus using the gold foil experiment, nuclear
model – Ernest Rutherford
discovery of charge of electron using the oil drop experiment –
Robert Millikan
energy levels, planetary model – Niels Bohr
periodic table arranged by atomic mass – Dmitri Mendeleev
periodic table arranged by atomic number – Henry Moseley
quantum nature of energy – Max Planck
uncertainty principle, quantum mechanical model – Werner
Heisenberg
wave theory, quantum mechanical model – Louis de Broglie.

differentiate between the historical and quantum models of the atom.
Chemistry SOL Review Packet
8. Write electron configurations for the following:
a. chlorine
b. magnesium
c. oxygen
CH 2 Problems:
1. Electrons have little mass and a __________ charge. They are
located in _____________, __________ the nucleus. Protons
have a ___________ charge. Neutrons have a ____________
charge. Protons and neutrons are located in the center or
________________ of the atom and comprise most its mass.
9. Define the periodic law.
2. An _____________ is an atom that has the same number of
protons as another atom, but has a different number of
__________. Some isotopes are radioactive; many are not.
10. Vertical columns are called _____________ and have similar
properties because _________________________________.
Horizontal rows are called ___________ and have predictable
properties based on an increasing number of electrons in the
outer orbitals.
3. The __________________ of an element is the same as the
number of protons. In a neutral atom the number of _______ are
always equal to the number of ______________. All atoms of the
same element have the same number of _______.
11. Electronegativity ____________ from left to right and
_________ from top to bottom within a group. Atomic radius
_____________ from left to right and __________ from top to
bottom within a group. Ionization energies generally
__________ from left to right and ___________ from top to
bottom within a group. Shielding effect is _____________ within
a given period and ____________ within given groups from top
to bottom.
4. The periodic table is arranged by increasing ______________.
5. Name the following elements:
Group 2, Period 5
Group 14, Period 2
6. Using the periodic table, determine the atomic #, mass #, #
protons, # electrons, and # neutrons of the following:
Element Atomic Mass # # p+
# e# n0
#
C
I
Ca
Mn
7. Determine the # protons, neutrons, electrons and mass # of the
following:
137
60 +3
31 -3
Ba+2
Ni
P
Protons
Neutrons
Electrons
Mass #
.
12. Name groups 1, 2, 3-12, 17, and 18 on the periodic table.
13. Name the metalloids.
14. Which of the following ahs the largest atomic radius? Ca Ga Li
15. Which of the following has the lowest ionization energy? Na K Rb
16. Which of the following has the greatest electronegativity? Li N F
Chemistry SOL Review Packet
17. States the Pauli Exclusion Principle.
18. State Hund’s Rule.
24. Explain the periodic trend of reactivity.
19. Identify the groups that represent the following orbitals: s, p, d, f
25. Briefly describe the contributions to the modern atomic theory of
the following scientists:
a. Democritus
20. When an atom gains an electron, it becomes ________ charged
and is called a(n) _______. When an atom loses and electron, it
becomes _______ charged and is called a(n) ________.
21. Define physical and chemical properties.
22. Write the formulas for the seven (7) diatomic molecules.
b. Dalton
c. JJ Thomson
d. Lord Rutherford
e. Millikan
f.
23. Classify the following as element (E), compound (C),
heterogeneous mixture (het), or homogeneous mixture (hom)
a.
b.
c.
d.
e.
f.
Water
Carbon
Salt water
Air
Tap water
Salad dressing
Bohr
g. Mendeleev
h. Plank
i.
Heisenberg
j.
de Broglie
Chemistry SOL Review Packet
CH 3 The student will investigate and understand how conservation
of energy and matter is expressed in chemical formulas
and balanced equations. Key concepts include
a) nomenclature;
b) balancing chemical equations;
c) writing chemical formulas;
d) bonding types;
e) reaction types; and
f) reaction rates, kinetics, and equilibrium.
 draw Lewis dot diagrams to represent valence electrons in elements
and draw Lewis dot structures to show covalent bonding.
 use valence shell electron pair repulsion (VSEPR) model to draw
and name molecular shapes (bent, linear, trigonal planar,
tetrahedral, and trigonal pyramidal).
 recognize polar molecules and non-polar molecules.
 classify types of chemical reactions as synthesis, decomposition,
single replacement, double replacement, neutralization, and/or
combustion.
 recognize that there is a natural tendency for systems to move in a
In order to meet this standard, it is expected that students will
direction of randomness (entropy).
 name binary covalent/molecular compounds.
 recognize equations for redox reactions and neutralization reactions.
 name binary ionic compounds (using the Roman numeral system
 distinguish between an endothermic and exothermic process.
where appropriate).
 predict, draw, and name molecular shapes (bent, linear, trigonal
planar, tetrahedral, and trigonal pyramidal).
 transform word equations into chemical equations and balance
chemical equations.
 write the chemical formulas for certain common substances, such as
ammonia, water, carbon monoxide, carbon dioxide, sulfur dioxide,
and carbon tetrafluoride.
 use polyatomic ions for naming and writing formulas of ionic
compounds, including carbonate, sulfate, nitrate, hydroxide,
phosphate, and ammonium.
 interpret reaction rate diagrams.
 identify and explain the effect the following factors have on the rate
of a chemical reaction: catalyst, temperature, concentration, size of
particles.
 distinguish between irreversible reactions and those at equilibrium.
 predict the shift in equilibrium when a system is subjected to a stress
(Le Chatelier’s Principle) and identify the factors that can cause a
shift in equilibrium (temperature, pressure, and concentration.)
Chemistry SOL Review Packet
CH 3 Problems:
1. State the law of definite proportions.
e. Carbon dioxide
f. Iron(III) sulfate
g. Sulfur dioxide
2. Define empirical formulas, molecular formulas, and structural
formulas.
3. What is the difference between an ionic bond and a covalent
bond in terms of electrons.
h. Carbon tetrachloride
i.
Methane
j.
Ammonia
4. Define ionization energy.
5. Define electronegativity.
9. Draw the lewis dot diagram for the following:
S
Br
Ca
6. Define polarity.
7. Name the following compounds:
a. PbCl2
b. Fe2O3
10. Draw examples of molecules with the following molecular
shapes:
Linear
Trigonal Planar
c. P2O5
d. Cu2CO3
Bent
Tetrahedral
e. BCl3
f. Au(NO3)3
Trigonal Pyramidal
g. Pb(C2H3O2)4
8. Write chemical formulas for the following:
a. Water
b. Carbon monoxide
c. Calcium carbonate
d. Lithium nitride
11. Reaction Type
______Write general form
a. Synthesis
b. Decomposition
c. Single replacement
d. Double replacement
e. Combustion
Chemistry SOL Review Packet
12. Define oxidation-reduction reaction, oxidation, reduction,
oxidizing agent, reducing agent.
13. Define exothermic and endothermic reactions.
14. State Le Chatelier’s Principle. Explain what stresses affect
reactions.
15. Write balanced chemical equations for the following
reactions and classify the reaction.
a. Phosphorus reacts with oxygen to product
c. Copper(II) hydroxide and potassium sulfate are
produced when potassium hydroxide reacts with
copper(II) sulfate.
16. In the following reactinos, tell which element is oxidized and
which is reduced and identify the oxidizing and reducing
agents:
a. 2HgO  2Hg + O2
b. S + O2 
SO2
c. Cu + 2AgNO3  Cu(NO3)2 + 2Ag
d. Mg + Cl2  2MgCl2
diphosphorus pentoxide.
b. Iron(II) oxide reacts with aluminum to produce
aluminum oxide and iron.
17. Identify the following as an endothermic reaction or an
exothermic reaction:
a. C3H8 + 5O2 
3CO2 + 4H2O + 2043kJ
b. C + H2O + 113kJ 
CO + H2
Chemistry SOL Review Packet
CH 4 The student will investigate and understand that chemical
quantities are based on molar relationships. Key
concepts include
a) Avogadro’s principle and molar volume;
b) stoichiometric relationships;
c) solution concentrations; and
d) acid/base theory; strong electrolytes, weak
electrolytes, and nonelectrolytes; dissociation and
ionization; pH and pOH; and the titration process.
In order to meet this standard, it is expected that students will
 perform conversions between mass, volume, particles, and moles of
a substance.
 perform stoichiometric calculations involving the following
relationships:
- mole-mole;
- mass-mass;
- mole-mass;
- mass-volume;
- mole-volume;
- volume-volume;
- mole-particle;
- mass-particle; and
- volume-particle.

compare and contrast the differences between strong, weak,
and non-electrolytes.

relate the hydronium ion concentration to the pH scale.
perform titrations in a laboratory setting using indicators.
CH 5 The student will investigate and understand that the phases
of matter are explained by kinetic theory and forces of attraction
between particles. Key concepts include
a) pressure, temperature, and volume;
b) partial pressure and gas laws;
c) vapor pressure;
d) phase changes;
e) molar heats of fusion and vaporization;
f) specific heat capacity; and
g) colligative properties.
In order to meet this standard, it is expected that students will
 explain the behavior of gases and the relationship between pressure
and volume (Boyle’s Law), and volume and temperature (Charles’
Law).
 identify the limiting reactant (reagent) in a reaction.
 solve problems and interpret graphs involving the gas laws.
 calculate percent yield of a reaction.
 identify how hydrogen bonding in water plays an important role in
 perform calculations involving the molarity of a solution, including
dilutions.
many physical, chemical, and biological phenomena.
 interpret vapor pressure graphs.
 interpret solubility curves.
 graph and interpret a heating curve (temperature vs. time).
 differentiate between the defining characteristics of the Arrhenius
 interpret a phase diagram of water.
theory of acids and bases and the Bronsted-Lowry theory of acids
and bases.
 identify common examples of acids and bases, including vinegar
and ammonia.
 calculate energy changes, using molar heat of fusion and molar heat
of vaporization.
 calculate energy changes, using specific heat capacity.
examine the polarity of various solutes and solvents in solution formation.
Chemistry SOL Review Packet
CH 4 Problems
1. How many liters of carbon dioxide will be produced if
1.47 mol of oxygen is used in the following reaction?
C3H8 + 5O2
3CO2 + 4H2O + 2043kJ
7. Aluminum reacts with sulfuric acid to produce aluminum
sulfate and hydrogen. How many grams of aluminum sulfate
will be produced from 0.58 mol of sulfuric acid?
8. List the postulates of the kinetic-molecular theory.
2. Methane (CH4) reacts with oxygen to produce carbon dioxide
and water. If 5.28L of oxygen is used in the reaction at STP,
what mass of water will be produced?
9. Write equations for Boyle’s Law, Charles’s Law, combined
gas law, and Dalton’ Law.
3. Calcium carbonate and hydrochloric acid react to produce
calcium chloride and carbonic acid. How much calcium
chloride will be produced if 7.89g of hydrochloric acid are
used?
4. How many moles of oxygen are produced from the
decomposition of 19.55 moles of water?
5. How many atoms of iron are required to react with 8.2x1024
molecules of oxygen according to the following equation:
4Fe + 3O2
2Fe2O3
6. How many liters of N2 are needed to produce 6.84L of NH3 in
the synthesis of ammonia?
10. The pressure and volume of a sample of gas at a constant
temperature are _________ proportional to each other.
(____________ Law) At constant pressure, the volume of a
fixed amount of gas is _________ proportional to its
temperature. (____________ Law)
11. If 75.3g of aluminum and 110.1g of oxygen react according
to the following equation, which is the limiting reactant?
4Al + 3O2
2Al2O3
12. 125g of Al2O3 is recovered from the above reaction, What is
the percent yield?
13. A gas occupies a volume of 60.0cm3 at 36°C. What will the
same gas occupy at standard temperature if the pressure
remains constant?
Chemistry SOL Review Packet
14. A mixture of gas has a pressure of 725mmHg. The mixture
contains hydrogen, nitrogen, and argon. The pressure of the
hydrogen and argon are 378mmHg and 64mmHg,
respectively. What is the pressure of the nitrogen in kPa?
19. What volume of 12M HCl is neeed to prepare 500mL of a 2M
HCl solution?
20. List five properties of acids and five properties of bases.
15. If some oxygen gas at 101 kPa and 25°C is allowed to
expand from 5.0dm3 to 10.0dm3 without changing the
temperature, what pressure will the oxygen gas exert?
16. How many moles can be obtained in a 1.44L flask at 32°C
and 93.5kPa?
21. Name the following and indicate whether it is an acid or
base:
a. KOH
b. HCl
c. H2SO4
d. NaOH
e. HNO3
f. H2CO3
22. What is an acid/base titration?
2.50x102mL
17. What is the molarity of
9.46g cesium bromide?
of solution containing
23. Explain the difference between a strong and a weak
electrolyte.
18. What is the molarity of 5.23g of iron(II) nitrate dissolved in
100.0cm3 of solution?
Chemistry SOL Review Packet
CH 5 Problems
Use the following heating curve for water to answer the questions.
6. An 18.7g sample of platinum metal increases in temperature by
2.3°C when 5.7J of heat are added. What is the specific heat of
platinum?
E
7. Define heat of fusion and heat of vaporization.
D
8. Polar substance dissolve ___________ substances and
nonpolar substances dissolve _____________ substances.
C
A
B
Heat Added
1. At which point on the heat curve is heat of fusion represented?
Heat of vaporization?
2. At which point(s) on the curve is there no increase in average
kinetic energy?
3. Label solid, liquid, gas, melting point, boiling point, freezing,
condensation, melting, and vaporization.
4. Define sublimation and deposition.
9. Label the following on the above phase diagram for water: solid,
liquid, gas, melting and boiling points at 1atm, critical point, and
triple point.
5. A 21.0g sample of water is cooled from 34.0°C to 28.0°C. How
many joules of heat were removed from the water?
10. Draw and label arrows that represent freezing, vaporization, and
sublimation.
Chemistry SOL Review Packet
Heats of vaporization and heats of fusion of some substances
Substance
Heat of
Heat of fusion
vaporization
Water
40.7 kJ/mol
6.00 kJ/mol
Methane
9.2 kJ/mol
0.84 kJ/mol
Mercury
59.4 kJ/mol
2.33 kJ/mol
11. How much energy is required to vaporize 22.5g of liquid
mercury?
d. NH3
e. Cl2
13. Distinguish between inter- and intra-molecular forces
12. Draw the following molecules and determine if they are polar or
non-polar molecules.
a. H2O
14. List the intramolecular forces in order of decreasing strength.
b. CH4
15. List the intermolecular forces in order of decreasing strength.
c. CO2
Chemistry SOL Review Packet
CH.6
The student will investigate and understand how basic
chemical properties relate to organic chemistry and
biochemistry. Key concepts include
a) unique properties of carbon that allow multi-carbon
compounds; and
b) uses in pharmaceuticals and genetics,
petrochemicals, plastics, and food.
In order to meet this standard, it is expected that students will
2. Which statement describes how plastics differ from nucleic
acids?
a. Plastics are synthetic polymers but nucleic acids are
natural
b. Plastics are formed from repeated subunits, but
nucleic acids are not
c. Plastics are formed from organic compounds, but
nucleic acids are not
d. Plastics are polymers, but nucleic acids are
monomers
3. Draw Lewis structures for the following and determine
molecular polarity:
a. Methane

describe how saturation affects shape and reactivity of carbon
compounds.

draw Lewis dot structures, identify geometries, and describe
polarities of the following molecules: CH4, C2H6, C2H4, C2H2,
CH3CH2OH, CH2O, C6H6, CH3COOH.
b. Ethane
recognize that organic compounds play a role in natural and
synthetic pharmaceuticals.
c. Ethene
recognize that nucleic acids and proteins are important natural
polymers.
d. Ethyne

recognize that plastics formed from petrochemicals are organic
compounds that consist of long chains of carbons.
e. Ethanol

conduct a lab that exemplifies the versatility and importance of
organic compounds (e.g., aspirin, an ester, a polymer).


f. Formaldehyde
g. Benzene
CH 6 Problems
1. Which of the following polymers are naturally occurring?
a. Nylon
b. Protein
c. Polyester
d. Teflon
e. DNA
h. Acetic Acid