1. science
2. chemistry

Honors Chemistry: MIDTERM REVIEW
The midterm consists of 60 multiple choice questions and two open responses.
Covers all content in Terms 1 & 2 including Chapters 1, 2, 3, 4, 5, 6, & 7.
Chapter 1–Chemistry: An Introduction
Objectives:
◦ To understand the importance of learning chemistry (Section 1.1)
◦ To define chemistry (Section 1.2)
◦ To understand scientific thinking (Section 1.3)
◦ To describe the method scientists use to study nature (Section 1.4)
◦ To develop successful strategies for learning chemistry (Section 1.5)
1. What is chemistry? Give a definition.
2. What is a theory? Give a definition.
3. Give two examples of scientific theories.
4. What is the difference between qualitative and quantitative
observations? Give an example of each.
5. Give an example of a natural law.
6. Explain what is meant by the term hypothesis, and give an example of one in either everyday
life or in chemistry.
Chapter 2 – Measurements and Calculations
Objectives:
◦ Expressing very large or very small numbers as the product of a number between 1 and 10 and a
power of 10 (Section 2.1)
◦ Learning the English, metric, and SI systems of measurement (Section 2.2)
◦ Understanding the metric system for measuring length, volume, and mass (Section 2.3)
◦ Understanding how uncertainty in a measurement arises (Section 2.4)
◦ Indicating a measurement's uncertainty by using significant figures (Section 2.4)
◦ Determining the number of significant figures in a calculated result (Section 2.5)
◦ Using dimensional analysis to solve various types of problems (Section 2.6)
◦ Learning the three temperature scales (Section 2.7)
◦ Converting from one scale to another (Section 2.7)
◦ Continuing to develop problem-solving skills (Section 2.7)
◦ Defining density and its units (Section 2.8)
Honors Chemistry: Review for Midterm (pg. 2 of 15)
Basic Conversion Problems and Significant Figures
1. How many digits are significant in each of the following measurements?
a. 0.000230
b. 1000
c. 1000.
d. 3.01 x 10-5
e. 804.4900
f. 0.020600
REMINDER: Determining Significant Figures in Calculations
A. Multiplication and Division:
a. The number of significant figures in your answer should be the same as the
measurement with the smallest number of significant figures
i. Example: 4.56 x
1.4
= 6.384 
6.4
3 SF
2 SF
Round result to 2 SF
B. Addition and Subtraction
b. The measurement with the fewest number of decimal places will determine how
many decimal places are in your result.
i. Example: 12.11 + 18.0 +
1.013 =
13.123  31.1
2 places 1 place
3 places Round result to 1st place (tenth)
2. Perform the following calculations and report your answer to the correct number of significant
figures:
a. 5.19 + 1.9 + 0.842
b. 1081 – 7.25
c. 2.3 x 3.14
d. 8.63 / 4.521
e. (1.33 x 2.8) + 8.41
f. (3.5 – 1.23) / 0.54
3. Perform the following conversions:
a. 55 mL to L
b. 2300 m to cm
c. 0.35 km to cm
d. 2 m3 to cm3
Honors Chemistry: Review for Midterm (pg. 3 of 15)
4. A volume of 1 mL is equivalent to
a. 1 cm3
b. 1 cm2
c. 1 dL
d. 1 mm3
5. The equivalent of 2.54 cm3 in units of in3 is
a. 1.00 in3
b. 2.54 in3
c. 6.45 in3
d. 16.4 in3
6. While driving in London you encounter a speed limit sign that reads 80 km/hr. How fast can
you legally travel in miles/hr?
a. 80
b. 70
c. 60
d. 50
7. Mercury is the only metal known to exist as a liquid at room temperature and pressure. It has
a very high density of 13.6 g/mL. Convert the density of mercury into units of lbs/in3.
8. The normal body temperature for a dog is approximately 102oF.
What is this equivalent to on the Kelvin temperature scale?
a. 373 K
b. 312 K
c. 289 K
d. 202 K
9. If I sleep 8 hours per day and I live to be 100 years old, how many years have I slept?
Chapter 3 – Matter
Objectives:
◦ To learn about matter and its three states (Section 3.1)
◦ To learn to distinguish between physical and chemical properties
(Section 3.2)
◦ To learn to distinguish between physical and chemical changes
(Section 3.2)
◦ To understand the definitions of elements and compounds
(Section 3.3)
◦ To learn to distinguish between mixtures and pure substances
(Section 3.4)
◦ To learn two methods of separating mixtures (Section 3.5)
Honors Chemistry: Review for Midterm (pg. 4 of 15)
Chemical vs. Physical Changes, Isotopes, Determining the number of Protons, Neutrons, and
Electrons in an atom
1. Describe the ways to tell if a chemical reaction has occurred.
2. Explain why undergoing a change in state (solid, liquid, gas) is a physical change.
3. In order to break down water into its constituent elements, water would have to undergo
a. distillation
b. fusion
c. chemical change
d. physical change
4. A mixture has a __________ composition, whereas a compound always has a _________
composition.
a. pure; complex
b. complex; pure
c. constant; variable
d. variable; constant
5. The brass in what might be a favorite candlestick is classified as a(n)
a. pure substance
b. element
c. heterogeneous mixture
d. homogeneous mixture
6. The brass in the ornamental tray you might use to serve guests could be classified as a(n)
a. solution
b. element
c. compound
d. pure substance
7. To separate a sand-saltwater mixture into pure substances one would have to employ
a. electrolysis
b. filtration
c. distillation
d. filtration followed by distillation
8. Pure substances consist of either
a. elements or compounds
b. elements or mixtures
c. elements or solutions
d. elements or energy
Honors Chemistry: Review for Midterm (pg. 5 of 15)
9. Decide whether each of the following scenarios involves a chemical or a physical change.
- Zinc when immersed in hydrochloric acid produces hydrogen gas.
- A nail rusts.
- A piece of paper burns.
- Water boils at 100 degrees Celsius
- Liquid nitrogen freezes a solid rubber ball
Chapter 4 – Chemical Foundations: Elements, Atoms, and Ions &
Chapter 19—Radioactivity and Nuclear Energy
Objectives:
◦ To learn about the relative abundances of the elements (Section 4.1)
◦ To learn the names of some elements (Section 4.1)
◦ To learn the symbols of some elements (Section 4.2)
◦ To learn about Dalton's theory of atoms (Section 4.3)
◦ To understand and illustrate the law of constant composition (Section 4.3)
◦ To learn how a formula describes a compound’s composition (Section 4.4)
◦ To learn about the internal parts of an atom (Section 4.5)
◦ To understand Rutherford's experiment to characterize the atom’s structure (Section 4.5)
◦ To understand some important features of subatomic particles (Section 4.6)
◦ To learn about the terms isotope, atomic number, and mass number (Section 4.7)
◦ To understand the use of the symbol to describe a given atom (Section 4.7)
◦ To learn the types of radioactive decay (Section 19.1)
◦ To learn to write nuclear equations that describes radioactive decay (Section 19.1)
1. The two most abundant elements in the earth’s crust, although they occur as parts of
compounds, are
a. nitrogen and oxygen
b. silicon and oxygen
c. nitrogen and silicon
d. carbon and oxygen
2. Which of the following is one of the statements that make up Dalton’s atomic theory?
a. All atoms contain electrons.
b. All atoms of a given element are identical.
c. Atoms are divisible.
d. Atoms gain and lose electrons in chemical reactions.
3. The pesticide known as DDT paralyzes insects by binding to their nerve cells, leading to
uncontrolled firing of the nerves. Before most uses of DDT were banned in the U.S., many
insects had developed a resistance to it. Write out the formula for DDT. It contains 14 carbon
atoms, 9 hydrogen atoms, and 5 atoms of chlorine.
Honors Chemistry: Review for Midterm (pg. 6 of 15)
4. The scientist who used alpha particles to bombard a thin film of gold, and proposed that most
of the volume of an atom is empty space because most of the alpha particles went straight
through the film:
a. Rutherford
b. Kelvin
c. Thomson
d. Dalton
5. Thomson discovered the electron when experimenting with
a. radioactive elements
b. alpha particles
c. thermometers
d. cathode ray tubes
6. The chemical properties of a particular element are largely determined by the number of
__________ an atom of that element possesses.
a. protons
b. neutrons
c. electrons
7. Lead-210 is used in radioactive dating of sediment cores. The number of protons, electrons,
and neutrons in an atom of lead-210 respectively is variable
a. 82, 82, 128
b. 210, 82, 128
c. 128, 128, 82
8. Positive ions, known as __________ can be formed when a metal atom gives up one or more
__________ to a nonmetal, which simultaneously forms a negatively charged ___________.
a. cations, electrons, anion
b. anions, electrons, cation
c. cations, electrons, allotrope
d. isotopes, electrons, cation
9. The periodic table is very helpful in assisting in figuring out the charge an atom is likely to have
if it accepts or loses electrons to form an ion. When halogens, as typical nonmetals, _____
electrons, they always form ions with a charge of ____.
a. give up, 2b. accept, 1c. give up, 2+
d. accept, 2+
Honors Chemistry: Review for Midterm (pg. 7 of 15)
10. When aluminum foil is dropped into liquid bromine the ionic compound aluminum bromide
forms. This compound’s formula is
a. AlBr
b. AlBr2
c. AlBr3
d. Al3Br
11. 60.11% of Ga has a mass number of 69, the rest have a mass number of 71. Calculate the
average atomic mass.
12. Complete the following chart:
Element Symbol
Fe
Atomic Number
Mass
# Neutrons # Electrons
Number
Charge
25
3
84
105
-2
54
135
106
104
265
# Protons
Sb
13. Define isotope:
14. Identify the number of protons, neutrons, and electrons in the atom 13O -2.
15. What are the relative masses of a proton, neutron, and an electron in amu?
16. Identify the number of each type of atom in the following compound. (How many Ca atoms
are there? How many O atoms are there? etc.)
Ca2(PO4)3
Ca:
P:
O:
17. Write a balanced equation for the following radioactive decay processes:
a. alpha decay of uranium-238
b. nitrogen-13 undergoes beta decay
18. What type of radioactive particle does NOT have a charge?
Honors Chemistry: Review for Midterm (pg. 8 of 15)
19. What is an alpha particle?
20. What is a beta particle?
Chapter 5 – Nomenclature
Objectives:
◦ To understand why it is necessary to have a system for naming compounds (Section 5.1)
◦ To learn to name binary compounds of a metal and a nonmetal (Section 5.2)
◦ To learn how to name binary compounds containing only nonmetals (Section 5.3)
◦ To review the naming of Type I, Type II, and Type III binary compounds (Section 5.4)
◦ To learn the names of common polyatomic ions and how to use them in naming compounds
(Section 5.5)
◦ To learn how the anion’s composition determines the acid’s name and to learn names for common
acids (Section 5.6)
◦ To learn how to write the formula of a compound given its name.
Naming and Writing Formulas
1)
H2SO3______________________________________________
2)
HC2H3O2 ______________________________________________
3)
P2O5 ______________________________________________
4)
Co2(Cr2O7)3 ______________________________________________
5)
MnSO4 ______________________________________________
6)
H2CO3 ______________________________________________
7)
NiHPO4 ______________________________________________
8)
FePO4 ______________________________________________
9)
SF6 ______________________________________________
10)
C5H10 ______________________________________________
11)
Ca3N2 ______________________________________________
12)
HClO2 ______________________________________________
13)
CuOH ______________________________________________
14)
Sn(CO3)2 ______________________________________________
Honors Chemistry: Review for Midterm (pg. 9 of 15)
15)
H2SO4 ______________________________________________
16)
IF7 _______________________________________________
17)
HClO________________________________________________
18)
H2O ______________________________________________
19)
Cs2Se ______________________________________________
20)
HI ______________________________________________
Write the formula:
21)
zinc dichromate __________________
22)
barium hydroxide __________________
23)
hydrochloric acid __________________
24)
silver nitrate __________________
25)
perchloric acid __________________
26)
tricarbon octahydride __________________
27)
phosphoric acid __________________
28)
strontium oxide __________________
29)
chlorous acid__________________
30)
calcium hydrogen phosphate __________________
31)
aluminum acetate __________________
32)
manganese (II) hydrogen sulfate __________________
33)
strontium cyanide __________________
34)
ammonium selenide __________________
35)
carbonic acid __________________
36)
chloric acid __________________
37)
sulfurous acid __________________
Honors Chemistry: Review for Midterm (pg. 10 of 15)
38)
phosphorus pentachloride __________________
39)
Tin (II) carbonate __________________
40)
Tin (IV) sulfite __________________
Chapter 6 – Chemical Reactions: An Introduction
Objectives:
◦ To learn the signals that show a chemical reaction has occurred (Section 6.1)
◦ To learn to identify the characteristics of a chemical reaction and the information given by a
chemical equation (Section 6.2)
◦ To learn how to write a balanced equation for a chemical reaction (Section 6.3)
1. Which of the following indicates that a chemical reaction has occurred?
a. Liquid water boils to produce steam.
b. Burning firewood give off heat.
c. Mixing two colorless liquids produce a bright yellow solid.
d. Solid NaHCO3 dissolves in water.
2. Why is it important that chemical equations be balanced?
3. Count the number of each kind of atom on both sides of the equation, and decide which
reactions are balanced and which are not.
a. H2 + Br2  HBr
b. KClO3  KCl + O2
c. 2NaOH + CO2  Na2CO3 + H2O
d. C2H5OH + 3O2  2CO2 + 3H2O
e. 3Cu + HNO3  3Cu(NO3)2 + NO + H2O
4. Use the following word descriptions to write unbalanced chemical equations showing the
formulas of reactants and products. Make sure you include the physical states of reactants
and products.
a. Solid iron metal reacts with oxygen in the atmosphere to form rust, iron (III) oxide.
Honors Chemistry: Review for Midterm (pg. 11 of 15)
b. Solid magnesium metal reacts with aqueous hydrochloric acid to produce hydrogen gas
and an aqueous solution of magnesium chloride.
c. Solid silver oxide decomposes upon heating to produce solid silver metal and oxygen gas.
d. Aqueous sodium hydroxide reacts with aqueous nitric acid to produce aqueous sodium
nitrate and liquid water.
5. Balance these chemical equations. Check your work by counting the number of each kind of
atom on both sides of the equation.
a.
KOH(aq) + H2S(aq)  K2S(aq) + H2O(l)
b.
HNO2(aq)  N2O3(g) + H2O(l)
c.
NaOH(aq) + H2SO4(aq)  Na2SO4(aq) + H2O(l)
d.
(NH4)2S(aq) + Pb(NO3)2(aq)  PbS(s) + NH4NO3(aq)
e.
Al(s) + O2(g)  Al2O3(s)
Chapter 7 – Reactions in Aqueous Solutions
Objectives:
◦ To understand some of the factors that cause reactions to occur (Section 7.1)
◦ To identify the solid that forms in a precipitation reaction (Section 7.2)
◦ To describe reactions in solutions by writing molecular, complete ionic and net ionic equations
(Section 7.3)
◦ To identify the characteristics of the reactions between strong acids and strong bases (Section 7.4)
◦ To describe the general characteristics of a reaction between a metal and a nonmetal (Section 7.5)
◦ To describe electron transfer as a driving force for a chemical reaction (Section 7.5)
◦ To identify various classification schemes for reactions (Section 7.6)
◦ To learn additional classes of chemical reactions (Section 7.7)
1. Which of the following is a common driving force for a reaction (something that makes the
reaction occur)?
a. Formation of a solid
b. Formation of a gas
c. Formation of water
d. All of the above
Honors Chemistry: Review for Midterm (pg. 12 of 15)
2. A reaction in which a solid is formed is referred to as a(n) _______ reaction.
a. electrolyte
b. precipitation
c. solidification
d. decomposition
3. When drilling irrigation wells in coastal areas, the salinity of the well water is always of
concern because of the negative impact of salt water on vegetation. One common way of
testing water for salinity is to add a solution of AgNO3 to a sample of the well water. If the
concentration of salt is too high, a precipitate will form. Write the equation for the reaction of
silver nitrate with sodium chloride and determine the identity of the precipitate using the
solubility rules.
Reaction Types: Predicting the Products of a Reaction and applying Solubility Rules
For each of the following reactions, translate and balance the equation. Then write the reaction type
next to the balanced equation. (NOTE: Some synthesis reactions may also be considered an
oxidation-reduction reaction)
1. Solid iron (III) and hydrochloric acid gas react
Reaction type:
2. calcium hydroxide (aq) and nitric acid (aq)
Reaction type:
Write the net ionic equation for the reaction:
3. calcium hydroxide (aq) + potassium carbonate (aq) 
Reaction type:
Write the net ionic equation for the reaction:
Honors Chemistry: Review for Midterm (pg. 13 of 15)
4. Iron (III) metal + oxygen 
Reaction type:
5. dicarbon hexahydride + oxygen 
Reaction type:
6. aluminum hydroxide (aq) + hydrochloric acid (aq) 
Reaction type:
7. What is an acid base reaction? What are the products of an acid base reaction?
8. What is a precipitate?
9. What happens to the ions in a double replacement reaction that do not form a precipitate?
10. What happens to electrons in a red-ox reaction?
11. Circle the compounds that ARE SOLUBLE in water:
a. ammonium carbonate
b. iron (III) sulfide
c. iron (III) sulfate
d. silver nitrate
e. silver chloride
f. barium chlorate
Honors Chemistry: Review for Midterm (pg. 14 of 15)
12. Circle the compounds that are NOT soluble in water:
a. sodium phosphate
b. lead (II) nitrate
c. calcium carbonate
d. barium sulfate
e. aluminum sulfate
f. barium phosphate
g. lead (II) acetate
13. Mixing which of the pairs of solutions listed below will result in the formation of a precipitate?
a. NaCl + K2CO3
b. NaOH + Mg(NO3)2
c. KCl + Ba(NO3)2
d. Na2S + KNO3
14. When a piece of aluminum foil is added to a container of liquid bromine a white salt forms.
Write out the balanced equation for the reaction and indicate which element is reduced and
which is oxidized in the reaction.
15. The oxidation-reduction reaction that furnishes the energy to launch the space shuttle via the
solid-fuel rockets is represented below:
3NH4ClO4(s) + 3Al(s)
Al2O3(s) +AlCl3(s) + 3NO(g) + 6H2O(g) + energy
The element that is oxidized in the reaction is
a. N
b. Cl
c. O
d. Al
16. The reaction between hydrogen and oxygen to form water
2H2O
2H2 + O2 
can be classified as a(n) ___________ reaction.
a. oxidation–reduction
b. synthesis
c. combustion
d. all of the above
OTHER Random Bits of Information you should know!!!
- Know the basic terminology of laboratory equipment (funnel, flask, etc).
- Know the definition of a calorie
- Know the charge on ions in their ionic compounds.
o Example: Identify the charge on the following ions in their ionic compounds:
1. K
4. Se
2. Sr
5. Cl
3. P
Honors Chemistry: Review for Midterm (pg. 15 of 15)
How To Study For the Midterm:
-
Organize and review your Chemistry Binder. This is your learning guide for honors chemistry.
Do all of the practice questions in the study guide and check your answers
Review topics that you have trouble with by looking back at your notes for that section,
retrying homework problems that were assigned, reviewing Note Sheets and Problem Sheets.
If you want some extra help, you need to come to me with VERY SPECIFIC QUESTIONS!! I am
here to help you, but I will not respond to “I don’t get anything!!”.
I EXPECT YOU TO STUDY (for more than 45 minutes!!) FOR THIS EXAM. THE MIDTERM IS 7.5%
OF YOUR GRADE. YOU CAN NOT EXPECT TO BE SUCCESSFUL WITHOUT STUDYING!!!!!!
GOOD LUCK!!!!!