Fall Semester Summary Review
Be able to define the following vocabulary terms:
Chapter 1:
Chemistry
Hypothesis
Quantitative
Observation
Theory
Inference
Natural Law
Scientific Method
Qualitative
Chapter 2:
Matter
Element
Physical Property
Mixture
Heterogeneous Mixture
Atom
Solid
Chemical Property
Alloy
Distillation
Compound
Liquid
Physical Change
Homogeneous Mixture
Filtration
Molecule
Gas
Chemical Change
Solution
Chapter 3:
Atomic Theory
Proton
Mass Number
Alkaline Earth Metals
Metals
Ion
Chemical Formula
Nucleus
Period
Halogens
Nonmetals
Cation
Electron
Isotope
Family
Noble Gases
Metalloids
Anion
Neutron
Atomic Number
Alkali Metals
Transition Metals
Diatomic Molecule
Chapter 7:
Chemical Reaction
Chemical Equation
Reactants
Products
Chapter 8:
Precipitate
Complete Ionic Equation
Decomposition Reaction
Aqueous Solution
Net Ionic Equation
Combustion Reaction
Soluble Solid
Spectator Ions
Single Replacement RXN
Insoluble Solid
Synthesis Reaction
Double Replacement
Chapter 11:
Photons
Configuration
Actinides
Wave Mechanical Model
Orbital Diagram
Atomic Radius
Orbital
Valence Electrons
Ionization Energy
Electron
Lanthanides
Bond Energy
Nonpolar Covalent
Unshared Electron Pairs
Ionic Bond
Electronegativity
Resonance
Covalent Bond
Lewis Dot Structure
Molecular Structure
Chapter 12:
Bond
Polar Covalent Bond
Octet Rule
VESPR
Practice Problems:
Chapter 1:
1) Which of the following is another term for quantitative observation?
a. Theory
b. Measurement
c. Hypothesis
d. Natural Law
Use the information in the following paragraph for questions 2 – 4.
Ronika and Thomas are eating raisins and drinking ginger ale. Thomas accidentally drops a raisin into his ginger
ale. Both he and Ronika notice that the raisin falls to the bottom of the glass. Soon, the raisin rises to the surface
of the ginger ale, and then sinks again. Within a couple of minutes, it rises and sinks again. Ronika asks “I don’t
know, but let’s see if it works in water.” Ronika fills a glass with water and drops a raisin into the glass. After a few
minutes, Thomas says, “No, it doesn’t go up and down in the water.” Ronika closely observes the raisins in the two
cups and states, “Look, there are bubbles on the raisin in the ginger ale but not on the raisin in the water.” Thomas
says “It must be the bubbles that make the raisin rise.” Ronika asks, “OK, but then why does it sink again?”
2) Which of the following items from the passage is an observation?
a. Accidentally dropping the raisin into the ginger ale
b. Claiming that the bubbles make the raisin rise
c. Asking “I wonder why that happened?”
d. Noticing the raisin sinks in the ginger ale
3) Which of the following from the passage is a hypothesis?
a. Asking “I wonder why that happened?”
b. Noticing that the raisin does not rise and sink in the water
c. Claiming that the bubbles make the raisin rise
d. Wondering why the raisin sinks after it rises to the surface of the ginger ale
4) Which of the following from the passage is an experiment?
a. Claiming that the bubbles make the raisin rise
b. Dropping a raisin into water
c. Asking “I wonder why that happened?”
d. Wondering why the raisin sinks after it rises to the surface of the ginger ale
For questions 5-8, label each of the following statements as true or false. Provide an explanation for the
statements that are false.
5) We can prove a theory to be correct by performing the right experiment.
6) If a theory is accepted for a long time, it eventually becomes a law.
7) A law is a summary of observed behavior.
8) A theory is an attempt to explain what happens in an experiment.
Chapter 2:
9) Copper is a reddish-brown metal that is easily stretched to make wires. These characteristics are examples of
__________ properties of copper.
10) When copper metal is heated in concentrated nitric acid, the copper dissolves to form a deep blue solution,
and a brown gas is evolved from the acid. These characteristics are examples of __________ changes.
Classify the following as physical changes, chemical changes, physical properties, and/or chemical properties.
11) An iron scorches a shirt when you leave it on one spot too long.
12) The tires on your car seem to be getting low in very cold weather.
13) Your grandmother’s silver tea set gets black with tarnish over time.
14) Acids produced by bacteria in plaque cause teeth to decay.
15) Hydrogen peroxide (H2O2) fizzes when applied to a wound.
16) Dry ice evaporates without melting as time passes.
17) Which of the following is an element?
a. Air
b. Water
c. Salt
d. Helium
18) Which of the following describes a physical change?
a. Cookies burn in the oven
c. sugar dissolves in coffee
b. A banana ripens
d. leaves turn colors in the fall
19) Which of the following is a chemical change?
a. Water condenses on a mirror
c. a damp towel dries
b. A nail rusts
d. peanuts are crushed
20) Consider the following substances: sodium, sugar, air, iron. How many are pure compounds?
a. 1
b. 2
c. 3
d. 4
21) A homogeneous mixture is also called _____.
a. A heterogeneous mixture
c. a compound
b. A pure substance
d. a solution
22) Which of the following processes requires chemical methods?
a. Separating a homogeneous mixture into pure substances
b. Breaking a compound into its constituent elements
c. Separating a heterogeneous mixture into pure substances
d. Distilling a saltwater mixture
Chapter 3:
23) Which element includes the first letter of its name as the first letter of the symbol for the element?
a. Potassium
b. lead
c. copper
d. sodium
24) Which of the following postulates of Dalton’s atomic theory is no longer scientifically accepted?
a. All matter is made up of atoms
b. All atoms of the same element are identical
c. Compounds are combinations of different atoms
d. A chemical reaction changes the way atoms a
25) Consider isotopes, ions, protons, and electrons. How many of these did Dalton NOT discuss in his atomic
theory?
a. 1
b. 2
c. 3
d. 4
26) Which of the following represents a pair of isotopes?
a. 23Na and 23Na+
c. 14C and 12C
b. 14C and 14N
d. 16O and 16O227) An ion is formed
a. Either by adding or by taking away protons from the atom
b. Either by adding or by taking away electrons from the atom
c. Either by adding or by taking away neutrons from the atom
d. At least two of the above statements correctly explain how an ion is formed
28) How many protons and electrons does the most stable ion for oxygen have?
a. 10 protons, 8 electrons
c. 8 protons, 10 electrons
b. 8 protons, 8 electrons
d. 6 protons, 8 electrons
29) A certain ion has a charge of 2+ and 27 electrons. Which ion is it?
a. Mn2+
b. Cu2+
c. Co2+
d. Ga2+
30) You are given a compound with the formula CaX2, in which X is a nonmetal. You are told that the nonmetal ion
has 10 electrons. What is the symbol of the nonmetal?
a. F
b. Cl
c. O
d. Ne
31) Be able to describe Ernest Rutherford’s gold foil experiment.
Chapter 4:
32) Write the proper chemical name for each combination of cations and anions made from table below.
(You will want to do the table, or names, on a separate sheet of paper.)
IONS
Fe2+
Al3+
Na+
Ca2+
NH4+
Fe3+
Ni2+
CO32OHPO43SO32SO42O2Cl33) Write the proper chemical formula for each combination of ions made from the table below.
(You will want to do the table, or formulas, on a separate sheet of paper.)
IONS
Nitrate
Sulfate
Oxide
Calcium
Ammonium
Aluminum
Iron (III)
Silver
Gold (III)
Potassium
34) When dihydrogen sulfide is dissolved in water, it is called
a. Sulfuric acid
b. sulfurous acid
c. hydrosulfuric acid d. dihydrosulfuric acid
Chapter 7:
35) Which of the following is not a clue that a chemical reaction has taken place?
a. A solid is formed when two clear solutions are mixed
b. A clear solution is added to a red solution, and the result is a blue solution
c. A solid is added to water, and bubbles form
d. A pure solid is heated and turns into a pure liquid
36) What does it mean for a chemical equation to be balanced?
a. The sums of the coefficients on each side of the equation are equal
b. The same number of each type of atom appears on both sides of the equation
c. The formulas of the reactants and the products are the same
d. The sums of the subscripts on each side of the equation are equal
Chloride
37) Which of the following physical states is not used for H2O in a chemical equation?
a. (s)
b. (l)
c. (g)
d. (aq)
38) Which of the following is the coefficient for O2 when the equation is balanced?
C4H10(l) + O2(g)  CO2(g) + H2O(g)
a. 4
b. 8
c. 10
d. 13
39) What is the SUM of the coefficients of the following equation when it is balanced?
FeS(s) + HCl(g)  FeCl2(s) + H2S(g)
a. 5
b. 4
c. 3
d. 2
40) When the equation representing the reaction between iron (II) oxide and carbon to form iron and carbon
dioxide is balanced, the coefficient for iron is
a. 1
b. 2
c. 3
d. 4
Write and balance the chemical equations for the following 3 problems.
41) When magnesium metal is added to water, hydrogen gas is produced along with a solution of magnesium
hydroxide.
42) When an aqueous solution of lead (II) nitrate is added to an aqueous solution of sodium iodide, the yellow
solid lead (II) iodide is produced along with a solution of sodium nitrate.
43) Propane gas (C3H8) reacts with oxygen in the air to form carbon dioxide and water vapor.
Chapter 8:
For each of the following two reactions, write the balanced molecular equation,
44) Aqueous sodium chloride is added to aqueous silver nitrate to form solid silver chloride plus aqueous sodium
nitrate.
45) Aqueous potassium hydroxide is mixed with aqueous iron (III) nitrate to form solid iron (III) hydroxide and
aqueous potassium nitrate.
Predict whether each of the following will be soluble in water.
46) Potassium nitrate
47) Zinc hydroxide
48) Calcium carbonate
49) Ammonium chloride
Chapter 11:
50) How many electrons can be contained in all of the orbitals with a principal energy level of 3 (n=3)?
a. 8
b. 10
c. 18
d. 32
51) In general, the rows on the periodic table correspond to ________ and the columns numbered 1A, 2A,…8A
correspond to ________.
a. The orbital of the valence electrons; the number of total electrons
b. The energy level of the valence electrons; the number of valence electrons
c. The energy level for the core electrons; the orbital of the valence electrons
d. The number of valence electrons; the energy level of the valence electrons
52) An orbital is best described as
a. The pathway for an electron
c. the space in which only valence electrons exist
b. The region of probability of finding an electron d. a physical structure which holds the electrons
c.
53) Which of the following is true about the trend of ionization energy across a row on the periodic table?
a. Ionization energy generally increases to the right because the number of protons increases from left
to right
b. Ionization energy generally decreases to the right because the number of electrons increases from left
to right
c. Ionization energy generally decreases to the right because the number of protons increases from left
to right
d. Ionization energy is constant since all atoms in a row have the same valence energy level
54) For the atoms Li, N, F, and Na, which of the following is the correct order from smallest to largest atomic radius?
a. Na, F, N, Li
b. Na, Li, N, F
c. N, F, Na, Li
d. F, N, Li, Na
55) Which of the following correctly ranks the ionization energies of O, F, Na, S, and Cs from smallest to largest?
a. Cs, Na, S, O, F b. Cs, S, Na, O, F
c. F, O, Na, S, Cs
d. F, O, S, Na, Cs
56) Write the electron configuration for iron.
57) Write out the orbital diagram for oxygen.
Chapter 12:
58) Which of the following atoms is the most electronegative?
a. Na
b. P
c. Cl
d. I
59) Which of the following is true concerning trends on the periodic table?
a. In general, smaller atoms have larger ionization energies and smaller electronegativity values
b. In general, smaller atoms have smaller ionization energies and smaller electronegativity values
c. In general, smaller atoms have smaller ionization energies and larger electronegativity values
d. In general, smaller atoms have larger ionization energies and larger electronegativity values
60) Diatomic molecules that are formed from two different types of nonmetal atoms generally from ________.
a. Ionic bonds
c. nonpolar covalent bonds
b. Polar covalent bonds
d. no bonds
61) Which of the following does not have a noble gas electron configuration?
a. The Na+ ion
b. the Mg2+ ion
c. the S2- ion
d. the Fe3+ ion
2 2
6 2
6
62) The electron configuration 1s 2s 2p 3s 3p is the correct electron configuration for the most stable form of
which ion?
a. The calcium ion
c. the fluoride ion
b. The magnesium ion
d. the oxide ion
63) What is the expected ground state electron configuration for the most stable ion of bromine?
a. [Ar] 4s23d104p5
c. [Ar] 4s24d104p6
b. [Ar] 4s23d104p6
d. [Ar] 4s24d104p5
64) How many resonance structures can be drawn for the carbonate ion?
a. 1
b. 2
c. 3
d. 4
65) Be able to identify the following molecular shapes:
Linear, bent, trigonal planar, trigonal pyramidal, tetrahedral