1.
Which of the following is a chemical change? a. Evaporation b. Freezing c. rusting d. Boiling
2.
Which of the following is NOT a physical property? a. flammability b. Melting point c. solubility d. density
3.
What is the difference between a homologous mixture and a heterogeneous mixture. Give an example of each.
4.
The diameter of a sulfur atom is 0.000 000 00 293 L. What is this number expressed in scientific notation?
5.
The diameter of a sulfur atom is 0.000 000 00 293 L. How many significant figures are there?
6.
How many significant figures are in the measurement 361.98 grams?
7.
What is the measurement 2039 L rounded off to three significant digits?
8.
What is the temperature of absolute zero measured in C?
9.
What is the density of an object with a mass of 25 g and a volume of 15 cm 3 ? Will this object float in water? Why or why not.
10.
All atoms of the same element have the same ____. a. number of neutrons b. number of protons
11.
Which of the following sets of symbols represents isotopes of the same element? a.
C C C c.
E E E b.
H H H c. mass numbers d. mass d.
M M M
12.
How do you figure out the number of neutrons in an atom using the periodic table?
13.
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements? (KNOW YOUR SCIENTITSTS!!!)
14.
In looking at the periodic table, which are there more of? Metals or Nonmetals?
15.
Of the elements Ti, Ag, K, and He, which is a nonmetal?
16.
What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p, 4s?
17.
What is the number of electrons in the outermost energy level of a nitrogen atom?
18.
What is the electron configuration of calcium?
19.
How many electrons does fluorine gain in order to achieve a noble-gas electron configuration?
20.
Know the difference between an ionic bond and a covalent bond.
21.
What is the shape of the water molecule? What is the shape of CO
2
?
22.
Which atom in a water molecule has the greatest electronegativity? (The oxygen atom or the hydrogen atoms?)
23.
Name the following polyatomic ions? HCO , CO , NO , SO , CrO , Cr O
24.
Write the formula for the following ions in a – d. (REMEMBER TO CRISS-CROSS IF NEEDED) a. Ca 2+ , F = b. Na , Cl
= c. Ba , O
= d. Pb , O
=
25.
Write the correct formula for the ionic compound in a – d. a. iron(III) sulfide c. tin(II) nitride b. aluminum fluoride d. potassium bromide
26.
Which set of chemical name and chemical formula for the same compound is correct? a. ammonium sulfite, (NH ) S c. lithium carbonate, LiCO b. iron(III) phosphate, FePO d. magnesium dichromate, MgCrO
27.
What is the formula for sulfurous acid?
28.
List the 7 diatomic molecules?
29.
How many moles of copper are in 4.8 10 atoms of copper?
30.
How many molecules are in 2.10 mol SO ?
31.
What is the molar mass of AgBr
3
?

32.
What is the volume (in liters) of one mole of a gas under STP conditions?
33.
What is the percent by mass of hydrogen in acetone, C H O?
34.
What is the empirical formula of C
8
H
24
O
64
?
35.
What is the empirical formula of a substance that is 52.2% C, 17.4% H, and 30.4% N by weight?
36.
Balance the following chemical equation?
CuCl + KOH Cu(OH) KCl
37.
In order for the reaction 2Fe 6HCl 2FeCl 3H to occur, which of the following must be true? a. Fe must be above Cl on the activity series. b. Fe must be above H on the activity series. c. Heat must be supplied for the reaction. d. A precipitate must be formed.
38.
Which of the following is a balanced equation representing the decomposition of tin (IV) oxide?
a. SnO Sn 2O c. Sn O 2Sn O b. SnO Sn O d. SnO Sn O
39.
A double-replacement reaction takes place when aqueous Na CO reacts with aqueous Sn(NO ) . What are the 2 products in this reaction?
40.
The equation Mg(s) 2HCl(aq) MgCl (aq) H g is an example of which type of reaction? (YOU MUST KNOW
THE 5 TYPES OF CHEMICAL REACTIONS!)
41.
Balance the following equation and determine what type of reaction this is:
S(s) + O (g) SO (g)
42.
Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 13.2 mol of aluminum?
2Al(s) + 3H SO (aq) Al (SO ) (aq) + 3H (g)
43.
The equation below shows the decomposition of lead (II) nitrate. How many grams of oxygen are produced when
12.7 g NO is formed?
44.
How many liters of NH are needed to react completely with 21.4 L of NO (at STP)?
4NH (g) + 6NO(g) 5N (g) + 6H O(g)
45.
Which of the following is NOT true about limiting and excess reagents? a. The amount of product obtained is determined by the limiting reagent. b. A balanced equation is necessary to determine which reactant is the limiting reagent. c. Some of the excess reagent is left over after the reaction is complete. d. The reactant that has the smallest given mass is the limiting reagent.
46.
How many liters of fluorine gas can be produced when 0.98 L of HF react with excess O at STP?
4HF(g) + O (g) 2F (g) + 2H O(g)
47.
Identify the limiting reagent and the volume of NO formed when 11 L NS reacts with 18 L O to produce NO gas and SO gas at STP.
NS (g) + 3O (g) NO (g) + 2SO (g)