NAME ___________________________________________
PERIOD _________
DATE _________________________________
SAGE Review #2 Worksheet
Write A, B, C, or D on the blank next to each question. You will be graded on whether or not you are
correct. 20 points possible.
1. _____ Which of the following aqueous solutions has the lowest freezing point?
a. 1.0 M C6H12O6
c. 1.0 M CH3COOH
b. 1.0 M C2H5OH
d. 1.0 M NaCl
2. _____ If an equation is balanced properly, both sides of the equation should have the same
number of which of the following?
a. Moles of molecules
c. Coefficients
b. Molecules
d. Atoms
3. _____ According to this reaction: H2(g) + I2(g) → 2HI(g) + Heat. If the concentration of iodine (I2)
were increased, which of the following would happen as the reaction established equilibrium?
a. Less HI and heat would be produced
b. More H2 would be produced
c. The pressure of the reaction would increase
d. More HI and heat would be produced
4. _____ Which pair of atoms is held together by a covalent bond?
a. NaCl
c. HCl
b. LiCl
d. KCl
5. _____ A solid has a high melting point, is not soluble in water, conducts electricity, and is
malleable. What type of bonding is present in the solid?
a. Ionic
c. Metallic
b. Polar covalent
d. Covalent
6. _____ What is the molarity of a solution made with 128 g of magnesium chloride dissolved in
one liter of water?
a. 2.1 M
c. 1.34 M
b. 3.6 M
d. 5.0 M
7. _____ Which of the following would show up blue on a litmus test?
a. Baking soda
c. Soda
b. Tomato
d. Coffee
8. _____ When compared to H2S, H2O has a higher boiling point because H2O contains stronger
what?
a. Hydrogen bonds
c. Covalent bonds
b. Metallic bonds
d. Ionic bonds
9. _____ A student observed that when sodium hydroxide was dissolved in water the temperature
of the water increased. The student should conclude that the dissolving of sodium hydroxide:
a. Is endothermic
c. Produces an acid solution
b. Is exothermic
d. Produces a salt solution
10. _____ Which type of bond is formed when an atom of potassium transfers an electron to a
bromine atom?
a. Metallic
c. Nonpolar covalent
b. Ionic
d. Polar covalent
11. _____ What element is the most abundant in the universe?
a. Oxygen
c. Helium
b. Hydrogen
d. Carbon
12. _____ The Rutherford Model of the atom was created using a gold foil experiment. What did
this experiment show?
a. That the electrons spin outside the nucleus.
b. That the nucleus is small but dense and the atom is mostly empty space.
c. That the protons are equal in mass to the neutrons.
d. That the atom is far smaller than gold.
13. _____ Which of the following elements would you expect to have similar reactive properties to
magnesium?
a. Iron
c. Strontium
b. Nickel
d. Cadmium
14. _____ Which of the following colors of visible light has the longest wavelength?
a. Orange
c. Green
b. Yellow
d. Blue
15. _____ Nuclear emissions occur when which of the following changes happen in an atom?
a. Electrons move to higher energy levels
b. Electrons move to lower energy levels
c. Changes occur in the nucleus
d. No changes need to occur
16. _____ When an atom loses an electron, the atom becomes an ion that is:
a. Positively charged and loses an insignificant amount of mass
b. Positively charged and gains an insignificant amount of mass
c. Negatively charged and gains an insignificant amount of mass
d. Negatively charged and loses an insignificant amount of mass
17. _____ Given the equation: H2(g) + Cl2(g) → 2HCl(g). What is the total number of moles of HCl(g)
produced when 3 moles of H2(g) are completely consumed?
a. 5 moles
c. 6 moles
b. 2 moles
d. 3 moles
18. _____ Which of the following is true of the water molecule?
a. Bent shape and polar
c. Linear shape and polar
b. Bent shape and nonpolar
d. Linear shape and nonpolar
19. _____ What is the structure of a krypton-85 atom?
a. 49 e-, 49 p+, 85 n
c. 36 e-, 36 p+, 85 n
b. 49 e-, 49 p+, 49 n
d. 36 e-, 36 p+, 49 n
20. _____ A student could identify that a certain element is present by:
a. The color of a flame test
c. Neither choices
d. Both choice
b. The emissions spectrum