Download Practice final questions

A little practice for the big final
____
1. Chemical properties
a. include changes of state of a substance.
b. include mass and color.
c. include changes that alter the identity of a substance.
d. can be observed without altering the identity of a substance.
____ 2. An example of a chemical change is
a. sanding wood.
c. milk going sour.
b. melting ice.
d. vaporizing gasoline.
____ 3. Physical means can be used to separate
a. elements.
c. mixtures.
b. pure substances.
d. compounds.
____ 4. Quantitative observations are recorded using
a. numerical information.
c. non-numerical information.
b. a control.
d. a system.
____ 5. The symbol for the metric unit used to measure mass is
a. m.
c. g.
b. mm.
d. L.
____ 6. What is the density of 37.72 g of matter whose volume is 6.80 cm3?
a. 0.18 g/cm3
c. 30.92 g/cm3
b. 5.55 g/cm3
d. 256.4 g/cm3
____ 7. 0.05 cm is the same as
a. 0.000 05 m.
b. 0.005 mm.
c. 0.05 m.
d. 0.5 mm.
____ 8. Five darts strike near the center of the target. Whoever threw the darts is
a. accurate.
c. both accurate and precise.
b. precise.
d. neither accurate nor precise.
____ 9. The number of significant figures in the measurement 170.040 km is
a. 3.
c. 5.
b. 4.
d. 6.
____10. Dalton's atomic theory did NOT explain the law of
a. whole-number ratios.
c. conservation of mass.
b. definite proportions.
d. conservation of energy.
____11. Isotopes are atoms of the same element that have different
a. principal chemical properties.
c. numbers of protons.
b. masses.
d. numbers of electrons.
____12. Zn-66 (atomic number 30) has
a. 30 neutrons.
b. 33 neutrons.
c. 36 neutrons.
d. 96 neutrons.
____13. The mass of a sample of nickel (atomic mass 58.69 amu) is 176.07 g. It contains
a. 1.7607  1024 atoms.
c. 5.869  1023 atoms.
b. 1.806  1024 atoms.
d. 5.869  1024 atoms.
____14. What does the 4 in
represent?
a. the mass number
b. the atomic number
c. the number of protons
d. the number of neutrons
____15. Balance the following equation:
+ _____ 
a.
c.
b.
d.
____16. The number of orbitals for the d sublevel is
a. 1.
c. 5.
b. 3.
d. 7.
____17. The Aufbau principle states that an electron
a. can have only one spin number.
b. occupies the lowest available energy level.
c. must be paired with another electron.
d. must enter an s orbital.
____18. The number of electrons in the highest energy level of the argon atom (atomic
number 18) is
a. 10.
c. 6.
b. 2.
d. 8.
____
19. Mendeleev is credited with developing the first successful
a. periodic table.
b. method for determining atomic number.
c. test for radioactivity.
d. use of X rays.
____20. The most reactive group of the nonmetals are the
a. lanthanides.
c. halogens.
b. transition elements.
d. rare-earth elements.
____21. A negative ion is known as a(n)
a. ionic radius.
b. valence electron.
c. cation.
d. anion.
____22. The number of valence electrons in Group 17 elements is
a. 7.
c. 17.
b. 8.
d. equal to the period number.
____23. A covalent bond results when ____ are shared.
a. ions
c. electrons
b. Lewis structures
d. dipoles
____24. What is the Lewis structure for carbon tetraiodide, which contains one carbon atom
and four iodine atoms?
a. A
c. C
b. B
d. D
____25. A polar molecule contains
a. ions.
b. a region of positive charge and a region of negative charge.
c. only London forces.
d. no bonds.
____26. What is the formula for the compound formed by lead(II) ions and chromate ions?
a. PbCrO4
c. Pb2(CrO4)3
b. Pb2CrO4
d. Pb(CrO4)2
____27. Name the compound Ni(ClO3)2.
a. nickel chlorate
b. nickel chloride
c. nickel chlorite
d. nickel peroxide
____28. Name the compound Hg2(NO3)2.
a. mercury(II) nitrate
b. dimercury dinitrate
c. mercury(I) nitrate
d. mercuric nitrate
____29. Name the compound N2O4.
a. sodium tetroxide
b. dinitrogen tetroxide
c. nitrous oxide
d. binitrogen oxide
____30. What is the percentage composition of CF4?
a. 20% C, 80% F
c. 16.8% C, 83.2% F
b. 13.6% C, 86.4% F
d. 81% C, 19% F
____31. Which equation is NOT balanced?
a. 2H2 + O2  2H2O
b. 4H2 + 2O2  4H2O
c. H2 + H2 + O2  H2O + H2O
d. 2H2 + O2  H2O
____32. In what kind of reaction do two or more substances combine to form a new
compound?
a. decomposition reaction
c. double-replacement reaction
b. ionic reaction
d. synthesis reaction
____33. In what kind of reaction do the ions of two compounds exchange places in aqueous
solution to form two new compounds?
a. synthesis reaction
c. decomposition reaction
b. double-replacement reaction
d. combustion reaction
____34. What is the balanced equation when aluminum reacts with copper(II) sulfate?
a. Al + Cu2S  Al2S + Cu
c. Al + CuSO4  AlSO4 + Cu
b. 2Al + 3CuSO4  Al2(SO4)3 +
d. 2Al + Cu2SO4  Al2SO4 + 2Cu
3Cu
1.
6.
11.
16.
21.
26.
31.
C
B
B
C
D
A
D
2.C
7.D
12.C
17.B
22.A
27.A
32.D
3.C
8.C
13.B
18.D
23.C
28.C
33.B
4.A
9.D
14.A
19.A
24.B
29.B
34.B
`
5.C
10.D
15.B
20.C
25.B
30.B