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/cm3b. / 5.55 g/cm3 / d. / 256.4 g/cm3
____ 7. 0.05 cm is the same as
a. / 0.000 05 m. / c. / 0.05 m.b. / 0.005 mm. / 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. / c. / 36 neutrons.b. / 33 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 / c. / the number of protonsb. / the atomic number / 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. / c. / cation.b. / valence electron. / 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. / electronsb. / 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. / Cb. / 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)3b. / Pb2CrO4 / d. / Pb(CrO4)2
____ 27. Name the compound Ni(ClO3)2.
a. / nickel chlorate / c. / nickel chloriteb. / nickel chloride / d. / nickel peroxide
____ 28. Name the compound Hg2(NO3)2.
a. / mercury(II) nitrate / c. / mercury(I) nitrateb. / dimercury dinitrate / d. / mercuric nitrate
____ 29. Name the compound N2O4.
a. / sodium tetroxide / c. / nitrous oxideb. / dinitrogen tetroxide / d. / binitrogen oxide
____ 30. What is the percentage composition of CF4?
a. / 20% C, 80% F / c. / 16.8% C, 83.2% Fb. / 13.6% C, 86.4% F / d. / 81% C, 19% F
____ 31. Which equation is NOT balanced?
a. / 2H2 + O2 ® 2H2Ob. / 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 reactionb. / 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 reactionb. / 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 + Cub. / 2Al + 3CuSO4 ® Al2(SO4)3 + 3Cu / d. / 2Al + Cu2SO4 ® Al2SO4 + 2Cu
1. C 2.C 3.C 4.A 5.C
6. B 7.D 8.C `9.D 10.D
11. B 12.C 13.B 14.A 15.B
16. C 17.B 18.D 19.A 20.C
21. D 22.A 23.C 24.B 25.B
26. A 27.A 28.C 29.B 30.B
31. D 32.D 33.B 34.B