Review

17. The atomic mass of an element is the weighted average of
the
(1) number of protons in the isotopes of that element
(2) number of neutrons in the isotopes of that element
(3) atomic numbers of the naturally occurring isotopes of
that element
(4) atomic masses of the naturally occurring isotopes of
that element
18. The modern model of the atom is based on the work of
(1) one scientist over a short period of time
(2) one scientist over a long period of time
(3) many scientists over a short period of time
(4) many scientists over a long period of time
19. In the wave-mechanical model, an orbital is a region of
space in an atom where there is
(1) a high probability of finding an electron
(2) a high probability of finding a neutron
(3) a circular path in which electrons are found
(4) a circular path in which neutrons are found
20. During a flame test, ions of a specific metal are heated in
the flame of a gas burner. A characteristic color of light is
emitted by these ions in the flame when the electrons
(1) gain energy as they return to lower energy levels
(2) gain energy as they move to higher energy levels
(3) emit energy as they return to lower energy levels
(4) emit energy as they move to higher energy levels
21. Which of these phrases best describes an atom?
(1) a positive nucleus surrounded by a hard negative shell
(2) a positive nucleus surrounded by a cloud of negative
charges
(3) a hard sphere with positive particles uniformly
embedded
(4) a hard sphere with negative particles uniformly
embedded
22. Recovering the salt from a mixture of salt and water could
best be accomplished by
(1) evaporation (3) paper chromatography
(2) filtration (4) density determination
23. Which element is malleable and conducts electricity?
(1) iron (3) sulfur
(2) iodine (4) phosphorus
24. At STP, an element that is a brittle solid and a poor
conductor of heat and electricity could have an atomic
number of
(1) 12 (3) 16
(2) 13 (4) 17
25. What are two properties of most nonmetals?
(1) high ionization energy and poor electrical conductivity
(2) high ionization energy and good electrical conductivity
(3) low ionization energy and poor electrical conductivity
(4) low ionization energy and good electrical conductivity
26. Which substance can not be decomposed by a chemical
change?
(1) Ne (3) HF
(2) N2O (4) H2O Base your answers to questions 27 and 28 on the information
below.
Naturally occurring elemental carbon is a mixture of
isotopes. The percent composition of the two most
abundant isotopes is listed below.
• 98.93% of the carbon atoms have a mass of 12.00
atomic mass units.
• 1.07% of the carbon atoms have a mass of 13.00
atomic mass units.
27. Describe, in terms of subatomic particles found in the
nucleus, one difference between the nuclei of carbon-12
atoms and the nuclei of carbon-13 atoms. The response
must include both isotopes.
28. In the space provided in your answer booklet, show a
correct numerical setup for calculating the average atomic
mass of carbon.
29. Which pair of symbols represents a metalloid and a noble
gas?
(1) Si and Bi (3) Ge and Te
(2) As and Ar (4) Ne and Xe
30. Which element is a solid at STP?
(1) H2 (3) N2 (2) I2 (4) O2 31. Given the particle diagram:
At 101.3 kPa and 298 K, which element could this diagram
represent?
(1) Rn (3) Ag
(2) Xe (4) Kr
32. Which list consists of elements that have the most similar
chemical properties?
(1) Mg, Al, and Si (3) K, Al, and Ni
(2) Mg, Ca, and Ba (4) K, Ca, and Ga
33. Which list of elements contains a metal, a metalloid, and a
nonmetal?
(1) Zn, Ga, Ge (3) Cd, Sb, I
(2) Si, Ge, Sn (4) F, Cl, Br
34. The elements in Period 5 on the Periodic Table are arranged
from left to right in order of
(1) decreasing atomic mass
(2) decreasing atomic number
(3) increasing atomic mass
(4) increasing atomic number
35. What is the density of N2 at STP?
(1) .00100 g/cm 3
(3) .00143 g/cm 3
(2) .00125 g/cm 3
(4) .00198 g/cm 3
36. Explain, in terms of atomic structure, why germanium is
chemically similar to silicon.