Download AP Chemistry-Chapter 6 MC Questions

Name: _____________________ Date: _______________
AP Chemistry-Chapter 6 MC Questions
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Which periodic group or series of elements is not correctly matched with its common family name?
IIA
a. alkaline earth metals
IIIA
b. alkali metals
lanthanides
58Ce - 71Lu
c.
halogens
VIIA
d.
VIIIA
e. noble gases
____
2. Of the following, which element does not match its designation?
representative metal
a. 38Sr
In
representative nonmetal
b. 49
metalloid
c. 14Si
d-transition metal
d. 74W
f-transition metal
e. 90Th
____
3. Of the following, which periodic group(s) do not match their designation?
a. d-transition metals
IIIB
IIB
IA, IIA
b. representative metals
VIIIB
c. noble gases
IIA
d. alkaline earth metals
halogens
VIIA
e.
____
4. __________ is a noble gas.
a. 22Ti
b. 42Mo
c. 81Tl
d. 36Kr
e. 92U
____
5. __________ is an actinide.
a. 22Ti
b. 42Mo
c. 81Tl
d. 36Kr
e. 92U
____
6. Which one of the following is an inner transition (f-transition) element?
a. Rb
b. Ho
c. Co
d. Ru
e. Bi
____
7. What would be the outer electron configuration of group IIIB (Sc, Y, La . . .)?
a. ns2nd2np0
b. nd1ns2
c. ns2(n-1)d1
d. ns1np3
e. (n-1)d1ns2
____
8. What would be the outer electron configuration of alkaline earth metals?
a. ns2np2
b. np2
c. ns0np2
d. nd2
e. ns2
____
9. Choose the term that best describes all members of this series of elements:
K, Ca, Ba, Cl, N
a.
b.
c.
d.
e.
metalloids
d-transition elements
alkaline earth metals
alkali metals
representative elements
____ 10. Which of the following statements is false?
a. The effective nuclear charge experienced by an electron in an outer shell is less than the
actual nuclear charge.
b. Within a family (vertical group in the periodic table) of representative elements atomic
radii increase from top to bottom.
c. Electrons in inner shells screen, or shield, electrons in outer shells from the full effect of
the nuclear charge.
d. The atomic radii of representative elements decrease from left to right across a period
(horizontal row in the periodic table).
e. Transition elements have larger atomic radii than the preceding IA and IIA
elements in the same period because transition elements have electrons in their d orbitals.
____ 11. Which element has the largest atomic radius?
a. Al
b. Si
c. P
d. S
e. Cl
____ 12. Which element has the largest atomic radius?
a. F
b. Cl
c. Sn
d. Kr
e. Se
____ 13. Which element has the smallest radius?
a. Na
b. Mg
c. Al
d. Si
e. P
____ 14. Arrange the following elements in order of increasing atomic radii.
Sr, Rb, Sb, I, In
a.
b.
c.
d.
e.
Rb < Sr < In < Sb < I
I < Sb < In < Rb < Sr
In < Sb < I < Sr < Rb
Sb < I < In < Sr < Rb
I < Sb < In < Sr < Rb
____ 15. The first ionization energy of sulfur is less than that of phosphorus. A reasonable explanation for this fact
involves
a. the stability of the half-filled subshell in atomic sulfur.
b. pairing of two electrons in one 3p orbital in sulfur atoms.
c. the smaller size of sulfur atoms relative to phosphorus atoms.
d. the ease with which phosphorus attains a noble gas electronic configuration.
e. the higher electronegativity of sulfur relative to phosphorus.
____ 16. Which element has the highest first ionization energy?
a. Be
b. B
c. C
d. N
e. O
____ 17. The amount of energy absorbed in the process in which an electron is added to a neutral gaseous atom is
defined as __________.
a. shielding effect
b. electronegativity
c. electron affinity
d. first ionization energy
e. standard reduction potential
____ 18. Which one of the following species is not isoelectronic with neon?
a. Mg2+
b. Na+
c. O2d. Cle. Al3+
____ 19. Which ion has the largest radius?
a. O2b. S2c. Se2d. Te2e. Po2-
____ 20. Consider the group of ions that are isoelectronic with krypton. Which response contains all the true statements
and no others?
I.
II.
III.
IV.
V.
a.
b.
c.
d.
e.
The ion with the highest positive charge is the largest ion.
The ion with the highest atomic number bears the highest positive charge.
The ion with the lowest atomic number bears the least negative charge.
The ion with a 1- charge is obtained by adding one electron to a Group VIIA
element.
All the ions have a noble gas electronic configuration.
II and III
I, II, and V
II, IV, and V
I and IV
II, III, IV, and V
____ 21. Which ion has the smallest radius?
a. As3b. Se2c. Brd. Rb+
e. Sr2+
____ 22. A property that measures the ability of an atom to attract electrons in a chemical bond is
a. binding energy.
b. mass defect.
c. electron affinity.
d. ionization energy.
e. electronegativity.
____ 23. Which element has the highest electronegativity?
a. N
b. Si
c. As
d. P
e. C
____ 24. Which pair of elements below would be least likely to form an ionic bond between them?
a. Na and S
b. C and N
c. Al and F
d. Mg and Br
e. Cs and O
____ 25. In general, ionization energies
a. increase down a group and increase across a period.
b. increase down a group and decrease across a period.
c. decrease down a group and increase across a period.
d. decrease down a group and decrease across a period.
e. increase with atomic mass and increase with atomic radii.
____ 26. In general, atomic radii
a. increase down a group and decrease across a period.
b. increase down a group and increase across a period.
c. decrease down a group and decrease across a period.
d. are proportional to atomic mass.
e. decrease down a group and increase across a period.
____ 27. Which of the following chemical expressions refers to the first ionization energy of calcium?
a. Ca(s) Ca+(s) + eb. Ca(g) + e- Ca+(g)
c. Ca(s) + e- Ca+(s)
d. Ca(g) Ca+(g) + ee. Ca(g) Ca2+(g) + e____ 28. Which statement is false?
a. Cations are smaller than their corresponding neutral atom.
b. Anions are smaller than their corresponding neutral atom.
c. Mg2+ is larger than Be2+.
d. O2- is larger than F-.
e. Br- is smaller than I-.
____ 29. Which element has the largest first ionization energy?
a. Be
b. Ca
c. Mg
d. Sr
e. Ba
____ 30. The change in energy for the following reaction is referred to as the ____ for fluorine.
F(g) + ea.
b.
c.
d.
e.
F-(g)
oxidation energy
electron affinity
electronegativity energy
first ionization energy
second ionization energy