Chemistry 10th Edition International Edition by Kenneth W - Test Bank
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Chemistry 10th Edition International Edition by Kenneth W - Test Bank

Chemistry 10th Edition International Edition by Kenneth W - Test Bank   Instant Download - Complete Test Bank With Answers     Sample Questions Are Posted Below   Chapter 5—Chemical Periodicity     MULTIPLE CHOICE   According to the periodic law the properties of elements repeat at regular intervals when the elements are arranged in …

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Chemistry 10th Edition International Edition by Kenneth W – Test Bank

 

Instant Download – Complete Test Bank With Answers

 

 

Sample Questions Are Posted Below

 

Chapter 5—Chemical Periodicity

 

 

MULTIPLE CHOICE

 

  1. According to the periodic law the properties of elements repeat at regular intervals when the elements are arranged in order of
a. their increasing atomic mass.
b. their increasing atomic size.
c. their increasing number of neutrons in the nucleus.
d. their increasing number of isotopes.
e. their increasing number of protons in the nucleus.

 

 

ANS:  E

OBJ:   Understand the periodic law.

TOP:   More About the Periodic Table

 

  1. Which electrons have the greatest influence on the properties of elements?
a. those electrons in s orbitals
b. those electrons in d orbitals
c. core electrons
d. the outermost electrons
e. none of these

 

 

ANS:  D

OBJ:   Understand the importance of the outermost electrons in chemistry.

TOP:   More About the Periodic Table

 

  1. Of the following, which element does not match its designation?
a. 38Sr  /  representative metal
b. 49In  /  representative nonmetal
c. 14Si  /  metalloid
d. 42Mo  /  d-transition metal
e. 90Th  /  f-transition metal

 

 

ANS:  B

OBJ:   Classify an element.

TOP:   More About the Periodic Table

 

  1. Of the following, which periodic group(s) do not match their designation?
a. d-transition metals  /  IIIB ® IIB
b. representative metals  /  IA, IIA
c. noble gases  /  VIIIB
d. alkaline earth metals  /  IIA
e. halogens  /  VIIA

 

 

ANS:  C

OBJ:   Match the family of elements with the group number(s).

TOP:   More About the Periodic Table

 

 

  1. ____ is a d-transition metal.
a. Cr
b. Ga
c. Sn
d. Sb
e. Li

 

 

ANS:  A

OBJ:   Identify a d-transition metal.

TOP:   More About the Periodic Table

 

  1. ____ is a noble gas.
a. 22Ti
b. 42Mo
c. 81Tl
d. 54Xe
e. 92U

 

 

ANS:  D

OBJ:   Identify a noble gas.

TOP:   More About the Periodic Table

 

  1. ____ is an actinide.
a. 22Ti
b. 42Mo
c. 81Tl
d. 36Kr
e. 93Np

 

 

ANS:  E

OBJ:   Identify an actinide.

TOP:   More About the Periodic Table

 

  1. Which one of the following is an inner transition (f-transition) element?
a. Rb
b. Ho
c. Co
d. Ru
e. Bi

 

 

ANS:  B

OBJ:   Identify an inner transition element.

TOP:   More About the Periodic Table

 

  1. Which of the following is not a representative element?
a. Cl
b. Sr
c. Co
d. K
e. N

 

 

ANS:  C

OBJ:   Identify the element that is least representative of a family.

TOP:   More About the Periodic Table

 

 

  1. Choose the response that includes all of the listed elements that are d-transition elements, and no others.
I. 22Ti
II. 42Mo
III. 81Tl
IV. 36Kr
V. 92U

 

a. I and II
b. II and III
c. III and IV
d. IV and V
e. I, III, and V

 

 

ANS:  A

OBJ:   Identify d-transition metals.

TOP:   More About the Periodic Table

 

  1. What would be the outer electron configuration of group VIA (O, S, Se, . . .)?
a. ns2np6
b. ns2np2
c. ns2np4
d. np6
e. ns0np6

 

 

ANS:  C

OBJ:   Determine the electron configuration beyond the noble gas core given the group number.

TOP:   More About the Periodic Table

 

  1. 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

 

 

ANS:  E

OBJ:   Determine the electron configuration beyond the noble gas core given the group number.

TOP:   More About the Periodic Table

 

  1. What would be the outer electron configuration of alkaline earth metals?
a. ns2np2
b. np2
c. ns0np2
d. nd2
e. ns2

 

 

ANS:  E

OBJ:   Determine the electron configuration beyond the noble gas core given the group number.

TOP:   More About the Periodic Table

 

 

  1. Choose the term that best describes all members of this series of elements:
  Xe, Rn, He, Ne, Kr

 

a. metalloids
b. noble gases
c. alkaline earth metals
d. alkali metals
e. representative elements

 

 

ANS:  B

OBJ:   Classify a group of elements.

TOP:   More About the Periodic Table

 

  1. 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.

 

 

ANS:  E

OBJ:   Understand the term effective nuclear charge. | Understand the term shielding. | Understand the general relationship between atomic radii and nuclear charge.                   TOP:   Atomic Radii

 

  1. Which element has the largest atomic radius?
a. Al
b. Si
c. P
d. S
e. Cl

 

 

ANS:  A

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

  1. Which element has the largest atomic radius?
a. B
b. Al
c. Ga
d. In
e. Tl

 

 

ANS:  E

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

 

  1. Which element has the largest atomic radius?
a. At
b. Pb
c. As
d. Sn
e. Xe

 

 

ANS:  B

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

  1. Which element has the largest atomic radius?
a. Ga
b. In
c. Ge
d. P
e. O

 

 

ANS:  B

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

  1. Which element has the largest atomic radius?
a. 3Li
b. 11Na
c. 37Rb
d. 9F
e. 53I

 

 

ANS:  C

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

  1. Which element has the largest atomic radius?
a. F
b. Cl
c. Sn
d. Kr
e. Se

 

 

ANS:  C

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

  1. Which element has the largest atomic radius?
a. Ca
b. Sr
c. Cr
d. P
e. Na

 

 

ANS:  B

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

 

  1. Which element has the largest atomic radius?
a. 9F
b. 16S
c. 11Na
d. 28Ni
e. 37Rb

 

 

ANS:  E

OBJ:   Identify the atom with the largest radius.

TOP:   Atomic Radii

 

  1. Which element has the smallest radius?
a. Na
b. Mg
c. Al
d. Si
e. P

 

 

ANS:  E

OBJ:   Identify the atom with the smallest radius.

TOP:   Atomic Radii

 

  1. Which element has the smallest radius?
a. F
b. Cl
c. Br
d. I
e. At

 

 

ANS:  A

OBJ:   Identify the atom with the smallest radius.

TOP:   Atomic Radii

 

  1. Which element has the smallest radius?
a. Mo
b. Au
c. Bi
d. In
e. Te

 

 

ANS:  E

OBJ:   Identify the atom with the smallest radius.

TOP:   Atomic Radii

 

  1. Which element has the smallest radius?
a. K
b. Na
c. Rb
d. Mg
e. Cl

 

 

ANS:  E

OBJ:   Identify the atom with the smallest radius.

TOP:   Atomic Radii

 

 

  1. Arrange the following elements in order of increasing atomic radii.
  Sr, Rb, Sb, I, In

 

a. Rb < Sr < In < Sb < I
b. I < Sb < In < Rb < Sr
c. In < Sb < I < Sr < Rb
d. Sb < I < In < Sr < Rb
e. I < Sb < In < Sr < Rb

 

 

ANS:  E

OBJ:   Arrange the atoms according to size (five atoms).

TOP:   Atomic Radii

 

  1. Arrange the following elements in order of increasing atomic radii.
  K, Na, Mg, Cs, Cl

 

a. Na < Mg < Cl < K < Cs
b. Cl < Mg < Na < K < Cs
c. Cs < K < Cl < Mg < Na
d. Cl < Mg < Cs < K < Na
e. Cl < Mg < Na < Cs < K

 

 

ANS:  B

OBJ:   Arrange the atoms according to size (five atoms).

TOP:   Atomic Radii

 

  1. Arrange the following elements in order of decreasing atomic radii.
  Pb, P, Cl, F, Si

 

a. Cl > F > Pb > Si > P
b. Pb > Si > P > F > Cl
c. Pb > Si > P > Cl > F
d. Pb > Cl > P > Si > F
e. Pb > Cl > P > Si > F

 

 

ANS:  C

OBJ:   Arrange the atoms according to size (five atoms).

TOP:   Atomic Radii

 

  1. As we move across the periodic table from left to right, atoms become smaller due to
a. increasing effective nuclear charge.
b. the p orbitals being filled.
c. electron-electron repulsions.
d. shell size increases.
e. none of these.

 

 

ANS:  A

OBJ:   Understand the effects of nuclear charge on atom size.

TOP:   Atomic Radii

 

 

  1. The minimum energy required to remove the most loosely held electron is
a. first ionization energy.
b. electron affinity
c. potential energy
d. kinetic energy
e. electronegativity.

 

 

ANS:  A

OBJ:   Define first ionization energy.

TOP:   Ionization Energy

 

  1. 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.

 

 

ANS:  B

OBJ:   Understand the causes of differences between ionization energies.

TOP:   Ionization Energy

 

  1. Which element has the lowest first ionization energy?
a. F
b. Cl
c. Br
d. I
e. At

 

 

ANS:  E

OBJ:   Identify the atom with the lowest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the lowest first ionization energy?
a. Cs
b. Rb
c. Ca
d. Ba
e. Na

 

 

ANS:  A

OBJ:   Identify the atom with the lowest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the lowest first ionization energy?
a. F
b. B
c. O
d. S
e. Sr

 

 

ANS:  E

OBJ:   Identify the atom with the lowest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the lowest first ionization energy?
a. Be
b. B
c. C
d. N
e. O

 

 

ANS:  B

DIF:    Harder Question

OBJ:   Identify the atom with the lowest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the highest first ionization energy?
a. B
b. Al
c. Ga
d. In
e. Tl

 

 

ANS:  A

OBJ:   Identify the atom with the highest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the highest first ionization energy?
a. Sn
b. Cd
c. As
d. Tc
e. Cl

 

 

ANS:  E

OBJ:   Identify the atom with the highest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the highest first ionization energy?
a. Li
b. Cs
c. Cl
d. I
e. Ar

 

 

ANS:  E

OBJ:   Identify the atom with the highest ionization energy.

TOP:   Ionization Energy

 

  1. Which element has the highest first ionization energy?
a. Be
b. B
c. C
d. N
e. O

 

 

ANS:  D

OBJ:   Identify the atom with the highest ionization energy.

TOP:   Ionization Energy

 

  1. Arrange the following elements in order of increasing first ionization energy.
  Mg, Al, Si, P, S

 

a. Al < Mg < Si < S < P
b. Mg < Al < Si < P < S
c. Al < Mg < Si < P < S
d. Mg < Al < Si < S < P
e. Al < Mg < P < Si < S

 

 

ANS:  A

DIF:    Harder Question

OBJ:   Arrange the atoms according to ionization energy (five atoms).

TOP:   Ionization Energy

 

  1. Arrange the following elements in order of decreasing first ionization energy.
  Rb, In, Sn, Sb, As

 

a. Sb > Sn > In > As > Rb
b. As > In > Sn > Sb > Rb
c. Rb > As > Sb > Sn > In
d. As > Sb > Sn > In > Rb
e. As > Sn > Sb > In > Rb

 

 

ANS:  D

OBJ:   Arrange the atoms according to ionization energy (five atoms).

TOP:   Ionization Energy

 

  1. Arrange the following elements in order of decreasing first ionization energy.
  Be, Ca, Cs, Mg, K

 

a. Mg > Be > Ca > K > Cs
b. Be > Mg > Ca > K > Cs
c. Cs > K > Ca > Be > Mg
d. Ca > Mg > Be > Cs > K
e. Ca > Mg > Be > K > Cs

 

 

ANS:  B

OBJ:   Arrange the atoms according to ionization energy (five atoms).

TOP:   Ionization Energy

 

  1. Arrange the following elements in order of decreasing first ionization energy.
  F, Be, O, N, C

 

a. F > O > N > C > Be
b. Be > C > O > N > F
c. F > N > O > C > Be
d. O > F > N > Be > C
e. Be > C > N > O > F

 

 

ANS:  C

DIF:    Harder Question

OBJ:   Arrange the atoms according to ionization energy (five atoms).

TOP:   Ionization Energy

 

 

  1. Which equation below depicts the reaction from which the first ionization energy would be determined?
a. Ca(g) ® Ca+(g) + e–
b. Ca(s) ® Ca+(g) + e–
c. Ca(s) + e– ® Ca–(g)
d. Ca(g) ® Ca2+ + e–
e. None of these

 

 

ANS:  A

OBJ:   Identify a chemical equation representing the first ionization energy of an atom.

TOP:   Ionization Energy

 

  1. 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

 

 

ANS:  C

OBJ:   Know the definition of electron affinity.

TOP:   Electron Affinity

 

  1. Which of the following elements has the most negative electron affinity?
a. Si
b. P
c. S
d. Se
e. Te

 

 

ANS:  C

OBJ:   Identify the atom with the most negative electron affinity.

TOP:   Electron Affinity

 

  1. Which of the following elements has the most negative electron affinity?
a. As
b. Al
c. K
d. Se
e. Sn

 

 

ANS:  D

OBJ:   Identify the atom with the most negative electron affinity.

TOP:   Electron Affinity

 

  1. The general electron configuration for the element group that would have the largest negative value for the electron affinity for its atoms is ____?
a. ns2np6
b. ns2np4
c. ns1
d. ns2np5
e. ns2np3

 

 

 

ANS:  D

OBJ:   Determine the electron configuration beyond the noble gas core for the group of elements with the most negative electron affinity.

TOP:   Electron Affinity

 

  1. Arrange the following elements in order of increasing values of electron affinity, i.e., from most negative to least negative. (Note: None of these elements is an exception to the general trends of electron affinities.)
  Cl, Se, S, Cs, Rb, Te

 

a. Cl < S < Se < Rb < Te < Cs
b. Cl > Te > Se > S > Rb > Cs
c. Cl > Se > S > Te > Rb > Cs
d. Cl < S < Se < Te < Cs < Rb
e. Cl < S < Se < Te < Rb < Cs

 

 

ANS:  E

OBJ:   Arrange the atoms according to electron affinities (five atoms).

TOP:   Electron Affinity

 

  1. Which of the following statements about ionization energy and electron affinity is true?
a. Elements with very high ionization energies usually have very negative electron affinities.
b. IE1 and EA are equal in value but with the sign reversed.
c. It is very easy to measure both IE and EA values.
d. Elements with low IE, as well as very negative EA, tend to form cations easily.
e. All of these statements are true.

 

 

ANS:  A

OBJ:   Understand both electron affinity and ionization energy.

TOP:   Electron Affinity

 

  1. Which one of the following species is not isoelectronic with neon?
a. Mg2+
b. Na+
c. O2–
d. Si2+
e. Al3+

 

 

ANS:  D

OBJ:   Determine all atoms or ions which are isoelectronic.

TOP:   Ionic Radii

 

  1. Which one of the following pairs contains isoelectronic species?
a. Na  /  Na+
b. S  /  Se
c. S2–  /  Se2–
d. F2  /  Cl2
e. Na+  /  O2–

 

 

ANS:  E

OBJ:   Determine atoms or ion pair which are isoelectronic.

TOP:   Ionic Radii

 

 

  1. Which of the following ions is not isoelectronic with the others?
a. I–
b. Sb3+
c. Te2–
d. Ba2+
e. Cs+

 

 

ANS:  B

OBJ:   Determine all atoms or ions which are isoelectronic.

TOP:   Ionic Radii

 

  1. Which of the following ions is not isoelectronic with a noble gas?
a. Mg2+
b. P2–
c. Cs+
d. Se2–
e. Ba2+

 

 

ANS:  B

OBJ:   Determine all atoms or ions which are isoelectronic.

TOP:   Ionic Radii

 

  1. Which ion has the largest radius?
a. O2–
b. S2–
c. Se2–
d. Te2–
e. Po2–

 

 

ANS:  E

OBJ:   Identify the ion with the largest radius.

TOP:   Ionic Radii

 

  1. Which ion has the largest radius?
a. F–
b. Cl–
c. Br–
d. I–
e. At–

 

 

ANS:  E

OBJ:   Identify the ion with the largest radius.

TOP:   Ionic Radii

 

  1. Which ion has the largest radius?
a. Li+
b. Na+
c. Be2+
d. Mg2+
e. Al3+

 

 

ANS:  B

OBJ:   Identify the ion with the largest radius.

TOP:   Ionic Radii

 

  1. Simple positively charged ions are always ____ than the neutral atoms from which they are formed.
a. smaller
b. larger
c. isoelectronic
d. the same size
e. more anionic

 

 

ANS:  A

OBJ:   Understand the relationship between the ionic radii and atomic radius of an atom.

TOP:   Ionic Radii

 

  1. Which ion has the smallest radius?
a. F–
b. Cl–
c. Br–
d. I–
e. At–

 

 

ANS:  A

OBJ:   Identify the ion with the smallest radius.

TOP:   Ionic Radii

 

  1. Which ion has the smallest radius?
a. O2–
b. S2–
c. Se2–
d. Te2–
e. Po2–

 

 

ANS:  A

OBJ:   Identify the ion with the smallest radius.

TOP:   Ionic Radii

 

  1. Which ion has the smallest radius?
a. As3–
b. Se2–
c. Br–
d. Rb+
e. Sr2+

 

 

ANS:  E

OBJ:   Identify the ion with the smallest radius.

TOP:   Ionic Radii

 

  1. Which ion has the smallest radius?
a. K+
b. Cs+
c. Sr2+
d. Ba2+
e. Tl3+

 

 

ANS:  E

DIF:    Harder Question

OBJ:   Identify the ion with the smallest radius.

TOP:   Ionic Radii

 

  1. Which ion or atom has the largest radius?
a. S
b. S2–
c. Se
d. Se2–
e. Br

 

 

ANS:  D

OBJ:   Identify the ion or atom with the largest radius.

TOP:   Ionic Radii

 

  1. Which ion or atom has the largest radius?
a. Sr2+
b. Rb+
c. Kr
d. Br–
e. Se2–

 

 

ANS:  E

OBJ:   Identify the ion or atom with the largest radius.

TOP:   Ionic Radii

 

  1. Arrange the following set of ions in order of increasing ionic radii.
  Ca2+, Cl–, K+, P3–, S2–

 

a. Ca2+ < K+ < P3– < S2– < Cl–
b. Ca2+ < K+ < Cl– < S2– < P3–
c. K+ < Cl– < Ca2+ < S2– < P3–
d. Cl– < S2– < P3– < Ca2+ < K+
e. P3– < S2– < Cl– < K+ < Ca2+

 

 

ANS:  B

OBJ:   Arrange the ions according to size (five ions).

TOP:   Ionic Radii

 

  1. Arrange the following set of ions in order of decreasing ionic radii.
  Al3+, Ga3+, Ca2+, Rb+, K+

 

a. Rb+ > Ga3+ > Ca2+ > K+ > Al3+
b. Rb+ > K+ > Ca2+ > Al3+ > Ga3+
c. Ga3+ > Al3+ > Ca2+ > Rb+ > K+
d. Rb+ > Ca2+ > K+ > Ga3+ > Al3+
e. Rb+ > K+ > Ca2+ > Ga3+ > Al3+

 

 

ANS:  E

OBJ:   Arrange the ions according to size (five ions).

TOP:   Ionic Radii

 

  1. Which of the lists of increasing ionic radii is not correct?
a. Cl– < Br– < I–
b. Al3+ < Mg2+ < Na+
c. Ca2+ < Sr2+ < Ba2+
d. S2– < Cl– < K+
e. Na+ < O2– < N3–

 

 

 

ANS:  D

OBJ:   Find the ions not arranged according to size (three ions).

TOP:   Ionic Radii

 

  1. Which of these comparisons according to radius is (are) correct?
I. Na+ > Mg2+
II. In3+ > Sr2+
III. Cl– > K+
IV. Cl > K

 

a. I and II
b. II and IV
c. I and III
d. II and III
e. III and IV

 

 

ANS:  C

OBJ:   Identify the correct atom or ion size comparisons (two atoms or ions).

TOP:   Ionic Radii

 

  1. 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.

 

 

ANS:  E

OBJ:   Define electronegativity.

TOP:   Electronegativity

 

  1. Which element has the lowest electronegativity?
a. H
b. Li
c. Na
d. K
e. Cs

 

 

ANS:  E

OBJ:   Identify the atom with the lowest electronegativity.

TOP:   Electronegativity

 

  1. Which element has the lowest electronegativity?
a. Mg
b. Na
c. Rb
d. Y
e. Sc

 

 

ANS:  C

OBJ:   Identify the atom with the lowest electronegativity.

TOP:   Electronegativity

 

 

  1. Which element has the lowest electronegativity?
a. K
b. Ca
c. Ga
d. Ge
e. As

 

 

ANS:  A

OBJ:   Identify the atom with the lowest electronegativity.

TOP:   Electronegativity

 

  1. Which element has the lowest electronegativity?
a. S
b. Sc
c. Sr
d. Se
e. Si

 

 

ANS:  C

OBJ:   Identify the atom with the lowest electronegativity.

TOP:   Electronegativity

 

  1. Which element has the highest electronegativity?
a. C
b. Si
c. Ge
d. Sn
e. Pb

 

 

ANS:  A

OBJ:   Identify the atom with the highest electronegativity.

TOP:   Electronegativity

 

  1. Which element has the highest electronegativity?
a. 3Li
b. 7N
c. 19K
d. 33As
e. 56Ba

 

 

ANS:  B

OBJ:   Identify the atom with the highest electronegativity.

TOP:   Electronegativity

 

  1. Which element has the highest electronegativity?
a. B
b. Ge
c. Ca
d. O
e. At

 

 

ANS:  D

OBJ:   Identify the atom with the highest electronegativity.

TOP:   Electronegativity

 

 

  1. Which element has the highest electronegativity?
a. N
b. Si
c. As
d. P
e. C

 

 

ANS:  A

OBJ:   Identify the atom with the highest electronegativity.

TOP:   Electronegativity

 

  1. Arrange the following elements in order of increasing electronegativities.
  Mg, Ra, P, Cl, Al

 

a. Mg < Ra < P < Al < Cl
b. Ra < Mg < Al < P < Cl
c. Mg < Ra < P < Cl <Al
d. Al < P < Cl < Mg < Ra
e. Al < P < Cl < Ra < Mg

 

 

ANS:  B

OBJ:   Arrange the atoms according to electronegativities (five atoms).

TOP:   Electronegativity

 

  1. Arrange the following elements in order of decreasing electronegativities.
  Al, Cs, Mg, Na, P

 

a. P > Al > Mg > Na > Cs
b. Cs > Na > Mg > Al > P
c. Al > Mg > Na > Cs > P
d. P > Al > Mg > Cs > Na
e. P > Cs > Na > Mg > Al

 

 

ANS:  A

OBJ:   Arrange the atoms according to electronegativities (five atoms).

TOP:   Electronegativity

 

  1. Which comparison of electronegativities is not correct?
a. Br > Se
b. K > Mg
c. O > S
d. N > Be
e. I > Ba

 

 

ANS:  B

OBJ:   Identify the incorrect electronegativity comparison (two atoms).

TOP:   Electronegativity

 

  1. Which comparison of electronegativities is not correct?
a. Ge > Ga
b. Ba > Cs
c. O > N
d. F > Cl
e. B > C

 

 

 

ANS:  E

OBJ:   Identify the incorrect electronegativity comparison (two atoms).

TOP:   Electronegativity

 

  1. Which of these elements has the greatest attraction for electrons in a covalent bond?
a. Ge
b. As
c. Se
d. Br
e. Kr

 

 

ANS:  D

OBJ:   Identify the atom with the highest electronegativity.

TOP:   Electronegativity

 

  1. Which of the following pairs of elements would be expected to form an ionic compound?
a. S  /  F
b. H  /  C
c. Rb  /  Cl
d. As  /  Br
e. C  /  I

 

 

ANS:  C

OBJ:   Identify the atom pair most likely to form an ionic compound.

TOP:   Electronegativity

 

  1. Which pair of elements below would be least likely to form an ionic bond between them?
a. Na  /  S
b. C  /  N
c. Al  /  F
d. Mg  /  Br
e. Cs  /  O

 

 

ANS:  B

OBJ:   Identify the atom pair most likely to form a covalent compound.

TOP:   Electronegativity

 

  1. Chlorine is most likely to form an ionic compound with ____.
a. F
b. O
c. C
d. N
e. Li

 

 

ANS:  E

OBJ:   Identify the atom pair most likely to form an ionic compound.

TOP:   Electronegativity

 

  1. Iodine is most likely to form an ionic compound with ____.
a. B
b. Si
c. Cl
d. N
e. Mg

 

 

 

ANS:  E

OBJ:   Identify the atom pair most likely to form an ionic compound.

TOP:   Electronegativity

 

  1. Which one of the following reactions does not produce H2(g)?
a. electrolysis of H2O
b. zinc with HCl(aq)
c. combustion of ethane, C2H6
d. iron with steam
e. steam cracking of hydrocarbons

 

 

ANS:  C

OBJ:   Recognize the reactions that produce hydrogen.

TOP:   Hydrogen and the Hydrides

 

  1. Which of the following statements about hydrogen is false?
a. Hydrogen occurs as a diatomic molecule.
b. Hydrogen can be produced by the reaction of an active metal and HCl(aq).
c. NH3, the binary hydride of nitrogen, is called ammonia.
d. Hydrogen forms only molecular compounds.
e. Metal hydrides are basic.

 

 

ANS:  D

OBJ:   Know the qualitative chemical facts about hydrogen.

TOP:   Hydrogen and the Hydrides

 

  1. Which pair of gases is the product of the “water gas reaction”?
a. H2O + H2
b. CO + H2O
c. O2 + H2O
d. CO + H2
e. H2 + O2

 

 

ANS:  D

OBJ:   Know the products of the water gas reaction.

TOP:   Hydrogen and the Hydrides

 

  1. Which one of the following reactions is the “water gas” reaction?
a. C(s) + H2O(g)  CO(g) + H2(g)
b. 2CH4(g) + 3O2(g)  2CO(g) + 4H2O(g)
c. CH4(g)  C(s) + 2H2(g)
d. 2Na(s) + 2H2O ® 2NaOH(aq) + H2(g)
e. C4H10(g)  2C2H2(g) + 3H2(g)

 

 

ANS:  A

OBJ:   Know the chemical equation for the water gas reaction.

TOP:   Hydrogen and the Hydrides

 

 

  1. Which one of the following (pure) compounds of hydrogen is ionic?
a. HF
b. HCl
c. NaH
d. H2O
e. H2Se

 

 

ANS:  C

OBJ:   Identify the ionic compound.

TOP:   Hydrogen and the Hydrides

 

  1. Which one of the following is an ionic hydride?
a. CH4
b. H2Se
c. AsH3
d. BaH2
e. B2H6

 

 

ANS:  D

OBJ:   Identify the ionic compound.

TOP:   Hydrogen and the Hydrides

 

  1. Which of the following responses lists only the molecular hydrides?
I. LiH
II. B2H6
III. GeH4
IV. HCl
V. BaH2

 

a. I
b. I, V
c. II, III
d. II, III, IV
e. I, II, V

 

 

ANS:  D

OBJ:   Identify the covalent (molecular) hydrides.

TOP:   Hydrogen and the Hydrides

 

  1. Which one of the following is a molecular hydride?
a. RbH
b. SrH2
c. KH
d. PH3
e. MgH2

 

 

ANS:  D

OBJ:   Identify the covalent (molecular) hydride.

TOP:   Hydrogen and the Hydrides

 

 

  1. Which of the following is incorrectly classified?
a. KH  /  ionic hydride
b. CH4  /  ionic hydride
c. HI  /  molecular hydride
d. CsH  /  ionic hydride
e. H2S  /  molecular hydride

 

 

ANS:  B

DIF:    Harder Question

OBJ:   Identify the incorrect compound classification.

TOP:   Hydrogen and the Hydrides

 

  1. Which response includes all the elements below whose compounds with hydrogen would be expected to be molecular hydrides, and no others?
  Br, K, P, B

 

a. K, B
b. Br, P
c. K, Br
d. Br, P, B
e. Br

 

 

ANS:  D

OBJ:   Identify the elements which produce covalent (molecular) hydrides.

TOP:   Hydrogen and the Hydrides

 

  1. Which one of the following hydrides is basic?
a. H2Te
b. B2H6
c. CaH2
d. HI
e. CH4

 

 

ANS:  C

OBJ:   Classify a hydride as basic, acidic, or neutral.

TOP:   Hydrogen and the Hydrides

 

  1. Which one of the following hydrides is not acidic?
a. HF
b. HCl
c. H2S
d. CaH2
e. H2Se

 

 

ANS:  D

OBJ:   Classify a hydride as basic, acidic, or neutral.

TOP:   Hydrogen and the Hydrides

 

  1. What would be the general balanced equation for the reaction of the ionic hydride MH2 with excess water?
a. MH2(s) + H2O ® MOH(aq) + H2(g)
b. MH2(s) + H2O ® MO(s) + 2H2(g)
c. MH2(s) + H2O ® MH2(s) + H2O(g)
d. MH2(s) + 2H2O ® M(OH)2(aq) + 2H2(g)
e. MH2(s) + 3H2O ® MO(s) + 4H2(g) + O2(g)

 

ANS:  D

DIF:    Harder Question

OBJ:   Know the products of reaction between an ionic hydride and water.

TOP:   Hydrogen and the Hydrides

 

  1. Write the balanced formula unit equation for the reaction of nitrogen with hydrogen at high temperature and pressure. What is the sum of the coefficients? (Do not forget coefficients of one.) Use the smallest whole number coefficients.
a. 6
b. 7
c. 8
d. 4
e. 5

 

 

ANS:  A

OBJ:   Write a balanced chemical equation for the reaction of a nonmetal with hydrogen. | Sum the coefficients.

TOP:   Hydrogen and the Hydrides

 

  1. Write the balanced formula unit equation for the reaction of magnesium with hydrogen at high temperature. What is the sum of the coefficients? (Do not forget coefficients of one.) Use the smallest whole number coefficients.
a. 5
b. 6
c. 3
d. 4
e. none of these

 

 

ANS:  C

OBJ:   Write a balanced chemical equation for the reaction of a metal with hydrogen. | Sum the coefficients.

TOP:   Hydrogen and the Hydrides

 

  1. Write the balanced formula unit equation for the reaction of magnesium with hydrochloric acid. What is the sum of the coefficients? (Do not forget coefficients of one.) Use the smallest whole number coefficients.
a. 5
b. 6
c. 3
d. 4
e. none of these

 

 

ANS:  A

OBJ:   Write a balanced chemical equation for the reaction of a metal with an acid. | Sum the coefficients.

TOP:   Hydrogen and the Hydrides

 

  1. Write the balanced formula unit equation for the reaction of sodium hydride with water. What is the sum of the coefficients in the balanced equation? Use the smallest whole numbers possible. (Do not forget coefficients of one.)
a. three
b. four
c. five
d. six
e. eight

 

ANS:  B

OBJ:   Write a balanced chemical equation for the reaction of an ionic hydride with water. | Sum the coefficients.

TOP:   Hydrogen and the Hydrides

 

  1. Magnesium hydride is ____.
a. basic
b. neutral
c. acidic
d. inert
e. non-reactive with water

 

 

ANS:  A

OBJ:   Classify a hydride as basic, acidic, or neutral.

TOP:   Hydrogen and the Hydrides

 

  1. Oxygen was discovered by Priestley in 1774 when he observed the ____.
a. electrolysis of water
b. thermal decomposition of mercury(II) oxide, HgO
c. reaction of sulfuric acid, H2SO4, with sodium
d. results of fractional distillation of air
e. the thermal decomposition of potassium chlorate, KClO3

 

 

ANS:  B

OBJ:   Know how Priestley discovered oxygen.

TOP:   Oxygen and the Oxides

 

  1. Which of the following statements about oxygen is false?
a. The most common form of oxygen is a diatomic molecule.
b. Ozone is an allotrope of oxygen.
c. Oxygen forms basic metal oxides.
d. Oxygen forms binary compounds with nonmetals called acid anhydrides.
e. Oxygen always forms -2 ions with metals.

 

 

ANS:  E

OBJ:   Know the qualitative chemical facts about oxygen.

TOP:   Oxygen and the Oxides

 

  1. Which one of the following will not react with oxygen to form a peroxide?
a. Be
b. Ca
c. Sr
d. Ba
e. all of these form peroxides

 

 

ANS:  A

OBJ:   Identify the element which will not form a peroxide.

TOP:   Oxygen and the Oxides

 

 

  1. Which statement does not accurately describe ozone?
a. Its molecules are angular.
b. Its density is about 1  times that of O2.
c. Its two oxygen-oxygen bond lengths are 1.23 Å and 1.48 Å.
d. It is unstable.
e. It is a very strong oxidizing agent.

 

 

ANS:  C

OBJ:   Know the structure, physical properties, and reactivity of ozone.

TOP:   Oxygen and the Oxides

 

  1. Which of the following anions represents a peroxide?
a. O–
b. O2–
c. O2–
d. O22–
e. O3–

 

 

ANS:  D

OBJ:   Identify the peroxide ion.

TOP:   Oxygen and the Oxides

 

  1. Which one of the following compounds is a superoxide?
a. Na2O2
b. SrO
c. KO2
d. Li2O
e. Cl2O7

 

 

ANS:  C

OBJ:   Identify the superoxide.

TOP:   Oxygen and the Oxides

 

  1. What is the principal product of the reaction of sodium with oxygen?
a. NaO
b. Na2O
c. Na2O2
d. NaO2
e. Na2O3

 

 

ANS:  C

OBJ:   Identify the principal product of reaction of sodium and oxygen.

TOP:   Oxygen and the Oxides

 

  1. Which one of the following does not represent correctly the major product formed by the reaction of an alkali metal with oxygen at ordinary temperatures and pressures?
a. Li2O2
b. Na2O2
c. KO2
d. RbO2
e. CsO2

 

 

 

ANS:  A

OBJ:   Identify the incorrect principal product of an alkali metal and oxygen reaction.

TOP:   Oxygen and the Oxides

 

  1. Which of the following statements about binary oxides is false?
a. Basic oxides are molecular.
b. Some oxides like BeO are amphoteric.
c. Nonmetal oxides are usually acidic.
d. Metal oxides are usually basic.
e. Acid anhydrides are molecular.

 

 

ANS:  A

OBJ:   Know the qualitative chemical facts about binary oxides.

TOP:   Oxygen and the Oxides

 

  1. Which response includes all the oxides below that are ionic and none that are molecular?
I. Na2O
II. MgO
III. As2O5
IV. SO3

 

a. II and IV
b. I, II, and III
c. I and II
d. III and IV
e. II and III

 

 

ANS:  C

OBJ:   Identify the ionic oxides.

TOP:   Oxygen and the Oxides

 

  1. Which response contains all the basic oxides listed below and no others?
I. NO
II. CaO
III. Li2O
IV. SO2
V. P4O10

 

a. I and IV
b. II and IV
c. I, III, and IV
d. IV and V
e. II and III

 

 

ANS:  E

OBJ:   Identify the basic oxides.

TOP:   Oxygen and the Oxides

 

  1. Which of the following oxides is a basic anhydride?
a. N2O
b. P4O6
c. CaO
d. OF2
e. H2O

 

 

 

ANS:  C

OBJ:   Identify the basic anhydride.

TOP:   Oxygen and the Oxides

 

  1. Which response includes all of the following oxides that are acid anhydrides?
I. CO2
II. CaO
III. ClO2
IV. Tl2O3

 

a. I and III
b. II and IV
c. I and IV
d. II, III, and IV
e. I

 

 

ANS:  A

OBJ:   Identify the acid anhydrides.

TOP:   Oxygen and the Oxides

 

  1. Which of the following oxides does not give an acidic solution when dissolved in water?
a. SO2
b. CO2
c. N2O5
d. P4O10
e. Na2O

 

 

ANS:  E

OBJ:   Identify the basic anhydride.

TOP:   Oxygen and the Oxides

 

  1. An amphoteric compound exhibits
a. acidic properties.
b. acidic and basic properties.
c. metallic properties.
d. basic properties.
e. ionic properties.

 

 

ANS:  B

OBJ:   Define amphoteric.

TOP:   Oxygen and the Oxides

 

  1. Which one of the following oxides is amphoteric?
a. Li2O
b. BeO
c. CO2
d. P4O6
e. Cl2O

 

 

ANS:  B

OBJ:   Identify the amphoteric oxide.

TOP:   Oxygen and the Oxides

 

 

  1. Which of the following oxides is not amphoteric?
a. Al2O3
b. BeO
c. SnO2
d. Br2O7
e. PbO2

 

 

ANS:  D

OBJ:   Identify the non-amphoteric oxide.

TOP:   Oxygen and the Oxides

 

  1. One of the following oxides is insoluble in water. Which one?
a. CO2
b. N2O5
c. SO2
d. SiO2
e. SO3

 

 

ANS:  D

DIF:    Harder Question

OBJ:   Identify the aqueous insoluble compound.

TOP:   Oxygen and the Oxides

 

  1. Arrange the following in order of increasing ionic character (most ionic at right).
  BaO, SiO2, SO2

 

a. BaO < SiO2 < SO2
b. SO2 < BaO < SiO2
c. SiO2 < SO2 < BaO
d. BaO < SO2 < SiO2
e. SO2 < SiO2 < BaO

 

 

ANS:  E

OBJ:   Order the compounds with respect to ionic character (three compounds).

TOP:   Oxygen and the Oxides

 

  1. Arrange the following in order of decreasing basicity.
  MgO, Cs2O, Cl2O7, SnO2, P4O10

 

a. Cs2O > MgO > SnO2 > P4O10 > Cl2O7
b. MgO > Cs2O > P4O10 > SnO2 > Cl2O7
c. Cs2O > SnO2 > MgO > P4O10 > Cl2O7
d. MgO > Cs2O > SnO2 > P4O10 > Cl2O7
e. Cl2O7 > P4O10 > SnO2 > Cs2O > MgO

 

 

ANS:  A

OBJ:   Order the compounds with respect to basic character (five compounds).

TOP:   Oxygen and the Oxides

 

 

  1. Arrange the following in order of increasing acidic character (most acidic at the right).
  Al2O3, Na2O, N2O5

 

a. Al2O3 < Na2O < N2O5
b. N2O5 < Al2O3 < Na2O
c. Al2O3 < N2O5 < Na2O
d. Na2O < Al2O3 < N2O5
e. Na2O < N2O5 < Al2O3

 

 

ANS:  D

OBJ:   Order the compounds with respect to acidic character (three compounds).

TOP:   Oxygen and the Oxides

 

  1. Which one of the following compounds would be expected to react with oxygen at elevated temperatures to produce both an acidic oxide and a basic oxide?
a. CH4
b. CS2
c. CaS
d. NO
e. H2S

 

 

ANS:  C

OBJ:   Identify the compound that combines with oxygen to form acidic and basic oxides.

TOP:   Oxygen and the Oxides

 

  1. The acid formed by dissolving Cl2O7 in water is ____.
a. HClO
b. HClO2
c. HClO3
d. HClO4
e. HCl

 

 

ANS:  D

OBJ:   Identify the acid produced from dissolution of a molecular oxide.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of sodium with oxygen (use the major product). What is the sum of the coefficients?
a. 2
b. 7
c. 3
d. 4
e. 5

 

 

ANS:  D

OBJ:   Write a balanced chemical equation for the reaction of a metal with oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

 

  1. Write the balanced formula unit equation for the reaction of rubidium, Rb, with oxygen (use the major product). What is the sum of the coefficients?
a. 3
b. 7
c. 8
d. 4
e. 5

 

 

ANS:  A

OBJ:   Write a balanced chemical equation for the reaction of a metal with oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of barium with a limited amount (low pressure) of oxygen. What is the sum of the coefficients?
a. 2
b. 6
c. 3
d. 4
e. 5

 

 

ANS:  E

OBJ:   Write a balanced chemical equation for the reaction of a metal with limited oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of barium with an excess (high pressure) of oxygen. What is the sum of the coefficients?
a. 2
b. 8
c. 3
d. 4
e. 5

 

 

ANS:  C

OBJ:   Write a balanced chemical equation for the reaction of a metal with excess oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of copper with excess O2 at elevated temperatures. What is the sum of the coefficients?
a. 6
b. 8
c. 3
d. 4
e. 5

 

 

ANS:  E

OBJ:   Write a balanced chemical equation for the reaction of a metal with excess oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

 

  1. Which of the following metal oxides would not be expected to form under conditions of limited oxygen?
a. FeO
b. PbO
c. Cu2O
d. CrO3
e. SnO

 

 

ANS:  D

OBJ:   Identify the oxide that is unlikely to be formed in limited oxygen.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of arsenic, As4, heated with an excess of oxygen (The molecular formula for the product is the same as the empirical formula). What is the sum of the coefficients?
a. 7
b. 8
c. 3
d. 4
e. 5

 

 

ANS:  B

OBJ:   Write a balanced chemical equation for the reaction of a nonmetal with excess oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of barium oxide with water. What is the sum of the coefficients?
a. 6
b. 8
c. 3
d. 4
e. 5

 

 

ANS:  C

OBJ:   Write a balanced chemical equation for the reaction of a metal oxide with water. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of lithium oxide with water. What is the sum of the coefficients?
a. 2
b. 6
c. 3
d. 4
e. 5

 

 

ANS:  D

OBJ:   Write a balanced chemical equation for the reaction of a metal oxide with water. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

 

  1. Lithium hydroxide is sometimes used to remove carbon dioxide from the atmosphere of disabled submarines. Write the balanced formula unit equation for this reaction if the products are lithium carbonate and water. What is the sum of the coefficients?
a. 7
b. 6
c. 5
d. 4
e. 8

 

 

ANS:  C

OBJ:   Write a balanced chemical equation given the reactants and products. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of dichlorine heptoxide with water. What is the sum of the coefficients?
a. 7
b. 8
c. 3
d. 4
e. 5

 

 

ANS:  D

OBJ:   Write a balanced chemical equation for the reaction of a nonmetal oxide with water. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of dinitrogen pentoxide with water. What is the sum of the coefficients?
a. 6
b. 8
c. 3
d. 4
e. 5

 

 

ANS:  D

OBJ:   Write a balanced chemical equation for the reaction of a nonmetal oxide with water. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Octane, C8H18, is a major component of gasoline. Write the balanced formula unit equation for the reaction of the complete combustion of octane. What is the sum of the coefficients?
a. 49
b. 73
c. 17
d. 61
e. 30

 

 

ANS:  D

OBJ:   Write a balanced chemical equation for the combustion of a hydrocarbon in excess oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

 

  1. Write the balanced formula unit equation for the reaction of the complete combustion of ethane, C2H6. What is the sum of the coefficients?
a. 19
b. 16
c. 17
d. 4
e. 5

 

 

ANS:  A

OBJ:   Write a balanced chemical equation for the combustion of a hydrocarbon in excess oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of the complete combustion of pentane, C5H12. What is the sum of the coefficients?
a. 16
b. 19
c. 20
d. 21
e. 22

 

 

ANS:  C

OBJ:   Write a balanced chemical equation for the combustion of a hydrocarbon in excess oxygen. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Write the balanced formula unit equation for the reaction of nitrogen oxide with oxygen. What is the sum of the coefficients?
a. 3
b. 6
c. 8
d. 4
e. 5

 

 

ANS:  E

OBJ:   Write a balanced chemical equation for the combustion of a nonmetal oxide. | Sum the coefficients.

TOP:   Oxygen and the Oxides

 

  1. Most of the air pollution resulting from combustion of (non-lead-containing) fossil fuels is due to oxides of ____.
a. N, P, and S
b. C, N, and S
c. C, P, and S
d. P and C
e. P, C, and N

 

 

ANS:  B

OBJ:   Know the oxides that result from the combustion of fossil fuels.

TOP:   Oxygen and the Oxides

 

 

  1. Combustion of fossil fuels and the roasting of metal ores often both produce oxides of
a. P
b. N
c. S
d. Si
e. C

 

 

ANS:  C

OBJ:   Know the oxides that result from the combustion of fossil fuels and roasting of ores.

TOP:   Oxygen and the Oxides

 

  1. The brownish color of photochemical smog is due to ____.
a. CO
b. NO2
c. NO
d. SO2
e. SO3

 

 

ANS:  B

OBJ:   Know the components of smog.

TOP:   Oxygen and the Oxides

 

  1. Combustion of fossil fuels contaminated with sulfur leads to what phenomena?
a. greenhouse effect
b. global warming
c. ozone destruction
d. photochemical smog
e. acid rain

 

 

ANS:  E

OBJ:   Know the effect of sulfur contamination in fossil fuels.

TOP:   Oxygen and the Oxides

 

  1. The two acids that are major contributors to “acid rain” are ____.
a. H2CO3 and HNO3
b. H2SO4 and H3PO4
c. H2CO3 and H2SO4
d. H2SO4 and HNO3
e. H3PO4 and HNO3

 

 

ANS:  D

OBJ:   Identify the acids which contribute to acid rain.

TOP:   Oxygen and the Oxides

 

  1. The ground-state valence-shell configuration of a particular atom is 4s24p6. This valence-shell electron configuration identifies the atom as

 

a. a noble gas.
b. a d-transition element.
c. an f-transition element.
d. an s-block representative element.
e. a p-block representative element.

 

 

 

ANS:  A

DIF:    easy

OBJ:   Classify a group of elements based on thier valence shell electron configuration.

TOP:   More About the Periodic Table

 

  1. An element that has the same ground state valence-shell electron configuration as silicon is

 

a. lead.
b. argon.
c. lithium.
d. magnesium.
e. gallium.

 

 

ANS:  A

DIF:    easy

OBJ:   Determine the configuration of an atom using the period and group numbers.

TOP:   electronic structure of atoms

 

  1. Rank the following atoms in order of the largest to smallest atomic radius: Se, K, As, Rb.

 

a. Rb > K > As > Se
b. K > Rb > As > Se
c. As > K > Rb > Se
d. K > As > Se > Rb
e. Rb > As > K > Se

 

 

ANS:  A

DIF:    moderate

OBJ:   Arrange the atoms according to size (four atoms).

TOP:   Atomic Radii

 

 

  1. The change in energy for which of the following processes corresponds to the first ionization energy of magnesium?
a.
b.
c.
d.
e.

 

 

ANS:  A

DIF:    easy

OBJ:   Identify the equation depicting the first ionization of an element.

TOP:   Ionization Energy

 

  1. An atom of which of the following elements has the largest second ionization energy?
a. Cs
b. At
c. Po
d. Pb
e. Ba

 

 

 

ANS:  A

DIF:    moderate

OBJ:   Identify the element with the largest second ionization energy.

TOP:   Ionization Energy

 

  1. Which of the following form the most stable anion in the gas phase?

 

a. Cl (electron affinity = -349 kJ/mol)
b. As (electron affinity = -77 kJ/mol)
c. P (electron affinity = -72 kJ/mol)
d. Al (electron affinity = -44 kJ/mol)
e. Na (electron affinity = -53 kJ/mol)

 

 

ANS:  A

DIF:    easy

OBJ:   Identify the most stable anion based on atom electron affinities.

TOP:   Electron Affinity

 

  1. Which of the following statements is true concerning a concentrated solution of lithium oxide in water?
a. The resulting solution is strongly basic.
b. The resulting solution is weakly acidic.
c. The resulting solution is neither acidic nor basic.
d. The resulting solution is weakly basic.
e. The resulting solution is strongly acidic.

 

 

ANS:  A

DIF:    easy

OBJ:   Recognize a basic oxide.

TOP:   Oxygen and the Oxides

 

  1. Which of the following species is isoelectronic with Ar?
a.
b.
c.
d.
e. Ne

 

 

ANS:  B

DIF:    easy

OBJ:   Identify the atom or ion that is isoelectronic with the given element.

TOP:   electronic structure of atoms

 

  1. Which of the following species would you expect to have the largest radius?
a.
b. P
c.
d.
e.

 

 

 

ANS:  D

DIF:    easy

OBJ:   Identify the element or ion with the largest radius.

TOP:   Ionic Radii

 

 

  1. Rank the following ions in order of decreasing ionic radii: K+, Cl–, Se2-, Br–.

 

a. Br– >  Se2- > Cl– > K+
b. Se2- > Br– > Cl– > K+
c.  K+> Cl– >  Se2- > Br–
d. Br– >  Cl– > Se2- > K+
e.  Cl– >  Se2- > K+ > Br–

 

 

ANS:  A

DIF:    easy

OBJ:   Rank the ions in order of decreasing ionic radius.

TOP:   Ionic Radii

 

 

  1. Which of the following elements would have the highest first ionization energy?
a. Beryllium b. Boron c. Carbon d. Lithium e. Silicon

 

 

ANS:  C

OBJ:   Identify the element with the highest first ionization energy.

TOP:   Ionization Energy

 

  1. Choose the statement that is true:
a. Outer electrons efficiently shield one another from nuclear charge
b. Core electrons effectively shield outer electrons from nuclear charge
c. Valence electrons are most difficult of all electrons to remove
d. Core electrons have the lowest ionization energies of all electrons
e. Two of the above are true.

 

 

ANS:  B

OBJ:   Identify the correct statement about shielding.

TOP:   Ionization Energy

 

  1. Arrange the following atoms in order of increasing atomic radius:

arsenic      oxygen       bromine

a. arsenic < bromine < oxygen
b. arsenic < oxygen < bromine
c. oxygen < bromine < arsenic
d. oxygen < arsenic < bromine
e. bromine < arsenic < oxygen

 

 

ANS:  C

OBJ:   Rank the elements according to atomic radii.

TOP:   Atomic Radii

 

 

  1. What is the oxidation state of arsenic in arsenic acid, H3AsO4?
a. +1 b. -1 c. +3 d. -5 e. +5

 

 

ANS:  E

OBJ:   Determine the oxidation state of an element in a compound.

TOP:   Oxidation States

 

  1. What is the oxidation state of sulfur in sulfur dioxide, SO2?
a. +1 b. -1 c. +2 d. -2 e. +4

 

 

ANS:  E

OBJ:   Determine the oxidation state of an element in a polyatomic ion.

TOP:   Oxidation States

 

  1. What is the oxidation state of phosphorus in POCl3?
a. 0 b. +3 c. -3 d. +5 e. -5

 

 

ANS:  D

OBJ:   Determine the oxidation state of an element in a compound.

TOP:   Oxidation States

 

  1. Arrange the following elements in order of lowest to highest electronegativity:

Sodium, rubidium, potassium, cesium

a. Na < Rb < K < Cs
b. Na < K < Rb < Cs
c. Cs < Rb < K < Na
d. Rb < Cs < Na < K
e. Cs < K < Na < Rb

 

 

ANS:  C

OBJ:   Rank the elements according to electronegativity.

TOP:   Electronegativity

 

CONCEPTUAL

 

  1. Use the screening effect to explain why a sodium atom has a larger radius than a lithium atom.

 

OBJ:   Explain nuclear shielding and its effect on the size of an atoms in the same group.

TOP:   Atomic Radii

 

  1. Explain why the 1st ionization energy of N is larger than that of O.

 

OBJ:   Contrast the first ionization energies of nitrogen and oxygen.

TOP:   Ionization Energy

 

  1. The 2nd ionization energy is the energy to remove a second electron. Why is IE2 of potassium much larger than IE1? Comment on the relative values of IE1 of Ne and the IE2 of Na.

 

OBJ:   Explain the large increase in the second ionization energy of the alkali metals.

TOP:   Ionization Energy

 

 

  1. Why are electronegativity values not usually given for Group VIIIA elements?

 

OBJ:   Explain the dearth of electronegativity values for the noble gases.

TOP:   Electronegativity

 

  1. Burning fossil fuels produces SO2, a pollutant responsible for acid rain. SO2 is formed when sulfur in the fossil fuels combines with oxygen during combustion. Give several ways to reduce the amount of acid rain produced by SO2.

 

OBJ:   Suggest ways to minimize the formation acid rain from sulfur dioxide pollution.

TOP:   Oxygen and the Oxides

 

  1. H2-O2 fuel cells are gaining popularity as “zero emission” methods of powering an automobile. Electricity is generated when H2 and O2 forms water. Describe some ways that hydrogen and oxygen could be produced for this reaction. Would these fuel cell cars really be zero emission?

 

OBJ:   Detail several methods for production of hydrogen and oxygen.

TOP:   Hydrogen and the Hydrides | Oxygen and the Oxides

 

  1. Explain why the ionic radii of cations is smaller than the atomic radii while the ionic radii of the anions are larger than the atomic radii.

 

OBJ:   Explain the size trends between ionic and atomic radii of the same element.

TOP:   Ionic Radii | Atomic Radii

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