Question 1

Which of the following electron configurations is impossible?

Accepted Answer

A)   1s22s22p63s23p4
B)   1s22s22p53s13p4
C)   1s22s22p63s23p63d104s2
D)   1s22s22p63s33p4
E)   1s12s22p63s23p4F) B) and E)
G) D) and E)

Question 2

Which of the following elements has the largest first ionization energy?

Accepted Answer

A)   Na
B)   Cl
C)   Ca
D)   Te
E)   BrF) A) and D)
G) A) and C)

Question 3

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Accepted Answer

A) True 
 B)False

Question 4

Atomic size decreases across a period due to an increase in the effective nuclear charge, Zeff.

Accepted Answer

A) True 
 B)False

Question 5

An atom of element number 33 (As)  is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Accepted Answer

A)   n = 2 l = 1 ml = -1 ms = +½
B)   n = 3 l = 0 ml = 0 ms = -½
C)   n = 3 l = 2 ml = -2 ms = -½
D)   n = 4 l = 0 ml = 0 ms = -½
E)   n = 4 l = 2 ml = 1 ms = +½F) All of the above
G) A) and D)

Question 6

In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Accepted Answer

A) True 
 B)False

Question 7

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471
IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

Accepted Answer

A)   Li
B)   B
C)   O
D)   Ne
E)   None of these choices are correct.F) B) and D)
G) C) and E)

Question 8

According to the exclusion principle, two is the maximum number of electrons in an atom which can share the same four quantum numbers.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following elements will form a cation with a +2 charge?

Accepted Answer

A)   Si
B)   Sr
C)   Ga
D)   Cs
E)   SF) C) and E)
G) B) and D)

Question 10

Which of the following sublevels is filled last? 3d, 4s, 4p, 4d, 5s

Accepted Answer

A)   3d
B)   4s
C)   4p
D)   4d
E)   5sF) B) and D)
G) A) and D)

Question 11

A negative electron affinity implies that the atom repels an approaching electron.

Accepted Answer

A) True 
 B)False

Question 12

Elements in the same period of the periodic table have similar valence shell electron configurations.

Accepted Answer

A) True 
 B)False

Question 13

Bigger atoms generally have smaller ionization energies.

Accepted Answer

A) True 
 B)False

Question 14

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Accepted Answer

A)   X(g)  → X+(g)  + e-
B)   X+(g)  → X+(aq) 
C)   X+(g)  + e- → X(g) 
D)   X(g)  + e- → X-(g) 
E)   X+(g)  + Y-(g)  → XY(s) F) A) and E)
G) D) and E)

Question 15

Which of the following fourth-period elements has the smallest atomic radius?

Accepted Answer

A)   K
B)   Ti
C)   Cu
D)   Ge
E)   KrF) B) and E)
G) A) and D)

Question 16

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Accepted Answer

A)   the first valence electron is removed.
B)   the second valence electron is removed.
C)   the eighth electron of is removed.
D)   the first core electron is removed.
E)   the last valence electron is removed.F) C) and D)
G) All of the above

Question 17

Which of the following elements has the largest second ionization energy (IE2) ?

Accepted Answer

A)   Li
B)   B
C)   O
D)   F
E)   NaF) A) and B)
G) A) and E)

Question 18

Which of the following elements has the greatest atomic radius?

Accepted Answer

A)   Li
B)   Ne
C)   Rb
D)   Sr
E)   XeF) A) and D)
G) A) and E)

Question 19

Which of the following has the most negative electron affinity?

Accepted Answer

A)   H
B)   Li
C)   Na
D)   K
E)   RbF) C) and D)
G) A) and B)

Question 20

Consider the set of isoelectronic atoms and ions A2-, B-, C, D+, and E2+. Which arrangement of relative radii is correct?

Accepted Answer

A)   A2- > B- > C > D+ > E2+
B)   E2+ > D+ > C > B- > A2-
C)   A2- > B- > C + 2+
D)   A2- -  D+ > E2+
E)   None of these choices are correct.F) C) and E)
G) All of the above

Exam 8: Electron Configuration and Chemical Periodicity

Elements in the same period of the periodic table have similar valence shell electron configurations.

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Which one of the following equations correctly represents the process involved in the electron affinity of X?

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Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471 IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

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Bigger atoms generally have smaller ionization energies.

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In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

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Which of the following sublevels is filled last? 3d, 4s, 4p, 4d, 5s

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Which of the following elements has the greatest atomic radius?

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Which of the following electron configurations is impossible?

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The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

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A negative electron affinity implies that the atom repels an approaching electron.

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Which of the following has the most negative electron affinity?

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When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

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According to the exclusion principle, two is the maximum number of electrons in an atom which can share the same four quantum numbers.

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Which of the following elements has the largest second ionization energy (IE2) ?

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Which of the following elements will form a cation with a +2 charge?

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Atomic size decreases across a period due to an increase in the effective nuclear charge, Zeff.

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Consider the set of isoelectronic atoms and ions A2-, B-, C, D+, and E2+. Which arrangement of relative radii is correct?

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An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

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Which of the following fourth-period elements has the smallest atomic radius?

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Which of the following elements has the largest first ionization energy?

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Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE₁, 1314 IE₂, 3389 IE₃, 5298 IE₄, 7471 IE₅, 10992 IE₆, 13329 IE₇, 71345 IE₈, 84087

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Which of the following elements has the largest second ionization energy (IE₂) ?

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Consider the set of isoelectronic atoms and ions A^2-, B^-, C, D⁺, and E²⁺. Which arrangement of relative radii is correct?

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