Chapter 8 Periodic Properties of the Elements

A

No two electrons can have the same four quantum numbers is known as the
A) Pauli exclusion principle
B) Hund's rule
C) Aufbau principle
D) Heisenberg uncertainty principle

C

Only two electrons, with opposing spins, are allowed in each orbital is known as the
A) Pauli exclusion principle
B) Hund's rule
C) Aufbau principle
D) Heisenberg uncertainty principle

B

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as
A) Pauli exclusion principle
B) Hund's rule
C) Aufbau principle
D) Heisenberg uncertainty principle

A

Which of the following statements is TRUE?
A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear
charge than an orbital that does not penetrate and therefore has a lower energy.
B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear
charge than an orbital that does not penetrate and therefore has a lower energy.
C) It is possible for two electrons in the same atom to have identical values for all four quantum
numbers.
D) Two electrons in the same orbital can have the same spin.
E) None of the above are true

C

The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is ________.
A) titanium
B) vanadium
C) chromium
D) manganese
E) iron

A

Give the ground state electron configuration for Se.
A) [Ar]4s23d104p4
B) [Ar]4s24d104p4
C) [Ar]4s23d104p6
D) [Ar]4s23d10
E) [Ar]3d104p4

B

Give the ground state electron configuration for I.
A) [Kr]5s24d105p6
B) [Kr]5s24d105p5
C) [Kr]4d105p6
D) [Kr]5s25p6
E) [Kr]5s25d105p6

C

Give the ground state electron configuration for Sr.
A) [Kr]5s24d2
B) [Kr]5s24d105p2
C) [Kr]5s2
D) [Kr]5s25d105p2
E) [Kr]5s24d10

D

Give the ground state electron configuration for Pb.
A) [Xe]6s26p2
B) [Xe]6s25d106p2
C) [Xe]6s25f146d106p2
D) [Xe]6s24f145d106p2
E) [Xe]6s24f145d106s26p2

E

Give the ground state electron configuration for Cd.
A) [Kr]5s25d10
B) [Kr]5s24d105p2
C) [Kr]4d10
D) [Kr]5s24d8
E) [Kr]5s24d10

C

Give the complete electronic configuration for Mn.
A) 1s22s22p63s23p64s24d5
B) 1s22s22p63s23p64s13d6
C) 1s22s22p63s23p64s23d5
D) 1s22s22p63s23p64s24p5

A

Identify the element that has a ground state electronic configuration of [Kr]5s24d5.
A) Tc
B) Mn
C) Nb
D) Ru

C

Give the number of core electrons for Cd.
A) 44
B) 48
C) 46
D) 45
E) 47

D

Give the number of valence electrons for Cd.
A) 8
B) 10
C) 12
D) 2
E) 6

D

How many valence electrons does an atom of Al possess?
A) 1
B) 2
C) 5
D) 3
E) 8

E

How many valence electrons do the halogens possess?
A) 5
B) 6
C) 2
D) 1
E) 7

B

How many valence electrons do the alkali earth metals possess?
A) 1
B) 2
C) 7
D) 6
E) 8

A

How many valence electrons do the alkali metals possess?
A) 1
B) 2
C) 7
D) 6
E) 8

E

How many valence electrons do the noble gases possess?
A) 1
B) 2
C) 7
D) 6
E) 8

C

Place the following elements in order of increasing atomic radius.
P, Ba, Cl
A) Ba < P < Cl
B) P < Cl < Ba
C) Cl < P < Ba
D) Cl < Ba < P
E) Ba < Cl < P

E

Place the following in order of increasing atomic radius.
As, O, Br
A) As < Br < O
B) O < As < Br
C) Br < As < O
D) As < O < Br
E) O < Br < As

A

A cation of +2 indicates that an element has
A) lost two electrons.
B) lost two protons.
C) lost two neutrons.
D) gained two electrons.
E) gained two protons

B

Place the following in order of increasing radius.
Br⁻ Na⁺ Rb⁺
A) Br⁻ < Rb⁺ < Na⁺
B) Na⁺ < Rb⁺ < Br⁻
C) Rb⁺ < Br⁻ < Na⁺
D) Br⁻ < Na⁺ < Rb⁺
E) Rb⁺ < Na⁺ < Br-

C

Place the following in order of decreasing radius.
Te2⁻ F⁻ O2⁻
A) F⁻ > O2⁻ > Te2⁻
B) F⁻ > Te2⁻ > O2⁻
C) Te2⁻ > O2⁻ > F⁻
D) Te2⁻ > F⁻ > O2⁻
E) O2⁻ > F⁻ > Te2-

B

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 are the easiest of all electrons to remove.
E) All of the above are true

D

Which reaction below represents the first ionization of O?
A) O⁺(g) + e⁻ → O(g)
B) O(g) + e⁻ → O⁻(g)
C) O⁻(g) → O(g) + e⁻
D) O(g) → O⁺(g) + e⁻
E) O⁻(g) + e⁻ → O2⁻(g)

E

Which reaction below represents the second ionization of Sr?
A) Sr(g) → Sr⁺(g) + e⁻
B) Sr2⁺(g) + e⁻ → Sr⁺(g)
C) Sr⁺(g) + e⁻ → Sr(g)
D) Sr⁻(g) + e⁻ → Sr2⁻(g)
E) Sr⁺(g) → Sr2⁺(g) + e-

C

What period 3 element having the following ionization energies (all in kJ/mol)?
IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200
A) Si
B) S
C) P
D) Cl
E) Mg

B

Place the following in order of increasing IE1.
N, F, As
A) N < As < F
B) As < N < F
C) F < N < As
D) As < F < N
E) F < As < N

C

Place the following in order of decreasing IE1.
Cs, Mg, Ar
A) Cs > Mg > Ar
B) Mg > Ar > Cs
C) Ar > Mg > Cs
D) Cs > Ar > Mg
E) Mg > Cs > Ar

D

Place the following in order of increasing IE1.
K, Ca, Rb
A) Ca < K < Rb
B) Rb < Ca < K
C) Ca < Rb < K
D) Rb < K < Ca
E) K < Ca < Rb

A

Identify the species that has the smallest radius.
A) cation
B) anion
C) neutral
D) they are all the same size