Deck 6: Electronic Structure and the Periodic Table

Question 1

A line in the Pfund series (n_lo = 5)occurs at 3.74 × 10−⁶ m.What is n_hi for this transition? The Rydberg constant equals 2.180 × 10−¹⁸ J.

A) 6
B) 7
C) 8
D) 9
E) 10

Answer 1

8

Question 2

The Pauli exclusion principle states that

A) no two electrons from a given atom can have the same spin.
B) no two electrons from a given atom can have the same four quantum numbers.
C) two electrons can occupy an orbital if they have the same spin.
D) two electrons can occupy an orbital if they have the same charge.
E) two electrons can occupy an orbital if they have opposite charges.

Answer 2

no two electrons from a given atom can have the same four quantum numbers.

Question 3

All of the following sets of quantum numbers are allowed EXCEPT

A) n = 1, $\ell$ = 0, $\mathrm{m}_{\ell}$ = 1,m_s = ? $1 / 2$ .
B) n = 2, $\ell$ = 1, $\mathrm{m}_{\ell}$ = 0,m_s = + $1 / 2$ .
C) n = 3, $\ell$ = 1, $\mathrm{m}_{\ell}$ = ?1,m_s = ? $1 / 2$ .
D) n = 4, $\ell$ = 3, $\mathrm{m}_{\ell}$ = ?1,m_s = ? $1 / 2$ .
E) n = 6, $\ell$ = 3, $\mathrm{m}_{\ell}$ = ?3,m_s = + $1 / 2$ .

Answer 3

n = 1, $\ell$ = 0, $\mathrm{m}_{\ell}$ = 1,m_s = ? $1 / 2$ .

Question 4

According to the Bohr model for the hydrogen atom,the energy necessary to excite an electron from n = 2 to n = 3 is ____ the energy necessary to excite an electron from n = 3 to n = 4.

A) greater than
B) equal to
C) less than
D) either equal to or greater than
E) either less than or equal to

Question 5

The Schrödinger wave equation

A) proves electrons have positive and negative spins.
B) calculates the precise position and momentum of an electron at any given time.
C) is used to compute the wavelength of small particles.
D) can be solved to find the probability of finding an electron in a region of space.
E) proves that photons are particles.

Question 6

Calculate the wavelength of the line in the Lyman series that results from the transition n = 3 to n = 1.The Rydberg constant equals 2.180 × 10−¹⁸ J.

A) 45.59 nm
B) 72.81 nm
C) 91.12 nm
D) 102.5 nm
E) 136.7 nm

Question 7

If the energy of 1.00 mole of photons is 245 kJ,what is the wavelength of the light?

A) 122 nm
B) 488 nm
C) 1220 nm
D) 787 nm
E) 811 nm

Question 8

What type of orbital is designated n = 3, $\ell$ = 2, $\mathrm{m}_{\ell}$ = -2?

A) 3s
B) 3p
C) 3d
D) 2f
E) 2d

Question 9

The ____ of a photon of light is ____ proportional to its frequency and ____ proportional to its wavelength.

A) energy,directly,inversely
B) energy,inversely,directly
C) velocity,directly,inversely
D) intensity,inversely,directly
E) amplitude,directly,inversely

Question 10

Excited sodium atoms emit light in the infrared at 589 nm.What is the energy of a single photon with this wavelength?

A) 5.09 × 10¹⁴ J
B) 1.12 × 10^-27 J
C) 3.37 × 10^-19 J
D) 3.37 × 10^-28 J
E) 1.30 × 10^-19 J

Question 11

Some digital cordless phones operate at 2.4 GHz (1 GHz = 10⁹ Hz).What is the energy,in joules,of a single 2.4 GHz photon?

A) 8.3 × 10−³⁵ J
B) 1.6 × 10−²⁴ J
C) 5.4 × 10−¹⁹ J
D) 0.96 J
E) 0.13 J

Question 12

What is the frequency of a gamma ray radiation that has a wavelength of 11.4 pm?

A) 3.80 × 10^-20 s^-1
B) 1.74 × 10^-14 s^-1
C) 2.63 × 10⁷ s^-1
D) 3.42 × 10⁹ s^-1
E) 2.63 × 10¹⁹ s^-1

Question 13

How many orbitals have the following set of quantum numbers: n = 5, $\ell$ = 3, $m_{\ell}$ = +2?

A) 0
B) 1
C) 3
D) 6
E) 7

Question 14

For which of the following transitions would a hydrogen atom absorb a photon with the longest wavelength?

A) n = 1 to n = 2
B) n = 4 to n = 6
C) n = 5 to n = 4
D) n = 7 to n = 6
E) n = 6 to n = 7

Question 15

Which of the following sets of quantum numbers refers to a 2s orbital?

A) n = 1, $\ell$ = 2, $\mathrm{m}_{\ell}$ = 2,m_s = + $1 / 2$
B) n = 1, $\ell$ = 2, $\mathrm{m}_{\ell}$ = 1,m_s = + $1 / 2$
C) n = 2, $\ell$ = 2, $\mathrm{m}_{\ell}$ = 0,m_s = + $1 / 2$
D) n = 2, $\ell$ = 1, $\mathrm{m}_{\ell}$ = ?1,m_s = + $1 / 2$
E) n = 2, $\ell$ = 0, $\mathrm{m}_{\ell}$ = 0,m_s = + $1 / 2$

Question 16

Calculate the energy of a photon in the Balmer series that results from the transition n = 3 to n = 2.What is the region of the electromagnetic spectrum? The Rydberg constant equals 2.180 × 10−¹⁸ J.

A) 3.028 × 10−¹⁹ J;visible
B) 4.578 × 10−¹⁹ J;infrared
C) 3.633 × 10−¹⁹ J;visible
D) 3.633 × 10−¹⁸ J;ultraviolet
E) 2.180 × 10−¹⁸ J;ultraviolet

Question 17

Green laser pointers emit radiation at 532 nm.What is the frequency of this radiation?

A) 8.12 × 10¹³ Hz
B) 5.64 × 10¹⁴ Hz
C) 1.60 × 10¹⁵ Hz
D) 9.10 × 10¹⁵ Hz
E) 1.60 × 10¹⁶ Hz

Question 18

What is the total number of orbitals having n = 4 and $\ell$ = 2?

A) 3
B) 5
C) 7
D) 9
E) 10

Question 19

When Cs-137 decays,it emits gamma radiation.The energy of one photon is 1.06 × 10−¹³ J.What is the wavelength of this radiation?

A) 1.87 × 10−¹² m
B) 2.08 × 10−¹² m
C) 2.44 × 10−¹² m
D) 1.88 × 10−¹¹ m
E) 1.58 × 10−¹⁰ m

Question 20

Place the following regions of the electromagnetic spectrum in order from highest to lowest energy.

A) infrared > gamma rays > x-rays > visible > radio
B) gamma rays > x-rays > visible > infrared > radio
C) x-rays > gamma rays > infrared > visible > radio
D) radio > x-rays > gamma rays > visible > infrared
E) visible > infrared > radio > x-rays > gamma rays

Question 21

What is the ground state electron configuration for Cr³⁺?

A) [Ar]
B) [Ar]3d⁷4s²
C) [Ar]3d¹4s²
D) [Ar]3d²4s¹
E) [Ar]3d³

Question 22

What is the total capacity of electrons in n = 3?

A) 5
B) 10
C) 18
D) 32
E) 50

Question 23

What is the electron configuration of S²⁻?

A) 1s²2s²2p⁶
B) 1s²2s²2p⁶3s²
C) 1s²2s²2p⁶3s²3p⁴
D) 1s²2s²2p⁶3s²3p⁶
E) 1s²2s²2p⁶3s²3p⁶4s¹

Question 24

What is the electron configuration of ₈₀Hg?

A) [Xe]6s²6d¹⁰
B) [Kr]5d¹⁰6s²
C) [Xe]4f¹⁴5d¹⁰6s²
D) [Xe]5d¹⁰6s²
E) [Kr]4d¹⁰4f¹⁴6s²

Question 25

Place the following atoms in order of increasing atomic radii: K,Na,Be,and Li?

A) Li < Na < K < Be
B) Be < K < Na < Li
C) Be < Li < Na < K
D) K < Na < Li < Be
E) Li < Be < Na < K

Question 26

Place the following atoms or ions in order of increasing radius: O,O²⁻,S²⁻,and Se²⁻.

A) O²⁻ < O < S²⁻ < Se²⁻
B) Se²⁻ < S²⁻ < O²⁻ < O
C) O²⁻ < O < Se²⁻ < S²⁻
D) Se²⁻ < S²⁻ < O < O²⁻
E) O < O²⁻ < S²⁻ < Se²⁻

Question 27

What is the ground state electron configuration of ₉₄Pu?

A) [Xe]5f⁶6s²
B) [Xe]6f⁶7s²
C) [Rn]6f⁶7s²
D) [Rn]5f⁶7s²
E) [Rn]5f⁶6d¹⁰7s²

Question 28

Which of the following properties is associated with the value of the quantum number $\ell$ ?

A) The shape of an orbital
B) The size of an orbital
C) The number of electrons in an orbital
D) The energy of an orbital
E) The orientation in space of an orbital

Question 29

What type of orbital is designated by n = 5, $\ell$ = 2, $\mathrm{m}_{\ell}$ = +1?

A) 5d
B) 2f
C) 5p
D) 2s
E) 5p..

Question 30

What is the electron configuration of Ga⁺?

A) [Ar]3d¹⁰4s²
B) [Ar]3d¹⁰4p²
C) [Ar]3d⁸4s²4p²
D) [Ar]3d¹⁰4s²4d⁴
E) [Ar]3d¹⁰4s²4p²

Question 31

Which of the following sets of quantum numbers refers to a 4f orbital?

A) n = 4, $\ell$ = 1, $\mathrm{m}_{\ell}$ = 0,m_s = + $\frac{1}{2}$
B) n = 4, $\ell$ = 2, $\mathrm{m}_{\ell}$ = -1,m_s = + $\frac{1}{2}$
C) n = 4, $\ell$ = 3, $\mathrm{m}_{\ell}$ = ?2,m_s = ? $\frac{1}{2}$
D) n = 4, $\ell$ = 4, $\mathrm{m}_{\ell}$ = 0,m_s = + $\frac{1}{2}$
E) n = 4, $\ell$ = 4, $\mathrm{m}_{\ell}$ = ?4,m_s = + $\frac{1}{2}$

Question 32

What is the ground state electron configuration of ₂₅Mn?

A) 1s²2s²2p⁶3s²3p⁶3d⁶4s¹
B) 1s²2s²2p⁶3s²3p⁶3d⁵4s²
C) 1s²2s²2p⁶3s²3p⁶3d⁷
D) 1s²2s²2p⁶3s²3p⁶3d⁵
E) 1s²2s²2p⁶3s²3p⁶4s²4d⁵

Question 33

Place the following atoms in order of increasing atomic radius: Al,Cl,Mg,O,and P.

A) Cl < O < P < Al < Mg
B) Cl < P < Al < Mg < O
C) O < Cl < P < Al < Mg
D) O < Mg < Al < P < Cl
E) none of the above

Question 34

Rank F,Cl,and Br in order of increasing first ionization energy.

A) F < Cl < Br
B) Cl < F < Br
C) Cl < Br < F
D) Br < F < Cl
E) Br < Cl < F

Question 35

Hund's rule predicts that

A) the most stable electronic structure of an atom has electron spins paired.
B) no two electrons will share the same orbital.
C) electrons in an orbital have equal but opposite charges.
D) electrons must have opposite spins to share an orbital.
E) when several orbitals of equal energy are available,as in a given subshell,electrons enter singly with parallel spins.

Question 36

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.

Question 37

Elements and compounds with unpaired electrons are attracted to a magnetic field.These materials are called paramagnetic.Which of the following ions are paramagnetic in the ground state?

A) I−
B) Ni²⁺
C) P³⁻
D) Ca²⁺
E) Ti⁴⁺

Question 38

What is the total capacity of electrons in n = 5, $\ell$ = 3?

A) 2
B) 6
C) 10
D) 14
E) 32

Question 39

Place the following ions in order of increasing radius: Al³⁺,F−,Mg²⁺,and N³⁻.

A) F− < Mg²⁺ < N³⁻ < Al³⁺
B) F− < N³⁻ < Al³⁺ < Mg²⁺
C) F− < N³⁻ < Mg²⁺ < Al³⁺
D) N³⁻ < F− < Mg²⁺ < Al³⁺
E) Al³⁺ < Mg²⁺ < F− < N³⁻

Question 40

Which of the following ions have the same ground state electron configuration: S^2-,N^3-,Mg²⁺,and Br^-?

A) N^3- and Mg²⁺
B) S^2-,N^3-,and Br^-
C) S^2- and Br^-
D) Mg²⁺ and Br^-
E) S^2-,N^3-,Mg²⁺,and Br^-

Question 41

Place the following atoms in order of increasing ionization energy: N,O,and P.

A) N < P < O
B) O < P < N
C) P < N < O
D) N < O < P
E) P < O < N

Question 42

Which of the following elements is assigned an electronegativity value of 4.0,which is the greatest electronegativity value?

A) H
B) Au
C) F
D) He
E) Cs

Question 43

Place the following ions in order of increasing size: Al³⁺,P³⁻,and S²⁻

A) P³⁻ < S²⁻ < Al³⁺
B) Al³⁺ < P³⁻< S²⁻
C) Al³⁺ < S²⁻ < P³⁻
D) P³⁻ < Al³⁺ < S²⁻
E) S²⁻ < Al³⁺ < P³⁻

Question 44

Which of the following chemical expressions refers to the first ionization energy of calcium?

A) Ca(s)→ Ca⁺(s)+ e−
B) Ca(g)+ e− → Ca⁺(g)
C) Ca(s)+ e− → Ca⁺(s)
D) Ca(g)→ Ca⁺(g)+ e−
E) Ca(g)→ Ca²⁺(g)+ e−

Question 45

The color of the shell of a cooked lobster is due to

A) the denaturing of the protein crustacyanin releasing astaxanthin a pigment that absorbs blue light.
B) the denaturing of the protein crustacyanin releasing astaxanthin a pigment that absorbs red light.
C) the temperature of the shell.
D) the reaction of the water with the pigments in the lobster shell.
E) the pigments dissolved in the water absorbing into the lobster shell.

Question 46

Glenn Seaborg is known for the discovery of many elements.What do these elements have in common?

A) They all occur in nature
B) They all contain 5f electrons
C) They are all isotopes of uranium
D) They are all required to prepare a nuclear bomb
E) They are all used in the electronics industry

Question 47

Which of the five atoms Na,N,Cl,Mg,or Al has the largest atomic radius?

A) Na
B) N
C) Cl
D) Mg
E) Al

Question 48

Electronegativity increases

A) moving down a group in the periodic table.
B) moving from left to right across the periodic table.
C) with increasing atomic mass.
D) when electrons are paired.
E) with increasing atomic radii.