Deck 7: Electron Configurations and the Periodic Table

Question 1

Light has a wavelength of 582 nm. What is its frequency? The speed of light is 3.00 × 10⁸ m/s.

A) 1.75 × 10²⁰ Hz
B) 5.15 × 10¹⁴ Hz
C) 1.94 × 10¹³ Hz
D) 1.94 × 10³ Hz
E) 1.75 × 10² Hz

Answer 1

5.15 × 10¹⁴ Hz

Question 2

Which new idea was proposed by Louis de Broglie?

A) Electrons are located in orbits.
B) Electrons can be viewed in terms of their wave and particle properties.
C) Energy in the atom is quantized.
D) An excited hydrogen atom emits a line spectrum.
E) Excited state orbits have higher energy than ground state orbits.

Answer 2

Electrons can be viewed in terms of their wave and particle properties.

Question 3

Light has a frequency of 5.45 × 10¹⁴ hertz. What is its wavelength? The speed of light is 3.00 × 10⁸ m/s.

A) 1.82 × 10⁶ nm
B) 1.82 × 10^-3 nm
C) 1.82 × 10⁵ nm
D) 5.50 × 10^-7 nm
E) 550 nm

Answer 3

550 nm

Question 4

Which of the following is not a characteristic of the Bohr model of the atom?

A) Orbits have variable radii.
B) An electron is restricted to specific energy levels around the nucleus.
C) Each orbit has a discrete energy associated with it.
D) An electron is located in an orbit around the nucleus.
E) Orbits have a defined circumference.

Question 5

Arrange the following four electromagnetic spectral regions in order of decreasing energy.

A) microwave, radio, X-ray, visible
B) microwave, visible, X-ray, radio
C) radio, visible, X-ray, microwave
D) X-ray, radio, visible, microwave
E) X-ray, visible, microwave, radio

Question 6

Which statement regarding the Bohr model of the atom is true?

A) Hydrogen produces a continuous spectrum.
B) Electrons lose quantized amounts of energy when moving to an excited state.
C) Electrons cannot be located between energy levels.
D) Light is emitted when an electron moves from the ground state to an excited state.
E) Electrons in the lowest energy level are in an excited state.

Question 7

Which statement regarding atomic orbitals is false?

A) Atomic orbitals are three dimensional.
B) Only one electron is allowed per orbital.
C) An electron shell consists of a collection of orbitals with the same principal quantum number.
D) An orbital may be designated with the letters s, p, d, f.
E) An orbital describes the location of the electron 90% of the time.

Question 8

Light has a wavelength of 444 nm. What is its frequency? The speed of light is 3.00 × 10⁸ m/s.

A) 1.48 × 10^-6 Hz
B) 1.48 × 10^-15 Hz
C) 1.48 × 10² Hz
D) 6.76 × 10¹⁴ Hz
E) 6.76 × 10^-4 Hz

Question 9

Which wavelength of light has the greatest speed?

A) 418.6 nm
B) 554.9 nm
C) 626.1 nm
D) 563.8 nm
E) All have the same speed.

Question 10

Which statement about light is true?

A) Light oscillates back and forth between wave and particle-like behavior.
B) Light exhibits both wave and particle-like behavior at the same time.
C) Light has neither wave nor particle-like behavior.
D) Light behaves as a particle only.
E) Light behaves as a wave only.

Question 11

What is the phenomenon that occurs when excited gaseous elements emit only a few colored lines?

A) Planck's constant
B) photoelectric effect
C) line spectrum
D) quantum theory
E) electromagnetic spectrum

Question 12

Which word or phrase least applies to the quantum number represented by the symbol n?

A) shell
B) size
C) principal
D) distance from nucleus
E) shape

Question 13

Determine the energy of a photon that has a wavelength of 714 nm. The speed of light is 3.00 × 10⁸ m/s and h = 6.63 × 10^-34 J s.

A) 1.58 × 10^-48 J
B) 1.42 × 10^-31 J
C) 1.42 × 10^-22 J
D) 6.34 × 10^-21 J
E) 2.79 × 10^-19 J

Question 14

Which word or phrase least applies to the quantum number represented by the symbol l?

A) subshell
B) s, p, d, f
C) orbital type
D) orientation
E) shape

Question 15

What is a major shortcoming of the Bohr model?

A) It explains the spectral characteristics of hydrogen.
B) It accounts for the existence of line spectra.
C) It requires that the energy in the atom be quantized.
D) It implies that a one electron system can have four colors of light in its line spectrum.
E) It does not explain the spectra of multielectron atoms.

Question 16

Which statement below is false?

A) The wavelength of light is the distance between two corresponding points in the wave pattern.
B) The frequency of light is the number of waves that pass a given point in a second.
C) The frequency of light increases as wavelength decreases.
D) The higher the frequency of light, the greater its energy.
E) The higher the frequency of light, the longer the wavelength.

Question 17

Light has a frequency of 7.21 × 10¹³ hertz. What is its wavelength? The speed of light is 3.00 × 10⁸ m/s.

A) 2.16 × 10⁹ nm
B) 2.40 × 10⁵ nm
C) 4.16 × 10³ nm
D) 2.40 × 10^-4 nm
E) 4.16 × 10^-6 nm

Question 18

What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light?

A) Planck's constant
B) photoelectric effect
C) emission spectrum
D) quantum theory
E) electromagnetic spectrum

Question 19

Determine the energy of a photon that has a frequency of 5.23 × 10¹⁴ Hz. Given: h = 6.63 × 10^-34 J s.

A) 1.27 × 10^-48 J
B) 1.16 × 10^-27 J
C) 3.47 × 10^-19 J
D) 1.04 × 10^-10 J
E) 7.87 × 10⁴⁷ J

Question 20

Which idea was proposed by Werner Heisenberg?

A) Certain metals emit electrons when illuminated by light with low enough wavelength.
B) Light waves passing through a diffraction grating produce a diffraction pattern.
C) Light waves have particle properties, and particles of matter have wave-like properties.
D) Photons used to determine the location of electrons have no measurable effect on electrons.
E) Simultaneously determining the exact momentum and exact position of an electron is impossible.

Question 21

If l = 2, what value(s) can m_l have?

A) m_l = 0, +1, +2
B) m_l = +1
C) m_l = +2
D) m_l = -2, -1, 0, +1, +2
E) m_l = -1, 0, +1

Question 22

Which statement is true?

A) The 3d orbitals have lower energy than the 2p orbitals.
B) The 4p orbitals hold more electrons than the 3d orbitals.
C) The 2p orbitals hold up to 6 electrons.
D) Two electrons in the 1s orbital will have the same spin.
E) The p orbitals occur in groups of 5.

Question 23

When n = 3, l can equal ____.

A) l = 0
B) l = 0, 1
C) l = 0, 1, 2
D) l = 0, 1, 2, 3
E) l = 0, 1, 2, 3, 4

Question 24

The d orbitals occur in groups of ____ and hold up to ____ electrons.

A) 3; 6
B) 4; 8
C) 5; 10
D) 6; 12
E) 7; 14

Question 25

What is the correct shorthand notation for the electron configuration given?

A) [Ar]5s²
B) [Ar]3s²3p⁶3d¹⁰4p⁶5s²
C) [Ca]3d¹⁰4p⁶5s²
D) [Kr]5s²
E) [Rb]5s¹

Question 26

Which atom or ion does not have the electron configuration [Ne]3s²3p⁶?

A) Ar
B) Br^-
C) Ca²⁺
D) Cl^-
E) K⁺

Question 27

What is the correct electron configuration for aluminum?

A) 1s²2s¹
B) 1s²2s²2p⁴3s²3p³
C) 1s²2s²2p⁶3s²3p¹
D) 1s²2s²2p²3s²3p²3d²4s¹
E) 1s²2s²2p²3s²3p²4s²5s¹

Question 28

How many electrons can be contained in the 2p subshell?

A) 1
B) 2
C) 3
D) 4
E) 6

Question 29

What is the correct electron configuration for arsenic?

A) 1s²2s²2p⁶3s²3p³
B) 1s²2s²2p⁶3s²3p⁶4s²4p³
C) 1s²2s²2p⁶3s²3p⁶3d⁹4s²4p³
D) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p³
E) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶

Question 30

What is the electron configuration of Br^-?

A) 1s²2s²2p⁴
B) 1s²2s²2p⁶
C) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶
D) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁵
E) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁴

Question 31

What is the electron configuration of Li⁺?

A) 1s¹
B) 1s²
C) 1s²2s¹
D) 1s²2s²
E) 1s²2s²2p¹

Question 32

Which set of quantum numbers is not allowed?

A) n = 0, l = 0, m_l = 0, m_s = +1/2
B) n = 1, l = 0, m_l = 0, m_s = +1/2
C) n = 2, l = 1, m_l = 1, m_s = +1/2
D) n = 3, l = 1, m_l = 0, m_s = +1/2
E) n = 4, l = 3, m_l = 0, m_s = -1/2

Question 33

What is the electron configuration of O₂^-?

A) 1s²2s²2p⁵
B) 1s²2s²2p⁶
C) 1s²2s²2p⁴
D) 1s²2s²2p²
E) 1s²2s²2p³

Question 34

How many orbitals are contained in the 4d subshell?

A) 2
B) 5
C) 6
D) 10
E) 14

Question 35

Give the element that has the electron configuration:

A) In
B) Pd
C) Fe
D) Ni
E) Sr

Question 36

Which type(s) of atomic orbital(s) has (have) two lobes of electron density?

A) s
B) p
C) d
D) s and p
E) p and d

Question 37

Which corresponds to the electron configuration of a noble gas?

A) 1s²2s²
B) 1s²2s²2p⁴
C) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p²
D) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p³
E) 1s²2s²2p⁶3s²3p⁶

Question 38

What is the electron configuration of Al³⁺?

A) 1s²2s²2p⁵
B) 1s²2s²2p⁴
C) 1s²2s²2p²
D) 1s²2s²2p⁶
E) 1s²2s²2p⁶3s²3p¹

Question 39

What is the correct electron configuration for beryllium (Be)?

A) 1s²2s²
B) 1s²2s²2p¹
C) 1s²2s²2p²
D) 1s²2s²2p⁴
E) 1s²2s²2p⁶

Question 40

How many electrons can the second principal quantum level hold?

A) 2
B) 8
C) 16
D) 18
E) 32

Question 41

The first ionization energy is the amount of energy required to remove one ____________ from a neutral atom.

Question 42

Arrange these elements in order of increasing ionization energy.

A) P < Cl < Ar < Li < Na
B) Na < Li < P < Cl < Ar
C) Ar < Cl < Na < Li < P
D) Cl < Ar < Na < Li < P
E) P < Cl < Ar < Na < Li

Question 43

Xenon atoms, iodide ions, and cesium ions are:

A) paramagnetic.
B) diamagnetic.
C) ferromagnetic.
D) lanthanides.
E) isoelectronic.

Question 44

Which ion has the largest ionic radius?

A) Li⁺
B) F^-
C) S^2-
D) Na⁺
E) O^2-

Question 45

Which halogen has the most negative electron affinity?

Question 46

The time span between wave peaks is called a(n) _____________.

Question 47

Which element has the largest first ionization energy?

A) Be
B) Ca
C) Mg
D) Sr
E) Ba

Question 48

Electrons in the lowest _____________ level are in the ground state.

Question 49

Arrange these elements in order from largest to smallest atomic radii.

A) Ar > K > Na > Ne > P
B) K > Ar > P > Na > Ne
C) Ar > P > Na > Ne > K
D) Ne > Ar > P > Na > K
E) K > Na > P > Ar > Ne

Question 50

Atoms or ions that have the same electron configurations are:

A) paramagnetic.
B) diamagnetic.
C) ferromagnetic.
D) lanthanides.
E) isoelectronic.

Question 51

As one moves closer to the nucleus, what happens to the value of the principal quantum number?

Question 52

In a vacuum, all light travels with the same _____________

Question 53

Which element has the largest atomic radius?

A) As
B) P
C) Se
D) Br
E) F

Question 54

Which statement is false?

A) Br^- is larger than Kr.
B) Cl^- is smaller than S^2-.
C) K⁺ is smaller than Ca²⁺.
D) Mg²⁺ is smaller than Ca²⁺.
E) N^3- is larger than Ne.

Question 55

_____________ is the number of peaks or troughs of electromagnetic radiation that pass a point per second.

Question 56

Which element has the largest atomic radius?

A) F
B) He
C) O
D) H
E) Na

Question 57

Atoms or ions with no unpaired electrons are:

A) isoelectronic.
B) paramagnetic.
C) diamagnetic.
D) ferromagnetic.
E) lanthanides.

Question 58

Which element has an electron affinity greater than zero?

A) Br
B) I
C) Te
D) As
E) Kr

Question 59

____ substances are permanent magnets.

A) paramagnetic.
B) diamagnetic.
C) ferromagnetic.
D) lanthanides.
E) isoelectronic.

Question 60

Which statement about the formation of solid sodium chloride from sodium metal atoms and chlorine atoms is false?

A) Sodium atoms transfer electrons to chlorine atoms.
B) The sodium cation has an octet of outer electrons.
C) Sodium chloride contains alternating atoms in a crystal lattice.
D) The chloride anion has an octet of outer electrons.
E) The formation of sodium chloride from the elements releases energy to the surroundings.

Question 62

Each electron in an atom or ion must have a unique set of four _____________.

Question 63

Atomic radii _____________ going from left to right across a row of the periodic table.

Question 64

Match the following:

Question 65

Which halogen atom has the smallest atomic radius?