Deck 7: Atomic Structure and Periodicity

Question 1

Which of the following frequencies corresponds to light with the longest wavelength?

A)3.00 $\times$ 10¹³ s^-1
B)4.12 $\times$ 10⁵ s^-1
C)8.50 $\times$ 10²⁰ s^-1
D)9.12 $\times$ 10¹² s^-1
E)3.20 $\times$ 10⁹ s^-1

Answer 1

4.12 $\times$ 10⁵ s^-1

Question 2

The four lines observed in the visible emission spectrum of hydrogen tell us that:

A)The hydrogen molecules they came from have the formula H₄.
B)We could observe more lines if we had a stronger prism.
C)There are four electrons in an excited hydrogen atom.
D)Only certain energies are allowed for the electron in a hydrogen atom.
E)The spectrum is continuous.

Answer 2

Only certain energies are allowed for the electron in a hydrogen atom.

Question 3

When a strontium salt is ignited,it burns with a red flame.The frequency of the light given off by this flame is greater than

A)yellow light
B)infrared light
C)ultraviolet light
D)radio waves
E)x-rays

Answer 3

infrared light

Question 4

What is the wavelength of a photon of red light (in nm)whose frequency is 4.55 $\times$ 10¹⁴ Hz?

A)659 nm
B)1.52 $\times$ 10⁶ nm
C)152 nm
D)455 nm
E)none of these

Question 5

Which of the following are incorrectly paired?

A)wavelength - $\lambda$
B)frequency - $v$
C)speed of light - c
D)hertz - s^-1
E)x-rays - shortest wavelength

Question 6

From the following list of observations,choose the one that most clearly supports the following conclusion:
a)emission spectrum of hydrogen
b)the photoelectric effect
c)scattering of alpha particles by metal foil
d)diffraction
e)cathode "rays"
Electrons in atoms have quantized energies.

A)observation a
B)observation b
C)observation c
D)observation d
E)observation e

Question 7

All matter exhibits either particulate or wave properties exclusively.

Question 8

When ignited,a uranium compound burns with a green flame.The wavelength of the light given off by this flame is greater than that of

A)red light
B)infrared light
C)radio waves
D)ultraviolet light
E)none of these

Question 9

From the following list of observations,choose the one that most clearly supports the following conclusion:
a)emission spectrum of hydrogen
b)the photoelectric effect
c)scattering of alpha particles by metal foil
d)diffraction
e)cathode "rays"
Electromagnetic radiation has wave characteristics.

A)observation a
B)observation b
C)observation c
D)observation d
E)observation e

Question 10

The SI unit for frequency is cycles per second.

Question 11

A line in the spectrum of atomic mercury has a wavelength of 254 nm.When mercury emits a photon of light at this wavelength,the frequency of this light is

A)8.47 $\times$ 10^-16 s^-1
B)7.82 $\times$ 10^-19 s^-1
C)1.18 $\times$ 10¹⁵ s^-1
D)76.1 s^-1
E)none of these

Question 12

Spacing between atoms in a crystal is on the same order as the de Broglie wavelength of accelerated electrons.

A)observation a
B)observation b
C)observation c
D)observation d
E)observation e

Question 13

Which form of electromagnetic radiation has the longest wavelengths?

A)gamma rays
B)microwaves
C)radio waves
D)infrared radiation
E)x-rays

Question 14

From the following list of observations,choose the one that most clearly supports the following conclusion:
a)emission spectrum of hydrogen
b)the photoelectric effect
c)scattering of alpha particles by metal foil
d)diffraction
e)cathode "rays"
Electrons have wave properties.

A)observation a
B)observation b
C)observation c
D)observation d
E)observation e

Question 15

What is the energy of a photon of blue light that has a wavelength of 453 nm?

A)4.53 $\times$ 10^-7 J
B)4.39 $\times$ 10^-19 J
C)6.62 $\times$ 10¹⁴ J
D)9.00 $\times$ 10^-32 J
E)2.28 $\times$ 10¹⁸ J

Question 16

Which one of the following types of radiation has the shortest wavelength,the greatest energy,and the highest frequency?

A)Ultraviolet radiation.
B)Infrared radiation.
C)Visible red light.
D)Visible blue light.
E)None,because short wavelength is associated with low energy and low frequency,not high energy and high frequency.

Question 17

How many of the following is/are incorrect? i.The importance of the equation E = mc² is that energy has mass.
Ii.Electromagnetic radiation can be thought of as a stream of particles called photons.
Iii.Electromagnetic radiation exhibits wave properties.
Iv.Energy can only occur in discrete units called quanta.

A)0
B)1
C)2
D)3
E)4

Question 18

Diffraction results when light is scattered from a regular array of points or lines.

Question 19

Consider an atom traveling at 1% of the speed of light.The de Broglie wavelength is found to be 1.46 $\times$ 10^-3 pm.Which element is this?

A)Be
B)Zr
C)Kr
D)Fe
E)P

Question 20

Green light can have a wavelength of 543 nm.The energy of a photon of this light is

A)1.08 $\times$ 10^-31 J
B)5.43 $\times$ 10^-7 J
C)3.66 $\times$ 10^-19 J
D)5.52 $\times$ 10¹⁴ J
E)2.73 $\times$ 10¹⁸ J

Question 21

Which of the following is a reasonable criticism of the Bohr model of the atom?

A)It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus.
B)It does not adequately predict the line spectrum of hydrogen.
C)It does not adequately predict the ionization energy of the valence electron(s)for elements other than hydrogen.
D)It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen.
E)It shows the electrons to exist outside of the nucleus.

Question 22

What is the wavelength of light that is emitted when an excited electron in the hydrogen atom falls from n = 5 to n = 1?

A)1.05 $\times$ 10⁷ m
B)9.50 $\times$ 10^-8 m
C)2.09 $\times$ 10^-18 m
D)9.12 $\times$ 10^-8 m
E)none of these

Question 23

The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 $\times$ 10^-7 m.By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li²⁺ ion?

A)1/9
B)1/7
C)1/4
D)1/3
E)1

Question 24

Which of the following best describes an orbital?

A)space where electrons are unlikely to be found in an atom
B)space which may contain electrons,protons,and/or neutrons
C)the space in an atom where an electron is most likely to be found
D)small,walled spheres that contain electrons
E)a single space within an atom that contains all electrons of that atom

Question 25

A gamma ray of wavelength 1.00 $\times$ 10^-8 cm has enough energy to remove an electron from a hydrogen atom.

Question 26

How many f orbitals have n = 6?

A)2
B)7
C)10
D)5
E)18

Question 27

Which of the following is incorrect?

A)The emission spectrum of hydrogen contains a continuum of colors.
B)Diffraction produces both constructive and destructive interference.
C)All matter displays both particle and wavelike characteristics.
D)Niels Bohr developed a quantum model for the hydrogen atom.
E)The lowest possible energy state of a molecule or atom is called its ground state.

Question 28

The energy of the light emitted when a hydrogen electron goes from n = 2 to n = 1 is what fraction of its ground-state ionization energy?

A)3/4
B)1/2
C)1/4
D)1/8
E)1/9

Question 29

In Bohr's atomic theory,when an electron moves from one energy level to another energy level more distant from the nucleus:

A)Energy is emitted.
B)Energy is absorbed.
C)No change in energy occurs.
D)Light is emitted.
E)None of these.

Question 30

A given set of p orbitals consists of ______ orbitals.

A)1
B)2
C)3
D)4
E)5

Question 31

Consider the following portion of the energy-level diagram for hydrogen:
n = 4 $\quad$ -0.1361 $\times$ 10^-18 J
n = 3 $\quad$ -0.2420 $\times$ 10^-18 J
n = 2 $\quad$ -0.5445 $\times$ 10^-18 J
n = 1 $\quad$ -2.178 $\times$ 10^-18 J

-For which of the following transitions does the light emitted have the longest wavelength?

A)n = 4 to n = 3
B)n = 4 to n = 2
C)n = 4 to n = 1
D)n = 3 to n = 2
E)n = 2 to n = 1

Question 32

Bohr's model correctly describes the hydrogen atom and other small atoms.

Question 33

If n = 2,how many orbitals are possible?

A)3
B)4
C)2
D)8
E)6

Question 34

In the hydrogen spectrum,what is the wavelength of light associated with the n = 3 to n = 1 electron transition?

A)3.97 F $\times$ 10^-25 nm
B)8.21 $\times$ 10² nm
C)9.75 $\times$ 10⁶ cm
D)1.94 $\times$ 10^-18 m
E)1.03 $\times$ 10^-7 m

Question 35

When an electron in a 2p orbital of a particular atom makes a transition to the 2s orbital,a photon of approximate wavelength 629.1 nm is emitted.The energy difference between these 2p and 2s orbitals is

A)3.16 $\times$ 10^-28 J
B)3.16 $\times$ 10^-19 J
C)3.16 $\times$ 10^-17 J
D)1.25 $\times$ 10^-31 J
E)none of these

Question 36

In an investigation of the electronic absorption spectrum of a particular element,it is found that a photon having $\lambda$ = 500 nm provides just enough energy to promote an electron from the second quantum level to the third.From this information,we can deduce

A)the energy of the n = 2 level
B)the energy of the n = 3 level
C)the sum of the energies of n = 2 and n = 3
D)the difference in energies between n = 2 and n = 3
E)all of these

Question 37

When a hydrogen electron makes a transition from n = 3 to n = 1,which of the following statements is true?
I.Energy is emitted.
II.Energy is absorbed.
III.The electron loses energy.
IV.The electron gains energy.
V.The electron cannot make this transition.

A)I,IV
B)I,III
C)II,III
D)II,IV
E)V

Question 38

How many f orbitals have the value n = 3?

A)0
B)3
C)5
D)7
E)1

Question 39

Which of the following is not determined by the principal quantum number,n,of the electron in a hydrogen atom?

A)The energy of the electron.
B)the minimum wavelength of the light needed to remove the electron from the atom.
C)The size of the corresponding atomic orbital(s).
D)The shape of the corresponding atomic orbital(s).
E)All of the above are determined by n.

Question 40

Which of the following statements best describes the Heisenberg uncertainty principle?

A)The exact position of an electron is always uncertain.
B)The velocity of a particle can only be estimated.
C)It is impossible to accurately know both the exact location and momentum of a particle.
D)The location and momentum of a macroscopic object are not known with certainty.
E)The location and momentum of a particle can be determined accurately,but not the identity of the particle.

Question 41

The small,but important,energy differences between 3s,3p,and 3d orbitals are due mainly to

A)the number of electrons they can hold
B)their principal quantum number
C)the Heisenberg uncertainty principle
D)the penetration effect
E)Hund's rule

Question 42

If l = 3,how many electrons can be contained in all the possible orbitals?

A)7
B)6
C)14
D)10
E)5

Question 43

Which of the following combinations of quantum numbers (n,l,m_l,m_s)do not represent permissible solutions of the Schrödinger equation for the electron in the hydrogen atom (i.e. ,which combination of quantum numbers is not allowed)?

A)9,8,-4,1/2
B)8,2,2,1/2
C)6,-5,-1,1/2
D)6,5,-5,1/2
E)All are allowed.

Question 44

Who was the first chemist to recognize patterns in chemical properties of the elements?

A)Mendeleev
B)Newlands
C)Meyer
D)Dobereiner
E)Bohr

Question 45

The size of an orbital is arbitrarily defined.

Question 46

The magnetic quantum number is related to the orientation of the orbital in space relative to the other orbitals in the atom.

Question 47

How many electrons can be contained in all of the orbitals with n = 4?

A)2
B)8
C)10
D)18
E)32

Question 48

Mendeleev is given the most credit for the concept of a periodic table of the elements because:

A)He had the longest history of research in elemental properties.
B)He emphasized its usefulness in predicting the existence and properties of unknown elements.
C)His representation of the table was the most understandable.
D)His periodic table was arranged in octaves.
E)He grouped elements into triads of similar properties.

Question 49

Consider the following representation of a 2p-orbital: Which of the following statements best describes the movement of electrons in a p-orbital?

A)The electrons move along the outer surface of the p-orbital,similar to a "figure 8" type of movement.
B)The electrons move within the two lobes of the p-orbital,but never beyond the outside surface of the orbital.
C)The electrons are concentrated at the center (node)of the two lobes.
D)The electrons are only moving in one lobe at any given time.
E)The electron movement cannot be exactly determined.

Question 50

How many electrons in an atom can have the quantum numbers n = 4,l = 2?

A)14
B)12
C)5
D)10
E)6

Question 51

Which of the following combinations of quantum numbers is not allowed?

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

Question 52

What is the l quantum number for a 4s orbital?

A)1
B)0
C)3
D)2
E)more than one of the above

Question 53

How many electrons in an atom can have the quantum numbers n = 3,l = 2?

A)2
B)5
C)10
D)18
E)6

Question 54

A point in the wave function where the amplitude is zero defines

A)the node
B)the excited state
C)the amplitude of the wave function
D)the frequency of radiation
E)none of the above

Question 55

Which of the following could not be a valid m_l quantum number for a 4d orbital?

A)2
B)0
C)-2
D)1
E)4

Question 56

Which of the following was not an elemental property usually predicted by Mendeleev for as-yet-unknown elements?

A)electron configuration
B)atomic mass
C)density
D)boiling point
E)oxide formula

Question 57

The number of orbitals having a given value of l is equal to

A)2l + 1
B)2n + 2
C)3l
D)l + m_l
E)the number of lobes in each orbital

Question 58

How many electrons can be described by the quantum numbers n = 3,l = 3,m_l = 1?

A)0
B)2
C)6
D)10
E)14

Question 59

Which of the following atoms or ions has three unpaired electrons?

A)N
B)O
C)Al
D)S^2-
E)Ti²⁺

Question 60

Which of the following is an incorrect designation for an atomic orbital?

A)1s
B)3d
C)1p
D)4f
E)6s

Question 61

An element with the electron configuration [Xe] 6s²4f¹⁴5d⁷ would belong to which class on the periodic table?

A)transition elements
B)alkaline earth elements
C)halogens
D)rare earth elements
E)none of the above

Question 62

The complete electron configuration of tin is

A)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5d¹⁰5p²
B)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4d¹⁰4p²
C)1s²2s²2p⁶3s²3p⁶4s²4p⁶5s²4d¹⁰5d¹⁰5p²
D)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p²
E)none of these

Question 63

An atom of fluorine contains nine electrons.How many of these electrons are in s orbitals?

A)2
B)4
C)6
D)8
E)none

Question 64

The electron configuration for the carbon atom is:

A)1s²2s²2p²
B)[He]2s⁴
C)[Ne]2s²2p²
D)1s²2p⁴
E)none of these

Question 65

Of the following elements,which needs three electrons to complete its valence shell?

A)Ba
B)Ca
C)Si
D)P
E)Cl

Question 66

Which of the following atoms has three electrons in p orbitals in its valence shell?

A)Ba
B)Ga
C)V
D)Bi
E)none of these

Question 67

Which of the following statements is false?

A)An orbital can accommodate at most two electrons.
B)The electron density at a point is proportional to $\varPsi$ ² at that point.
C)The spin quantum number of an electron must be either + or - .
D)A 2p orbital is more penetrating than a 2s;i.e. ,it has a higher electron density near the nucleus and inside the charge cloud of a 1s orbital.
E)In the usual order of filling,the 6s orbital is filled before the 4f orbital.

Question 68

Fe has __________ that is (are)unpaired in its d orbitals.

A)one electron
B)two electrons
C)three electrons
D)four electrons
E)none of these

Question 69

Which of the following statements is true?

A)The exact location of an electron can be determined if we know its energy.
B)An electron in a 2s orbital can have the same n,l,and m_l quantum numbers as an electron in a 3s orbital.
C)Ni has two unpaired electrons in its 3d orbitals.
D)In the buildup of atoms,electrons occupy the 4f orbitals before the 6s orbitals.
E)Only three quantum numbers are needed to uniquely describe an electron.

Question 70

All alkaline earths have the following number of valence electrons:

A)1
B)3
C)6
D)2
E)none of these

Question 71

Of the following elements,which has occupied d orbitals in its ground-state neutral atoms?

A)Ba
B)Ca
C)Si
D)P
E)Cl

Question 72

Which of the following statements about quantum theory is incorrect?

A)The energy and position of an electron cannot be determined simultaneously.
B)Lower energy orbitals are filled with electrons before higher energy orbitals.
C)When filling orbitals of equal energy,two electrons will occupy the same orbital before filling a new orbital.
D)No two electrons can have the same four quantum numbers.
E)All of these are correct.

Question 73

An element has the electron configuration [Kr] 5s²4d¹⁰5p².The element is a(n)

A)nonmetal
B)transition element
C)metal
D)lanthanide
E)actinide

Question 74

Germanium has __________ in its 4p orbitals.

A)one electron
B)two electrons
C)three electrons
D)four electrons
E)none of these

Question 75

Which of the following electron configurations is correct?

A)Ga: [Kr]4s²3d¹⁰4p¹
B)Mo: [Kr]5s²4d⁵
C)Ca: [Ar]4s¹3d¹⁰
D)Br: [Kr]4s²3d¹⁰4p⁷
E)Bi: [Xe]6s²4f¹⁴5d¹⁰6p³

Question 76

Ti has __________ in its d orbitals.

A)one electron
B)two electrons
C)three electrons
D)four electrons
E)none of these

Question 77

The electron configuration for the barium atom is:

A)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰
B)[Xe]6s²
C)1s²2s²2p⁶3s²3p⁶4s¹
D)1s²2s²2p⁶3s²3p⁶4s²
E)none of these

Question 78

An element E has the electron configuration [Kr] 5s²4d¹⁰5p².The formula for the fluoride of E is most likely

A)EF₁₄
B)EF₄
C)EF
D)EF₆
E)EF₈

Question 79

The statement that "the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals" is known as

A)the aufbau principle
B)Hund's rule
C)Heisenberg uncertainty principle
D)the Pauli exclusion principle
E)the quantum model

Question 80

How many unpaired electrons are there in an atom of sulfur in its ground state?

A)0
B)1
C)2
D)3
E)4