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General Chemistry - Chemistry I and Lab > Module 6 - Electronic Structure of Atoms V5 > Flashcards

Module 6 - Electronic Structure of Atoms V5 Flashcards

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1
Q

Electromagnetic radiation refers to waves that move through a vacuum at the speed of light.

A

true

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2
Q

A nanometer is how many meters?

A

10-9

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3
Q

A wavelength refers to the number of waves passing through a given point in a specific amount of time.

A

false

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4
Q

A quantum is a fixed amount of the smallest amount of electromagnetic radiation that can be absorbed or released by an object.

A

true

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5
Q

Which of the following multiples of h\nu are allowed?

A

3 h/nu

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6
Q

The unit for energy is Hz.

A

false

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7
Q

Ground state is the highest energy state for an electron.

A

false

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8
Q

Each element has its own unique atomic emission spectrum.

A

true

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9
Q

Which scientist came up with the concept of principal quantum numbers?

A

Bohr

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10
Q

All orbitals that have the same values of n and l are known as e-shells.

A

false

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11
Q

An orbital is where electrons can be found inside an atom, each one having its own unique set of energies and shapes.

A

true

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12
Q

What does the quantum number “ml” represent?

A

the orientation of the orbital

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13
Q

The following energy diagram is drawn correctly.

A

false

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14
Q

The Aufbau principle states that electrons must fill orbitals of __________ energy before occupying orbitals of __________ energy.

A

lower; higher

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15
Q

A many-electron atom is an atom with two or more electrons.

A

true

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16
Q

Valence electrons are the electrons used in bonding.

A

true

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17
Q

What is the electron configuration for chlorine?

A

1s22s22p63s23p5

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18
Q

The electrons not involved in bonding are known as __________ electrons.

A

core

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19
Q

The speed of light is used to calculate…

A

wavelength and frequency.

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20
Q

All electromagnetic radiation is visible light.

A

false

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21
Q

Which type of radiation has the lowest energy?

A

red

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22
Q

Atoms move to a higher level when they__________energy and move to a lower level when they__________energy.

A

absorb; release

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23
Q

What is the wavelength (in meters) of blue light that has a frequency of 4.60 x 109 Hz?

A

0.0065m

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24
Q

Who is responsible for the explanation of the photoelectric effect?

A

Albert Einstein

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25
Q

Photons have a quantum amount of energy.

A

true

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26
Q

Based on the photoelectric effect, if you shine high-frequency light on a clean sheet of metal…

A

electrons are emitted from the metal

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27
Q

What is the energy of a photon with a frequency of 1.1 x 1026 Hz?

A

7.3 x 10-8

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28
Q

What is the energy of radiation with a wavelength of 3.4 x 10-5 meters?

A

5.842 x 10-21

29
Q

Elements in the same period have the same atomic emission spectrum.

A

false

30
Q

Based on Bohr’s model, which is the lowest energy level?

A

n = 4

31
Q

While the__________quantum number tells the shape of the orbital, the __________quantum number tells the orientation of the orbital shape.

A

angular momentum; magnetic

32
Q

As the principal quantum number, n, increases…

A

the number of orbitals increases.

33
Q

What are the quantum numbers for an electron in the 3p orbital (+1 orientation)?

A

n = 3, l = 1, ml = 1

34
Q

What are the quantum numbers for an electron in the 4d orbital (-2 orientation)?

A

n = 4, l = 2, ml = -2

35
Q

The Pauli exclusion principle states that…

A

no two electrons can have the same four quantum numbers.

36
Q

What element is represented by the following electron configuration? 1s22s22p63s23p5

A

chlorine

37
Q

Planck concluded that objects…

A

absorb a fixed amount of energy.

38
Q

The Aufbau principle states that orbitals of the lowest energy must be filled first.

A

true

39
Q

Which list correctly shows visible light in increasing energy?

A

red, orange, green, violet

40
Q

Which list correctly shows electromagnetic radiation in decreasing energy?

A

gamma, x-ray, visible light, infrared

41
Q

Which form of electromagnetic radiation listed here has the highest energy?

A

x-ray

42
Q

What is the speed for the constant c (speed of light constant)?

A

3.0 x 108 m/s

43
Q

What is the wavelength (in meters) of blue light that has a frequency of 6.3 x 1014 Hz?

A

4.8 x10-7 meters

44
Q

Within the equation E = hv, h stands for what?

A

Planck’s constant

45
Q

Which of the following provides the best explanation for the photoelectric effect?

A

When light of a certain frequency is shined on a clean metal surface, electrons are emitted from the surface.

46
Q

Within the equation E = hv, v stands for what?

A

frequency

47
Q

What is the energy of a photon with a frequency of 3.8 x 1014 Hz?

A

2.5 x 10-19 J

48
Q

What is the frequency of a photon whose energy is 9.2 x 10-18 joules?

A

1.4 x 1016 Hz

49
Q

__________ refers to the generic lab for observing light being emitted from excited electrons within an atom.

A

a flame test

50
Q

Line spectra observed through gaseous elements in a glass tube being sent energy in the form of electricity is…

A

an atomic emission spectrum.

51
Q

Which of the following would give a continuous spectrum when its light is broken up by a prism?

A

sunlight

52
Q

Which principal quantum number has the lowest energy?

A

n=1

53
Q

An electron in its __________ can absorb energy and jump up to an __________.

A

ground state, excited state

54
Q

What does the quantum number “l” represent?

A

the shape of the orbital

55
Q

What specific orbital aligns with the following quantum numbers?

n=2
l = 0
ml = 0

A

2s

56
Q

The following picture represents which orbital shape?

A

s

57
Q

What are the quantum numbers for an electron in 3d orbital (+1 orientation)?

A

n=3, l = 2, ml = +1

58
Q

What are the quantum numbers for an electron in 5p orbital (0 orientation)?

A

n=5, l = 1, ml = 0

59
Q

The two quantum numbers for electron spin are…

A

-½ , and +½.

60
Q

The Pauli exclusion principle states that no __________ electrons can have the same set of __________ quantum numbers.

A

2; 4

61
Q

Identify the correct order for the following orbitals in order of lowest energy to highest energy for a many-electron atom: “4s, 2p, 3s, 5d, 4f, 6s.”

A

2p, 3s, 4s, 6s, 4f, 5d

62
Q

The electron circled in the energy level diagram is found in the _________ energy level and has an electron spin of __________.

A

2; +½

63
Q

A diagram showing relative energies of shells, subshells, and orbitals of a hydrogen or many-electron atom is a(n)…

A

energy level diagram.

64
Q

How many valence electrons does carbon have? Carbon’s electron configuration is 1s22s22p2.

A

4

65
Q

Fluorine has __________ paired electron(s) and __________ unpaired electron(s) in the 2p subshell.

A

2;1

66
Q

Calcium has __________ valence electrons.

A

2

67
Q

What element has the following electron configuration: 1s22s22p4?

A

oxygen

68
Q

Potassium has __________ valence electron(s) and __________ core electron(s).

A

1;18

General Chemistry - Chemistry I and Lab (10 decks)

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