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Chemistry > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

(Honors) What is the letter code for a sublevel with l = 1?

A

p

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1
Q

All the forms of electromagnetic radiation together comprise the…

A

Electromagnetic spectrum

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2
Q

(Honors) Is the following set of quantum numbers allowed? If no, why not?

n =4, l = -1, ml = 0, ms = +1/2

A

No. l must be from 0 to (n-1). l cannot be a negative number.

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2
Q

(Honors) Complete the table:

A
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3
Q

A unit of frequency equal to 1 wave per second.

A

Hertz (Hz)

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4
Q

Consider the following orbital diagram for nitrogen. Is the ground state electron configuration given acceptable? If no, why not?

A

Yes.

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4
Q

A spectrum containing all visible wavelengths of light

A

Continuous spectrum

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5
Q

What energy is associated with a photon of electromagnetic radiation whose frequency is 3.6x1012 Hz?

A
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6
Q

How much energy is associated with microwave radiation whose wavelength is 3.00mm (3.00x10-3m)?

A
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7
Q

A form of energy that exhibits wavelike behavior as it travels through space.

Or

Oscillating (changing in a regular, repeating way over time) electric and magnetic fields that travel through empty space

A

Electromagnetic Radiation

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7
Q

A 3D region around the nucleus that indicates the probable location of an electron

A

Orbital

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8
Q

Ultraviolet radiation with a wavelength of less than 280nm may be used as a germicide. What is the frequency of this radiation?

A
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9
Q

The height of the wave above the x-axis

A

Amplitude

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9
Q

A state in which an atom has a higher potential energy than it has in its ground state

A

Excited state

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10
Q

(Honors) Is the following set of quantum numbers allowed? If no, why not?

n = 5, l = 1, ml = -1, ms = -1

A

No. The only allowed values for ms are +1/2 or -1/2.

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11
Q

A particle of electromagnetic radiation having zero mass and carrying a quantum of energy

A

Photon

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11
Q

Complete the table

A
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12
Q

(Honors) The quantum number that indicates the two fundamental spin states of an electron

A

The spin quantum number (ms)

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14
Q

How many sublevels are there in the 3rd energy level (n=3)? What are their names?

A

3: 3s, 3p, 3d

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15
Q

A human body emits infrared radiation of around 7.95x10-21J per photon. What is the frequency associated with this radiation?

A
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16
Q

(Honors) What are the values for n and l for a 3p sublevel?

A

n = 3

l = 1

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16
Q

The lowest energy state of an atom

A

Ground state

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17
Q

The distance between corresponding points on adjacent waves.

A

Wavelegnth (λ)

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19
Q

(Honors) If n=3, what are the possible values for l?

A

l may be equal to 0, 1, or 2 (corresponding to an s, p, and d sublevel)

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19
Q

If n=7, what are the possible values for l?

A

l may be equal to 0, 1, 2, 3, 4, 5, or 6. Note that the 7th energy level has 7 different sublevels.

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20
Q

What is the orbital diagram for the ground state electron configuration of tin? What is the accompanying electron configuration?

A
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21
Q

Describes mathematically the wave properties of electrons and other very small particles

A

Quantum Theory

21
Q

(Honors) The range of allowed values for the angular momentum quantum number (l)

A

0 to (n-1)

23
Q

The blue-violet line in hydrogen’s emission spectrum corresponds to a wavelength of 0.434µm. What is the frequency of this radiation?

A
24
Q

(Honors) Is the following set of quantum numbers allowed? If no, why not?

n = 5, l = 2, ml = -2, ms = -1/2

A

Yes, it is allowed

26
Q

Gamma radiation has freqencies ranging from about 1.0x1020 Hz to 1.0x1024 Hz. Calculate the wavelength of gamma radiation whose frequency is 1.0x1024 Hz.

A
26
Q

States that electrons occupy the orbitals of lowest energy first

A

Aufbau (Building Up) Principle

27
Q

(Honors) The quantum number that specifies the sublevel

A

The angular momentum quantum number (l)

27
Q

Make a sketch showing how a 1s, 2s, and 3s orbital differ from each other

A
29
Q

Is the following set of quantum numbers allowed? If no, why not?

n = 6, l = 0, ml = 0, ms = +1/2

A

Yes, it is allowed.

29
Q

(Honors) The range of allowed values for the spin quantum number (ms)

A

+1/2 or -1/2

31
Q

Find the energy of yellow light whose wavelength is 550nm (5.5x10-7m).

A
32
Q

(Honors) The quantum number that indicates the specific orbital in which an electron is located

A

The Magnetic Quantum Number (ml)

33
Q

(Honors) What are the values of n and l for a 5s sublevel?

A

n = 5

l = 0

35
Q

(Honors) Is the following set of quantum numbers allowed? If no, why not?

n = 7, l = 4, ml = 5, ms = -1/2

A

No. ml must be from -l to +l. In this specific case, ml anything from -4 up to +4.

36
Q

The number of wavelengths of a wave that pass a fixed point in one unit of time (usually a second)

A

frequency (ν)

37
Q

Consider the following orbital diagram for nitrogen. Is the ground state electron configuration given acceptable? If no, why not?

A

No. According to the Aufbau Principle, lower energy sublevels should fill before higher energy sublevels.

39
Q

How many sublevels in the 2nd energy level (n=2)? What are their names?

A

2: 2s, 2p

40
Q

A particular distribution of electrons among available sublevels

A

Electron configuration

41
Q

(Honors) The range of allowed values for the magnetic quantum number (ml)

A

-l to +l

42
Q

The value of the speed of light in a vacuum (c).

A

3.00x108 m/s

44
Q

Consider the following orbital diagram for nitrogen. Is the ground state electron configuration given acceptable? If no, why not?

A

No. According to the Pauli Exclusion Principle, there can be no more than two electrons in an orbital.

45
Q

The value of Planck’s constant (h)

A

6.626x10-34 J·s

45
Q

Make a sketch showing the different p orbitals.

A
46
Q

A microwave emits radiation with a wavelength of 0.12m. What is the frequency of these microwaves?

A
47
Q

Consider the following orbital diagram for nitrogen. Is the ground state electron configuration given acceptable? If no, why not?

A

No. According to the Pauli Exclusion Principle, two electrons in the same orbital must have opposite spin.

48
Q

A radio station broadcasts at a frequency of 940kHz. What is the wavelength of these radio waves?

A
49
Q

Refers to the emission of electrons from a metal when light shines on the metal

A

The photoelectric effect

50
Q

Consider the following orbital diagram for nitrogen. Is the ground state electron configuration given acceptable? If no, why not?

A

No. According to Hund’s Rule, electrons should go into the orbitals of a sublevel one at a time, unpaired, with the same spin, before any electrons are paired in that sublevel.

51
Q

How much energy is associated with a photon of radiation whose frequency is 9.2x1015Hz?

A
53
Q

What is the freqency of electromagnetic radiation whose energy is 9.45x10-20J per photon?

A
54
Q

States that no two electrons in the same atom can have the same set of four quantum numbers.

Can be also stated that two electrons must be spinning in opposite directions in order to be in the same orbital

A

Pauli Exclusion Principle

56
Q

A spectrum showing only certain specific wavelengths of light produced by a hot, glowing gas

A

Emission (line) spectrum

58
Q

The minimum quantity of energy that can be gained or lost by an atom

A

Quantum

59
Q

The quantum number that indicates the main energy level occupied by the electron.

A

Principal Quantum Number (n)

61
Q

What is the orbital diagram for the ground state electron configuration of sulfur? What is the accompanying shorthand notation?

A
62
Q

(Honors) What is the letter code for a sublevel with l = 3?

A

f

63
Q

States that the lowest energy arrangement of electrons in a sublevel is obtained by putting electrons into separate orbitals of the sublevel with the same spin before pairing any electrons

A

Hund’s Rule

64
Q

The statement that it is impossible to determine simultaneously both the position and velocity of an electron

A

Heisenberg’s Uncertainty Principle

65
Q

(Honors) Is the following set of quantum numbers allowed? If no, why not?

n = 4, l = 4, ml = -2, ms = +1/2

A

No. l must be from 0 to (n-1). In this specific case, l could be 0, 1, 2, or 3.

66
Q

The range of allowed values for the principal quantum number (n)

A

1 to infinity

Chemistry (13 decks)

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