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Chemistry 121 > Quantum Theory > Flashcards

Quantum Theory Flashcards

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1
Q

Spectroscopy

A

The method for finding out about the structure of molecules that depends on the interaction of molecular compounds with radiation.

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2
Q

Absorption Spectrum

A

A plot of radiation energy versus the percentage of radiation transmitted

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3
Q

Frequency

A

“nu” - the number of wave peaks that pass by a fixed point per until time.

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4
Q

Wavenumber

A

The number of repeating units of a wave in a unit of space (rather than time). This is a reciprocal of frequency.

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5
Q

What happens when molecules absorb microwaves?

A

Molecular tumbling

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6
Q

What happens when molecules absorb ultraviolet light?

A

Covalent bonds can rupture

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7
Q

What happens when molecules absorb infrared light?

A

Molecular vibration

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8
Q

How do atoms become excited?

A

Atoms absorb energy.

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9
Q

How do atoms return to their ground state?

A

Atoms release their extra energy by emission of radiation.

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10
Q

Line Emission Spectrum

A

Excited atoms emit only particular wavelengths of light - when this light is passed through a prism, only a few coloured lines are seen.

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11
Q

What does it mean for the energy of electrons to be quantized?

A

They can only have particular amounts of energy and not values between the “allowed” levels.

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12
Q

Lyman Series

A

A series of emission lines having energies in the ultraviolet region.

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13
Q

Balme Series

A

A series of emission lines have energies in the visible region.

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14
Q

What is the l value for the s orbital?

A

0

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15
Q

What is the l value for the p orbital?

A

1

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16
Q

What is the l value for the d orbital?

A

2

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17
Q

What is the l value for the f orbital?

A

3

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18
Q

What orbital has the l value of 0?

A

s orbital

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19
Q

What orbital has the l value of 1?

A

p orbital

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20
Q

What orbital has the l value of 2?

A

d orbital

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21
Q

What orbital has the l value of 3?

A

f orbital

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22
Q

What is an orbital?

A

Refers to a mathematical function, which is one part of the solution to the wave equation for each stationary wave. Non-uniform distributions of electron matter over space around the nucleus.

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23
Q

Orbitals of an atom that have been derived by use of the same value of n in the Schrodinger equation are said to be in the same _____.

A

Shell

Example: The 2s orbital (n=2, l=0) and the three 2p orbitals (n=2, l=1) are all part of the same n=2 shell.

24
Q

In a given shell, each set of orbitals derived by use of a particular value of l in the Schrodinger equation are said to be in the same ________.

A

Sub-shell

Example: in the n=3 shell, the 3s subshell is comprised of the 3s orbital (l=0,m1 =0)

25
Q

What type of wave is an electron?

A

A standing wave

26
Q

How can you find the number of orbitals in a sub-shell?

A

2(L) + 1

27
Q

How many orbitals in sub-shell s?

A

1

28
Q

How many orbitals in sub-shell p?

A

3

29
Q

How many orbitals in sub-shell d?

A

5

30
Q

How many orbitals in sub-shell f?

A

7

31
Q

Diamagnetic

A

Substances that are slightly repelled by a magnet

32
Q

Paramagnetic

A

Substances that are attracted to a magnetic field. They have unpaired electrons.

33
Q

What is the shape of s orbitals?

A

They are spherically symmetrical.

34
Q

Principal QN n

A

n = 1,2,3…

35
Q

How do you find the density of the electron wave?

A

Wavefunction^2

36
Q

As the principal QN n increases, the number of nodes in a wavefunction ____________.

A

increases

37
Q

At a node, the sign of the wavefunction is _______.

A

zero

38
Q

On either side of a node, the sign of the wavefunction __________.

A

changes phase

39
Q

A node is a region of _______ electron density.

A

zero

40
Q

Radial node

A

a region of zero electron density that exists at a specific radial distance from the nucleus. In 3D a radial node is a sphere, but a 2D cross section represents such a node as a circle.

41
Q

Angular Node

A

a plane of zero electron density that exists at a specific angle from a particular axis. In 3D, a angular node is a plane, but 2D cross section represents such a node as a line

42
Q

The total number of nodes depends on principal QN n, and is equal to _____.

A

n-1

43
Q

As the principal quantum number increases, the orbital size ___________.

A

increases

44
Q

In an s-orbital, the angular QN, l, is always equal to______.

A

zero

45
Q

In an s-orbital, the number of angular nodes is always equal to ______.

A

zero

46
Q

In a p-orbital, the angular QN, l, is always equal to ____.

A

one

47
Q

In a p-orbital, the number of angular nodes is always equal to ____.

A

one

48
Q

In both s and p orbitals, the number of angular nodes equals _____.

A

l

49
Q

The number of angular nodes in a d-orbital is always equal to _______.

A

two

50
Q

The value of the principal QN n determines the number of _________ nodes.

A

total

51
Q

The value of the principal QN n determines the ______ of the orbital.

A

size

52
Q

The value of the angular QN l determines the number of ________ nodes.

A

angular

53
Q

The value of the angular QN l determines the ______ of the orbitals.

A

shape

54
Q

How do you find the energy of an electron at a certain energy state?

A

Equation: E = -(1/n^2)RH

55
Q

What is the equation for wavelength of a photon?

A

“lambda” = hc/E

56
Q

What is the equation for wavelength of a particle?

A

“lambda” = h/mv

57
Q

How many atomic orbitals are in the sub-shell with quantum numbers n = 6 and l =2?

A

Five. This is a 6d orbital. All d orbitals have 5 orbitals.

Chemistry 121 (1 decks)

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