Quantum Theory Flashcards

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
What type of wave is an electron?
A standing wave
26
How can you find the number of orbitals in a sub-shell?
2(L) + 1
27
How many orbitals in sub-shell s?
1
28
How many orbitals in sub-shell p?
3
29
How many orbitals in sub-shell d?
5
30
How many orbitals in sub-shell f?
7
31
Diamagnetic
Substances that are slightly repelled by a magnet
32
Paramagnetic
Substances that are attracted to a magnetic field. They have unpaired electrons.
33
What is the shape of s orbitals?
They are spherically symmetrical.
34
Principal QN n
n = 1,2,3...
35
How do you find the density of the electron wave?
Wavefunction^2
36
As the principal QN n increases, the number of nodes in a wavefunction ____________.
increases
37
At a node, the sign of the wavefunction is _______.
zero
38
On either side of a node, the sign of the wavefunction __________.
changes phase
39
A node is a region of _______ electron density.
zero
40
Radial node
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
Angular Node
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
The total number of nodes depends on principal QN n, and is equal to _____.
n-1
43
As the principal quantum number increases, the orbital size ___________.
increases
44
In an s-orbital, the angular QN, l, is always equal to______.
zero
45
In an s-orbital, the number of angular nodes is always equal to ______.
zero
46
In a p-orbital, the angular QN, l, is always equal to ____.
one
47
In a p-orbital, the number of angular nodes is always equal to ____.
one
48
In both s and p orbitals, the number of angular nodes equals _____.
l
49
The number of angular nodes in a d-orbital is always equal to _______.
two
50
The value of the principal QN n determines the number of _________ nodes.
total
51
The value of the principal QN n determines the ______ of the orbital.
size
52
The value of the angular QN l determines the number of ________ nodes.
angular
53
The value of the angular QN l determines the ______ of the orbitals.
shape
54
How do you find the energy of an electron at a certain energy state?
Equation: E = -(1/n^2)RH
55
What is the equation for wavelength of a photon?
"lambda" = hc/E
56
What is the equation for wavelength of a particle?
"lambda" = h/mv
57
How many atomic orbitals are in the sub-shell with quantum numbers n = 6 and l =2?
Five. This is a 6d orbital. All d orbitals have 5 orbitals.