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AH Chemistry > 1.1 and 1.2 > Flashcards

1.1 and 1.2 Flashcards

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1
Q

velocity, frequency, wavelength relationship

A

C (velocity) = f x wavelength

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2
Q

EM radiation order from high energy/frequency to low energy/frequency

A

Gamma rays
X rays
UV Radiation
Visible light
Infra red
Microwaves
Radio and TV

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3
Q

EM radiation order from high energy/frequency to low energy/frequency

A

Gamma rays
X rays
UV Radiation
Visible light
Infra red
Microwaves
Radio and TV

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4
Q

What is wavelength and units

A

The distance between two wave crests

Measured in m or nm

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5
Q

The distance between two wave crests

Measured in m or nm

A

Wavelength

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6
Q

What is frequency and units

A

The number of waves per second

Hz

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7
Q

The number of waves per second

Hz

A

Frequency

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8
Q

What is velocity and units

A

Speed of waves

It is always 3 x 10^8

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9
Q

Speed of waves

It is always 3 x 10^8 m s

A

Velocity

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10
Q

Velocity

A

Speed of waves

It is always 3 x 10^8

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11
Q

Wave - particle duality

A

Under some circumstances, EM radiation can be regarded as a stream of very small particles called photons rather than waves

These photons transfer small bundles of energy

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12
Q

Energy of photons of radiation calculation

A

E = h x f

Where E is energy in Joules

h is planks constant in J s

f is frequency in Hz

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13
Q

E = h x f

Where E is energy in Joules

h is planks constant in J s

f is frequency in Hz

A

Energy of photons of radiation

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14
Q

Energy of one mole of photons

A

E = L x hf OR E = Lhc / wavelength

Where E is energy in Joules

L is avogrados constant

h is planks constant in J s

f is frequency in Hz

c is constant

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15
Q

Wave number

A

m^-1 or cm^-1

1 / wavelength

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16
Q

m^-1 or cm^-1

1 / wavelength

A

Warenumber

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17
Q

What does em radiation behave as when absorbed by matter

A

A stream of particles. These particles are known as photons

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18
Q

What does a photon carry

A

Quantised energy proportional to the frequency of radiation

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19
Q

What happens to electrons when a photon is absorbed or emitted

A

Energy is gained or lost by electrons within the substance

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20
Q

Photons in high frequency radiation can transfer greater amounts of energy than photons in low frequency radiation

A

Greater

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21
Q

Photons in _______ can transfer greater amounts of energy than photons in low frequency radiation

A

High frequency radiation

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22
Q

_____ in high frequency radiation can transfer greater amounts of energy than _____ in low frequency radiation

A

Photons

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23
Q

What happens when energy is transferred to atoms

A

Electrons within the atoms may be promoted to higher energy levels

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24
Q

What causes electrons within the atoms may be promoted to higher energy levels

A

Energy being transferred to atoms

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25
Q

What does an atom emit when an excited electron moves from a higher energy level to a lower energy level

A

A photon of light energy

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26
Q

What causes an atom to emit a photon of light energy

A

when an excited electron moves from a higher energy level to a lower energy level

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27
Q

What does the light energy emitted by an atom produce

A

A spectrum that is made up of a series of lines at discrete (quantised) energy levels

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28
Q

What produces a spectrum that is made up of a series of lines at discrete (quantised) energy levels

A

The light energy emitted by an atom

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29
Q

What provides energy for the existence of energy levels

A

Spectrum that is made up of a series of lines at discrete energy levels

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30
Q

Each element produces a unique and characteristic…

A

Absorption and emission spectra

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31
Q

What can absorption and emission spectra be used for

A

To identify and quantify the element

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32
Q

What can be used to identify and quantify the element

A

Absorption and emission spectra

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33
Q

What happens in absorption spectroscopy

A

EM radiation is directed at an atomised sample

Radiation is absorbed as electrons are promoted to higher energy levels

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34
Q

EM radiation is directed at an atomised sample

Radiation is absorbed as electrons are promoted to higher energy levels

A

Absorption spectroscopy

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35
Q

How is an absorption spectrum produced

A

Measuring how the intensity of light varies with wavelength

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36
Q

What is produced by measuring how the intensity of light varies with wavelength

A

Absorption spectrum

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37
Q

What happens in emission spectroscopy

A

High temperatures are used to excite electrons within atoms.

As the electrons drop to lower energy levels, photons are emitted

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38
Q

High temperatures are used to excite electrons within atoms.

As the electrons drop to lower energy levels, photons are emitted

A

Emission spectroscopy

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39
Q

How is an emission spectrum produced

A

By measuring the intensity of light emitted at different wavelengths

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40
Q

What is produced by measuring the intensity of light emitted at different wavelengths

A

Emission spectrum

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41
Q

What relates together in atomic spectroscopy

A

The concentration of an element within a sample is related to the intensity of light emitted or absorbed

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42
Q

The concentration of an element within a sample is related to the intensity of light emitted or absorbed

A

Atomic spectroscopy

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43
Q

each line on an emission spectrum corresponds to what

A

the energy given out when an excited electron moved to a lower level

44
Q

what corresponds to the energy given out when an excited electron moved to a lower level

A

each line on an emission spectrum

45
Q

electrons have the properties of..

A

both waves and particles

46
Q

principal quantum number, n

A

the main energy level of an electron and is related to the size of the orbital

47
Q

the main energy level of an electron and is related to the size of the orbital

A

principal quantum number, n

48
Q

angular momentum quantum number, l

A

the shape of the subshell

values from zero to n-1

49
Q

the shape of the subshell

values from zero to n-1

A

the angular momentum quantum number, l

50
Q

the shape of the subshell

values from zero to n-1

A

angular momentum quantum number, l

51
Q

the orientation of the orbital

values between -l and +l

A

ml

52
Q

ml

A

the orientation of the orbital

values between -l and +l

53
Q

spin quantum number, ms

A

the direction of spin

values of +1/2 or -1/2

54
Q

the direction of spin

values of +1/2 or -1/2

A

spin quantum number, ms

55
Q

how do electrons behave as in an atom

A

behave as standing (stationary) waves

56
Q

when do electrons behave as standing (stationary) waves

A

in an atom

57
Q

electrons as waves in atoms

A

waves that vibrate in time but do not move in space

58
Q

electrons as waves in atoms

A

waves that vibrate in time but do not move in space

59
Q

there are different _______ of standing wave possible around the nucleus, known as ______

A

sizes and shapes

orbitals

60
Q

maximum number of electrons in orbitals

A

two

61
Q

different shapes of orbitals identified that

A

s

p

d

f

62
Q

s

p

d

f

A

different shapes of orbitals

63
Q

electrons within atoms have a ___ amount of energy

A

fixed

64
Q

electrons within _____ have a fixed amount of energy

A

atoms

65
Q

fixed amount of energy of electrons within atoms

A

quanta

66
Q

fixed amount of energy of electrons within atoms

A

quanta

67
Q

you can describe any electron in an atom with..

A

four quantum numbers:

n
l
ml
ms

68
Q

what can be explained using the four quantum numbers

A

electrons in atoms

69
Q

electrons are arranged according to…

A

aufbau principle

hunds rule

the pauli exclusion principle

70
Q

the aufbau principle

A

electrons fill orbitals in order of increasing energy

71
Q

electrons fill orbitals in order of increasing energy

A

aufbau principle

72
Q

electrons fill orbitals in order of increasing energy

A

aufbau principle

73
Q

hunds rule

A

when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts

74
Q

when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts

A

hunds rule

75
Q

Pauli exclusion principle

A

No two electrons in one atom can have the same set of four quantum numbers, therefore, no orbital can hold more than two electrons and the electrons must have opposite spins

76
Q

No two electrons in one atom can have the same set of four quantum numbers, therefore, no orbital can hold more than two electrons and the electrons must have opposite spins

A

Pauli exclusion principle

77
Q

What are orbitals in an isolated atom

A

Degenerate

78
Q

What are orbitals a part of

A

Subshell

79
Q

What four blocks can the periodic table be divided into

A

S
P
D
F

80
Q

What do the blocks making up the periodic table correspond to

A

Their outer electron configuration

81
Q

What can explain the differences in ionisation energies for an element

A

The relative stability of different subshell electron configurations

82
Q

What provides evidence for electronic configurations

A

Differences in first second etc ionisation energies

83
Q

Significant stability of atoms is associated with what subshells

A

Half filled and full subshells

84
Q

VSEPR

A

Valence
shell
electron
pair
repulsion

85
Q

What can VSEPR be used for

A

Predict the shapes of molecules and polyatomic ions

86
Q

What to use to predict the shapes of molecules and polyatomic ions

A

VSEPR

87
Q

How to find the number of electron pairs on a central atom

A
  • take total number of outer electrons on the central atom and add one for each atom attached
  • Adding an electron for every negative charge
  • removing an electron for every positive charge
  • divide by two
88
Q
  • take total number of outer electrons on the central atom and add one for each atom attached
  • Adding an electron for every negative charge
  • removing an electron for every positive charge
  • divide by two
A

How to find number of electron pairs surrounding a central atom

89
Q

What do electrons do because they are negatively charged

A

Repel Eachother

90
Q

What two things to electrons arrange based on

A

Minimise repulsion

Maximise separation

91
Q

Arrangement of electron pairs for two electron pairs

A

Linear

92
Q

Arrangement of electron pairs for three electron pairs

A

Trigonal planar

93
Q

Arrangement of electron pairs for four electron pairs

A

Tetrahedral

94
Q

Arrangement of electron pairs for five electron pairs

A

Trigonal bipyramidal

95
Q

Arrangement of electron pairs for six electron pairs

A

Octahedral

96
Q

How many electron pairs in linear arrangement

A

Two

97
Q

How many electron pairs in trigonal planar arrangement

A

Three

98
Q

How many electron pairs in tetrahedral arrangement

A

Four

99
Q

How many electron pairs in trigonal bipyramidal arrangement

A

Five

100
Q

How many electron pairs in octahedral arrangement

A

Six

101
Q

Arrangement of electron pairs ——> ______

A

Shapes of atoms

102
Q

________ ——> shapes of atoms

A

Arrangement of electron pairs

103
Q

Shapes of atoms ——> ________

A

Shapes of molecules or polyatomic ions

104
Q

_____ ——> shapes of molecules or polyatomic ions

A

Shapes of atoms

105
Q

Electron pair repulsions strength from strongest to weakest

A

Non bonding pair / non bonding pair

Non bonding pair / bonding pair

Bonding pair / bonding pair

106
Q

Non bonding pair / non bonding pair

Non bonding pair / bonding pair

Bonding pair / bonding pair

A

Electron pair repulsion from strongest to weakest

AH Chemistry (7 decks)

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