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Advanced Higher Chemistry > Unit 1 - Organic Chemistry > Flashcards

Unit 1 - Organic Chemistry Flashcards

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1
Q

What is electromagnic radiaton

A

Form of radiation released by an electomagnetic process

-physical interaction between charged particles

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2
Q

What happens when charged particles are accelerate

A

They produce electromagnetic waves

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3
Q

The longer/shorter the wavelength, the greater the energy of the wave

A

Shorter

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4
Q

What is the electromagnetic spectrum

A

Range of all possible frequencies in electromagnetic radiation

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5
Q

What does rlectromagnetic radiation include

A

Light
Xray
Radio waves

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6
Q 
Violet = (1) wavelength
Red = (2) wavelength
A

1 longest

2 shortest

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7
Q

Define wavelength

A

Distance between adjacent crest of wave

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8
Q

What is the adjacent crest of the wave

A

Highest point

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9
Q

Define frequency

A

Number of wavelengths that pass a fixed point in time unit

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10
Q

Define valency

A

Speed of light (constant of 3x10^8)

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11
Q

What is wave particle duality

A

Electromagnetic radiation can be considered both, waves and particles

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12
Q

What is a quanta

A

Can transfer a specific amount of Energy

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13
Q

What information can light provide about an atom

A

Quantity and type

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14
Q

What is an atomic spectra

A

Caused by electroms moving between different E levels

=fixed for one atom

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15
Q

Quantum theory

A

Matter can only emit/ absorb E in small fixed amount

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16
Q

When an electron absorbs a photon of E it moves from lower/higher E level to a lower/higher level

A

Lower

Higher

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17
Q

How is light emitted

A

When the electron that has been promoted to a higher E level drops back down

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18
Q

What is evidence for the existence of Energy levels

A

The light E emitted by an atom produces a spectrum that is made up of a series of lines descrete (quantised) E levels

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19
Q

Photons of high/low radiation can transfer greater amounts of energy

A

High

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20
Q

Radiation is absorben when electrons are promoted to a lower/higher level

A

Higher

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21
Q

What is an absorption spectrum

A

Produced by measuring how the intensity of absorbed light varies with wavelength

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22
Q

Why are high temperatures used in emission spectroscopy

A

To excite electrons within atoms

When e- drops= quantum emitted

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23
Q

What is an emission spectrum

A

Produced by measuring the intensity of light emitted or absorbed

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24
Q

What is the concentration of an element related to in atomic spectroscopy

A

Intensity of emitted or absorbed light

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25
Q

What is referred to as ground state

A

Lowest possible electronic configuration the electrons in an atom can adopt

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26
Q

Levels become closer/further apart as n increases

A

Closer

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27
Q

What is rhe convergence limit

A

Point at which E levels become so close together that they converge

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28
Q

State the Aufbau Principle

A

Orbitals are filled in order of increasing energy

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29
Q

State the Pauli Exclusion Principle

A

No 2 electrons in one atom can have the same set of 4 quantum numbers

  • no orbital can hold more than 2 electrons
  • electrons have opposite spin
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30
Q

State Hunds Rule

A

When degenerate orbitals are available, electrons fill each singly, keeping spins parallel before pairing starts

31
Q

Why does 4s get filled up before 3d

A

Because it has a lower energy state

32
Q

Whats an isolated atom

A

Exists separately without any bonding

-orbitals in each subshell are degenerate

33
Q

Whats ionisation energy

A

Energy required to remove one mole of electron from one mole of gaseous atom

34
Q

Full shell = (1) = high/low IE

half full shell = (2) = high/low IE

A

1 very stable, high

2 stable, high

35
Q

Why is IE higher for stable molecules

A

More difficult to remove electron

36
Q

How are covalent bonds formed

A

Formed when aromic orbitals overlap to form molecular orbital

37
Q

What are molecular orbitals

A

Overlapping atomic orbitals

-form covalent bonds

38
Q

Whats VSEPR

A

valency shell electron pair repulsion

Theory that pairs of e- that surround central atom of a molecule or ion are arranged as far apart as possible to minimise electron repulsion

39
Q

What can vsepr be used for

A

Can be used to predict shapes of molecules and polyatomic ions

40
Q

What must be considered for vsepr

A

Bonding and non bonding pairs

41
Q

Whats a dative bond

A

Both electrons come from one of the elements involved in bond

-covalent

42
Q

Why do bonding e- repell less than non nonding e-

A

Because they are attracted by 2 nuclei

43
Q

Transition metals have at least one ion with (1)

A

And incomplete subshell

44
Q

Are 4s filled before or after 3d for transition metals

A

Before

45
Q

High oxidation number= 1

Low oxidation number= 2

A

1 oxidation

2 reduction

46
Q

Compounds with high oxidation states 1

Compounds with low oxidation state 2

A

1 oxidising agend

2 reducing agend

47
Q

What di transition metal complexes consist of

A

Central metal ion surrounded by ligands

48
Q

What are ligands

A

Molecules/ neg ions that donate electron pairs into unfilled d orbitals

49
Q

Whats monodentate

A

Donates 1 e- pair eg water

50
Q

Whats bidentate

A

Donates 2 e- pairs eg oxalate

51
Q

Whats hexadentate

A

Donates 6 e- pairs eg EDTA4-

52
Q

What does colour depend on in transition metals

A

Oxidation state

53
Q

Properties of ligands (3)

A

Have at least one lone pair

Usually neg/molecule

54
Q

What is coordination number

A

Total number of binds from ligand to central mental

55
Q

What is the shape of an ion complex determined by

A

Coordination number

56
Q

What dies colour of transition metals depend on

A

Oxidation state
Identity
Ligands attached

57
Q

Some of visible spectrum absorbed=

A

Colourr

58
Q

Non of visible spectrum absorbed

A

Colourless

59
Q

All of visible spectrum absorbed

A

Black

60
Q

How are transition metal complexes able to absorb light

A

Because of 5 degenerate d orbitals splitting in terms of energy

61
Q

What properites does energy have in free transition metal ions

A

Degenerate

62
Q

What are ftee transition metal ions

A

Transition metals with no ligands

63
Q

What is the spectrochemical series

A

A list of ligands according to how strongly they split d orbitals in transition metal complexes

64
Q

Spectrochemical series from strongest to weakest

A

CN->NH3>H2O>OH->F->Cl->Br->I-

65
Q

What is crystal field strength

A

Difference in energy between two subshells of d orbitals

66
Q

When one colour is absorbed, what colour is emitted

A

Complementary colour eg green/purple

67
Q

How do d orbitals split in higher/lower energies

A

E- present in approaching ligands cause e- in orbutals lying along axes to be repelled

68
Q

When is light emitted

A

When e- jump from higher to lower energy level

69
Q

When is light absorbed

A

When e- from lower energy level are promoted to higher

70
Q

What are strong field ligands

A

More likely to occur in UV region

71
Q

What are heterogenous catalysts

A

In different state to reactant

72
Q

What are homogenous catalysts

A

Same state as reactant

73
Q

How can heterogenous catalysts be explained

A

Formation of activated complexes and absorption of reactive molecules into active site

Presence of unpaired e- or unfilled d orbitals allow complexes to form

74
Q

How can homogenous catalysts be explained

A

Changing oxidation states cause formation of complexes

Advanced Higher Chemistry (4 decks)

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