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chem atomic Flashcards

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1
Q

1661

A

Robert Boyle
Some supbstances can’t be made simpler
These are chemical elements

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2
Q

1803

A

John dalton
Elements composed indivisible atoms
Not broken down
Atoms same element have same mass

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3
Q

1896

A

Henri bewuerel
Radioactivity
Particles come from inside of atom
Not indivisible

Then jj
Electron

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4
Q

1911

A

Ernest Rutherford
Most mass and all pos charge of the atom was in tiny central nucleus

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5
Q

Proton mass

A

1

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6
Q

Neutron mass

A

1

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7
Q

Electron mass

A

1/1840

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8
Q

Protion charge

A

+1

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9
Q

Neutron charge

A

0

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10
Q

Electron charge

A

-1

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11
Q

Atomic number

A

Proton number
Z

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12
Q

Mass number

A

A
Protons + neutrons

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13
Q

Isotopes

A

Atoms of elements with same proton and electron numbers but diff neutron numbers
React chemical.y same way
Same configuration
Mass number varies due to diff neutrons

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14
Q

1913

A

Neil’s Bohr
Tiny positive nucleus orbited by electron
Shells of fixed sizes

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15
Q

1926

A

Erwin Schrödinger
Equation where electrons had some of the wave properties and particles
Predict behaviour of subatomic particles

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16
Q

1932

A

James Chadwick and the neutron

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17
Q

Lewis theory

A

1)inertness of noble gases related to their having full outer shell
2)ions formed by atoms losing or gaining electrons for full outer shells
3)atoms bond by sharing electrons to form full outer shells

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18
Q

Why daltons model used

A

Explain geometries I’d crystals

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19
Q

Why bohrs model used

A

Ionic and covalent nsi ding
Easy to draw and understand

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20
Q

Number of electrons on each shell

A

2n^2

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21
Q

First shell electrons

A

2

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22
Q

Second shell electrons

A

8

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23
Q

Third shell electrons

A

18

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24
Q

Why mass spectrometer is important

A

Accurate determination of ram

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25
Q

Why carbon 12 is used

A

Measured on a scale on which the mass of an atom of c12 is exactly 12g

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26
Q

Ram equation

A

Average mass molecule \ 1 twelfth mass of one c12

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27
Q

IRL what is mass spectrometer used for

A

Identify substances such as illegal drugs

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28
Q

Wuantam mechanics and Schrödinger

A

Solutions to his equation gives the probability of finding an electron in a given volume of space called atomic orbital

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29
Q

What do orbital shapes represent

A

A volume of space in which there is a 95% probability of finding an electron and they influence the shapes of molecules

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30
Q

Energy level 1

A

S sub levels
1 orbitak
2 electrons

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31
Q

Energy level 2

A

S and p sub levels
8 electrons

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32
Q

Energy shell 3

A

S p d
18 electrons

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33
Q

Energy level 4

A

S p d f
32 electrons

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34
Q

Spun

A

Electrons in same orbital have opposite spins
Arrows

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35
Q

Time takes to detects shows

A

What ion

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36
Q

Ions accelerate to the same

A

Ke

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37
Q

Why are transition metals specifical

A

Chromium and copper
Donate one of their 4s electors to the 3d sun shell
More stable with a full ir half full d sub shell
Lose 4s electrons before their 3d electrons

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38
Q

How many orbitals in s

A

1

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39
Q

How many orbitals in p

A

3

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40
Q

How many orbitals in d

A

5

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41
Q

How many orbitals in f

A

7

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42
Q

Which transition metals are partially filled

A

Vanadium
Chromium

43
Q

Similarity between chromium 50 and 53

A

24 protons and electrons

44
Q

Define relative atomic mass

A

Weighted average mass of an atom of an element taking into account its naturally occurring isotopes relative to 1/12 the ram of an atom if carbon 12

Average mass of an atom of an element /1/12 mass of one atom of carbon 12

45
Q

Now compared to rutherford

A

Current has neutrons and protons and orbital levels

46
Q

What are energy levels divided into

A

Sub shells which have different energies and shape

47
Q

Orbital definition.

A

Areas of space that predicts where an electron may be

48
Q

What does the letter of orbitals show

A

Shape of orbital

49
Q

What determines how atoms interact with each other

A

The arrangement of electrons

50
Q

Spectra order

A

1)ionisation
2)acceleration
3)ion drift
4 detection
5)analysis

51
Q

Now compared to Rutherford

A

Current has neutrons and protons and orbital levels

52
Q

Rules for writing electron configuration

A

1)lowest energy orbital filled first aufbau principle

2)hunds rule do not pair u Tim electrons have to be paired

When in orbitals of dual energy electrons will try and remain unpaired

3)no single orbital holds more than 2 electrons

4)Pauli exclusion principle electrons have two possible states with arrows one up and one down different spin states

53
Q

Electro spray ionisation

A

Sample dissolved in volatile substances and pushed through a small needle at high pressure

Connect to positive terminal at high voltage

Each particle gains h+ ions sample tuners into gas

54
Q

Electron Impact ionisation

A

Sample is vapourised and high energy electrons are fired at it

Knowcks one electron off each particle so they become +1 ions

All under a high vacuum

55
Q

Why vacuum used

A

To prevent the ions that are produced colliding with molecules from air so they don’t react inside the spectrometer

56
Q

Acelleration

A

Positive ions attracted to negatively charged plate and accelerated towards it so they have the same KE

Lighter ions move faster than heavier ions

57
Q

Ion drift

A

Ions pass through negatively charged plate with mi electric field. They drift
Pass through holed in negatively charged plate forming a beam and travel a to a detector

58
Q

Detections

A

Ions with same charge arrive at detectors
Lighter ones first as they have higher velocity
Flight times recorded
Pos ions pick up electron from the detector which causes current to flow

59
Q

Data analysis

A

Signal from the detector passed to s computer which generates a mass spectrum

60
Q

Getting a mass spectrum for molecular sample

A

1)molecular ion - m+ formed when electron removed
2)peak in a spectrum equal to relative molecular mass of molecule
3)identify unknown compound

61
Q

tof calculation steps

A

1) find the mass of theions times top number and divide by avagadros
2)find velocity/ke
3)find time/distance find length of tube or how long th flight takes

62
Q

elrctron config

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p…

63
Q

Ionisation energy

A

A measure of how easily an atom loses electrons to form positive ions
The first ionisation energy = the energy required to remove 1 electron from each atom in 1 mole of gaseous atoms of an element to form 1 mole of gaseous 1+ ions

64
Q

The first ionisation energy

A

the energy required to remove 1 electron from each atom in 1 mole of gaseous atoms of an element to form 1 mole of gaseous 1+ ions

65
Q

Endo sign

A

Plus

66
Q

Factors affecting ionisation energy

A

Nuclear charge
Distance from the nucleus
Shielding
Spin pair repulsion
Type of orbital
Occupancy of orbital
Effective nucleus charge

67
Q

Nucleus charge

A

More protons ,mor positive charge stinger attraction of electrons to nucleus

68
Q

Distance from nucleus

A

Further away weaker attraction

69
Q

Shielding

A

Further away more shells more shielding weaker attraction

70
Q

Spin pair repulsion

A

When electrons are paired
There is a repulsion from each other as they have the same charge this counteracts the attraction of the nucleus they are easy to remove

71
Q

High ionisation energy

A

A high attraction between the electron and the nucleus so more energy is needed to remove the electron

72
Q

How type of orbital effects ionisation energy

A

Some atoms have a stable electronic configuration will resist releasing an electron so have a higher ionisation energy required to overcome the stable configuration

73
Q

How occupancy of orbital affect nuclear charge

A

Half filled orbitals will have less tendency to release electrons therefore higher energy

74
Q

How effective nucleus charge affects ionisation energy

A

Higher orbital is subjected to the shielding effect generated by the nergstive charged electron and doesn’t experience the full nuclear charge

75
Q

What decreases ionisation

A

Greater period
Further away from nucleus
Lower nuclear charge
Less attraction more shielding
Easier to remove electrons

76
Q

Ionisation energy decreases down the group why

A

-proton in atom increases nucleus charge increases
-atomic radius increases due to more shells so bugger atom
-distance beteeen electron and nucleus increases
-shielding increases due to more shells of electrons
-these factors outweigh the increased nucleus charge so it’s easier to remove the outer electron as u go down

77
Q

Along the period inoinsqtion energy

A

Increases

78
Q

Ionic bonding

A

Strong electrostatic forces of attraction between positive ions and negative ions
Ions are formed when one or more electrons are transferred from oNe atom to another

79
Q

Why group four doesn’t forma charged ion

A

Form covalent bonds so no charge

80
Q

Compound ions to remember

A

So4 2- SULFATE
OH- HYDROXIDE
NO3 -
NH4+
CO3 2-

81
Q

Structure of ionic compounds

A

Each ion attracts oppositely charged ions in all directions
Giant ionic lattice

82
Q

First electron needs the least energy

A

Being removed from a neutral stom

83
Q

Second electron needs more energy

A

Because removed from +1ion

84
Q

2nd ionisation equation

A

X=x2+ +2e-

85
Q

ideal gas equation

A

pV=nRT
r is molar gas constant

86
Q

BOYLES LAW

A

PV=constant
constant as long as temperature remains constant

87
Q

Charles law

A

V/T=constant
vol of gas is proportional to the temp as long as the pressures remains the constant

88
Q

gas lussac law

A

P/T = constant
pressure is proportional to the temp as long as volume remains constant

89
Q

combining the laws give

A

pv/t = constant for a fixed mass of gas

90
Q

r value is

A

8.31 j/K.mol

91
Q

si units for ideal gas equation

A

p=pascal xkpa by 1000
v=cubic meters
t=kelvin- add 273 to degrees Celsius
r=j/k mol

92
Q

why would a lighter ion be more likely to be deflected

A

The amount of ion drift depends upon the:
The mass of the ion - the lighter the ion the more it will be deflected.
The charge of the ion - the higher the charge the more it will be deflected.

93
Q

covalent bonding

A

when non metals shared pair of electrons to get a full outer shell
the overlap of atomic orbitals each containing one electron to give a shared pair of electron
the shared pair of electrons are attracted to the nucleus of both the bonding atoms

93
Q

graphite

A

each. carbon covalently binder to 3 other carbons
1 delocalised electron conducts electrons
high m+b
weak intermolecular forces

94
Q

sillicon dioxide

A
95
Q

graphene

A
95
Q

Empirical formula

A

The simplest whole number ratio of moles of elements in a compound

96
Q

Solid to liquid

A

Fusion
Energy is supplied to weaken the forces acting between particles
Latent heat of melting
Enthrall y change of melting

97
Q

Enthalpy

A

The heat energy change measured under constant pressure whilst temperature depends on the average KE of particles and is therefore related to their speed
Greater energy -faster

98
Q

Liquid to gas

A

Vaporisation
Energy supplied to break all intermolecular forces between particles
Energy needed =latent heat of vapourisation
Aka enthalpy change of vapourisatioin

99
Q

Four types of Chrystal structures

A

Ionic -sodium chloride
Metallic - magnesium
Macromelular (giant covalent) - graphite and diamond
Molecular - iodine and ice

100
Q

Explain why the third ionisation energy of magnesium is much higher than the
second ionisation energy of magnesium.

A

Electron is removed from 2p subshell
Electron being removed is less shielded

101
Q

Molecular formula

A

The actual ratio of moles of elements in a compound
The two can be the same

102
Q
A

chem (34 decks)

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