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chemistry: physical chemistry 1 > atomic structure > Flashcards

atomic structure Flashcards

1
Q

what do atoms consist of?

A

● central, small nucleus

● protons and neutrons in nucleus

● surrounded by electrons in energy levels

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2
Q

how are the electrons arranged?

A

2 . 8 . 8 . 2

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3
Q

what is the relative mass of a proton?

A

1

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4
Q

what is the relative charge of a proton?

A

1+

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5
Q

what is the relative mass of a neutron?

A

1

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6
Q

what is the relative charge of a neutron?

A

0

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7
Q

what is the relative mass of an electron?

A

1/2000

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8
Q

what is the relative charge of an electron?

A

1-

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9
Q

what is the atomic number?

A

● number of protons in nucleus

● way to remember: atomic so at the bottom because it’s so small

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10
Q

what is the mass number?

A

● number of protons + number of neutrons

● way to remember: MASSive so at the top

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11
Q

what do atoms of the same element all have the same number of?

A

● protons

● protons determines what type of atom it is

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12
Q

what are isotopes?

A

● atoms of the same element with same number of protons and different number of neutrons

●same atomic number but different mass number

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13
Q

what did john dalton describe atoms as?

A

● solid spheres

● spheres made up different elements

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14
Q

what did j.j thomson discover and what model did he propose?

A

● electron

● new model made ‘plum pudding model’

● positively charged pudding, electrons inside

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15
Q

what experiment did rutherford conduct?

A

gold foil experiment

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16
Q

what was the gold foil experiment?

A

● fired positive alpha particles at thin gold sheet

● most particles passed through but some deflected

● so must be positive nucleus

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17
Q

what was the nuclear model?

A

● tiny positively charged nucleus surrounded by a ‘cloud’ of negative electrons

● most of atom is empty space

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18
Q

why was nuclear model wrong?

A

cloud around nucleus of atom would spiral into nucleus causing atom to collapse

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19
Q

what was the model niels bohr proposed?

A

electrons are in shells

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20
Q

how was the bohr model refined?

A

included sub-shells

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21
Q

why is the bohr model still used today?

A

simple and explains many experimental observations

22
Q

what do all types of TOF mass spectrometry rely on?

A

● forming ions from samples

● separating ions depending on their m/z (mass charge) ratio

23
Q

what are the types of ionisation in TOF mass spectrometry?

A

● electron impact (aka electron bombardment)

● electron spray ionisation

24
Q

what is electron impact ionisation?

A

● sample analysed is vaporised

● high energy electrons fired at it (from electron gun)

● knocks off 1 electron from each particle forming a 1+ ion

● fragmentation occurs

● for smaller molecules

25
Q

what is the symbol equation for electron impact ionisation?

A

● X(g) -> X⁺(g) + e⁻

● include state symbols

26
Q

what does volatile mean?

A

easily evaporates

27
Q

what is electron spray ionisation?

A

● sample dissolved in volatile solvent (water)

● injected through fine hypodermic needle to give fine mist (aerosol)

● tip of needle attached to positive terminal of high voltage power supply

● particles ionised by gaining proton (ie H⁺ which is 1 proton) from solvent as they leave needle

● producing XH⁺ ions (ions with single positive charge and mass of Mr + 1)

● solvent evaporates away while XH⁺ ions are attracted towards a negative plate where they are accelerated

28
Q

what is the symbol equation for electron spray ionisation?

A

● X(g) + H⁺ -> XH⁺ (g)

29
Q

what is the technique of electron spray ionisation used for?

A

● substances with higher molecular mass
● including biological molecules like protein

30
Q

what is the technique of electron spray ionisation known as?

A

soft ionisation as fragmentation rarely takes place

31
Q

explain acceleration in TOF mass spectrometry

A

positive ions accelerated using electric field so they all have same KE

32
Q

what is the equation for kinetic energy?

A

KE + 1/2mv^2

KE - (J)
m - (kg)
v - (m/s)

33
Q

what is the equation for velocity?

A

v = √ 2KE / m

34
Q

what does the velocity of each particle depend on?

A

● mass

● lighter particles have faster velocity

● heavier particles have slower velocity

35
Q

explain ion drift in the flight tube in TOF mass spectrometry

A

● positive ions travel through hole in negatively charged plate into tube

● time of flight of each particle through flight tube depends on velocity which depends on mass

36
Q

what is the equation for time of flight?

A

t = d / v

t = d x √m /2KE

t = (s)
d = (m)
v = (m/s)

37
Q

explain detection in TOF mass spectrometry

A

● positive ions hit a negatively charged electric plate

● when they hit detector plate, positive ions are discharged

● by gaining electrons from the plate

● this generates a movement of electrons and an electric current that is measured

● size of current measured is proportional to the abundance

38
Q

what are the rules of putting electrons into atomic orbitals?

A

● spin - 2 electrons in same orbital must have opposite spin

● aufbau principle - atomic orbitals with lower energy filled first

● hund’s rule - atomic orbitals of same energy fill singly before starting pair (of opposite spin)

39
Q

how do you do electron configuration short structure?

A

put noble gas before: [Ne] 3s1

40
Q

what are rules for electron configuration of transition metals?

A

● electron lost from 4s level first (fills first, empties first)

● as soon as electron enters the 4s orbital, energy increases to be greater than 3d

41
Q

what are main levels and sub levels?

A

● main levels - 1, 2, 3 etc

● main levels have sub levels - s, p, d, f

42
Q

how many orbitals do each sub level have?

A

● s has 1 orbital (holds 2 electrons)

● p has 3 orbitals (holds 6 electrons)

● d has 5 orbitals (holds 10 electrons)

● f has 7 orbitals (holds 14 electrons

43
Q

what is the order of electron arrangement?

A

1s 2s 2p 3s 3p 4s 3d 4p

44
Q

what is the electron configuration for copper?

A

● 1s2 2s2 2p6 3s2 3p6 4s1 3d10

● more stable configuration

45
Q

what is the electron configuration for chromium?

A

● 1s2 2s2 2p6 3s2 3p6 4s1 3d5

● more stable configuration

46
Q

what is ionisation energy?

A

● energy required to remove one mole of electrons from one mole of atoms in the gaseous state (kjmol-1)

● state symbols are essential when writing equation

47
Q

what is the first ionisation energy?

A

● energy required to remove 1 electron from each atom in a mole of gaseous atoms producing one mole of unipositive gaseous ions

● Na(g) -> Na+ (g)+ e-

48
Q

what is the second ionisation energy?

A

● energy required to move the second electron (not both)

● Na+(g) -> Na2+(g) + e-

49
Q

what is the trend in ionisation energy down a group?

A

● generally decreases

● increased nuclear charge (more protons)

● atoms get bigger

● more shielding

● therefore, weaker attraction from nucleus to electron in outer shell

50
Q

what is the trend in ionisation energy across a period?

A

● generally increases

● increased nuclear charge (more protons)

● atoms get smaller

● shielding stays the same

● therefore, stronger attraction from nucleus to electron in outer shell

51
Q

what is the exception in the trend across a period?

A

● Mg -> Al

● electron lost from Al is lost from the p orbital, while that lost from Mg is from the s orbital

● P orbital has higher energy than S orbital, so easier to lose electrons

● N -> O

● in O, electrons are paired in the 2p orbital

● therefore, the repulsion between electrons make it easier to remove one of them

● P -> S

● in S, electrons are paired in 3p orbital

● therefore the repulsion between electrons makes it easier to remove one of them

52
Q

why does atomic radius decrease across a period?

A

increase in nuclear charge attracts electrons more strongly, pulling them to nucleus

chemistry: physical chemistry 1 (5 decks)

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