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chemistry: physical chemistry 1 > atomic structure > Flashcards

atomic structure Flashcards

(52 cards)

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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?

Study These Flashcards
A

simple and explains many experimental observations

22
Q

what do all types of TOF mass spectrometry rely on?

Study These Flashcards
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?

Study These Flashcards
A

● electron impact (aka electron bombardment)

● electron spray ionisation

24
Q

what is electron impact ionisation?

Study These Flashcards
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
what is the symbol equation for electron impact ionisation?
● X(g) -> X⁺(g) + e⁻ ● include state symbols
26
what does volatile mean?
easily evaporates
27
what is electron spray ionisation?
● 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
what is the symbol equation for electron spray ionisation?
● X(g) + H⁺ -> XH⁺ (g)
29
what is the technique of electron spray ionisation used for?
● substances with higher molecular mass ● including biological molecules like protein
30
what is the technique of electron spray ionisation known as?
soft ionisation as fragmentation rarely takes place
31
explain acceleration in TOF mass spectrometry
positive ions accelerated using electric field so they all have same KE
32
what is the equation for kinetic energy?
KE + 1/2mv^2 KE - (J) m - (kg) v - (m/s)
33
what is the equation for velocity?
v = √ 2KE / m
34
what does the velocity of each particle depend on?
● mass ● lighter particles have faster velocity ● heavier particles have slower velocity
35
explain ion drift in the flight tube in TOF mass spectrometry
● 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
what is the equation for time of flight?
t = d / v t = d x √m /2KE t = (s) d = (m) v = (m/s)
37
explain detection in TOF mass spectrometry
● 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
what are the rules of putting electrons into atomic orbitals?
● 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
how do you do electron configuration short structure?
put noble gas before: [Ne] 3s1
40
what are rules for electron configuration of transition metals?
● 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
what are main levels and sub levels?
● main levels - 1, 2, 3 etc ● main levels have sub levels - s, p, d, f
42
how many orbitals do each sub level have?
● 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
what is the order of electron arrangement?
1s 2s 2p 3s 3p 4s 3d 4p
44
what is the electron configuration for copper?
● 1s2 2s2 2p6 3s2 3p6 4s1 3d10 ● more stable configuration
45
what is the electron configuration for chromium?
● 1s2 2s2 2p6 3s2 3p6 4s1 3d5 ● more stable configuration
46
what is ionisation energy?
● 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
what is the first ionisation energy?
● 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
what is the second ionisation energy?
● energy required to move the second electron (not both) ● Na+(g) -> Na2+(g) + e-
49
what is the trend in ionisation energy down a group?
● generally decreases ● increased nuclear charge (more protons) ● atoms get bigger ● more shielding ● therefore, weaker attraction from nucleus to electron in outer shell
50
what is the trend in ionisation energy across a period?
● 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
what is the exception in the trend across a period?
● 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
why does atomic radius decrease across a period?
increase in nuclear charge attracts electrons more strongly, pulling them to nucleus

chemistry: physical chemistry 1 (6 decks)

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