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chem > topic 1: atomic structure and the periodic table > Flashcards

topic 1: atomic structure and the periodic table Flashcards

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1
Q

structure of atom

A
  • protons and neutrons in nucleus
  • electrons in orbitals
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2
Q

rel charge proton

A

+1

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3
Q

rel mass proton

A

1

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4
Q

rel charge neutron

A

0

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5
Q

rel mass neutron

A

1

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6
Q

rel charge electron

A

-1

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7
Q

rel mass electron

A

1/1836

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8
Q

atomic number

A
  • number of protons in nucleus of atom
  • Z
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9
Q

mass number

A

total number of protons and neutrons in nucleus of atom (also known as nucleon number)
- symbol A

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10
Q

isotopes

A

same number of protons but different number of neutrons

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11
Q

properties of isotopes

A
  • similar chemical properties but different physical properties
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12
Q

why do isotopes have similar chemical properties (2)

A
  • same electron configuration
  • same number of outer shell electrons so react similarly
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13
Q

relative isotopic mass

A

mass of one atom of an isotope relative to the mass of 1/12 of a carbon-12 atom

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14
Q

relative atomic mass

A

MEAN mass of an atom relative to the mass of 1/12 of a carbon-12 atom

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15
Q

chlorine ATOM mass spec

A
  • 2 molecular ion peaks as exists as TWO ISOTOPES
    -35 Cl and 37 Cl
  • peak heights ratio is 3:1 as abundance of 35Cl is 3* that of 37 Cl
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16
Q

diatomic chlorine molecule mass spec

A

-3 molecular ion peaks
- 35Cl+35Cl
-35Cl + 37Cl
-37Cl + 37Cl
RATIO of peaks: multiply probability of each; eg for 35, 35 3/4*3/4

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17
Q

one BROMINE atom mass spec

A
  • 2 isootopes
  • so 2 molecular ion peaks
    -79Br and 81 Br
  • 1:1 abundance
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18
Q

diatomic bromine moleculemass spec

A
  • 3 molecular ion peaks
  • 79Br, 79Br
    -79Br,81Br
    -81Br,81Br
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19
Q

peak with highest m/z value…

A

molecular ion peak which gives info about MOLECULAR MASS

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20
Q

FIRST ionisation energy

A

amount of energy required to remove one mole of electrons from one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

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21
Q

first ionisation energy of calcium

A

Ca(g) -> Ca+(g) + e-

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22
Q

second ionisation energy

A

energy required to remove one mole of electrons from one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions

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23
Q

second IE calcium

A

Ca+(g) -> Ca2+(g) + e-

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24
Q

why do successive ionisation energies increase (generally)

A
  • when an electron is removed, a positive ion is formed
  • less electrons for same number of protons
  • larger effective nuclear charge- STRONEGER ES ATTRACTION (decreasing p to e ratio)
  • more energy required
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25
Q

shape of s orbital

A

spherical (draw a circle)

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26
Q

shape of p orbital

A

infinity sign (facing upwards)

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27
Q

what is an orbital

A

a region within an atom that can hold up to 2 electrons with opposite spins

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28
Q

IE across period

A

increases

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29
Q

IE down group

A

decreases

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30
Q

IE across period explanation

A
  • increases
  • nuclear charge increases
  • atomic radius decreases as stronger attraction, so distance decreases
  • CONSTANT shielding as electrons added to same shell
  • more energy needed to remove an electron
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31
Q

beryllium to boron ionisation energy

A

DECREASE:
- boron electron in 2p
- - higher energy subshell
- more sheilding
- weaker attraction , smaller radius, less energy required

32
Q

nitrogen to oxygen (same for phosphorus to sulphur)

A

DECREASE
- in oxygen , 2 electrons in 2p orbital
- in nitrogen , only 1 electron in 2p orbital
- repulsion in electrons means easier to remove

33
Q

from one period to the next

A

LARGE DECREASE in IE
- increased distance between nucleus and outer shell e- as NEW SHELL
- more sheilding
- OUTWEIGHT increased nuclear charge

34
Q

IE down group explanation

A
  • DECREASES
  • more protons, higher nuclear charge
  • atomic radius INCREASES
  • distance increases
  • shielding increases
  • factors outweighs increased nuclear charge
35
Q

shell CLOSEST to nucleus

A

n=1 quantum shell

36
Q

number of electrons that can be hold in each shell

A

2n^2
eg: in shell 4, 32 e-

37
Q

no. of electrons per orbital

A

2

38
Q

no. orbitals in s subshell

A

1 (2e-)

39
Q

no. orbitals in p subshell

A

3 (6e-)

40
Q

no. orbitals in d subshell

A

5 (10e-)

41
Q

no. orbitals in f subshell

A

7 (14e-)

42
Q

orbitals in same subshell are

A

equal in energy (degenerate)

43
Q

how are subshells filled

A

in order of increasing energy

44
Q

Chromium electron config

A

[Ar] 3d5 4s1

45
Q

Copper electron config

A

[Ar] 3d10 4s1

46
Q

s d p blocks

A

left, middle, right

47
Q

random decrease in IE across period (eg Mg to Al, Be to B)

A

electron removed from HIGHER energy level subshell, so less IE

48
Q

periodicity defintion

A

trends that repeatedly occur across a period

49
Q

state how to find relative abundance of isotopes

A

measure number of particles for each isotope detected in a mass spectrometer

50
Q

chlorine mass spec ratios

A

for 35,35: 0.752
for 35,37: 0.750.35 2
for 37,37: 0.250.25
9:6:1 ratio

51
Q

mass spec deflection

A
  • by electromagnets
  • ions with higher mass are deflected LESS
  • ions with smaller mass (or higher charge) deflected more
52
Q

why does mass spec happen in a vacuum

A

to prevent collisions with air particles

53
Q

meaning of the arrows in boxes

A
  • 2 electrons with opposite spins in the same orbital
54
Q

y might 2 elements react similarly (2)

A
  • same number of outer shell electrons
  • governs their chemical reactions
55
Q

deductions from ionisation energy graphs

A
  • big jumps between x and x
  • therefore ELECTRON CONFIGURATION ….
56
Q

why is there a bigger increase in 2nd and 3rd IE compared to 1st and 2nd? (group 2)

A
  • 1 and 2 from same subshell
  • similar shielding
  • 3 from subshell CLOSER TO NUCLEUS
  • less shielding
  • weaker attraction so less energy required
57
Q

why use logs for IE

A
  • range too big
  • numbers too large so y axis too large
58
Q

why might x have a lower IE

A
  • electron removed from higher energy subshell
  • more shielded from nucleus
59
Q

in mass spec, which is the molecular ion peak

A

the one with the highest m/z

60
Q

why is ionisation energy always positive

A
  • endothermic
  • energy taken in by the reaction
61
Q

orbitals can hold

A

up to 2 electrons with OPPOSITE SPINS

62
Q

ion making 4s

A

empty 4s BEFORE 3d

63
Q

big jump in successive ionisation energy indicates…

A

what group is in
- eg big jump between 2 and 3 means group 2. more nergy required to remove 3 as was in an electron shell closer to nucleus so less shielding so stronger attraction

64
Q

what element has the largest first ionisation energy

A

helium
- first shell so no shielding
- more than hydrogen as has one more proton

65
Q

why big decrease in ionisation energy from Ne to Na

A
  • different periods
    -Na electron in a 3s shell further from nucleus,
    -more shielding
    -weaker attraction so more energy required
66
Q

decrease in IE from P to S

A
  • S has 4 electrons in 3p and, with the 4th starting to doubly fill the first 3p orbital
  • slight repulstion between the 2 negatively charged electrons so second electron is easier to remove
67
Q

melting and boilung point across period3

A

Na- Al : metallic bonding. Increase as smaller ion with a higher charge on ion, stronger attraction to outer shell e-, more energy required
Si: peaks here. giant covalent, lots of energy required to break many strong covalent bonds
P4, (slight increase to S8) ,Cl2 (simple molecular): london forces increase with more e-
Ar: LOWEST, monatomic, very weak london forces

68
Q

melting and boiling point of B and C

A
  • similar to S8
  • very high mp
    -C IS HHIGHEST
69
Q

HOW to find relative abundance of 2 isotopes (2)

A
  • measure intensity of each isotope
  • in a mass spectromoter
70
Q

why mass spec under vaccum

A

prevents collisions with air molecules that could deflect the ions

71
Q

atomic emmission spectra provide evidence for …

A

existence of quantum shells

72
Q

SUCCESSIVE ionisation energies provide evidence for …

A

the existence of quantum shells AND THE GROUP OF THE ELEMENT

73
Q

first ionisation energy for elements proves evidence for…

A

electron subshells

74
Q

why is there not a big difference between ist IE of those next to each other

A
  • electorns moved from SAME subshell
  • same distance from nucleus etc
75
Q
A

chem (16 decks)

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