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Chemistry A Level > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is an atomic number

A

the number of protons in the nucleus of that atom

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2
Q

What is the relative atomic mass

A

the average mass of an atom relative to 1/12th the mass of carbon 12

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3
Q

what is relative molecular mass

A

the average mass of a molecule relative to 1/12th the mass of carbon 12

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4
Q

what is relative formula mass

A

the average mass of a formula relative to 1/12th the mass of carbon 12

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5
Q

what is the mass of an electron

A

1/1840

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6
Q

what is relative isotopic mass

A

this is the mass of an isotope relative to
1/12th of the mass of a carbon12 atom

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7
Q

how do you measure the abundance of different isotopes

A

mass spectrometry

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8
Q

what is relative atomic mass

A

this is the weighted average mass of an atom divided by 1/12th the mass of a carbon-12 atom

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9
Q

what are the 5 main stages of the mass spectrometer

A

-vaporisation
-ionisation
-acceleration
-deflection
-detection

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10
Q

how to identify a compound using its mass spectrum

A

-find out the molecular ion peak
-divide this by 12 to see how many carbons there are and the remainder is the amount of hydrogens left

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11
Q

WHAT IS THE MOLECULAR/PARENT ION PEAK

A

this is the last peak in the mass spectrum

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12
Q

what are the three uses of mass spectrometry

A

=to check for drugs in urine
-carbon-14 dating
-determine relative atomic mass of an element

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13
Q

what is the first ionsation energy

A

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

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14
Q

what is second ionisation energy

A

the energy needed to remove one electron from each ion in one mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions

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15
Q

orbitals

A

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

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16
Q

sub shells

A

a group of electrons in the same type of orbital within a shell

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17
Q

what are the 4 types of subshells

A

s,p,d,f

18
Q

write these down in order of biggest to smallest: quantum shells, orbitals, subshells,electrons

A

quantum shells, subshells, orbitals, electrons

19
Q

what happens to the first ionisation energy in a period

A

the energy increases as the number of protons (nuclear charge) in the nucleus increase so the attraction will increase. the size of the atom will decrease, as there at more protons to be attracted to and shielding will stay the same

20
Q

what happens to the first ionisation energy as you go down a group

A

the energy decreases as there is more electron shielding which decreases the attraction between protons and electrons and also the size increases

21
Q

what is electron shielding

A

this is the number of electrons inbetween the nucleus and the outer most electron

22
Q

what is the formula to work out how many electrons can fit in a shell

A

2nsquared

23
Q

what is the probability that there is an electron in an orbital

A

90%

24
Q

how are s-orbitals shaped

A

like a sphere

25
Q

how many orbitals does s have

A

1

26
Q

how any orbitals does p have

A

3

27
Q

how many orbitals does d have

A

5

28
Q

how many orbitals does f have

A

7

29
Q

what is the full electron structure of carbon

A

1s2 2s2 2p2

30
Q

how is a p orbital shaped

A

like a dumbell

31
Q

how do you draw the short hand notations of subshells

A

write the symbol of the last noble gas in brackets and add whatever is left

32
Q

what happens in the ionisation stage of mass spectrometry

A

-we place the sample of all the isotopes of the element we are interested in and place it into the sample chamber
-all these atoms are ionised into positive ions

33
Q

what happens in the acceleration stage of mass spectrometry

A

-these positive ions will then be attracted to a negatively charged plate
-this will cause them to accelerate
-all of them will accelerate at the same speed

34
Q

what happens in the deflection stage of mass spectrometry

A

these ions will pass through a magnetic field and are deflected according to their mass and charge, the light ones will travel quicker

35
Q

what happens in the detection stage of mass spectrometry

A

-ion detector at the end of the tube reponds to ions of a particular mass/charge ratio and a mass spectrum is formed. the abundance is recorded as a peak

36
Q

what are the 3 things that affect ionisation energy

A

-size
-nuclear charge
-shielding

37
Q

what are the two anomalies in the electronic configuration

A

chromium and copper

38
Q

what is periodicity

A

this is the repeating trends in the physical and chemical properties of the elements across each period

39
Q

why does the first ionisation energy drop in the between the group 2 and 3

A

this is because group 3 elements have their outer electron in their p orbital but group 2 have theirs in their s orbital. the p orbital has a higher energy than an s orbital so it is further away from the nucleus. this means it requires less energy to remove.

40
Q

why does the first ionisation energy drop in between the group 5 and 6

A

this is because the electron from group 6 is getting removed from a full p shell orbital. this means that there is electron-electron repulsion which then makes it easier to remove an electron

Chemistry A Level (5 decks)

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