AQA A LEVEL CHEMISTRY PAPER 1 Study Guide Rated A+
TOF steps
Electron impact
electrospray ionization
Acceleration (TOF)
Ion drift (TOF)
Detection (TOF)
Analysis (TOF)
Electron spin
Orbitals
Hund's Rule
Electron configuration
exceptions to electron configuration
Why does ionization ener...
Ans: Sample vaporised and electron gun fires high energy electrons at it which knock
off 1 electron from each particle, making them 1+ ions
NB- can knock off more than one e or break molecular ion
3). Electrospray ionization
Ans: Sample dissolved in volatile solvent then injected through needle to give fine mist
which is attached to positive end of high voltage power supply, particles gain proton
NB- Mr of substance is actually one less than shown due to extra H+
4). Acceleration (tof)
Ans: positive ions accelerated using electric field so they all have the same kinetic
energy
5). Ion drift (tof)
Ans: particles with small mass have larger velocity do ions start to separate with
lightest ions reaching detector first
6). Detection (tof)
Ans: positive ions hit negatively charged plate and gain an electron which forms a
current, the larger the current the higher the abundance
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, 7). Analysis (tof)
Ans: -computer uses data to produce mass spectrum which shows mass m / charge z
ratio
-mr or ar is furthest right peak (small peaks larger than mr are due to isotopes)
-may be large peaks at lower mr due to fragmentation
8). Electron spin
Ans: Property of electron (CW or ACW)
Represented by up and down arrows
9). Orbitals
Ans: Defined regions of space around nucleus where electrons most likely to be found,
each orbital holds 2 electrons
10). Hund's rule
Ans: Electrons prefer to occupy orbitals on their own and only pair up when no empty
or bait ask of same energy are available
11). Electron configuration
Ans: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10
12). Exceptions to electron configuration
Ans: chromium and copper, only take one electron in 4s orbital
13). Why does ionization energy decrease down a group?
Ans: Atoms get bigger so electrons further away from nucleus, greater shielding
14). Why does ionization energy increase across a period?
Ans: Atoms get smaller, nuclear charge increases, similar shielding
15). Dip in ionisation energy groups 2-3
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