atomic structure Flashcards

1
Q

write an example of an ionisation equation

A

k(g)—>k+(g)+e-

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2
Q

why is the outer most electron the highest energy electron

A

it is furthest from the nucleus

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3
Q

why does 4s fill up before 3d

A

4s has lower energy
electrons fill up in lower energy order

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4
Q

what is the atomic number

A

number of protons

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5
Q

what is the atomic mass

A

number of neutrons + protons

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6
Q

what is a positive ion

A

cation
has lost electrons and has more protons that electrons

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7
Q

what is a negative ion

A

anion
has gained electrons and has more electrons that protons

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8
Q

what is a isotope

A

atoms of the element which have the same number of protons but different number of neutrons

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9
Q

what factors affect ionisation energy

A

-nuclear charge(number of protons in the nucleus)-more protons, stronger electrostatic attraction between nucleus and outermost electron so there is more energy needed to remove the outer most electron.
-shielding-electrons on a shell further away from the nucleus means there is more shielding, weaker electrostatic attraction so less energy needed to remove outermost electron.

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10
Q

what does the mass spectrometer measure

A

-relative abundance
-mass/charge ratio (m/z)

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11
Q

what do jumps in ionisation energy mean

A

jumps in values of consecutive ionisation energy means that the electron with a higher ionisation energy is being removed from a shell closer to the nucleus so it has a stronger electrostatic attraction and there is a big difference in its ionisation energy compared to the one before.

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12
Q

what are the units of ionisation energy

A

kj/mol

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13
Q

trends in first IE across a period

A

atomic radius decreases - higher proton number so higher electrostatic attraction between nucleus and outermost electron
-higher first ionisation energy

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14
Q

time of flight equation

A

t=d/v
t=time (sec)
v=velocity of ion(m/s)
d= distance or length of flight tube (m)

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15
Q

shape of s and p orbital

A

s= sphere
p=dumbbell shape with a cross

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16
Q

results of a TOF mass spectrometer

A

if a single element is injected into a mass spectrometer it will be sperated into its isotopes
each peak is an isotope and height of the peak is the relative abundance of each isotope

17
Q

number of electrons in each shell

A

1-2
2-8
3-18
4-32

18
Q

kinetic energy equation

A

KE=1/2mv^2
kinetic energy is the energy that objects possess due to their motion
m=mass(kg)
v=velocity(m/s)
KE=kinetic energy(J)

19
Q

isotopes have the same chemical properties because..

A

they have the same electronic configuration

20
Q

how to calculate Ar

A

sum of (isotope abundance x isotope mass number)/sum of (isotope abundance)

21
Q

how many orbitals does each subshell have

A

S-1
P-3
D-5
F-7
each orbital holds 2 electrons

22
Q

exceptions of ‘normal’ electronic configuration

A

chromium and copper

23
Q

electrospray

A

sample is dissolved in volatile solvent and injected through a fine hypodermic needle to give a fine mist
tip of the needle is attatched to a positive terminal
particles gain a proton
x(g) + H+——->xH+(g)
used on higher molecular mass subtances

24
Q

electron impact

A

sample analysed is vapourised and high energy electrons are fired at it which come from an ‘electron gun’ - hot wire filament
knocks off an electron to form a 1+ ion
x(g)—>x+(g)+e-
used on substances with low formula mass

25
Q

draw and label the stages of a mass spectrometer

A

1-ionisation-2 methods but in both the sample particles get a positive charge
2-acceleration-postive ions are attracted towards the negative plate and accelerate towards it. Once accelerates all ions have the same kinetic energy
3-ion drift-ions drift towards the detector the speed they reach teh detector depends on their size
smaller ions reach faster and larger ions take longer
4-detector-each ion gains an electron then a current is generated which is proportional to the abundance of ions
5-analysis-signal from detector is passed to computer which generates a mass spectrum

26
Q

deviations in ionisation energy

A

3rd element-
The first e- removed from (element before) is from a 2s sub level
The first e- removed from(element) is from a 2p sub level
2s sub level is lower in energy than 2p so less energy needed to remove e- from (element)

6th element-
The first e- removed from(element before) is from a 2p sub level and is unpaired
The first e- removed from (element) is from a 2p sublevel and is paired
(element) has lower ionisation energy due electron paired repulsion so needs less energy to remove the electron

27
Q

describe the bohr model

A

-protons and neutrons inside the nucleus and can be called nucleons
-electrons orbit the nucleus in shells or energy levels

28
Q

describe rutherfords test

A

he fired He2+ ions at a sheet of gold foil
when the ions arrived at point p he concluded that most of the atom is empty space
some ions were deflected to point q and so he concluded that an atom must have a small positive nucleus

29
Q

definition: ionisation energy

A

the amount of energy needed to remove a mole of electrons from a mole of atoms in a gaseous state

30
Q

attraction rules to compare the size and IE’s of different elements

A

-write electronic configuration
-write number of protons
-compare shielding
if its the same compare number of protons
-compare attraction between nucleus and outer electron