atomic structure (physical)

Question 1

what is atomic number

Answer 1

number of protons

Question 2

what is mass number

Answer 2

total protons and neutrons

Question 3

what is an isotope

Answer 3

the same element with the same protons and electrons but with a different amount of neutrons

Question 4

what are the 3 types of hydrogen

Answer 4

hydrogen
deuterium
tritium

Question 5

what is mass spectrometer

Answer 5

francis aston found 2 isotopes of neon with mass numbers of 20 and 22.
Any substance that can be vapourised without decomposing can be analysed in the same way by mass spectrometry

Question 6

how does the time of flight spectrometer work

Answer 6

accelerates an ionised sample and calculates mass per charge based on how long each object is in flight for

Question 7

what are the 2 types of ionisation

Answer 7

electrospray and electron impact

Question 8

what is electrospray

Answer 8

sample gains a H+ ion (mass increases by 1)
uses high voltage

Question 9

what is electron impact

Answer 9

sample uses an electron (mass stays the same)
fires e- at sample

Question 10

what is fragmentation

Answer 10

when a molecule passes through the mass spectrometer, it is broken into fragments which form ions and are detected

Question 11

what is quantum theory

Answer 11

electrons are only stable when they have a particular multiple of energy (corresponds to the shells)
Shells are numbered with a principle quantum number (corresponds to period level)

Question 12

what is an orbital

Answer 12

region where you are most likely to find an electron around a nucleus.
Energy levels of principle quantum numbers are subdivided into orbitals.
There are 4 different orbitals (subshells)

Question 13

how many orbitals does S have

Answer 13

1

Question 14

how many orbitals does P have

Answer 14

3

Question 15

How many orbitals does D have

Answer 15

5

Question 16

how do orbitals fill up

Answer 16

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p

Question 17

what is pauli exclusion principle

Answer 17

any individual orbital can hold a maximum of 2 electrons.
electrons can repel eachother so each electron spins in the opposite direction to the other when in the orbital- reduces the effect of repulsion.
first electron is clockwise

Question 18

what is Hunds rule

Answer 18

electrons will occupy orbitals singly where possible.
when the same orbitals are all full, electrons will spin pair

Question 19

how does chromium fill

Answer 19

1 electron goes to 4s and the other goes to 3d because 5 single electrons in each orbital is more stable

Question 20

how does copper fill

Answer 20

1 electron in 4s allowing 10 to go into d orbitals and giving a stable pair in each d orbital

Question 21

what happens when a transition metal loses electrons in terms of orbitals

Answer 21

they lose 4s electrons first

Question 22

what is the general equation for first ionisation

Answer 22

X(g) -> X+(g) + e-

Question 23

what is the general equation for 2nd ionisation

Answer 23

X+(g) -> X2+(g) + e-

Question 24

general equation for 3rd ionisation

Answer 24

X2+(g) -> X3+(g) +e-

Question 25

why do noble gases have a higher first ionisation energy

Answer 25

more stable and require more energy

Question 26

why do group 1 have lower first ionisation energy

Answer 26

they only need to lose 1 electron to gain a full shell

Question 27

Why does group 3 have a slightly higher first ionisation energy than group 1 but still low

Answer 27

require less energy to lose outermost electron in p subshell. p subshell is further from the nucleus and slightly shielded by s electrons

Question 28

whats the general trend for 1st IE across a period

Answer 28

more protons/ nuclear charge increases. outer electrons filling same shell so the same amount of shielding greater force of attraction between nucleus and outer electrons

Question 29

whats the general trends for 1st IE down a group

Answer 29

increases in shielding increases in number of protons increases in distance of the outer electrons less attraction between outer electrons and the nucleus