1.2. electronic shells

Question 1

what was the theory about electronic shells

Answer 1

electrons have fixed shell energy shells. each shell is given a number called the principal quantum number. the further the shell is to the nucleus the higher the principal quantum number

Question 2

what do experiments show

Answer 2

they show that bot all the elctrons in a shell have exactly the same energy. the atomic model shows that shells are split u into sub-shells. different shells have different numbers of sub shells which all have different energy levels.

Question 3

name of shells

Answer 3

s, d, p, f sub shell

Question 4

sub shells

Answer 4

sub shells have different number of orbital which can hold up to 2 electrons

Question 5

s

Answer 5

number of orbital 1

2 electrons

Question 6

p

Answer 6

number of orbital 3

6 electrons

Question 7

d

Answer 7

vnumber of orbital 5

10 electrons

Question 8

f

Answer 8

number of orbital 7

14 electrons

Question 9

sub shell notation

Answer 9

1s2 2s2 2p6

Question 10

arrows in a box

Answer 10

each box represents one orbital each arrow represents one electron

Question 11

energy level diagram

Answer 11

shows the energy of one of the electrons in different orbits

Question 12

working out electron con fig

Answer 12

1. electrons fill up the lowest sub shells first
2. electrons fill orbital in a sub shell singly before they start sharing
3. config of ions from the s and p blocks of the periodic table just remove the electrons to or from the highest energy occupied sub-shell

Question 13

noble gases

Answer 13

you square them e.g (ar)42^2

Question 14

ions

Answer 14

they need to be ions or they won be able to be accelerated or detected by the mass spectrum’s ion detector

Question 15

transition metal configuration

Answer 15

chromium and coppy donate one of the 4s electrons to the 3d sub shell. it is because they prefer a more stable full or half full d sub shell

Question 16

electron config for chromium

Answer 16

1s2 2s2 2p6 3p2 3p6 3d5 4s1

Question 17

electron config for copper

Answer 17

1s2 2s2 2p6 3p2 3p6 3d10 4s1

Question 18

electronic structure and chemical properties

Answer 18

the numbers of outer shell electrons decides the chemical properties of the element. you can use the periodic table to help you to work theme out

Question 19

the s block elements

Answer 19

group 1 and 2

Question 20

the s block elements qualities

Answer 20

have 1 or 2 outer shell electron these are easily lost to form positive ions with an inert gas config

Na 1s 2 2s 2 2p 6 3s 1 —- 1s 2 2s 2 2p 6

this is the same configuation as neon

Question 21

electronic structure in the p block

Answer 21

group 5 6 7

Question 22

electronic structure in the p block qualities

Answer 22

these gain 1 2 3 electrons to form negative ions
group 4 to group 7 can share electrons to form covalent bonds - covalent bonds can only occur between non metals mostly anyways

Question 23

electronic structure in group 0

Answer 23

group 0 has completely filleds and p sub-shells and dont gain or lose electrons. their full sub shells make them inert

Question 24

ionisation meaning

Answer 24

when electrons have been removed from an atom or molecule, it has been ionised.