Sub-shells

Question 1

what is the periodic table

Answer 1

a list of all known elements, with the first 92 occuring naturally and the remaining being man-made

Question 2

how do electrons fill their shells

Answer 2

the fill the shells closest to the nucleus first as it takes less energy to do so and to travel to these shells

Question 3

what are sub-shells

Answer 3

shells within each electron shell, identified by the letter s,p,d,f

Question 4

shell 1 subshells

Answer 4

1 only, s

Question 5

shell 2 subshells

Answer 5

2, s, p

Question 6

shell 3 subshells

Answer 6

3, s,p,d

Question 7

shell 4 subshells

Answer 7

4, s,p,d,f

Question 8

what are electron orbitals

Answer 8

the three dimensional space around the nucleus which electrons may occupy

Question 9

how many obitals does subshell s have

Answer 9

1, 2 electrons

Question 10

how many obitals does subshell p have

Answer 10

3 orbitals, 6 electrons

Question 11

how many obitals does subshell d have

Answer 11

5 orbitals, 10 electrons

Question 12

how many obitals does subshell f have

Answer 12

7 orbitals, 14 electrons

Question 13

how many electrons can an orbital hold

Answer 13

2

Question 14

energy levels of subshells/ in which order they fill up

Answer 14

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

Question 15

what is condenseed electron configuration/ noble gas notation

Answer 15

when the symbol of the noble gas in the period before the element is written in square brackets, the extra electrons are written as normal

Question 16

why do we use condensed notation

Answer 16

simpler, less time consuming and emphasises the valence shell electrons which are the most important

Question 17

what are the exceptions to the schroginer model

Answer 17

chromium (Cr) and copper (Cu)

Question 18

electron configuration of chromium

Answer 18

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

Question 19

electron configuration of copper

Answer 19

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

Question 20

why is chromiums electron configuration this way

Answer 20

there is little energy difference between 3d and 4s subshells and certain stability associated with elements have orbitals half filled, so an electron from the s subshell is borrowed to make the 3d subshell half filled

Question 21

why is coppers electron configuration this way

Answer 21

there is little energy difference between 3d and 4s subshells so an electron from the s subshell is borrowed to make the 3d subshell fully filled

Question 22

what do the subshell blocks indicate

Answer 22

they share the subshell of its highest energy electrons

Question 23

s block

Answer 23

alkaline metals and alkaline earth metals

Question 24

p block

Answer 24

halogens and noble gases

Question 25

d block

Answer 25

transition metals

Question 26

f block

Answer 26

lanthanides and actinides