2.2.2 Sub-shells and energy levels

Question 1

how are orbitals organised in a shell?

Answer 1

within each shell, orbitals of the same type are grouped together to form a sub-shell

Question 2

what does a sub shell contain?

Answer 2

orbitals of only one type

Question 3

how do electrons occupy subshells

Answer 3

in order of increasing energy levels

Question 4

what is the Aufbau Principle?

Answer 4

the rules to figure out electronic configuration

Question 5

what are the rules of the Aufbau Principle?

Answer 5

-electrons are added one at a time
-the lowest energy level is filled first
-each energy level must be full before the next begins to fill

Question 6

how are sub-shells filled?

Answer 6

each orbital is filled singly, before pairing starts (sitting on a bus rule)

Question 7

which orbital is a lower energy level, 4s or 3d

Answer 7

4s orbital is a lower energy level than 3d orbital

Question 8

which sub-shell fills first?

Answer 8

the orbital with the lowest energy level (closest to the nucleus)

Question 9

what is electron configuration?

Answer 9

the arrangements of electrons in an atom or ion

Question 10

how can you figure out electron configuration?

Answer 10

using the Aufbau Principle

Question 11

what is the formula for electron configuration?

Answer 11

nx^y

Question 12

what does the n stand for in nx^y?

Answer 12

shell number

Question 13

what does the x stand for in nx^y?

Answer 13

type of orbital

Question 14

what does the y stand for in nx^y?

Answer 14

number of electrons in the orbitals, making up sub-shells

Question 15

which electrons are lost/gained first if an atom is ionised to become a positive ion?

Answer 15

the electrons found in the highest energy levels are lost first

Question 16

how will the electron configuration change, if the atom becomes a positive ion?

Answer 16

it will show fewer electrons at the highest energy levels

Question 17

which electrons are lost/gained first if an atom is ionised to become a negative ion?

Answer 17

the electrons gained will continue to fill the sub-shells as the other electrons did

Question 18

what is the electron configuration of nitrogen?

Answer 18

1s^2 ,2s^2 ,2p^3

Question 19

what is the shorthand electron configuration of chlorine?

Answer 19

[Ne] 3s^2, 3p^5

Question 20

how to do shorthand electron configuration?

Answer 20

go to noble gas previously in the periodic table, place in square brackets and do regular configuration for the remainder

Question 21

exam question: how many full orbitals are in an atom of sulfur? (using 1s^2, 2s^2, 2p^6, 3s^2, 3p^4)

Answer 21

7

Question 22

instead of “it formed a full outer shell”, what should you say?

Answer 22

it formed a negative/positive ion, depending