1.25 electronic configuration

Question 1

what are the general trends regarding ionisation energy?

Answer 1

increases across a period, decreases down a group

Question 2

what causes anomalies to occur in ionisation energy values?

Answer 2

the more stable the electronic configuration, the higher the ionisation energy. stability can be associated with a filled or half-filled subshell

Question 3

which part of the periodic table makes up the f block?

Answer 3

lanthanides and actinides

Question 4

which part of the periodic table makes up the d block?

Answer 4

the transition metals

Question 5

which groups make up the p block?

Answer 5

groups 3-8 (except helium)

Question 6

which groups make up the s block?

Answer 6

groups 1,2, and helium

Question 7

which two transition metals do not follow the Aufbau principle and why?

Answer 7

copper - due to the extra stability gained from a full d subshell
chromium - due to the extra stability gained from a half-full d subshell

Question 8

which subshell is emptied first - 4s or 3d?

Answer 8

4s

Question 9

which subshell is filled first - 4s or 3d?

Answer 9

4s

Question 10

what happens in orbitals when ions are formed?

Answer 10

electrons are added to/removed from the highest energy orbital available

Question 11

how can larger electronic configurations be simplified?

Answer 11

by using the nearest noble gas e.g. [Ar]

Question 12

which type of notation uses boxes to represent the energy level and letters to represent the subshell?

Answer 12

orbital box notation

Question 13

which type of notation uses numbers to represent the energy level and letters to represent the subshell?

Answer 13

spectroscopic

Question 14

what does Hund’s rule state?

Answer 14

that when degenerate orbitals are available, electrons fill each singly keeping their spins parallel before spin pairing occurs

Question 15

what is the order of filling of electron orbitals?

Answer 15

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

Question 16

what does the Aufbau principle state?

Answer 16

that electrons fill orbitals in order of increasing energy

Question 17

what can the Pauli exclusion principle be used to explain?

Answer 17

the fact that no orbital can hold more than two electrons and those two electrons must have opposite spins

Question 18

what does the Pauli exclusion principle state?

Answer 18

that no two electrons in the one atom can have the same set of four quantum numbers