Electron Configuration

Question 1

Excited state

Answer 1

When an electron absorbs energy/ increase to a higher subshell or energy level

Question 2

Grounded state/relaps

Answer 2

Lowest possible subshell, and energy level an electron can occupy. Observed when a photon on electromagnetic radiation is released in wavelength of light

Question 3

Nucleus of atom

Answer 3

Small dense protons and neutrons

Question 4

Electrin cloud

Answer 4

Region of space where there is probability of electron being found.

Question 5

Electron shell

Answer 5

An energy level within an atom that may be occupied by a number of fixed electrons

Question 6

Subshells

Answer 6

Subdivision of electron shells containing fixed number of orbital at the same energy level

Question 7

Orbital

Answer 7

A region of space containing up to 2 electrons

Question 8

Subshell names, and Max electrons

Answer 8

S= 2 in every shell- sphere 
P= 6 oriented in 3 dif positions 
D= 10
F= 14

Question 9

Subshell notation

Answer 9

1,S,2 2,S,2 2,P,6 3,S,2

1 shell, s sub shell, 2 electrons

Question 10

Abrivated notation

Answer 10

Use lightest noble gas, then use normal notation

(Ar) 4,S,2

Question 11

Pauli exclusion principle

Answer 11

Maximum 2 electrons in orbital

If 2 full, opposite spin

Question 12

Aufbau principle

Answer 12

Subshells fill from lowest energy to highest

This means overlap, 4S Filled before 3D

Question 13

Hunds rule

Answer 13

Every orbital must be filled half in each subshell before fully filled

Question 14

Exceptions to hunds rule

Answer 14

Copper 4,S,1 3,D,10

Chromium 4,S,1 3,D,5

Question 15

Ions forming

Answer 15

Outermost shell electrons are lost because occupy highest energy

4,s electron lost before 3,d

Question 16

Trends in electronegativty

Answer 16

High when atomic radius is low/ increase room in valence shell for shared electrons

Core charge is high because nuclear charge high electron shielding low

Move down column-

Core charge no change increase electron shielding

Question 17

Electronegativty

Answer 17

Strength which atom of an element attract electron when they combined with another electron

In covalent bonds electrons more likely to be closer to atom with greater electroneg

Question 18

Core charge

Answer 18

Effective nuclear charge is a measure of net attractive force felt by valence shell electrons towards nuclei

Down column constant core energy

Across group core energy increase

Question 19

Atomic radius across a period

Answer 19

Decrease

N/o of occupied energy levels remain contst

Core energy increase resulting in valence electron being more strongly attracted to nucleus

Question 20

Atomic radius down a group

Answer 20

Increase

N/o of energy levels occupied by electrons increases

Core energy remains constant

Question 21

Atomic radius

Answer 21

Half the distance between 2 nuclei of a molecule

Assuming a singular covalent bind exists between 2 identical atoms

Question 22

Ionisation

Answer 22

Energy required to remove an electron from each mole of gaseous atom

Produces gaseous ion charge of 1 plus

Na=Na+ + e-

Question 23

Trends in ionisation energy

Answer 23

Greater pull between electrons and nucleus are harder to pull electrons away Need greater amounts of ionisation energy

Repulsion of electrons= easier to pull away

Core charge= if higher require more ionisation energy

Atomic radius= if greater needs less ionisation energy because further from nucleus

Question 24

Ionisation energy across a period

Answer 24

Increase- atomic radius decreases/ core charge increase

Question 25

Ionisation energy down a group

Answer 25

Decreased- atomic radius increase/ core energy stays the same

Question 26

Successive ionisation

Answer 26

Cation becomes more positive, but becomes more difficult to pull electrons away- requires more energy

2nd ionisation energy always greater then 1st

Question 27

Relative atomic mass

Answer 27

Average mass of all the isotope of an element weighted for their relative abundance