Electronic Structure

Question 1

Energy levels

Answer 1

Quantum shells which the electrons in an atom are arranged

Question 2

Shells

Answer 2

Numbered from one- the lowest energy level, shells further from the nucleus have a higher energy level

Question 3

Shell 1 can hold ..,

Answer 3

2

Question 4

Shell 2 can hold

Answer 4

8

Question 5

Shell 3 can hold

Answer 5

18

Question 6

Shell 4 can hold

Answer 6

32

Question 7

S subshell

Answer 7

Contains one orbital. Hold max of 2 electrons. Spherical shapes

Question 8

P subshell

Answer 8

Contains 3 orbitals, therefore 6 electrons. Dumbbell shape. Right angles to eschtoehr

Question 9

D subshell

Answer 9

Contains 5 orbitals so 10 electrons.

Question 10

F subshell

Answer 10

Contains 7 sub shells so 14 electrons

Question 11

Orbitals

Answer 11

Bit if space that an electron moves in , orbitals within same subshell have same amount of energy. Orbital can be empty, contain one or two. If two, must have oppistite spins

Question 12

Aufbau principle

Answer 12

Electrons fill subshells in order of increasing energy

Question 13

Hunds rule

Answer 13

Within subshell, orbitals first occupier singularly

Question 14

Paulis exclusion principle

Answer 14

2 electrons in an orbital must have opposite spins

Question 15

Chromium and copper

Answer 15

Exceptions, they donate one of their 4s electrons to the 3d subshell, as they are more stable

Question 16

Ionisation enthalpy

Answer 16

Involves loss of an electron to form positive ion. Ions can be further ionised. Energy is needed for ionisation to happen, therefore endothermic reaction

Question 17

First ionisation energy

Answer 17

Energy needed to remove one electron from each atom in 1 mole of gaseous atoms to form 1 moles of gaseous ions with single positive charge

Question 18

Ionisation enthalpy depend on.,,

Answer 18

Nuclear charge
-more protons there are in nucelius, stronger attraction
Electron shell
-further away from nucleus, weaker forces of attraction are
Shielding
-weaker forces of attraction

Question 19

Down a groups, the ionisation energy…

Answer 19

Decreases, becomes easier to remove outer electrons

Question 20

Across a period, ionisation energy…

Answer 20

Increases as it becomes harder to remove outer electron

Question 21

Why do ionisation energies rise

Answer 21

Closer to shell
Less shielding
Positive ions
Other subshell

Question 22

Steps of mass spectrometry- vapourisation

Answer 22

Sample is turned into gas

Stage 1

Question 23

Steps of mass spec

Ionisation

Answer 23

Gas particles bombarded with high energy electrons to ionise them. Knocked off particles leaving positive ions

Stage 2

Question 24

Steps of mass spec

Acceleration

Answer 24

Positive ions are accelerated by electric field

Stage 3

Question 25

Steps of mass spec

Deflection

Answer 25

Positive ions path is altered with magnetic field, lighter ions have less momentum and are deflected more than heavier ion

Stage 4

Question 26

Steps of mass spec

Detection

Answer 26

Magnetic field strength slowly increases, chances m/z ratio of ions that can reach detector

Stage 5

Question 27

Evidence for electronic structure

Answer 27

Atomic emission spectra