Atomic Structure and the Periodic Table Ch2

Question 1

Sub-Atomic Particle

Name + Relative Mass + Charge

Answer 1

Proton ~ 1 ~+1
Neutron ~ 1 ~ 0
Electron ~ 1/1840 ~ -1

Question 2

Definition:

Isotopes

Answer 2

Atoms of the same element with the same atomic number but a different mass number

Question 3

Mass Spectrometry

5 steps

Answer 3

1. Vapourisation
2. Ionisation
3. Acceleration
4. Deflection
5. Detection

Question 4

What is it?

Vaporisations

Answer 4

Samples turning into gases

By heating

Question 5

What is it ?

Ionisation

Answer 5

Vapour samples bombarded with high energy elections from an election gun

‘knocks off’ an elections from atom

Positive charge

Question 6

What is it ?

Acceleration

Answer 6

An electic field is used to accelerate the ions

positive samples attracted to the negative electric field

Question 7

What is it ?

Deflection

Answer 7

Positive ions deflected by an uniform magnetic field

deflection
mass:charge
velocity of the ion
strenght of magnetic fiel

Question 8

What is it?

Detection

Answer 8

Ions hit plate, convert into electrical current - convert into peak on the mass spectrum

Question 9

Formula

Relative Isotopic Mass

Answer 9

(Abundance x m/z) total / total m/z value

Question 10

Mass spectrometry

Diatomic Molecules

Answer 10

The whole molecule could be charged positively OR molecule spilts and one becomes postive and the other becomes a radical

Create multiple peaks

Question 11

Mass spectrometry

Poyatomic Molecule

Answer 11

The high energy elctions may break the bonds, allowing posistively charged fractions to pass.

Contains carbon theres a ‘M+1’ peak due to presence of carbon- 13

Question 12

Definition

Orbital

Answer 12

A region within an atom that can hold up to 2 electrons with opposite spins

Question 13

Shape

s - Orbital

Answer 13

Spherical in shape
center is the nucleus
Down the group, orbital increase in size and more energy

Question 14

Shape

p - Orbital

Answer 14

Dumbell shaped

Px + Py + Pz (dofferent axis)

Question 15

’s’+ ‘p’+’d’ block ions

Which electrosn they lose first?

Answer 15

When the atoms become ions, they lose the highest principal number first

Question 16

Definition

First Ionisation Energy

Answer 16

The energy required to remove one electron in each atom, in a mole of atoms, in the gaseous state

Enn dothermic Process

Question 17

Definition

Successive ionisation energies

Answer 17

energy required to remove each electron, one by one until none are left

Question 18

Provides evidence for?

Successive ionisation energies

Answer 18

1. Group - number of lectron removed before first big jump
2. Period - number of shelss in an atom = (n+1) of the big jumps

Question 19

Factors Affecting

Ionisation energy

Answer 19

1. size of nuclear charge
2. Orbital/subshell from which electron being removed
3. Shielding

1 increase IE increase
2 further IE decrease
3 repel IE decrease

Question 20

Trends

Ionisation Energy

Down a group

Answer 20

Nuclear charge Increase
Electron being removed further from nucleus - decrease force of attraction
increase Shielding

IE decreases

Question 21

Trends

Ionisation Energy

Across a period

Answer 21

Nuclear charge Increase
Increase of electrons = more repulsion
Shielding stays the same

IE generally increases

Question 22

Graph

First ionisation energies

Boron and Beryllium

Answer 22

Outer electeron in B in 2P, has more energy
easier to remove than Be out electon in 2s

Question 23

Graph

First ionisation energies

Nitrogen and oxygen

Answer 23

Nitrogen singly oxccupied
oxygen in a pair (force of repulsion)

Less energy required

Question 24

Definition

Periodicity

Answer 24

Repeating pattern of physical and chemical properites across each period

Question 25

Trends

Atomic Radius

Answer 25

Increase down a group
decrease across a period