Topic 1

Question 1

What is an isotope

Answer 1

Are atoms of the same element with different number of neutrons but same number of electrons

Question 2

Atomic Number

Answer 2

The Number of protons in an atoms Nucleus

Question 3

Mass Number

Answer 3

Total Number of protons + neutrons

Question 4

Relative Atomic Mass

Answer 4

Mean weighted mass of an atom of an element compared to 1/12 mass of one carbon-12 atom

Question 5

Relative Isotopic Mass

Answer 5

Mean weighted mass of an atom of one isotope compared to 1/12 mass of one atom of carbon-12

Question 6

Relative Formula Mass

Answer 6

Mean weighted mass of a molecule of a compound compared to 1/12 mass of one atom of carbon-12

Question 7

RAM equation

Answer 7

(mass x abundance)+(mass x abundance) / Total abundance

Question 8

Abundance equation

Answer 8

(? x Ar1) + [ (100-?) x Ar2 ] / 100

Question 9

Mass spectrometry

Answer 9

A device that’s used to measure the mass of positive ions and calculating molar mass

Question 10

First step to mass spectrometry

Answer 10

Ionisation : Sample enters the mass spectrometer in a gaseous form and are bombarded by a beam of high energy electrons which knock off electrons of the atom causing it to become a positive ion

Question 11

Second step to mass spectrometry

Answer 11

Acceleration: The positive ions then pass through electric plates which cause the ion to accelerate

Question 12

Third step of mass spectrometry

Answer 12

Deflection: A strong magnetic field causes the ions to defelct their path , ions with a higher mass are deflected less

Question 13

Fourth step to mass spectrometry

Answer 13

Detection: The on then gets detected by detector. The more ions hit a certain part of the detector it suggests that theres more of that type of isotope

Question 14

What are Quantam shells

Answer 14

Well defined levels where electrons can exist

Question 15

what are sub-shells

Answer 15

The path taken by electrons as they move around shell

Question 16

What are the 4 types of sub-shells and their maximum electron occupancy

Answer 16

S=2
P=6
D=10
F=12

Question 17

First ionisation energy

Answer 17

Energy change required to remove 1 mole of gaseous electrons from 1 mole of gaseous atoms to form 1 mole of gaseous +1 ions

Question 18

Second ionisation energy

Answer 18

Energy change required to remove 1 mole of electrons from 1 mole of gaseous +1 ions to from gaseous +2 ions

Question 19

How does Nucleur Charge effect IE

Answer 19

If there is higher proton muber there is a h=higher force of attraction between positively charged nucleus and negative charged last electron therefore higher amount of energy is required to remove the electron from the atom

Question 20

How does Atomic radii effect IE

Answer 20

If there’s higher radii between positive nucleus and negative last electron there is less force of attraction therefore less energy is required to remove the electron

Question 21

How does Electronic Repulsion Effect IE

Answer 21

When 2 electrons are in the same orbital they repel each other which means less energy is required to remove the electron

Question 22

How does Electron Shielding effect IE

Answer 22

If there is shielding between sub-shells there is repulsion between the sub-shells leading to less energy being required to remove the electron

Question 23

What is the trend of IE along period

Answer 23

The IE increases due to higher nucleur charge while the atomic raduis and shielding stays the same.
There is higher repulsion but nucleur charge has stronger effect on IE

Question 24

What is the trend of IE down a group

Answer 24

The IE decreases as there is higher atomic radii due to new sub-shell being added

Question 25

What is periodicity

Answer 25

Is the regular repeating pattern of physical and chemical properties with increasing atomic number along the period

Question 26

What happens to atomic raduis as go along the period

Answer 26

The raduis decreases

Question 27

Why is this

Answer 27

There is a higher nucleur charge which means there is stronger force of attraction between positive nucleus and negative electrons. This force of attraction brings the nucleus and shells closer thus reducing distance

Question 28

Exceptions in trends of IE along period in period 2

Answer 28

1. Boron:The IE decreases as we are removing an electron from a p-subshell which has higher atomic radii and shielding
2. Oxygen: The IE decreases as in the p-subshell we are removing the electron from an orbital where 2 electrons are held together which causes repulsion

Question 29

Exceptions for IE for a long period 3

Answer 29

1. Alluminuim: we are removing electrons from p-subshell which has higher shielding and radii
2. Sulphur: In the p-subshell there are 2 electrons in the same orbital which causes repulsion