Topic 1

Question 1

Atoms are made up of three types of subatomic particles…

Answer 1

Protons neutrons and electrons

Question 2

Mass number

Answer 2

Tells you the total number of protons and neutrons

Question 3

Atomic number

Answer 3

Tells you the number of protons in the nucleus

All atoms of the same element have the same number of protons

Question 4

Uncharged particles have…

Answer 4

The same number of protons as electrons

Question 5

Isotopes are…

Answer 5

The same element with different number of neutrons

Question 6

All isotopes have…

Answer 6

The same chemical properties

Question 7

Relative atomic mass define it

Answer 7

The relative atomic mass is the weighted mean mass of an atom of an element compared to 1/12 of the mass of an atom of carbon 12

It’s an average of all the relative isotopic masses

Question 8

Relative isotopic mass define it

Answer 8

Relative isotopic mass is the mass of an atom of an isotope compares with 1/12 of the mass of carbon 12

Question 9

Relative molecular mass Define it

Answer 9

The relative molecular mass is the average mass of a molecule or formula unit compared to 1/12 of the mass of carbon 12

Question 10

Isotopic abundance

Answer 10

Different isotopes of an element occur in different quantities or isotopic abundance’s

Question 11

How to work out the relative atomic mass of an element

Answer 11

Work out the average mass of all its atoms

Question 12

If given isotopic abundance as a percentage all you need to do is

Answer 12

Multiply its relative isotopic mass by its percentage relative isotopic abundance and add up the results
Divide by hundred

Question 13

How many electrons can the S Orbital hold

Answer 13

2

Question 14

How many electrons can the P orbital hold

Answer 14

6

Question 15

How many electrons can the D orbital hold

Answer 15

10

Question 16

How many electrons can the F orbital hold

Answer 16

14

Question 17

First ionisation energy

Answer 17

The energy needed to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ atoms

Question 18

Energy is… To ionise an atom so the reaction is…

Answer 18

Energy is put in to ionise an atom so the reaction is endothermic

Question 19

There are three factors that affect ionisation energy

Answer 19

Nuclear charge electron shells and shielding

Question 20

Nuclear charge

Answer 20

The more protons there are in a nucleus the more positively charged the nucleus is and the stronger the attraction for the electrons therefore increasing the first ionisation energy

Question 21

Electron shells

Answer 21

Attractions fall off very rapidly with distance.An electron in an electron shell close to the nucleus will be much more strongly attracted then one in a shell further away

Question 22

Shielding

Answer 22

As the number of electrons between the outer shell and the nucleus increases the outer electrons feel less attraction towards the nuclear charge. This lessening of the pull of the nucleus by inner shells of electrons is called shielding

Question 23

First ionisation energy

Answer 23

Decreases down the group

Question 24

Atomic radius… Across a period

Answer 24

Decreases
As the number of protons increases the positive charge of the nucleus increases. This means electrons are pulled closer to the nucleus making the atomic radius smaller

Question 25

Ionisation energy… Across the period

Answer 25

Increases
The number of protons is increasing which means a stronger nuclear attraction this makes it harder to remove the outer electrons

Question 26

The drop in ionisation energy between groups two and three are explained by…

Answer 26

SUB SHELL STRUCTURE

It requires more energy to remove an electron from a higher energy sub shell then a low energy sub shell

Question 27

The drop between group 5 and 6 can be explained by

Answer 27

ELECTRON REPULSION
Elements with Singly filled sub-shells are more stable than those with partially filled subshells so have higher first ionisation energy
In group 5 electron is being removed from a single occupied orbital.but in group 6 electron is being removed from orbital containing two electrons