Periodicity (7)

Question 1

What happens to the atomic number in the periodic table?

Answer 1

It increases as you go left to right

Question 2

Groups

Answer 2

Vertical columns of the periodic table, tells you how many electrons on your outermost shell

Question 3

Periods

Answer 3

Horizontal columns that tell you how many shells the element has

Question 4

Periodicity

Answer 4

Trends in the periodic table such as electron config, ionisation energy, structure and melting point

Question 5

S Block

Answer 5

Group 1+2

Question 6

P block

Answer 6

Groups 3-8

Question 7

D Block

Answer 7

Transition metals

Question 8

F Block

Answer 8

Bottom two rows

Question 9

Ionisation Energy

Answer 9

The energy required for an atom to lose an electron in order to become a positive ion

Question 10

First Ionisation Energy

Answer 10

The energy required to release 1 electron from one mole of gaseous atoms of an element to form 1 mole of gaseous cations.

Question 11

How do electrons sit on shells?

Answer 11

The electrons sit on shells as they are attracted to the nucleus, but the higher the shell number, the further away the electron will be from the nucleus so the weaker the bond will be.

Question 12

Factors Affecting Ionisation Energy

Answer 12

Size of atomic radius, Nuclear charge, Electron shielding

Question 13

Atomic Radius

Answer 13

The bigger the radius of the atom, the bigger the distance between the outermost electron and the nucleus which will weaken the bond so the electron can be lost easier.

Question 14

Nuclear Charge

Answer 14

The more protons that exist in the nucleus, the greater the attraction to the electron as protons are positive and attract the negative electrons

Question 15

Electron Shielding

Answer 15

The more shells that are between the nucleus and outermost electron, the more electron shielding there is and the more the innermost shells will repel the outermost electron so the bond between the nucleus and electron will be weaker.

Question 16

How many ionisation energies does an atom have?

Answer 16

It will have as many ionisation energies as there are electrons on its outer shell e.g Helium will have 2.

Question 17

Second Ionisation Energy

Answer 17

The energy needed to remove an electron from 1 mole of gaseous +1 ions of an element to form 1 mole of gaseous 2+ ions

Question 18

Is the second ionisation energy greater than the first?

Answer 18

Yes it is because in helium for example, after the first electron is removed, the remaining electron on the outer shell is pulled closer towards the nucleus which means more energy is required to remove this electron.

Question 19

How can you make predictions about an element?

Answer 19

Look at the table of ionisation energies and see how the energy is increasing. If it’s a steady slow increase, it means the electrons being removed are from the same shell. If there is a sharp jump, this indicates it’s moved to a lower shell.

Question 20

How does the ionisation energy trend in a period?

Answer 20

There is an increase of ionisation energies in a period, and a peak will be a noble gas as they are really hard to take electrons from. A sharp decrease in ionisation energy means you’ve started the next period.

Question 21

How does the ionisation energy trend in a group?

Answer 21

As you go down a group, the ionisation energy will decrease.

Question 22

Why is the trend like that in a period?

Answer 22

It will increase because the nuclear charge is increasing as there are more protons. The atomic radii also decrease which makes the nucleus have a stronger bond with the electron. Electron shielding is the same as they have the same number of shells

Question 23

Why is the trend like that in a group?

Answer 23

It decreases within a group because the atomic radii increase, the nuclear charge and the electron shielding all increase because the atoms are getting bigger.

Question 24

Why does the energy level within the periods sometimes fall?

Answer 24

There are some drops when moving on to fill the next orbital e.g from 2s2 to 2p6

Question 25

Comparing beryllium and boron

Answer 25

Boron follows beryllium and is the start of the p 2p orbital so it has one electron in that orbital which is easier to remove than the two close electrons in beryllium

Question 26

Comparing oxygen and nitrogen

Answer 26

Oxygen follows nitrogen and is when you start filling in the opposite spin electrons for the 2p orbital so naturally, because the electrons repel each other, it is easier to remove the electron from the oxygen rather than the nitrogen that has a single electron in each orbital.

Question 27

Metallic Bonds

Answer 27

Strong electrostatic attraction between positive metal ions and negative delocalised electron floating within its structure

Question 28

Structure of metal

Answer 28

Metal atoms will donate their outer shell electrons in order to become stable metal cations and form a sea of delocalised electrons that can float around the structure. They are held together in a giant metallic lattice

Question 29

Properties of metal

Answer 29

High melting point because of strong bonds in it. Good conductor because of the delocalised electrons Malleable and ductile because the positive ions can be dispositioned without the lattice collapsing It is not soluble but could react with polar molecules

Question 30

Giant covalent structures

Answer 30

Diamond is a giant covalent lattice and uses all 4 of its covalent bonds to make a tetrahedral structure with 109.5 bond angle. Graphene and graphite are also giant covalent structures but the carbons bond to form planar hexagonal layers.

Question 31

Properties of giant covalent structures

Answer 31

High melting and boiling points because of the strong covalent bonds They are insoluble Diamond doesn't conduct electricity but graphite and graphene can as they only use three of the four covalent bonds

Question 32

Trend of melting points

Answer 32

The melting points increase from group 1 to 3 where all the metals are and then there is a sharp decrease where the non-metals are