Periodicity

Question 1

Groups on periodic table

Answer 1

Vertical columns of elements with the same chemical properties and outer electron arrangement.

Question 2

Periods on the periodic table

Answer 2

Horizontal rows of elements increasing in atomic number and outer electron arrangement as you go along from left to right.

Question 3

Metallic lattices examples

Answer 3

Lithium, Beryllium, sodium, calcium, aluminium magnesium, potassium.

Question 4

Covalent network examples

Answer 4

Boron carbon and silicon

Question 5

Covalent molecules example

Answer 5

Nitrogen, phosphorous, oxygen, sulphur, fluorine and chlorine and hydrogen

Question 6

Monatomic elements examples

Answer 6

helium, Neon and argon

Question 7

Metallic lattice properties

Answer 7

Metallic bonding
Lattice structure
High melting and boiling point
Conducts electricity

Question 8

Covalent molecular properties

Answer 8

Covalent bonding
Molecule structure
Low melting and boiling point due to weak intermolecular forces.
Doesn’t conduct electricity

Question 9

Covalent networks properties

Answer 9

Covalent bonding
Network structure
High melting and boiling points.

Question 10

Diatomic elements

Answer 10

hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, bromine.

Question 11

Forms of the element carbon

Answer 11

Diamond, graphite and buckyball (molecular)

Question 12

Fullerenes definition

Answer 12

Large carbon molecules which have covalent bonding and molecular structure.

Question 13

Phosphorous

Answer 13

P4

Question 14

Sulphur

Answer 14

S8

Question 15

Covalent radius definition

Answer 15

Half of the distance between the nuclei of two atoms that are covalently bonded together.

Question 16

Covalent radius rule down a group

Answer 16

As you go down a group the covalent radius increases because an extra outer electron shell is present, increasing the distance from the nucleus to the outer electron shell and also causing more electron shielding,

Question 17

Covalent radius rule along a period

Answer 17

As you go along a period the covalent radius decreases because a proton is added to the nucleus, giving it an extra positive charge, which pulls the electron shell closer to the nucleus (no extra electron shells are added).

Question 18

Covalent radius rule along a period

Answer 18

As you go along a period the covalent radius decreases because a proton is added to the nucleus, giving it an extra positive charge, which pulls the electron shell closer to the nucleus (no extra electron shells are added).

Question 19

Covalent radius rule for metal atoms turning into ions

Answer 19

Atoms lose their a outer electron shell when turning into ions, this decreases the covalent radius since the distance between the outer electron shell and the nucleus has decreased.

Question 20

Covalent radius metal atoms to ions

Answer 20

Atoms lose their a outer electron shell when turning into ions, this decreases the covalent radius since the distance between the outer electron shell and the nucleus has decreased.

Question 21

Covalent radius rule for non metal atoms to ions

Answer 21

When a non metal atom is turned into a non metal ion the ions covalent radius increases because electrons are received to fill the outer electron shell, this increases the outer electron shielding and no protons are added to the nucleus so the radius increases.

Question 22

First ionisation energy definition

Answer 22

The energy required for the first electron to be lost from all the atoms in one mole of free atoms.

Question 23

Things to remember about ionisation energies

Answer 23

They always form positive ions
They are always gas

Question 24

Ionisation equations

Answer 24

First A(g) —> A+(g) + e-
Second A+(g) —> A2+(g) + e-
Third A2+(g) —> A3+(g) + e-

Question 25

Going along a period ionisation energy rule

Answer 25

As you go along a period from left to right the ionisation energy increases because the positive charge in the nucleus increases due to additional numbers of protons, this causes the outer electrons to be held tighter and closer to the nucleus, and no extra electron shells are added.

Question 26

Going down a group ionisation energy rule

Answer 26

As you go down a group the ionisation energy decreases since their is more electron shells, this means that the outer electrons have more shielding and are further away from the nucleus, meaning they are less tightly held and so less energy is required for them to be lost.

Question 27

Electronegativity definition

Answer 27

The measure of the force of attraction an atom involved in a bond has for the shared electrons of the bond.

Question 28

Electronegativity along a period

Answer 28

As you go along a group the number of protons increases, this increases the strength of the positive charge of the nucleus, meaning the shared outer electrons are more tightly held, therefore meaning that as you go along the group the Electronegativity increases.

Question 29

Electronegativity down a group

Answer 29

As you go down a group the number of outer electron shell increases, this increases the electron shielding of the shared electron and the distance of the nucleus, therefore this means that as you go down a group the Electronegativity decreases.