Trends In The Periodic Table and Electronegativity

Question 1

As you go along the period…

Answer 1

1. An additional proton is added to the nucleus each time.

2. The nuclear charge increases.

Question 2

As you go down a group…

Answer 2

1. An electron shell is added.

2. Atom gets bigger

Question 3

Covalent radius is…

Answer 3

The measure of the size of an atom, half the distance between the nuclei of the two atoms.

Question 4

As you go along a period the covalent radius…

Answer 4

1. Decreases in atomic size.
2. Nuclear charge increases.
3. Increasing attraction for outer electrons, pulling them closer to the nucleus.

Question 5

As you go down a group the covalent radius…

Answer 5

1. Increases in atomic size.
2. Number of electron shells increase.
3. Inner electron shells shield the outer electrons from the pull of the nucleus.

Question 6

Ionisation energy is…

Answer 6

The Enthalpy change and is represented as a value

Question 7

First ionisation energy is…

Answer 7

The energy required to remove one electron from each atom in a mole of gaseous atoms of an element.
It is an endothermic process, you put energy in to remove an electron.

Question 8

As you go along a period ionisation energy…

Answer 8

1. Increases as nuclear charge increases.
2. Electrons are held more tightly to the positive nucleus as the atom gets smaller.
3. Electrons are more strongly attracted to the nucleus.

Question 9

As you down a group ionisation energy…

Answer 9

1. Decreases as atoms get bigger.
2. Outer electrons are less strongly attracted to the nucleus.
3. There are more electron shells so outer electrons are more shielded from the nuclear pull of the nucleus.

Question 10

Electronegativity is…

Answer 10

The measure of the ability of atoms to attract electrons in a covalent bond.
The higher the value, the better it is for attracting electrons.
The higher the value, the greater share it will have of the bonding electrons.

Question 11

As you go along a period electronegativity…

Answer 11

1. Increases as nuclear charge increases.
2. Electrons are held more tightly to the positive nucleus as the atom gets smaller.
3. Electrons are more strongly attracted to the nucleus.
4. Most electronegative elements are found at the top RHS.
5. Most electronegative elements are Cl, O, N, F.

Question 12

As you go down a period electronegativity…

Answer 12

1. Decreases as atoms get bigger.
2. Outer electrons are less strongly attracted to the nucleus.
3. There are more electron shells so outer electrons are more shielded from the nuclear pull of the nucleus.
4. Least electronegative elements are found on the bottom LHS.

Question 13

No difference in electronegativity is…

Answer 13

1. Pure covalent, electrons are shared equally.

2. Values are between 0.0 and 0.4.

Question 14

A small difference in electronegativity is…

Answer 14

1. Polar covalent, electrons are not shared equally.

2. Values between 0.5 and 1.9

Question 15

A large difference in electronegativity is…

Answer 15

1. Ionic, a transfer of electrons.

2. Value 2 or 2+