The Periodic Table

Question 1

What trend can be observed in electronegativity across a period (from left to right) and why?

Answer 1

Electronegativity increases across a period (from left to right)
as there is an increase in nuclear charge across a period with no significant change in shielding.

Question 2

What trend can be observed in electronegativity down a group and why?

Answer 2

Electronegativity decreases down a group because the size of the atoms increase

Question 3

What is electronegativity?

Answer 3

The electronegativity of an element is a measure of its ability to attract electrons from within a covalent bond.

Question 4

As a group is descended what trend can be observed in atomic radius?

From left to right of a period what trend can be observed in atomic radius?

Answer 4

Atomic radius increases down a group

Atomic radius decreases across a period

Question 5

What is ionisation energy and what trend can be observed in first ionisation energy down a group?

Answer 5

Ionisation energy is the minimum amount of energy required to remove an electron from a gaseous atom.

First ionisation energy deceases down a group because outer shell electrons are further away from the nucleus and so less energy is required to remove them.

Question 6

What trend can be observed in melting point as group 1 is descended and why?

Answer 6

As group 1 is descended the melting point decreases

because the atomic radius increases thus the outer shell electrons are further away from the nucleus making the attraction between them weaker —> less energy is required to break apart the lattice

Question 7

What will be observed when a basic oxide reacts with acid?

Answer 7

When a basic oxide reacts with acid a salt will be formed (if the oxide is soluble in water an alkaline solution will be formed).

Question 8

Please differentiate between basic and acidic oxides.

Answer 8

Basic oxides are metallic whereas acidic oxides are non-metallic