Trends in The Periodic Table CH7

Question 1

Atomic radius

Answer 1

Half the distance between nuclei of two atoms of the same element joined together by a single covalent bond.

Question 2

Atomic radius decreases

Answer 2

Decreases across a period due to increasing nuclear charge and no screening effect.

Question 3

Atomic radius increases

Answer 3

Increases down a group due to a new energy level and screening effect.

Question 4

1st ionisation energy

Answer 4

The minimum energy needed to completely remove an electron from the outmost energy level.

Question 5

Ionisation energy increases

Answer 5

Increases across a period due to increasing nuclear charge and deceasing atomic radius.

Question 6

Ionisation energy deceases

Answer 6

Deceases down a group due to increasing atomic radius and the screening effect.

Question 7

Why is there exceptions?

Answer 7

Any sublevel that is completely filled or exactly half filled has extra stability.

Question 8

2nd ionisation energy

Answer 8

Energy is the needed to remove an electron from an ion with one positive charge in the gaseous state.

Question 9

Electronegativity

Answer 9

The relative attraction that an atom in a molecule has for the sharing pair of electron in a covalent bond.

Question 10

Electronegativity values increase

Answer 10

Increases across a period due to increasing nuclear charge and deceasing atomic radius.

Question 11

Electronegative values decreases

Answer 11

Deceases down a group due to increasing atomic radius and the screening effect.

Question 12

Trends within groups

Answer 12

ionic bond formation is bonds formed by transfer on an electron and in covalent bond is formed by sharing electrons.

Question 13

Alkaii metals

Answer 13

Very reactive because they have a low first ionisation energy value.

Question 14

Halogen

Answer 14

Are the most electronegative element and reactive.