Periodicty and Reactivity Trends

Question 1

What is the definition for the <i>first ionisation energy</i> ?

Answer 1

The energy required to remove 1 electron from each atom in 1 mole of <i>gaseous atoms</i> of an element to form 1 mole of gaseous 1⁺ ions.

Question 2

The horizontal rows of the period table are called …

Answer 2

Periods

Question 3

What is the equation for the first ionisation energy of Helium?

Answer 3

He_(g) → He⁺ _{(g) +} e^-

Question 4

What are the factors affecting the first ionisation energy?

Answer 4

Atomic radius, electron shielding, and nuclear attraction.

Question 5

What is the equation for the second ionisation energy of Magnesium?

Answer 5

Mg⁺_(g) → Mg²⁺ _{(g) +} e^-

Question 6

How does the atomic radius affect the ionisation energy?

Answer 6

The greater the distance between the nucleus and the electrons, the less the nuclear attraction. This means that there is a decreased ionisation energy.

Question 7

Why is the <i>first ionisation</i> energy of Aluminium <b>lower</b> than that of Magnesium?

Answer 7

Because there is an unpaired electron in Aluminium’s outer shell, making it easier to remove.

Question 8

Describe and explain the trend in the first ionisation energy of Group 1.

Answer 8

First ionisation energy decreases. This is because there is an increased atomic radius further down the group, as well as increased shielding of electrons, meaning there is less nuclear attraction between the nucleus and the outer electrons so they are easier to remove.

Question 9

How many orbitals are there in the P shell and what is their shape?

Answer 9

There are 3 orbital in the P shell and their shape is a figure 8.
[insert image of p orbitals here]

Question 10

What is metallic bonding?

Answer 10

A strong electrostatic attraction between metal cations and a sea of <b>delocalised electrons.</b>