EL8:1 Spectacular Metals

Question 1

What are the most reactive metals in the periodic table?

Answer 1

Group 1 and 2.

Question 2

What are group 1 metals called?

Answer 2

Alkali metals.

Question 3

What are group 2 metals called?

Answer 3

The alkaline earth metals.

Question 4

What happens as you go down groups in the periodic table?

Answer 4

Elements get more metallic and therefore get more reactive.

Question 5

What happens as you go across a periods in the periodic table?

Answer 5

Elements become less metallic.

Question 6

What block are groups 1 and 2 in?

Answer 6

The s block.

Question 7

What do s block metals tend to be like?

Answer 7

Soft, weak metals with low boiling points but very reactive with water and oxygen.

Question 8

Why don’t metals in elemental form in groups 1 and 2 have many uses?

Answer 8

They are too reactive.

Question 9

What compounds are common and useful?

Answer 9

S block compounds.

Question 10

What is similar within groups in the periodic table?

Answer 10

Electron arrangements in their atoms.

Question 11

What is the cause of differences between groups in the periodic table?

Answer 11

The size of the atom, it increases down the group.

Question 12

What happens if sufficient energy is given to an atom (in group 1 and 2)?

Answer 12

An electron is lost and the atom becomes a positive ion.

Question 13

What is needed to remove electrons and why?

Answer 13

Energy, because the electrons are attracted to the nucleus.

Question 14

What is the first ionisation enthalpy of an element?

Answer 14

The energy needed to remove one electron from every atom in one mole of isolated gaseous atoms forming one mole of gaseous ions.

Question 15

What is the general equation for first ionisation enthalpy?

Answer 15

X(g)-X^+(g)+e^-

Question 16

What is the first ionisation enthalpy equation for oxygen?

Answer 16

O(g)-0^+(g)+e^-

Question 17

What is the first ionisation enthalpy for oxygen?

Answer 17

+1320 kJ/mol

Question 18

What electron does the first ionisation enthalpy remove and why?

Answer 18

One of the outer shell electrons, they are the most loosely held.

Question 19

What do group 0 have?

Answer 19

High first ionisation enthalpies.

Question 20

What does it mean if groups have a high first ionisation enthalpy?

Answer 20

They are hard to ionise.

Question 21

Why are group 0 elements hard to ionise?

Answer 21

They have full outer shells.

Question 22

What does it mean if groups have a low first ionisation enthalpy?

Answer 22

They are easy to ionise.

Question 23

What do group 1 have?

Answer 23

A low first ionisation enthalpy.

Question 24

Why are group 1 elements easy to ionise?

Answer 24

They have one electron in their outer shell.

Question 25

What are the peaks and troughs in a first ionisation enthalpy graph and why?

Answer 25

Peaks are group 0 as they are hard to ionise and troughs are group 1 as they are easily ionised.

Question 26

What is the electron shield theory?

Answer 26

Electron shielding from the nucleus increases as the number of shells increase, so less energy is needed to remove an outer shell electron.

Question 27

Why does it become harder to remove an outer shell electron as you go across the period?

Answer 27

The number of protons increases so nuclear charge increases.

Question 28

What causes variation of first ionisation enthalpy across periods?

Answer 28

The different energies and paired repulsions in sub-shells.

Question 29

What happens to the first ionisation enthalpies as you go down a group and why?

Answer 29

They decrease as the attraction between the nucleus and outer electrons decreases.

Question 30

What do group 1 and 2 metals first ionisation enthalpy correspond to?

Answer 30

It’s reactivity.

Question 31

What factors effect ionisation energy?

Answer 31

The size of the nuclear charge, the distance of the outer electrons to the nucleus, and the shielding effect on inner electrons.

Question 32

Why is it easier to remove an electron from a p-subshell than a s-subshell?

Answer 32

The p-subshell is further away from the nucleus and the s-subshell is shielding the electron so there is less attraction.

Question 33

Why is it easier to remove an electron from group 6 than group 5?

Answer 33

The p orbital starts to double fill in group 6 so there is a repulsion making it easier to remove the electron.

Question 34

What are the second, third, fourth and so on ionisation enthalpies?

Answer 34

The energy required to remove further electrons.

Question 35

What is the general equation for second ionisation enthalpy?

Answer 35

X^+(g)-X^2+(g)+e^-