The Periodic Table

Question 1

What colour does lithium produce in a flame test?

Answer 1

Red

Question 2

What colour does sodium produce in a flame test?

Answer 2

Yellow / Orange

Question 3

What colour does potassium produce in a flame test?

Answer 3

Lilac

Question 4

What colour does calcium produce in a flame test?

Answer 4

Brick Red

Question 5

What colour does strontium produce in a flame test?

Answer 5

Crimson

Question 6

What colour does barium produce in a flame test?

Answer 6

Apple Green

Question 7

What colour does magnesium produce in a flame test?

Answer 7

No Colour

Question 8

Which hydroxide is insoluble in water?

Answer 8

Magnesium hydroxide (Mg(OH)₂)

Question 9

Which hydroxide is sparingly soluble in water?

Answer 9

Calcium hydroxide (Ca(OH)₂)

Question 10

Which hydroxide is moderately soluble in water?

Answer 10

Strontium hydroxide (Sr(OH)₂)

Question 11

Which hydroxide is soluble in water?

Answer 11

Barium hydroxide (Ba(OH)₂)

Question 12

Are Group 2 carbonates soluble in water?

Answer 12

No, all Group 2 carbonates are insoluble.

Question 13

Which sulfates are soluble in water?

Answer 13

Magnesium sulfate (MgSO₄)

Question 14

Which sulfate is moderately soluble in water?

Answer 14

Calcium sulfate (CaSO₄)

Question 15

Which sulfates are sparingly soluble or insoluble in water?

Answer 15

Strontium sulfate (SrSO₄) - sparingly soluble
Barium sulfate (BaSO₄) - insoluble

Question 16

What type of oxides do s-block elements form?

Answer 16

Basic oxides (produce a salt and water)

Question 17

Are s-block elements oxidising or reducing agents?

Answer 17

Reducing agents (they donate electrons)

Question 18

What happens to the melting point of Group 1 & 2 metals down the group?

Answer 18

It decreases

Question 19

How do group 1 metals react with water?

Answer 19

They form hydroxides and release hydrogen gas (effervescence is observed).
Let M be the metal;

2M +H20 = 2MOH + H2

Question 20

What trend is seen in the reaction of Group 1 metals with water?

Answer 20

Reactivity increases down the group.
(Becomes more vigorous as you go down)

Question 21

What happens when potassium and heavier Group 1 metals react with water?

Answer 21

The hydrogen produced ignites.

Question 22

What type of oxides do p-block elements form?

Answer 22

Acidic oxides

Question 23

Are p-block elements oxidising or reducing agents?

Answer 23

Oxidising agents (they accept electrons)

Question 24

What happens to the melting point of Group 6 & 7 elements down the group?

Answer 24

It increases

Question 25

How do Group 6 and 7 elements form anions?

Answer 25

By gaining electrons (Group 6 → -2, Group 7 → -1)

Question 26

At room temperature, what colour and state is chlorine?

Answer 26

Chlorine is a green gas.

Question 27

At room temperature, what colour and state is Bromine?

Answer 27

Bromine is a red-brown liquid.

Question 28

At room temperature, what colour and state is Iodine?

Answer 28

Iodine is a grey solid.

Question 29

Why is chlorine added to water as a treatment method?

Answer 29

Chlorine is added to water to kill bacteria and viruses. It must be low concentrations to be safe.

Question 30

Why is Fluorine added to water as a treatment method?

Answer 30

Fluorine is added to water to reduce tooth decay. It also helps to strengthen bones.

Question 31

What is the trend in reactivity of group 7?

Answer 31

As you go down, reactivity decreases as more shielding makes it harder for nucleus to attract electrons.

Question 32

How do group 2 metals react with water?

Answer 32

They form hydroxides and release hydrogen gas (effervescence is observed). Let M be the either Ca, Sr or Ba; M + 2H20 = M(OH)2 + H2

Question 33

How is magnesium’s reaction with water different to other group 2 metals?

Answer 33

Magnesium reacts and produces an oxide instead of a hydroxide. Mg + H20 = MgO + H2