Groups in the Periodic Table

Question 1

What are typical properties of transition metals?

Answer 1

Hard, strong, shiny, malleable, good conductors of heat and electricity, high melting points, high densities, catalysts, form colourful compounds

Question 2

How does metallic bonding work?

Answer 2

Positive ions are surrounded by delocalised electrons and form strong bonds

Question 3

Why do metals conduct electricity?

Answer 3

They have delocalised electrons that can carry a charge

Question 4

Why do metals have high melting points?

Answer 4

There are strong bonds between negative electrons and positive ions

Question 5

Why are alloys stronger than pure metals?

Answer 5

Metals have layers of atoms in sheets that can slide over each other easily, so it can bend. Adding another element that has atoms of different sizes disrupts these sheets, so they cannot slide

Question 6

What are limits of atomic models?

Answer 6

Some are only two dimensional, rather than three in real life
Ions and particles are very large, while in real life they would be small, with lots of empty space between them

Question 7

What are the alkali metals and their symbols?

Answer 7

Lithium - Li
Sodium - Na
Potassium - K
Rubidium - Rb
Caesium - Cs
Francium - Fr

Question 8

Why are alkali metals more reactive as you go down the group?

Answer 8

There are more electron shells, so the outermost electron is further from the nucleus, so the attraction force is weaker, so it can be lost more easily

Question 9

What are properties of group 1 metals?

Answer 9

Soft, low melting and boiling points, float on water - low densities, very reactive with water, form an alkali in water

Question 10

How do alkali metals react with water?

Answer 10

They float, move around and fizz. Over time they disappeared as they turned into hydroxide and let off hydrogen gas.
Potassium produced a purple flame
Rubidium and caesium explode

Question 11

What is the reaction between alkali metals and water?

Answer 11

e.g. Lithium + water –> lithium hydroxide + hydrogen

2Li + 2H2O –> 2LiOH + H2

Question 12

What is the test for hydrogen?

Answer 12

Hold a test tube over it and hold a lit splint over it. If it makes a squeaky pop sound, hydrogen gas is present

Question 13

Why are halogens found in pairs?

Answer 13

They need to form a covalent bond to have a full outer shell. This is called diatomic, as opposed to monotomic

Question 14

What are the halogens and their symbols?

Answer 14

Fluorine - F
Chlorine - Cl
Bromine - Br
Iodine - I
Astatine - At

Question 15

What are the states and colours of the halogens?

Answer 15

Fluorine - gas - pale yellow
Chlorine - gas - green
Bromine - liquid - red
Iodine - solid - grey, purple vapour
Astatine - solid - black

Question 16

What is the test for chlorine gas?

Answer 16

Chlorine turns damp blue litmus paper red, then bleach it white

Question 17

How do halogens react with metals?

Answer 17

They react vigorously with some to form salts called metal halides
Sodium + chlorine –> sodium chloride
2Na + Cl2 –> 2NaCl

Question 18

How do halogens react with hydrogen?

Answer 18

They react to form soluble hydrogen halides
Hydrogen + chlorine –> hydrogen chloride
H2 + Cl2 –> 2HCl

Question 19

Why do halogens get less reactive as you go down?

Answer 19

There is less of a force to attract an electron to the nucleus, so it gets harder to attract the extra electron to fill the outer shell

Question 20

Why are halogen displacement reactions redox reactions? Give an example

Answer 20

The halogens lose electrons (oxidation)
Halide ions gain electrons (reduction)

Cl2 + 2KBr –> Br2 + 2KCl
Oxidised Reduced

Question 21

What are the noble gases and their symbols?

Answer 21

Helium - He
Neon - Ne
Argon - Ar
Krypton - Kr
Xenon - Xe
Radon - Rn

Question 22

Why are noble gases inert?

Answer 22

They have a full outer shell, so they don’t easily give up or gain electrons

Question 23

What are properties of noble gases?

Answer 23

Colourless, gases at room temperature, inert, non-flammable, hard to observe

Question 24

What are uses of noble gases?

Answer 24

Providing an inert atmosphere, light bulbs and welding (to stop metals from burning or being oxidised), and airships and balloons (low densities and inert)

Question 25

What are patterns in the noble gases?

Answer 25

Boiling points and melting points increase as you go down

Density increases as you go down the group