Groups Of The Peridoic Table

Question 1

What are the properties of alkali metals?

Answer 1

Soft
Low melting point 
Dull colour
React with water and oxygen 
Gives of hydrogen

Question 2

What group and charge are the alkali metals in?

Answer 2

1 so they all have a 1+ charge as they want to loose an electron to gain a full outer shell
-the more readily this is lost the more reactive it is

Question 3

Why are alkali metals stored under oil?

Answer 3

As it stops them reacting with the oxygen in the air

Question 4

Why are these elements called alkali metals?

Answer 4

Because they produce an alkali solution when reacted with water -hydrogen and metal hydroxide
Ph of 13/14

Question 5

What happens to the trend of appearance as you go down the alkali metals group?

Answer 5

The inside stays shiny but the outside becomes a lighter version of black/grey

Question 6

What is the trend of effervescing when reacted with water as you go down the alkali metals group?

Answer 6

The element effervesces (fizz) more, meaning more hydrogen is given off. It also moves around more as it is more reactive and potassium gives off a purple flame

Question 7

What is the general equation to show an alkali metal reaction with water?

Answer 7

2Alkali metal + 2water — 2metal hydroxide + hydrogen

Question 8

What is the affect of an alkali metal having more shells?

Answer 8

The more shells an atom has the further the outer shell electron is from the nucleus. This decreases the attraction between the outer shell electrons and the nucleus, so makes the alkali metal more reactive as the outer electron is easier to remove.

Question 9

What happens to the size of the atoms as you go down the alkali metal group?

Answer 9

They get bigger as they have more electron shells.

Question 10

What group and charge are the halogens in?

Answer 10

7 so they have a 1- charge as they want to gain an electron in order to create a full outer shell
-this means they have similar chemical properties and react similarly

Question 11

What is the appearance and state if the first 3 halogens?

Answer 11

Chlorine = yellowy/green = gas
Bromine = Brown/orange = liquid at room temperature
Iodine = grey = solid

Question 12

What happens to the trend pf the halogens and alkali metal boiling points as you go down the group?

Answer 12

Halogens =Their boiling points get higher

Alkali metals = boiling point decreases

Question 13

What are the halogen molecules?

Answer 13

Diatomic so are written as (e.g. Cl2, Br2, I2)

-this is because by sharing a pair of electrons they gain a full outer shell

Question 14

What is the test for chlorine gas?

Answer 14

That it turns light blue litmus paper red and then bleaches white

Question 15

What do halogens make when they react with metals and hydrogen?

Answer 15

With metals they form Salts called metal halides

Or with hydrogen to form hydrogen halides (these can dissolve in water to form acidic solutions as they are Soluble)

Question 16

How do you balance a metal halide reaction?

Answer 16

Cl2 (gas) + H2 (gas) — 2 HCl (gas)

Question 17

What happens when hydrogen chloride is put into water?

Answer 17

Is dissociates into hydrogen ions (H+) and (Cl-)

Hydrogen chloride + water — hydro-chloric acid

Question 18

What is a displacement reaction?

Answer 18

A displacement reaction happens when a more reactive element displaces a less reactive element

Question 19

Why can chlorine displace bromine and iodine?

Answer 19

Because it is the most reactive halogen (top of the group)

This means if you add chlorine water to any of them it will displace it and be reduced while the other compound oxidised

Question 20

Chlorine + potassium bromide —

Answer 20

Potassium chloride + bromine

Question 21

Why do halogens become less reactive as you go down the group?

Answer 21

As you go down the group the elements have more outer shells so the outer most electrons are further away from the nucleus. This means it is harder to gain electrons as the attraction is weaker

Question 22

What group are Nobel gases in?

Answer 22

8/0

Question 23

Why does helium make your voice go high?

Answer 23

Because the speed of sound is faster in lighter gases

Question 24

What are the properties of Nobel gases?

Answer 24

Colourless, odourless, tasteless
Low melting point and boiling point
Low density 
Inert (stable and un-reactive)
Single atoms (monatomic) as they have a full outer shell

Question 25

What does it mean if Nobel gases have a full outer shell?

Answer 25

This means they do not need to gain or lose an election is they were to react. This makes them stable and inert

Question 26

What is the property of the Nobel gas helium for balloons?

Answer 26

As helium has a low density, even lower then air, it will float and rise into the air making it suitable for a balloon. It will also float without combusting making it safer than hydrogen

Question 27

What is the property if the Nobel gas Neon making it suitable for lights?

Answer 27

Neon gives out ‘white’ light when high voltage electricity passes through it and so is useful as a source of light

Question 28

What is the property that makes argon useful for filament bulbs?

Answer 28

• it isn’t flammable so it stops the very hot filament from burning away, flags photography uses this
• stops the filament reacting with the oxygen in the air, welding metals uses this process as well

Question 29

What is the trend in reactivity of halogens as you go down the group?

Answer 29

The atoms get larger, so the attraction is weaker between the outer shell electrons and the nucleus. Therefore the less easily an electron is gained so the less reactive it is the further down you go.

Question 30

What does OIL RIG stand for?

Answer 30

Oxidation is loss (of electrons)

Reduction is gain (or electrons)

Question 31

What are the properties of transition metals?

Answer 31

• higher melting points and densities than other groups
• very ductile
• malleable
• less reactive so more useful
• can be used as catalysts
• solutions are colourful

Question 32

Where are transition metals found?

Answer 32

In the middle rectangle if the periodic table

Question 33

Transition metals form coloured compounds, how can we use this property?

Answer 33

To identify which transition metal is present in a solution

-they can also be used as dyes in products

Question 34

What are some uses linked to properties of transition metals?

Answer 34

Copper is ductile and can conduct electricity making it useful for wires and frying pans

• aluminium might be used in mirrors due to its shiny property and in overhead cables as is less dense than e.g. copper so can hang in the air but is also resistant to corrosion so suitable for all weather
• gold is used in jewellery as is shiny, ductile and expensive

Question 35

What are some uses of alloys?

Answer 35

Magnalium (95% aluminium, 5% magnesium) is less dense and four times stronger than normal aluminium having a better resistance to corrosion -used in aircraft parts
-brass is made of copper and zinc and is used in electrical plug pins as conducts electricity and is stronger than normal copper

Question 36

What transition metals are used as catalysts?

Answer 36

• iron is used in the haber process

- vanadium pentoxide is used in the contact process

Question 37

Why are alloys strong?

Answer 37

• normal metals have rows of regularly arranged metal cations that can slide over one another
• the presence of another size atom disrupts the regular arrangement so metals cannot slide and are stronger
• alloys can be designed for specific uses as well
• a mixture of a metal with one or more element

Question 38

Why might one make an alloy?

Answer 38

• increase strength or ductility or resistance
• lower or increase the melting point
• change the colour
• give better castings (moulds)
• change electrical or thermal properties

Question 39

Why is iron alloyed to produce steel?

Answer 39

• iron on its own will rust but by adding carbon is reduces this making it stronger and more resistant
• it is harder as can slide less easily