Topic 6 - Groups in the periodic table

Question 1

What are group 1 metals also known as?

Answer 1

Alkali Metals

Question 2

What are group 7 also known as

Answer 2

Halogens

Question 3

What are group 0 also known as?

Answer 3

Noble gases

Question 4

Names some physical properties of Alkali metals

Answer 4

Very soft so can be cut with a knife

Low melting points

Question 5

What kind of compounds do group 1 form? and Why?

Answer 5

Ionic compounds because they lose their outer shell electron very easily

Question 6

What is the pattern f reactivity going down the group 1

Answer 6

Increases/ more reactive

Question 7

What happens when lithium sodium and potassium react with water

Answer 7

Produces a metal hydroxide and hydrogen gas

fizzes and bubbles in the water

Question 8

How do we test for hydrogen

Answer 8

squeaky pop test

Question 9

Why do group 1s get more reactive

Answer 9

because their outer shell electron is lost more easily as its further from the nucleus

Question 10

Why does potassium ignite when reacting with water??

Answer 10

Because it gets hot enough to ignite the hydrogen gas being produced

Question 11

What is the balanced symbol equation for Alkali metal reacting with water (for sodium)

Answer 11

2Na + 2H2O&raquo_space;» 2NaOH + H2

-Works for all group 1

Question 12

What is the half equation for lithium forming a 1+ ion in an ionic compound

Answer 12

Li&raquo_space;»> Li+ + e-

Question 13

What is the appearance and state of chlorine, bromine, and iodine at room temperature

Answer 13

Chlorine - fairly reactive, poisonous green gas
Bromine- poisonous brown liquid which gives off orange vapour
Iodine- dark grey crystal solid which gives off purple vapour when heated

Question 14

What are the trends in colour as you go down the group 7

Answer 14

The colours get darker

Question 15

How does reactivity change as you go down group 7

Answer 15

decreases as its harder to attract an extra electron as its outer shell is too far from the nucleus

Question 16

How do boiling and melting points change as you go down group 7

Answer 16

It increases as they become solids as you go down so more energy is needed to break bonds

Question 17

Predict the properties of Astatine (bottom of group 7)

Answer 17

Black solid with very high melting point of 300 degrees

Question 18

How do you test for chlorine gas?

Answer 18

Bleaches damp blue litmus after making it red as chlorine is acidic

Question 19

What do halogens make when reacting with hydrogen

and example

Answer 19

Hydrogen halides which are soluble in water to form acidic solutions
eg) Hydrochloric acid

Question 20

What is the balanced equation for the formation of a common hydrogen halide

Answer 20

H2 + Cl2&raquo_space;»» 2HCl

Question 21

What do halogens make when reacting with a metal

Answer 21

They react vigorusly to make a metal halide which is often with group 1 eg) sodium chloide
- Halogens higher up on the group react easier as they attract an outer shell electron more easily

Question 22

What is a balanced equation for the formation of a metal halide (sodium chloride)

Answer 22

2Na + Cl2&raquo_space;»> 2NaCl

Question 23

What is a chemical property of a hydrogen halide

Answer 23

Soluble in water

HCl is aqueous

Question 24

How can the reactivity of a halogen be worked out from displacement reactions

Answer 24

A more reactive halogen will displace a less reactive one from a compound

Question 25

Describe what you would see if you added chlorine water to a potassium bromide solution

Answer 25

The more reactive chlorine would displace the bromine to make potassium chloride making the solution orange leaving it as excess in solution

Question 26

Why is a displacement reaction a redox reaction

Answer 26

Because the halogens are reduced and gain electrons whilst halide ions are oxidised and lose electrons

Halide ion = The salt solution
Halogen = is the halogen being added

Question 27

What is the ionic equation for chlorine displacing

bromine

Answer 27

Cl2 + 2Br-&raquo_space;»> Br2 + 2Cl-

Question 28

How could you show the reactivity trends of halogens

Answer 28

add halide salt solution to test tube and add halogen

and if colour change then displacement reaction has occurred.

Question 29

Why are noble gases inert?

Answer 29

Because they contain a full outer shell of electrons so they dont easily give up or gain electrons

Question 30

Name some properties of group 0

Answer 30

Colourless gases at room temperature
Monotomic - single atoms not molecules
Non-flammable

Question 31

what is the trend for boiling and melting points going down group 0

Answer 31

increases

Question 32

what is the trend for density going down group 0

Answer 32

increases

Question 33

Name some everyday uses of Noble gases

Answer 33

• Argon is used in filament bulbs as its non-flammable
• Kypton and xenon are used in flash photos to stop flash burning up
• Argon and helum protect metals that are being welded to create inert atmosphere that doesnt react with oxygen
• Helium is used in airships and balloons as it has a density lower than air so can float (doenst ignite unlike hydrogen)