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Chemistry GCSE > Topic 6 - Groups in the Periodic Table > Flashcards

Topic 6 - Groups in the Periodic Table Flashcards

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1
Q

What are group 1 elements know as?

A

The alkali metals

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2
Q

What are the properties of group 1 metals?

A

Low mp/bp

Very soft

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3
Q

How reactive are group 1 metals?

A

Very reactive

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4
Q

What determines a metals reactivity?

A

How readily it loses its outer electron

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5
Q

What is the trend of reactivity for group 1?

A

As you go down, it gets more reactive

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6
Q

What happens when alkali metals are put in water?

A

They react vigorously

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7
Q

What is the word equation for the reaction between water and alkali metals?

A

Alkali Metal + Water -> Metal Hydroxide + Hydrogen

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8
Q

How do test for the presence of hydrogen gas?

A

By a lit splint making a squeaky pop

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9
Q

Describe the observations when lithium is put into water?

A

It will move around the surface, fizzing furiously

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10
Q

Describe the observations when sodium is put into water?

A

It will move around the surface, fizzing furiously whilst also melting due to the heat of the reaction

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11
Q

Describe the observations when potassium is put into water?

A

It will move around the surface, fizzing furiously whilst also igniting the hydrogen gas produced

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12
Q

Write a balance symbol equation for the reaction between potassium and water

A

2K + 2H2O -> 2KOH + H2

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13
Q

What are group 7 elements known as?

A

The halogens

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14
Q

What do the halogens exist as?

A

Diatomic molecules

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15
Q

What do you notice as you go down the halogens?

A

The melting points and boiling points increase

Colour gets darker

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16
Q

Describe chlorine

A

A fairly reactive, poisonous, green gas

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17
Q

Describe bromine

A

A poisonous, red-brown liquid, which gives off an orange vapour at room temperature

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18
Q

Describe iodine

A

A dark grey crystalline solid which gives off a purple vapour when heated

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19
Q

How do you test for chlorine?

A

By holding a piece of damp blue litmus paper which will bleach if chlorine is present, turning it white
It may also turn red for a moment first

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20
Q

What is the trend of reactivity for halogens?

A

Decreases as you go down

21
Q

What is the word equation between metals and halogens?

A

Metal + Halogen -> Metal Halide

22
Q

What do metals and halogens react to form?

A

Metal halides

23
Q

What are metal halides?

A

Salts formed when halogens react with metals

24
Q

What is the word equation between hydrogen and halogens?

A

Hydrogen + Halogens -> Hydrogen Halide

25
Q

Write a balanced symbol equation for the reaction between bromine and sodium?

A

Br2 + 2Na -> 2BrNa

26
Q

What is a displacement reaction?

A

Where a more reactive element displaces a less reactive element from a compound

27
Q

What type of reactions are halogen displacement reactions?

A

Redox

28
Q

Why are halogen displacement reactions redox?

A

Because halide ions lose electrons whilst halogens gain elecrons

29
Q

A student adds a few drops of a halogen solution to a potassium iodide solution
The solution turned brown
Explain what the student should do to help him identify the halogen solution

A

He should add a few drops of the solution to a bromine salt solution
If the solution turns orange, the halogen solution contains chlorine

30
Q

What are group 0 elements?

A

Inert and colourless gases

31
Q

What are group 0 elements called?

A

Noble gases

32
Q

What does monatomic mean?

A

They are gases made up of single atoms

33
Q

Are noble gases diatomic or monatomic?

A

Monatomic

34
Q

What are the properties of the noble gases?

A

Monatomic
Inert
Colourless
Non-flammable

35
Q

What are the uses of noble gases?

A

Stopping burning in filament lamp
Welding in metals
Airships
Balloons

36
Q

Why are noble gases used in filament lamps?

A

Because they’re non-flammable

37
Q

Why does helium float?

A

Because it’s density is lower than air

38
Q

Why is helium used over hydrogen?

A

Because hydrogen is extremely flammable

39
Q

What is the trend as you go down the noble gases?

A

Boiling point, melting point and density all increase

40
Q

Use the densities off helium (0.2 kg/m³) and argon (1.8 km/m³) to predict the density of neon

A

(0.2 + 1.8) / 2 = 2.0 / 2 = 1

Neon should have a density of about 1.0 kg/m³

41
Q

Give two properties of the group 1 metals?

A

Low mp/bp

Very soft

42
Q

Explain why group 1 metals are so reactive?

A

Because all group 1 metals have only 1 outer electron meaning there is only 1 electron that needs to be lost meaning it is very reactive

43
Q

Put all these alkali metals in order of reactivity, staring with the least reactive:
Potassium, Caesium, Lithium and Sodium

A

Lithium, Sodium, Potassium and Caesium

44
Q

How many electrons do halogens have in their outer shell?

A

7

45
Q

Why can halogen displacement reactions be described as redox reactions?

A

Because halogens gain electrons whilst the halide ions lose electrons

46
Q

If chlorine water is added to potassium bromide solution, what colour will the solution turn?

A

Orange solution formed

47
Q

At room temperature, what colour are the Group 0 gases?

A

Colourless

48
Q

Why are balloons filled with helium able to float in the air?

A

Because helium has a lower density than air meaning it will float

Chemistry GCSE (9 decks)

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