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A - Chemistry GCSE > Topic 6 - Groups in the periodic table > Flashcards

Topic 6 - Groups in the periodic table Flashcards

1
Q

What are group 1 metals also known as?

A

Alkali Metals

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2
Q

What are group 7 also known as

A

Halogens

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3
Q

What are group 0 also known as?

A

Noble gases

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4
Q

Names some physical properties of Alkali metals

A

Very soft so can be cut with a knife

Low melting points

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5
Q

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

A

Ionic compounds because they lose their outer shell electron very easily

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6
Q

What is the pattern f reactivity going down the group 1

A

Increases/ more reactive

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7
Q

What happens when lithium sodium and potassium react with water

A

Produces a metal hydroxide and hydrogen gas

fizzes and bubbles in the water

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8
Q

How do we test for hydrogen

A

squeaky pop test

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9
Q

Why do group 1s get more reactive

A

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

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10
Q

Why does potassium ignite when reacting with water??

A

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

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11
Q

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

A

2Na + 2H2O&raquo_space;» 2NaOH + H2

-Works for all group 1

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12
Q

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

A

Li&raquo_space;»> Li+ + e-

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13
Q

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

A

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

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14
Q

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

A

The colours get darker

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15
Q

How does reactivity change as you go down group 7

A

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

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16
Q

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

A

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

17
Q

Predict the properties of Astatine (bottom of group 7)

A

Black solid with very high melting point of 300 degrees

18
Q

How do you test for chlorine gas?

A

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

19
Q

What do halogens make when reacting with hydrogen

and example

A

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

20
Q

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

A

H2 + Cl2&raquo_space;»» 2HCl

21
Q

What do halogens make when reacting with a metal

A

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

22
Q

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

A

2Na + Cl2&raquo_space;»> 2NaCl

23
Q

What is a chemical property of a hydrogen halide

A

Soluble in water

HCl is aqueous

24
Q

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

A

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

25
Q

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

A

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

26
Q

Why is a displacement reaction a redox reaction

A

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

27
Q

What is the ionic equation for chlorine displacing

bromine

A

Cl2 + 2Br-&raquo_space;»> Br2 + 2Cl-

28
Q

How could you show the reactivity trends of halogens

A

add halide salt solution to test tube and add halogen

and if colour change then displacement reaction has occurred.

29
Q

Why are noble gases inert?

A

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

30
Q

Name some properties of group 0

A

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

31
Q

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

A

increases

32
Q

what is the trend for density going down group 0

A

increases

33
Q

Name some everyday uses of Noble gases

A
  • 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)

A - Chemistry GCSE (11 decks)

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