Topic 6 - Groups In The Periodic Table Flashcards

1
Q

What are the group 1 metals?

A

Alkali metals

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2
Q

How can elements be classified as alkali metals based on their position on the periodic table?

A

They all have one outer electron on their outer shell so they’re group 1

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3
Q

How can elements be classified as halogens based on their position on the periodic table?

A

They all have 7 electrons in their outer shell so are in group 7

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4
Q

How can elements be classified as noble gases based on their position on the periodic table?

A

They have a full outer shell so are group 0

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5
Q

Physical properties of alkali metals

A

Low melting and boiling points

Very soft

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6
Q

Describe the reaction of lithium with water

A

Lithium will move around the surface, fizzing furiously

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7
Q

Describe the reaction of sodium with water

A

Move around quickly and fizz. Also melts in the heat of reaction

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8
Q

Describe the reaction of potassium with water

A

Moving around violently and fizzes. Gets hot enough to ignite the hydrogen produced

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9
Q

Describe the pattern in reactivity of the alkali metals.

A

Reactivity increases down the group

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10
Q

Explain the pattern of reactivity in group 1 in terms of electronic configurations

A

Group 1 lose their outer electron to form +1 ion. As you go down the outer electron is more easily lost because it’s further from the nucleus so it’s attraction is weaker and less energy needed to remove it

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11
Q

What is chlorine at room temperature?

A

Green gas

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12
Q

What is bromine at room temperature?

A

Red brown liquid which gives off an orange vapour

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13
Q

What is iodine at room temperature?

A

Dark grey crystalline solid which gives off a purple vapour when heated

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14
Q

What are halogens?

A

Diatomic molecules sharing one pair of electrons in a covalent bond giving both atoms a full outer shell.

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15
Q

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

A

As you go down the melting and boiling points of halogens increase. Going from gas to solid. Also colours get darker

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16
Q

Describe the chemical test for chlorine

A

Hold a piece of damp blue litmus paper over chlorine. At first it turns red and then the chlorine will bleach the litmus paper white.

17
Q

Explain the relative reactivity of the halogens in terms of

electronic configurations

A

Halogen atom only gains one electron to form 1- ion. As you go down halogens become less reactive because it gets harder to attract the extra electron to fill outer shell when it’s further away from nucleus.

18
Q

What happens when halogens react with metals?

A

They react vigorously to form salts called metal halides:

Sodium + chlorine -> sodium chloride

19
Q

What happens when halogens react with hydrogen?

A

They form hydrogen halides. They’re soluble and can dissolve in water to form acidic solutions:
Hydrogen + chlorine -> hydrogen chloride

20
Q

What is a displacement reaction?

A

When a more reactive element displaces a less restive element from a compound

21
Q

What are the halogen displacement reactions?

A

They’re redox reactions. The halogens gain electrons (reduction) whilst halide ions lose electrons (oxidation)

22
Q

Why are noble gases (group 0) inert?

A

They have a full outer shell of electrons so they don’t need to give up or gain electron

23
Q

What are the uses of noble gases due to their non flammability?

A

Argon is used in filament lamps so it stops the hot filament from burning.
Some are used in flash photography to stop flash filament from burning.

24
Q

What are the uses of noble gases due to their inertness?

A

Used to protect metals that are being welded to stop the hot metal reacting with oxygen.

25
Q

What are the uses of noble gases due to their low density?

A

Helium used in balloons + airships as it has lower density than air to so it floats.

26
Q

What are the patterns in the properties of group 0?

A

As you go down group 0 BP, MP + density increase due to intermolecular forces becoming stronger

27
Q

Describe the noble gases

A

They’re a colourless gas at room temperature
Monatomic - made up of single atoms
Inert