Topic 1 Periodic Table Flashcards

1
Q

What are elements in group 1 refered to

A

Alkali metals

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2
Q

What happens as you move down group 1

A

the reactions of alkali metals become quicker and more vigorous as The number of electron shells increases meaning there is a greater distance between the outer electron and the nucleus.

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3
Q

What happens when a metal floats on water

A

Becomes (metal) hydroxide

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4
Q

What group are the haolgens located in

A

Group 7

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5
Q

Why are halogens very reactive

A

Easily accept an electron into their outer shell

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6
Q

What are diatomic molecules

A

Molecules made of pairs of atoms

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7
Q

How are salts formed

A

When a metal atom transfers its outer electron to a non-metal atom

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8
Q

What happens when you go down group 7

A

Tye halogens become less reactive as the atoms gain more electron shells so therfore further from the nucleus

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9
Q

Name three halogens

A

Bromine
Chlorine
Iodine

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10
Q

At room temperature what are these 3 halogens like

A

Bromime - red/brown liquid
Iodine - dark grey solid
Chlorine - pale green gas

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11
Q

What is the test for chlorine

A

Insert damp litmus paper into a test tube containing a gas.

If the gas is chlorine, the litmus paper will bleach and change colour from red to white.

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12
Q

Wnat group are noble gases in

A

Group 0

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13
Q

Why are noble gases unreactive

A

Have a full outer shell so dont gain or lose any electrons

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14
Q

What can noble gases be used for

A

Light bulb

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15
Q

How are noble gases arranged

A

As they are unreactive they are single atoms ( monatomic)

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16
Q

What is tye boiling point like for noble gases

A

Low boiling point but does increase as you go down the periodic table as the relative atomic mass increases

17
Q

What forms when a halogen and metal react

A

Metal halides

18
Q

What is a spectator ion

A

An ion that doesnt change during a chemical reaction

19
Q

What is reduction

A

Where the atoms of the more reactive halogen displace the less reactive one and gain an electron

20
Q

What is oxidation

A

The ions of the less reactive halogen are displaced by the more reactive halogen.
They each lose an electron and are oxidised.