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GCSE Chemistry > Groups Of The Periodic Table > Flashcards

Groups Of The Periodic Table Flashcards

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1
Q

What physical properties do the group 1 alkali metals have?

A
  • Soft
  • Low melting and boiling points
  • Low density
  • Good conductors of heat and electricity
  • Shiny (when unreacted)
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2
Q

As you go down group 1 the reactivity _________

A

Increases

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3
Q

Which other group of the periodic table reacts easily with group 1?

A

Group 7

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4
Q

Which other group of the periodic table reacts easily with group 7?

A

Group 1

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5
Q

Group 1 metals have _ electron(s) in their outer shells

A

1

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6
Q

Describe the reactivity of group 1 metals

A

Highly reactive, therefore found as metal ores

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7
Q

Alkali metal + water ——> ???

A

Metal hydroxide + hydrogen

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8
Q

Lithium + water ——> ???

A

Lithium hydroxide + hydrogen

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9
Q

Why are group 1 metals more reactive as you go down the periodic table?

A

As you go down the group, the distance between the nucleus and the single electron increases, so there are weaker electrostatic forces so it is easier to lose that one electron

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10
Q

As you go down group 1 the melting points ________

A

Decrease

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11
Q

Why do the melting points of group 1 metals decrease as you go down the group?

A

There are weaker electrostatic forces so less energy is required to break the bonds

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12
Q

What are the group 1 elements known as?

A

The alkali metals

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13
Q

What are the group 7 elements known as?

A

Halogens

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14
Q

What state is fluorine at room temperature?

A

Gas

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15
Q

What state is chlorine at room temperature?

A

Gas

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16
Q

What state is bromine at room temperature?

A

Liquid

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17
Q

What state is iodine at room temperature?

A

Solid

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18
Q

What colour is fluorine at room temperature?

A

Green

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19
Q

What colour is chlorine at room temperature?

A

Yellow

20
Q

What colour is bromine at room temperature?

A

Brown/orange

21
Q

What colour is iodine at room temperature?

A

Grey-black

22
Q

All halogens are ________ and are connected by ________ bonds

A

Diatomic, covalent

23
Q

Why are group 7 elements more reactive as you go up the periodic table?

A

The outer electron is getting closer to the nucleus so forces of attraction are higher, so it is easier to gain an electron

24
Q

As you go down group 7 reactivity _________

A

Decreases

25
Q

As you go down group 7 the melting and boiling points ________

A

Increase

26
Q

Why do the melting and boiling points increase as you go down group 7?

A

As you go down group 7 the molecules become larger so there are stronger intermolecular forces, that require more energy to break

27
Q

All halogens are _____

A

Toxic

28
Q

Halogen + alkali metal ——> ???

A

Metal halide

29
Q

Lithium + chlorine ——> ???

A

Lithium chloride

30
Q

Halogen + hydrogen ——> ???

A

Hydrogen halide

31
Q

Hydrogen + bromine ——> ???

A

Hydrogen bromide

32
Q

Hydrogen halide + water ——> ???

A

Acid

33
Q

Hydrogen chloride + water ——> ???

A

Hydrochloric acid

34
Q

Sodium iodide + chlorine ——> ???

A

Sodium chloride + iodine

35
Q

Lithium fluoride + chlorine ——> ???

A

No reaction

36
Q

What are elements in group 0 known as?

A

The Noble Gasses

37
Q

Describe the reactivity of group 0 elements

A

Highly unreactive

38
Q

What are group 0 elements so unreactive?

A

They have full valence shells of electrons

39
Q

What state are group 0 elements at room temperature?

A

Gasses

40
Q

In group 0 elements melting and boiling points ________ going down the group

A

Increase

41
Q

In group 0 elements, density ________ going down the group

A

Increases

42
Q

Why do density, melting and boiling points increase going down group 0?

A

The elements have larger atoms so stronger intermolecular forces that require more energy to break

43
Q

Name 4 chemical properties of noble gases

A
  • Odourless
  • Colourless
  • Non-flammable
  • Extreme unreactive
44
Q

What is another name for the noble gasses?

A

The Inert Gasses

45
Q

What does inert mean?

A

Extremely unreactive

46
Q

Write a balanced equation for when chlorine reacts with hydrogen to form hydrogen chloride

A

H2+Cl2 ——> 2HCl

GCSE Chemistry (16 decks)

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