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Year 9 Chemistry > The Periodic Table > Flashcards

The Periodic Table Flashcards

1
Q

Where is the atomic mass found for an element?

A

It is the top number beside the atomic symbol

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2
Q

What does the atomic mass show?

A

The number of protons and neutrons added together

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3
Q

What is the atomic symbol?

A

The symbol of the element

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4
Q

Where is the atomic number found for an element?

A

It is the bottom number beside the atomic symbol

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5
Q

What does the atomic number show?

A

The number of protons, but also the number of electrons in an atom

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6
Q

What does the period number show us about the electronic configuration of an element?

A

The number of shells the atom has

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7
Q

What does the group number show us about the electronic configuration of an element?

A

The number of electrons it has in its’ outer shell

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8
Q

Which is which: groups and periods?

A

Groups are vertical

Periods are horizontal

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9
Q

What are properties of metals?

A

Shiny
high melting points (solid at room temperature- except mercury, which is a liquid)
High density- feel heavy for their size
Malleable (not brittle- so will bend without breaking)
Good conductors of heat and electricity
Magnetic (only iron, cobalt and nickel)
Are basic/ alkaline oxides
Ductile (can be drawn out into a long wire without snapping or breaking)

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10
Q

What are properties of non-metals?

A

Low melting points
Dull - not shiny
Low density (they feel light for their size)
Brittle(will break or shatter when hammered)
Poor conductors of heat and electricity (they are insulators)
Not magnetic
Are acidic oxides

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11
Q

Where is the line on the periodic table separating metals and non metals?

A 
Two from the very right,
Two up,
Two across,
One up,
One across,
One up,
One across
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12
Q

What are valence electrons?

A

The electrons in the outer shell

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13
Q

What are chemical properties?

A

A description of how a substance reacts with other substances

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14
Q

Why do elements in the same group have similar chemical properties?

A

They have the same number of valence electrons, therefore will react similarly to get a full outer shell of electrons

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15
Q

What are the noble gases?

A

Helium, Neon, Argon, Krypton, Xenon, Radon

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16
Q

What group are the Noble gases?

A

Group 0

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17
Q

Are the Noble Gases monatomic or diatomic gases?

A

Monatomic gases

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18
Q

What is meant by monatomic?

A

Have a full outer shell (except Helium) and hence are highly stable on their own and do not easily react

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19
Q

Why are the Noble gases unreactive?

A

Because they have a full outer shell and therefore do not readily react

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20
Q

What is Neon used for?

A

For glowing, neon signs with orange light

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21
Q

What is Argon used for?

A

For glowing, neon signs with blue/green light

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22
Q

What is Helium used for?

A

For breathing apparators because oxygen can be poisonous by itself, so it has to be mixed

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23
Q

What is Krypton used for?

A

Lights and photographic flash guns

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24
Q

What is Xenon used for?

A

For lights and lasers

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25
Q

What is Radon used for?

A

For cancer therapy

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26
Q

Why are noble gases useful?

A

They are stable and unreactive

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27
Q

What are ions?

A

Charged particles

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28
Q

What is the trend of the boiling points of noble gases?

A

As you go down the group, the boiling point increases

29
Q

What are Group 1 metals also called?

A

Alkali metals

30
Q

How many electrons do Group 1 metals have in their outer shell?

31
Q

What is the product of a metal + water?

A

Metal hydroxide + hydrogen

32
Q

Are metals found to the right or left of the periodic table?

A

To the left

33
Q

Do non metal oxides and water react to form acidic or basic solutions?

A

Acidic (pH lower than 7)

34
Q

Do metal oxides and water react to form acidic or basic solutions?

A

Basic (pH higher than 7)

35
Q

What is a base?

A

A substance that can react with acids and neutralise them

36
Q

What is the trend of reactivity in Group 1 metals?

A

As you go down the group, the metals become more and more reactive

37
Q

Why does the reactivity of Group 1 metals become stronger as you go down the group?

A
  • the atoms get larger as you go down the group
  • the outer electron gets further from the nucleus as you go down the group so the attraction between the nucleus and outer electron gets weaker as you go down the group - so the electron is more easily lost
38
Q

Why do the Group 1 metals react similarly in water?

A

Because they all have one electron in their outer shell

39
Q

What are the halogens?

A

Fluorine, Bromine, Iodine, Chlorine

40
Q

What is the physical state of Fluorine at room temperature?

41
Q

What is the physical state of Bromine at room temperature?

42
Q

What is the physical state of Iodine at room temperature?

43
Q

What is the physical state of Chlorine at room temperature?

44
Q

What is the colour of Fluorine?

45
Q

What is the colour of Bromine?

46
Q

What is the colour of Iodine?

A

Silver, grey

47
Q

What is the colour of Chlorine?

A

Greenish yellow

48
Q

What group are the halogens?

49
Q

What are trends in physical properties in halogens?

A

As you go down the group, the states go from gas to liquid to solid
The boiling points increase as you go down the group

50
Q

What is the trend in colour in the halogens?

A

As you go down the group, they become darker

51
Q

Are halogens metals or non metals?

A

Non-metals

52
Q

Are the halogens monatomic or diatomic?

A

Diatomic - they are made up of pairs of molecules

53
Q

What are displacement reactions in halogens?

A
  • the more reactive halogen will replace the less reactive halogen in a reaction
  • the metal in the reaction will stay the same
  • e.g chlorine + potassium bromide ➡️ potassium chloride + bromine
  • this can show us which halogen in a reaction is more reactive
54
Q

What happens to iodine when it is heated?

A

It turns into a purple gas

55
Q

What is the trend of reactivity in halogens?

A

As you go down the group, the halogens become less reactive

56
Q

What is the equation for when halogens and metals react?

A

Metal + halogen ➡️ metal halide

57
Q

What are the metals between groups 2 and 3 called?

A

Transition metals

58
Q

Why are group 1 metals unusual?

A

They have low melting points

59
Q

What gas is produced when group 1 metals react with water?

60
Q

How do we test for hydrogen?

A

a lighted spill will be put out with a squeaky pop if there is hydrogen

61
Q

When group 1 elements react with water, is the solution acidic or alkaline?

62
Q

What are two properties of the Noble gases?

A

They are colourless and odourless

63
Q

What are unusual properties of alkali metals?

A
  • low melting/boiling points
  • very soft and can be easily cut
  • very low densities
64
Q

Describe the reactions of the Group 1 metals (Lithium, Sodium, Potassium, Rhubidium and Cesium) with water

A

Lithium - floats on water surface (floats) fizzes then disappears

Sodium- floats on water surface (floats), fizzes, melts into a ball because of the heat given out by the reaction

Potassium- lilac flame, fizzes on water surface (floats)

Rubidium- explodes, very reactive

Cesium- huge explosion, very reactive

65
Q

What does period number show?

A

Number of electron rings in an element

66
Q

What does group number show?

A

Number of electrons in the outermost electron shell

67
Q

Metals vs non metals: reaction with acids

A

Many metals react with acids, whereas non metals do not

68
Q

Metals vs non metals: type of oxides

A

Metals have basic oxides (a few are amphoteric), whereas non metals have acidic oxides (some are neutral)

Year 9 Chemistry (5 decks)

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