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Chemistry GCSE > The Periodic Table > Flashcards

The Periodic Table Flashcards

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1
Q

What is a group?

A

Elements in the column

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2
Q

What is a period?

A

Elements in a row

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3
Q

Where are metals in the periodic table?

A

On the left and middle

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4
Q

Where are non metals in the periodic table?

A

On the right

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5
Q

Are metals electrically conductive?

A

Yes

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6
Q

Are non metals electrically conductive?

A

No

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7
Q

Are metal oxides acid or alkali?

A

Alkali

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8
Q

Are non metal oxides acid or alkali?

A

Acid

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9
Q

Why do elements in the same group of the periodic table have the same chemical properties?

A

Because they all have the same number of electrons in their outer shell and therefore give away or gain the same amount of electrons when they react with another element

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10
Q

What are the noble gases?

A

A group of inert gases

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11
Q

Why are noble gases extremely unreactive?

A

Because they all have a full outer shell of electrons and therefore have no need to gain or lose any electrons by reacting with another element

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12
Q

Describe the reaction of lithium with water

A

Lithium doesn’t melt but fizzes on the surface of the water and produces an alkaline solution

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13
Q

Describe the reaction of sodium in water

A

Sodium melts into a small ball on the surface of the water giving of hydrogen, producing an alkaline solution. Sodium catches fire with an orange flame on filter paper on top of the water.

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14
Q

Describe the reaction of potassium with water

A

Potassium melts giving off hydrogen which catches fire with a LILAC flame producing an alkaline solution.

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15
Q

How does the melting/boiling point of the group 1 metals change as you go down?

A

It decreases, i.e. Lithium is highest

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16
Q

How does the density of group 1 metals change as you go down the group?

A

It increases, i.e. lithium is least dense

Think about how lithium sodium and potassium are all less dense than water and float on it

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17
Q

How should you store group 1 metals and why?

A

Lithium, sodium and potassium should all be stored on oil because they all react quickly with air to form oxides and violently with water.

Rubidium and caesium are so reactivw that they have to be stored in a sealed glass container to stop any possibility of oxygen getting to them.

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18
Q

What colour are group 1 metal ions?

And so what colour are their compounds?

A

colourless

colourless or white unless they are paired with a coloured negative ion

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19
Q

How does the reactivity change as you go further down the group 1?

A

The elements become more reactive as you go further down the group

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20
Q

In conclusion group 1 elements:

(8)

A
  • are metals
  • are soft with melting points and densities that are very low for metals
  • have to be stored out of contact with air and water
  • react rapidly with air to form coatings of the metal oxide
  • react with water to produce an alkaline solution of the metal hydroxide and hydrogen gas
  • increase in reactivity as you go down the group
  • form compounds in which the metal has a 1+ ion
  • have mainly white compounds which dissolve to produce colourless solutions
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21
Q

What are the alkali metals?

A

Group 1 metals

22
Q

Why do elements in group 1 get more reactive as you move further down the group?

A

Because the outer electron is further from the nucleus which means the attraction between the nucleus and electrons is less and so the electron is more easily lost.

23
Q

What is the colour and state of chlorine at room temperature?

A

Green gas

24
Q

What is the colour and state of bromine at room temperature?

A

Brown liquid

25
Q

What is the colour and state of iodine at room temperature?

A

Grey solid

26
Q

Predict the properties of other halogens in this group

A

Black/grey solid 7 outer shell electrons Less reactive than other halogens

27
Q

How does the reactivity change in group 7?

A

Elements become less reactive as you go further down the group

28
Q

Why do elements in group 7 become less reactive as you go further down the group?

A

Because it’s harder to gain an extra electron because the outer shell is further from the nucleus and so there is less attraction.

29
Q

How are the halogens dangerous?

A

Fluorine is extremely reactive.

They all have very poisonous vapours and so should be handled in a fume cupboard.

Liquid bromine is corrosive

30
Q

Describe an experiment to show that a more reactive halogen will displace a less reactive halogen and form a solution of one of its salts.

A

Sodium bromide + chlorine = sodium chloride + bromine

Sodium iodide + chlorine = sodium chloride + iodine

31
Q

Make this equation into an ionic equation 2Na+ + 2Br- + Cl2 = 2Na+ + 2Cl- + Br2

A

2Br- + Cl2 = 2Cl- + Br2

32
Q

What are these displacement reactions known as?

A

Redox reactions

33
Q

In the reaction with sodium bromide and chlorine which element has been oxidised and which one has been reduced?

A

Bromide has been OXIDISED Chlorine has been REDUCED

34
Q

What is the atomic number?

A

The number of protons in the atoms of the element.

35
Q

Physical noble gas properties

A

The noble gases are all colourless, monatomic gases; this means their molecules consist of single atoms.

36
Q

Differences between metals and non-metals

A

Metals conduct electricity and heat Are shiny when polished and malleable Usually solids with high melting points Oxides which are alkaline Poor conductors of heat, don’t usually conduct electricity Have oxides which are acidic or neutral Usually brittle as solids Tend to have low melting and boiling points

37
Q

What happens to the melting point of group 1 metals as you go down the group?

A

Gets lower

38
Q

Why are group 1 metals stored in oil?

A

Because they react with water vapour and oxygen in the air.

39
Q

What does it mean if there are bubbles in a beaker of oil containing a group 1 metal?

A

There must have been a tiny bit of water in the oil.

40
Q

What is the periodic table arranged in the order of?

A

The atomic (proton) numbers of the elements.

41
Q

What colour are the compounds of group 1 elements usually?

A

White or colourless

42
Q

Fluorine at room temp

A

Yellow gas

43
Q

why must you be careful with halogens?

A

They have coloured poisonous vapours.

44
Q

LEARN HOW TO DRAW A METAL STRUCTURE AND ALL THE DIAGRAMS

A

Ugh ok fine

45
Q

In conclusion group 7 elements:

(7)

A
  • Have diatomic molecules, X2
  • Go from gases to liquid to solid as you move down the group
  • Have coloured, poisonous vapours
  • Form ionic salts with metals and covalent compounds with non-metals
  • become less reactive as you go down the group
  • are oxidising agents with oxidising ability decreasing down the group
  • will displace elements lower down the group from their salts
46
Q

Generally, what are the properties of the transition metals?

A

All typically metallic elements

good conductors of heat and electricity

Workable, strong and mostly with high densities

With the exception of liquid mercury they all have fairly high to very high melting points

47
Q

are transition metals more or less reactive than group 1 metals?

A

much less reactive and so they don’t react as rapidly with air or water

48
Q

What are the physical properties of the compounds of transition elements?

A

They usually form coloured compounds

49
Q

Transition metals are often useful catalysts, name 3 useful transition metals and their compounds that are useful catalysts:

A
  • iron in the manufacture of ammonia
  • vanadium (V) oxide, V2O5, in the manufacture of sulfuric acid
  • manganese (IV) oxide, MnO2, in the decomposition of hydrogen peroxide.
50
Q
A

Chemistry GCSE (21 decks)

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