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Z Chemistry GCSE > Periodic Table > Flashcards

Periodic Table Flashcards

1
Q

What are the qualities of metals?

A
  1. Metal oxides are basic
  2. Metals can conduct electricity
    They have positive ions
    (left of the zig zag)
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2
Q

What are the properties of non metals?

A
  1. Non-metal oxides are acidic
  2. Non-metals are poor conductor of electricity
    (right of the zig-zag)
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3
Q

What are the physical properties of noble gases?

A
  1. All colourless and odourless
  2. MONOatomic gases as their molecules consist of a single atom.
  3. Density increases as the atoms get heavier
  4. Bp increases as the intermolecular attractions between one molecule and its neighbour gets stronger as the atoms get bigger meaning more energy is needed to break the stronger attractions.
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4
Q

What are the chemical properties of noble gases?

A
  1. Don’t form ions as their outer shell is already full and so they are stable and so there is no need to loose or gain electrons
  2. Generally unreactive as too much energy is needed to rearrange the full shells to produce the single electron that as atom needs if it is to form simple covalent bonds by sharing electrons
  3. Family of inert gases
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5
Q

What are the properties of Group 1 (Alkali Metals)

A
  • As you go down the reactivity increase and the melting and boiling point increases
  • They are stored in oil as they would react with the oxygen in the air forming a coating of the metal oxide
  • They are soft and slippery (unlike ‘typical metals’)
  • Shiny and silver when freshly cut but tarnish within seconds on exposure to air
  • Have mainly white compounds which dissolve to produce colourless solutions (and all produce and alkaline solution)
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6
Q

What happens when a metal reacts with water?

A

metal hydroxide and hydrogen is produced

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7
Q

Describe the reaction of lithium with water

A
  • Moves slowly around the surface
  • It floats (as it is less dense than water)
  • It does not melt (since melting point is higher than sodiums and the heat is not produced so quickly)
  • It fizzes
  • No fire is produced
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8
Q

Describe the reaction of sodium with water

A
  • Slow
  • It floats (as it is less dense than water)
  • It does melt (as it has a low melting point and lots of heat is produced)
  • It vigorously fizzes
  • No fire is produced
  • There was a fire with filter paper and a yellow/orange flame is produced. This is because more hydrogen becomes trapped and so there is a higher concentration of hydrogen around the reaction and it is very flammable
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9
Q

Describe the reaction of potassium with water

A
  • Faster
  • It floats
  • It melts quickly
  • Very vigorous fizzing
  • It catches fire and a lilac flame is produced. The large amount of heat produced ignited the hydrogen
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10
Q

Why do you not react alkali metals with acids? What happens as you go down group 1?

A
  • The reactions would be even more vigorous and the acid (which is harmful) would spray out
  • The elements in group 1 get more reactive as the atomic number increases
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11
Q

What is the equation of alkali metals reacting with hydrogen? How can you tell those are the products formed?

A

2Na (s) + 2H2O (l) –> 2NaOH (aq) + H2 (g)
The universal indicator will turn purple
There was fizzing which shows the presence of hydrogen

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12
Q

What are the properties of Group 7 (Halogens)

A
  • As you go down group 7 the mp and bp increases as the molecules become bigger and so the number of electrons increases so the intermolecular forces become stronger, which need a greater amount of energy to be overcome and so the boiling point and melting point increase
  • Reactivity decreases
  • Oxidising ability decreases
  • Non-metallic elements with diatomic molecules
  • They are poor conductors of electricity and heat
  • When they are a solid their crystals will be brittle
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13
Q

Describe fluorine

A

State: gas
Colour: yellow
highly reactive

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14
Q

Describe chlorine

A

State: gas
Colour: green

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15
Q

Describe bromine

A

State: liquid
Colour: brown / dark red
corrosive

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16
Q

Describe iodine

A

State: solid
Colour: dark grey (purple vapour)

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17
Q

What happens when halogens react with hydrogen

A

Halogens react with hydrogen to form hydrogen halides

H2 (g) + Br2 (g) –> 2HBr (g)

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18
Q

What are the properties of hydrogen halides?

A
  • All steamy, acidic, poisonous gases
  • The gases are covalently bonded
  • Very soluble in water, reacting with it to produce solutions of acids
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19
Q

Describe the reaction of fluorine with hydrogen

A

Violent explosion, even in the cold and dark

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20
Q

Describe the reaction of chlorine with hydrogen

A

Violent explosion if exposed to a flame or to sunlight

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21
Q

Describe the reaction of bromine with hydrogen

A

Mild explosion if a bromine vapour/hydrogen mixture is exposed to a flame

22
Q

Describe the reaction of iodine with hydrogen

A

Partial reaction to form hydrogen iodide if iodine vapour is heating continuously with hydrogen

23
Q

Why do you not react fluorine or astatine studied in school laboratories?

A
  • Fluorine: very dangerously reactive and it produces an extremely poisonous vapour
  • Astatine: very rare and radiactive
24
Q

Why is there a change in reactivity as you go down the group?

A

The further down group 7 (1) you go the reactivity decreases (increases).
This is because the number of shells increases and so if the outer shell is further from the positive nucleus the attraction between the electrons and positive nucleus is weaker.
Therefore it more difficult to gain an electron and so reactivity decreases (easier to loose an electron so reactivity increases)

25
Q

What happens when you add NaCl to chlorine (displacement reactions: halogens)

A
  • No reaction

- The hexane is colourless

26
Q

What happens when you add NaCl to bromine (displacement reactions: halogens)

A
  • No reaction

- The hexane is orange

27
Q

What happens when you add NaCl to iodine (displacement reactions: halogens)

A
  • No reaction

- The hexane is orange/pink

28
Q

What happens when you add NaBr to chlorine (displacement reactions: halogens)

A
  • Reaction

- The hexane is orange

29
Q

What happens when you add NaBr to bromine (displacement reactions: halogens)

A
  • No reaction

- The hexane is orange

30
Q

What happens when you add NaBr to iodine (displacement reactions: halogens)

A
  • No reaction
  • I2 is brown solution
  • The hexane is orange/pink
31
Q

What happens when you add NaI to chlorine (displacement reactions: halogens)

A
  • Reaction

- The hexane is pink (water is orange)

32
Q

What happens when you add NaI to bromine (displacement reactions: halogens)

A
  • Reaction
  • The iodine solution left is brown
  • The hexane is pink
33
Q

What happens when you add NaCl to iodine (displacement reactions: halogens)

A
  • No reaction
  • The iodine solution is left brown
  • The hexane is orange/pink
34
Q

What is oxidisation?

A

The loss of electrons, the gain of oxygen

35
Q

What is reduction?

A

The gain of electrons, the loss of oxygen

36
Q

What is it called when reduction and oxidation occur at the same time?

A

A redox reaction (in displacement reactions oxidation and reduction happen simultaneously), so these displacement reactions are redox reactions

37
Q

Why does the oxidising ability decrease down group 7?

A

Since the number of shells increase the further down group 7 you go, the incoming electron is further and further away from the positive nucleus. This means that the incoming electron it less strongly attracted, meaning that the ion is less easily formed.
Similarly further up group 7 you go there is a smaller number of shells, so the electrons in the outer shell are more strongly attracted to the positive nucleus. Therefore the incoming electron will be more strongly and readily attracted since the attraction is stronger

38
Q

What are the rules of displacement reactions in halogens?

A
  • A less reactive halogen CANNOT displace more reactive halogen
  • Some mixtures reacted as the halogen added was MORE REACTIVE than the halide in the compound
39
Q

What is the oxidising agent?

A

The substance that accepts electrons and gets reduced

40
Q

What is the reducing agent?

A

The substance that donates electrons and gets oxidised

41
Q

What is the equation for halogen displacement reactions?

A

2NaBr (aq) + Cl2 (aq) –> 2NaCl (aq) + Br2 (aq)
2Br- + Cl2 –> 2Cl- + Br2
Chlorine is reduced
BromIDE is oxidised
(aq) in displacement reactions as we always use solutions. No charge needed on the element

42
Q

Describe the periods

A
  • The rows are called periods

- The properties of the elements change as you go along a period

43
Q

Describe the groups

A
  • The columns are called groups
  • Elements in the same group have similar chemical properties. This is because they have the same number of electrons in their outer shell
  • The properties of the elements (such as reactivity) often gradually change as you go down the group
44
Q

Describe the periodic table

A

-The modern periodic table shows the elements in order of increasing atomic number

45
Q

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

A

They have the same number of electrons in their outermost shell

46
Q

What happens as you go down group 7?

A
  • As the atomic number of the halogens increases, the elements have a darker colour and a higher boiling point, which is why they go from gases at the top of group 7 to solids at the bottom
  • The higher up group 7 an element is the more reactive it is, this is because the shell with the missing electron is nearer to the nucleus, so the pull form the positive nucleus is greater
47
Q

What is the difference between Hydrochloric acid and Hydrogen Chloride gas?

A
  1. Halogens can combine with hydrogen to form hydrogen halides, for example hydrogen chloride and hydrogen bromide
  2. Hydrogen Chloride has the chemical formula HCL and is a gas at room temperature
  3. When hydrogen chloride is dissolved in water the HCL molecules split up into H+ ions and Cl- ions, this process is called dissociation
  4. The solution that is formed is called hydrochloric acid
  5. Hydrochloric acid is an acidic solution because it contains H+ ions
    - If you test a solution of hydrochloric acid with blue litmus paper the paper will turn red/pink
48
Q

What happens when hydrogen chloride is dissolved in methylbenzene?

A
  1. If HCL is dissolved in an organic solvent like methylbenzene, it does not dissociate into H+ ions and Cl- ions
  2. This means there are no H+ ions produced so it is not acidic
  3. If you test a solution of HCL in methylbenzene with blue litmus paper the paper will stay blue. But if there is any moisture on the paper or in the bottle, the the HCL can dissociate and it will behave like an acid again
49
Q

What is a displacement reaction? How would you conduct an experiment?

A
  1. The elements in Group 7 take part in displacement reactions, and this is where a more reactive element displaces/”pushes out” a less reactive element from a compound
  2. For example Chlorine is more reactive than iodine as it is higher up group 7
  3. So if you add chlorine water to potassium iodide solution the chlorine will react with the potassium in the potassium iodide to form potassium chloride
  4. The iodine is displaced from the salt and gets left in the solution, turning it brown
    - Add a few drops of halogen solution to the salt solution and then look for a colour change
50
Q

What colour is hexane in halogens?

A
  1. Chlorine: colourless
  2. Bromine: orange
  3. Iodine: pink
51
Q

What colour are the halogen solutions?

A

The one not in the compound makes the colour of the solution

  1. Chlorine: colourless
  2. Bromine: orange
  3. Iodine: brown

Z Chemistry GCSE (16 decks)

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