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A-level Chemistry > EL 7 - Blood, sweat, and seas > Flashcards

EL 7 - Blood, sweat, and seas Flashcards

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1
Q

What reactants produce magnesium sulfate?

A

sulfuric acid + magnesium

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2
Q

What reactants produce lithium chloride?

A

hydrochloric acid + lithium oxide

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3
Q

What reactants produce barium sulfate?

A

barium chloride + magnesium sulfate

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4
Q

What reactants produce sodium ethanoate?

A

ethanoic acid + sodium carbonate

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5
Q

What reactants produce ammonium nitrate?

A

nitric acid + ammonium hydroxide

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6
Q

Give an example of a use of magnesium sulfate

A

bath salts

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7
Q

Give an example of a use of lithium chloride

A

lithium batteries

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8
Q

Give an example of a use of barium sulfate

A

‘barium meal’ shows up soft tissue on x-ray

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9
Q

Give an example of a use of sodium ethanoate

A

hand warmers

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10
Q

Give an example of a use of ammonium nitrate

A

fertiliser

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11
Q

Name all of the period 3 elements (in order)

A

Na, Mg, Al, Si, P, S, Cl and Ar

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12
Q

What do Na and Mg oxides (basic oxides) produce when they are added to water?

A

An alkali

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13
Q

How can aluminium oxide be described (what type of oxide)?

A

An amphoteric oxide - can react with acids/alkalis

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14
Q

What do Al and Si oxides produce when added to water?

A

The products are the same as the reactants as both Al and Si oxides don’t dissolve in water

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15
Q

What type of oxides are Na and Mg oxide?

A

basic oxides

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16
Q

What types of oxides are Si, P, S and Cl oxide?

A

acid oxides

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17
Q

What do Si, P, S and Cl oxides produce when they are added to water?

A

An acid

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18
Q

Define electronegativity

A

The tendency of an element to attract electrons in a covalent bond

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19
Q

How would you describe the difference in the electronegativity of ionic bonds?

A

Big difference in electronegativity

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20
Q

How would you describe the difference in the electronegativity of polar covalent bonds?

A

Medium

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21
Q

How would you describe the difference in the electronegativity of covalent bonds?

A

Small

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22
Q

What does an oxyanion consist of?

A

XOy^z-
X: another element
y: no. of oxygen atoms
z-: negative ion

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23
Q

What is the difference between a cation and an anion?

A

Cation: positive ion
Anion: negative ion

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24
Q

What products are made from acid + alkali?

A

salt + water

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25
Q

What products are made from acid + base?

A

salt + water

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26
Q

What products are made from acid + carbonate?

A

salt + water + carbon dioxide

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27
Q

What products are made from acid + metal?

A

salt + hydrogen

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28
Q

Many ionic substances dissolve in water but which ones don’t?

A
  • barium, calcium, lead and silver sulfates
  • silver + lead halides
  • all metal carbonates
  • metal hydroxides (except group 1 and ammonium hydroxides)
29
Q

What happens when ionic substances dissolve and what does this allow them to do?

A

The ions become surrounded by water molecules and spread out through the solution.
Once separated, behave independently of each other.
This presence of hydrated ions in solution explains why aqueous solutions of salts can conduct electricity.

30
Q

What are spectator ions?

A

The ions that are non involved in the reaction (+ not part of the ionic equation)

31
Q

What is ionic precipitation?

A

A suspension of solid particles is produced by a chemical reaction in solution

32
Q

Name the solution that is added to Cu2+, the name of the precipitate formed and what colour it is

A

Solution added: sodium hydroxide
Precipitate formed: copper hydroxide
Colour of precipitate: blue

33
Q

Name the solution that is added to Fe2+, the name of the precipitate formed and what colour it is

A

Solution added: sodium hydroxide
Precipitate formed: iron (II) hydroxide
Colour of precipitate: (dirty) green

34
Q

Name the solution that is added to Fe^3+, the name of the precipitate formed and what colour it is

A

Solution added: sodium hydroxide
Precipitate formed: iron(III) hydroxide
Colour of precipitate: orange/brown

35
Q

Name the solution that is added to Pb^2+, the name of the precipitate formed and what colour it is

A

Solution added: potassium iodide
Precipitate formed: lead iodide
Colour of precipitate: bright yellow

36
Q

Name the solution that is added to Cl^-, the name of the precipitate formed and what colour it is

A

Solution added: silver nitrate
Precipitate formed: silver chloride
Colour of precipitate: white

37
Q

Name the solution that is added to Br^-, the name of the precipitate formed and what colour it is

A

Solution added: silver nitrate
Precipitate formed: silver bromide
Colour of precipitate: cream

38
Q

Name the solution that is added to I^-, the name of the precipitate formed and what colour it is

A

Solution added: silver nitrate
Precipitate formed: silver iodide
Colour of precipitate: pale yellow

39
Q

Name the solution that is added to SO4^2-, the name of the precipitate formed and what colour it is

A

Solution added: barium chloride
Precipitate formed: barium sulfate
Colour of precipitate: white

40
Q

Give the ionic equation of Cu and sodium hydroxide

A

Cu^2+(aq) + 2OH^-(aq) -> Cu(OH)v2(s)

41
Q

Give the ionic equation of sulfate and barium chloride

A

Ba^2+(aq) + SOv4^2- -> BaSOv4(s)

42
Q

Give the ionic equation of iodine and silver nitrate

A

Ag^+(aq) + I^-(aq) -> AgI(s)

43
Q

What shape do ionic compounds often form?

A

lattice + regularly shaped crystals

44
Q

What substances have an ionic structure?

A

Compounds of metals with non-metals

45
Q

What substances have a covalent network structure?

A

Some elements in group 4 and some of their compounds

46
Q

What substances have a metallic structure?

A

Metals

47
Q

What substances have a simple molecular structure?

A

Some non-metal elements and some non-metal/non-metal compounds

48
Q

What substances have a macromolecular structure?

A

Polymers

49
Q

Give an example of a compound that has an ionic structure

A

NaCl and CaO

50
Q

Give an example of a compound that has a covalent structure

A

Diamond, graphite and silica

51
Q

Give an example of a compound that has a metallic structure

A

Na, Cu and Fe

52
Q

Give an example of a compound that has a simple molecular structure

A

COv2, Clv2 and Hv2O

53
Q

Give an example of a compound that has a macromolecular structure

A

poly(ethene), nylon, proteins and DNA

54
Q

What type of particles does an ionic structure contain?

A

ions

55
Q

What type of particles does a covalent network contain?

A

atoms

56
Q

What type of particles does a metallic structure contain?

A

positive ions surrounded by delocalised electrons

57
Q

What type of particles does a simple molecular structure contain?

A

small molecules

58
Q

What type of particles does a macromolecular structure contain?

A

long-chain molecules

59
Q

How are the particles bonded in an ionic structure?

A

Strong ionic bonds - attraction between oppositely charged ions

60
Q

How are the particles bonded in a covalent structure?

A

Strong covalent bonds - attraction of atom’s nuclei for shared electrons

61
Q

How are the particles bonded in a metallic structure?

A

Strong metallic bonds - attraction of atom’s nuclei for delocalised electrons

62
Q

How are the particles bonded in simple molecular structure?

A

Weak intermolecular bonds between molecules - strong covalent bonds between the atoms within molecules

63
Q

How are the particles bonded in a macromolecular structure?

A

Weak intermolecular bonds between the atoms within molecules - strong covalent bonds between the atoms within the molecules

64
Q

What are the typical properties/boiling or melting points of ionic, covalent (network), metallic, simple molecular and macromolecular structures?

A

Ionic: high
Covalent (network): very high
Metallic: generally high (except mercury)
Simple molecular: low
Macromolecular: moderate - often decompose on heating

65
Q

What is the hardness of an ionic, covalent (network), metallic, simple molecular and macromolecular structure?

A

Ionic: hard but brittle
Covalent (network): very hard (if three-dimensional)
Metallic: hard but malleable (except mercury)
Simple molecular: soft
Macromolecular: variable - many are soft but often flexible

66
Q

What is the electrical conductivity of ionic, covalent (network), metallic, simple molecular and macromolecular structures?

A

Ionic: electrolytes conduct when molten or dissolved in water
Covalent (network): do not normally conduct (except graphite)
Metallic: conduct when solid or liquid
Simple molecular: do not conduct
Macromolecular: do not normally conduct

67
Q

What is the solubility of an ionic, covalent (network), metallic, simple molecular and macromolecular structure like in water?

A 
Ionic: often soluble
Covalent (network): insoluble
Metallic: insoluble (but some react)
Simple molecular: usually insoluble, unless molecules contain groups which can hydrogen bond with water 
Macromolecular: usually insoluble
68
Q

What is the solubility of an ionic, covalent (network), metallic, simple molecular and macromolecular structure like in non-polar solvents (e.g hexane)?

A 
Ionic: insoluble
Covalent (network): insoluble
Metallic: insoluble
Simple molecular: usually soluble 
Macromolecular: sometimes soluble

A-level Chemistry (21 decks)

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