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Chemistry A-Level > EL 6, 7 > Flashcards

EL 6, 7 Flashcards

1
Q

what is the relative atomic mass of an element

A
  • the mass of an atom relative to carbon-12
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2
Q

what is avogadros constant and what does it mean

A
  • 6.02 x 10^23
  • that is how many particles one mole of any substance will contain
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3
Q

how do you calculate the NoM

A

mass / RFM

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4
Q

what is the difference between the molecular formula and the empirical formula

A
  • molecular formula tells you the actual amount of atoms in the molecule
  • empirical formula is the simplified ratio of the molecular formula
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5
Q

what is water of crystallisation

A
  • the molecules of water fitted within some crystals of ionic lattices in a regular manner
  • this means that the crystals are hydrated
  • when they are heated, the water is removed as steam and the solid is anhydrous
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6
Q

what are the factors that can reduce percentage yield

A
  • loss of products from reactant vessels
  • side reactions producing unwanted products
  • impurities in the reactants
  • changes in temperature and pressure
  • if the reaction is in an equilibrium system
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7
Q

how do you calculate percentage yield

A

( experimental yield / theoretical yield ) x 100

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8
Q

what is a:
- cation
- anion

A
  • positively charged ion
  • negatively charged ion
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9
Q

describe ionic bonding

A
  • occurs when a metal reacts with a non metal
  • electrons are transferred from the metal atom to the non metal, giving them a stable electronic structure
  • hold together by their opposite charges in an electrostatic bond
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10
Q

what is the formula are charge of the following ions:
- ammonium
- nitrate
- oxide
- lithium
- hydrogen carbonate
- sulphate

A
  • NH4 +
  • NO3 -
  • O 2-
  • Li +
  • HCO3 -
  • SO4 2-
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11
Q

what forms when you react the following:
- acid + alkali
- acid + base
- acid + carbonate
- acid + metal

A
  1. salt + water
  2. salt + water
  3. salt + water + carbo dioxide
  4. salt + hydrogen
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12
Q
  • what are the ions that are EXCEPTIONS and are not soluble
A
  • barium, calcium, lead and silver sulphates
  • silver and lead halides
  • all metal carbonates
  • metal hydroxides (NOT group 1, or ammonium hydroxide)
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13
Q

what happens when you react sodium chloride and silver nitrate

A
  • you form a white precipitate of silver chloride
  • the only ions that get involved in the reaction is Ag+ and Cl-
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14
Q

what are spectator ions

A

Ions that don’t get involved in an ionic reaction

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15
Q

how do you identify copper and iron ions

A
  • add sodium hydroxide to the sample
  • COPPER, copper hydroxide precipitate, blue
  • IRON (II), iron (II) hydroxide, dirty green
  • IRON (III), iron (III) hydroxide, orange/brown
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16
Q

how do you identify lead and sulphate ions

A

LEAD
- add potassium iodide
- lead iodide formed
- bright yellow precipitate formed
SULPHATE
- add barium chloride
- barium sulphate formed
- white precipitate

17
Q

how do you identify chloride, bromide and iodide ions

A
  • add silver nitrate
  • CHLORIDE, silver chloride, white precipitate
  • BROMIDE, silver bromide, cream precipitate
  • IODIDE, silver iodide, pale yellow precipitate
18
Q

describe the structure and properties of ionic structures

A
  • typically solids at room temperature and pressure
  • they have lattice structures consisting of repeating positive and negative ions in all three dimensions
  • so they form regularly shaped crystals
19
Q

why can molten ionic compounds conduct electricity

A
  • once melted, the ions in ionic compounds are free to move around
20
Q

what is large ionic bonding

A
  • the electrostatic attractions of oppositely charged ions over comes any repulsion between ions of the same charge, holding together the lattice structure
21
Q

describe the structure and bonding of a metal, and how it affects its properties

A
  • they have a lattice structure
  • metals appear in a giant lattice structure of metal cations in a sea of delocalised electrons
  • electrons are free to move
  • structure is held together by the attraction of metal cations and delocalised electrons
22
Q

describe the properties and structure of covalent networks

A
  • large covalently bonded networks
  • they have strong covalent bonds between the atoms
  • very high melting and boiling points
  • insoluble in water and do not conduct electricity

Chemistry A-Level (26 decks)

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