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Chemistry Flashcards 1.0

front 1

Structure of diamond

back 1

A tetrahedral shape, with each carbon atom bonded to 4 other carbons with strong covalent bonds.

front 2

Graphite structure

back 2

Layers of carbon atoms in a hexagon arrangement with weak intermolecular forces between them. Each carbon atom is bonded to 3 other carbons with covalent bonds with one free (delocalised) electron per carbon atom.

front 3

The structure of silicon dioxide

back 3

A tetrahedral structure where each silicon atom is bonded to 4 oxygen atoms, and each oxygen atom is bonded to 2 silicon atoms.

front 4

Why diamond is a cutting tool.

back 4

Rigid three-dimensional structure with many strong covalent bonds making it very hard.

front 5

Similarities od diamond and sio2

back 5

High melting and boiling points as strong covalent bonds, very hard as three-dimensional structure + strong bonds, no delocalised electrons so can't conduct

front 6

Metals are malleable and ductile because...

back 6

The layers of ions can slide over each other but are still held together by the delocalised electrons so can be bent into shape (malleable) and stretched out (ductile).

front 7

Ionic bond meaning

back 7

An electrostatic force between oppositely charged ions.

front 8

Covalent bond meaning

back 8

When a pair of electrons is shared between two atoms to gain full outer shells of electrons.

front 9

precipitation reaction

back 9

Two soluble reactants form an insoluble product and a soluble product.

front 10

Molecular formula

back 10

The number and type of different atoms in one molecule.

front 11

Relative atomic mass

back 11

The average mass of the isotopes of an element compared the mass of an atom of carbon-12.

front 12

Avogadro constant (number of particles one mole contains)

back 12

6.02 × 10(23)

front 13

Acid with metal

back 13

Salt and hydrogen

front 14

Acid with base

back 14

Neutralise to salt and water

front 15

Acid with carbonates

back 15

Salt, CO2, and water.

front 16

Acid properties

back 16

Sour, corrosive, below 7 PH, proton donor. Presence of H+ ions makes it acidic.

front 17

Alkali and ammonium salt

back 17

Water, salt and ammonia gas.

front 18

Symbol equation for to show HCl is a strong acid

back 18

HCl (aq) → H+(aq) + Cl –(aq)

front 19

Symbol equation to show ethnic acid is a week acid

back 19

CH3COOH(aq) ⇌ H+(aq) + CH3COO–(aq)

front 20

Neutral oxides.

back 20

carbon monoxide and nitrate oxides.

front 21

Preparing salt by titration.

back 21

Using pipette measure alkali into conical flask adding methyl orange. Add acid to burette noting starting volume. Slowly add acid to alkali until turns red. Record finishing volume and calculate how much acid was added. Add this amount of acid with same amount of alkali as first measured out without indicator. Form saturated solution by partially evaporating, then crystallise and dry.

front 22

Preparing salt with solid metal, base or carbonate.

back 22

Heat dilute acid in beaker over a Bunsen burner. Add insoluble metal, base or carbonate until in excess. Filter then evaporate into saturated solution. Leave to crystallise and dry crystals.

front 23

Hydrated substance

back 23

A substance chemically combined with water.

front 24

The term water of crystallisation.

back 24

The water molecules present in hydrated crystals.

front 25

Preparation of insoluble salts

back 25

Precipitation reaction: Dissolve soluble salts in water and mix together using a stirring rod in a beaker. Filter and wash filtrate with water to remove traces of other solutions. Dry.

front 26

Appearance of bromine, iodine and chlorine.

back 26

Bromine - red-brown liquid.

Chlorine - Yellow-green gas

Iodine - Grey black solid.

front 27

Metal and steam reaction

back 27

Form solid metal oxide and hydrogen gas.

front 28

Aluminium in overhead cables

back 28

Good conductivity and low density

front 29

Copper in overhead cables

back 29

Good conductivity and ductility.

front 30

Aluminium in food containers

back 30

Resistant to corrosion.

front 31

Brass made out of...

back 31

Mixture of copper and zinc.

front 32

Stainless steel made of...

back 32

Mixture of iron and other elements such as chromium, nickel and carbon.

front 33

Stainless steel is used for cutlery because...

back 33

It's hardness and resistance to corrosion.

front 34

Brass is used for instruments because...

back 34

Its resistance to corrosion and good malleability.

front 35

State the order of reactivity.

back 35

Potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold.

front 36

Reaction of calcium with water.

back 36

Fizzing, disappears, no flame, white precipitate formed.

front 37

Magnesium with steam reaction

back 37

Burns in steam to form white magnesium oxide and hydrogen.

front 38

Magnesium and hydrochloric acid.

back 38

Reacts rapidly and vigorously producing magnesium chloride and hydrogen gas.

front 39

Zinc and hydrochloric acid.

back 39

Also reacts but at a slower rate than magnesium, producing zinc chloride and hydrogen gas.

front 40

Iron and hydrochloric acid.

back 40

Reacts slowly forming iron(II) chloride and hydrogen gas.

front 41

Copper and hydrochloric acid.

back 41

Barely reacts.

front 42

Ionic half equations for extraction of aluminium

back 42

Al3+ + 3e- → Al

2O2- → O2 + 4e-

front 43

Water from natural sources may contain substances, including...

and which are helpful and not.

back 43

Dissolved oxygen, metal compounds, plastics, sewage, harmful microbes, nitrates from fertilisers, phosphates from fertilisers and detergents.

Dissolved oxygen for aquatic life, some metal compounds provide essential minerals for life but others are toxic, and nitrates and phosphates lead to deoxygenation of water and damage to aquatic life.

front 44

Steps of filtration

back 44

Sedimentation and filtration, use of carbon to remove tastes and odours, chlorination to kill microbes.

front 45

How is sulphur dioxide formed

back 45

From the combustion of fossil fuels which contain sulfur compounds.

front 46

Catalytic converters reaction.

back 46

2CO + 2NO → 2CO2 + N2

front 47

State the symbol equation for photosynthesis.

back 47

6CO2 + 6H2O → C6H12O6 + 6O2

front 48

What is kerosene / parrafin used for?

back 48

Jet fuel

front 49

What fuel oil fraction is used for.

back 49

Fuel for ships and home heating systems.

front 50

What the lubricating oil fraction is used for.

back 50

Lubricants, waxes and polishes.

front 51

Reactivity of alkanes

back 51

Generally unreactive, except in terms of combustion and substitution by chlorine.

front 52

Describe the manufacture of alkenes.

back 52

Cracking of larger alkane molecules using a high temperature and a catalyst

front 53

Describe the reasons for the cracking of larger alkane molecules.

back 53

Matches supply with demand, and alkenes are useful as feedstock in the photochemical industry.

front 54

Describe the properties of alkenes in terms of addition reactions with hydrogen with structural formula.

back 54

An alkane is formed, a hydrogen atom gets added to each bond where the C=C bond is broken.

front 55

Describe the properties of alkenes in terms of addition reactions with hydrogen in the presence of a nickel catalyst, with structural formula.

back 55

An alkane is formed, a hydrogen atom gets added to each bond where the C=C bond is broken.

front 56

Describe the properties of alkenes in terms of addition reactions with steam in the presence of an acid catalyst.

back 56

An alcohol is formed, it is also a hydration reaction as a water molecule is being added, C=C bond breaks and one water molecule is added to turn eg (ethene into ethanol or propane into propanol and so on).

front 57

Describe the manufacture of ethanol by fermentation.

back 57

Fermentation of aqueous glucose at 25–35 °C in the presence of yeast and in the absence of oxygen.

front 58

Describe the manufacture of ethanol by steam.

back 58

Catalytic addition of steam to ethene, at 300°C and 60 atm in the presence of an acid catalyst.

front 59

Describe the combustion of ethanol.

back 59

Ethanol burns with an almost invisible blue flame, burns cleanly, and without strong odours.

Alcohols undergo combustion to form carbon dioxide and water.

front 60

Describe the advantages and disadvantages of the manufacture of ethanol by:

(a) fermentation
(b) catalytic addition of steam to ethene

back 60

Fermentation: simple equipment and low temperatures required which saves money, and uses renewable recourses. It however produces greenhouse gas co2, is very slow and produces a dilute solution that needs further processing, also it is made in batches.

Hydration: Complex set up, uses non-renewable recourses but produces no greenhouse gases, is a fast continues process that produces pure ethanol, but high temperatures and pressures required increasing the energy input and cost.

front 61

Products of ethanoic acid and:

a. Metal 2CH3COOH + Mg → ?

b. base CH₃COOH + NaOH → ?

c. Carbonates 2CH₃COOH + Na₂CO₃ → ?

back 61

The name is the name of the metal before ethanoate.

a. (CH₃COO)₂Mg + H₂

b. CH₃COONa + H₂O

c. 2CH₃COONa + CO₂ + H₂O

front 62

Describe the formation of ethanoic acid by the oxidation of ethanol with acidified aqueous potassium manganate(VII).

back 62

Heating ethanol and acidified aqueous potassium manganate(VII) in the presence of an acid in a vessel with a condenser attached to stop the alcohol with its low boiling point escaping. goes from colourless to purple.

CH3CH2OH (aq) + 2[O] → CH3COOH (aq) + H2O (l)

front 63

Describe the formation of ethanoic acid by the oxidation of ethanol by bacterial oxidation during vinegar production.

back 63

Acetobacter bacteria uses atmospheric oxygen from air to oxidise ethanol in wine, producing a weak solution of ethanoic acid (vinegar) this is what makes one have an acidic vinegary taste after it has been opened for a while.

front 64

Ester reaction (ethanoic acid and ethanol)

back 64

Ethanoic acid will react with ethanol in the presence of concentrated sulfuric acid (catalyst) to form ethyl ethanoate and water.

front 65

Describe how the properties of plastics have implications for their disposal.

back 65

Many polymers are chemically unreactive so they are non-biodegradable and fill up land fill space and oceans. Many also create toxic gas if burned so incineration is very bad.

front 66

What a polyamide is made from and its link.

back 66

A dicarboxylic acid and a diamine.

front 67

What a polyester is made of and its link.

back 67

From a dicarboxylic acid and a diol.

front 68

draw the structure of nylon, a polyamide.

back 68

front 69

draw the structure of PET, a polyester

back 69

front 70

General structure of amino acid monomers.

back 70

where R represents different types of side chain

front 71

Draw the structure of proteins.

back 71

front 72

Test for nitrate, NO3 – ion.

back 72

Reduction with aluminium foil and aqueous sodium hydroxide and then testing for ammonia gas.

front 73

Test for sulfate, SO4 2-

back 73

Acidifying with dilute nitric acid and then adding aqueous barium nitrate.

front 74

Test for sulfite, SO3 2-

back 74

Reaction with acidified aqueous potassium manganate(VII).

front 75

Identify test and result for each.

(a) aluminium, Al 3+

(b) ammonium, NH4+

(c) calcium, Ca2+

(d) chromium(III), Cr3+

(e) copper(II), Cu2+

(f) iron(II), Fe2+

(g) iron(III), Fe3+

(h) zinc, Zn2+

back 75

a. Dilute NaOH or ammonia, white precipitate (soluble in excess NaOH, insoluble in excess ammonia)

b. Dilute warm NaOH, ammonia produced

c. Dilute NaOH, white precipitate (insoluble in excess NaOH)

d. Dilute NaOH or ammonia solution, grey-green precipitate (soluble in excess NaOH, insoluble in excess ammonia)

e. Dilute NaOH or ammonia solution, light blue precipitate (insoluble in excess NaOH, soluble in excess ammonia)

f. Dilute NaOH or ammonia solution, green precipitate (insoluble in excess both)

g. Dilute NaOH or ammonia solution, red-brown precipitate (insoluble in excess both)

h. Dilute NaOH or ammonia solution, white precipitate (soluble in excess both)