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BMAT > chemistry > Flashcards

chemistry Flashcards

1
Q

atomic number=?

A

number of protons

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2
Q

mass number=?

A

number of protons + number of neutrons

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3
Q

how should u write electron configurations in this clapped test?

A

2,8,8,2 (up to calcium)

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4
Q

what Is an isotope (yawn)

A

atoms of an element with the same number of protons but a different number of neutrons.

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5
Q

what are the useful properties of aluminium ?

A

properties: low density, non-toxic, high thermal conductivity, excellent corrosion resistance, can be easily cast, machined and formed (malleable and ductile), non-magnetic, non-sparking

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6
Q

what are some uses of aluminium?

A

cans, foils, kitchen utensils, window frames, beer kegs aeroplane parts, electrical transmission lines (cheaper than copper)

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7
Q

what is iron used for?

A

Most is used to manufacture steel, used in civil engineering (reinforced concrete, girders etc) ,in manufacturing, bridges, electricity pylons, bicycle chains, cutting tools and rifle barrels. stainless steel is v resistant to corrosion and 11% chromium, it’s used in architecture, bearings, cutlery, surgical instruments and jewellery. Iron catalysts are used in the Haber process for producing ammonia. +haemoglobin in blood.

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8
Q

what are the properties of iron?

A

shiny, bright white metal that is soft, malleable, ductile and strong. Its surface is usually discolored by corrosion, since it combines readily with the oxygen of the air in the presence of moisture.

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9
Q

how do copper’s properties relate to its functions?

A

1) Corrosion resistant-pipes, electrical cables, saucepans, radiators, jewellery, statues and parts of buildings
2) Antibacterial-food preparation, hospitals, coins, door knobs
3) Ductile- pipes and wires.
4) alloys easily into brass + bronze
5) can act as a catalyst eg found in some enzymes, one of which is involved in respiration

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10
Q

how do silver’s properties relate to its functions?

A

1) scarcity, brilliant white colour, malleability, ductility, and resistance to atmospheric oxidation-manufacture of coins, ornaments, and jewelry.
2) electrical and thermal conductivity -fabricating printed electrical circuits and as a vapour-deposited coating for electronic conductors.

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11
Q

how do gold’s properties relate to its functions?

A

1) can be beaten into very thin sheets (gold leaf) to be used in art, for decoration and as architectural ornament
2) protecting electrical copper components because it conducts electricity well and does not corrode, which would break the contact.

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12
Q

how is tin used + why/

A

takes a high polish and is used to coat other metals to prevent corrosion, such as in tin cans, which are made of tin-coated steel.Most window glass is made by floating molten glass on molten tin to produce a flat surface. Tin salts sprayed onto glass are used to produce electrically conductive coatings.

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13
Q

what are most metal ores?

A

the oxides of metals

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14
Q

what does the extraction of metals always involve?

A

reduction processes.

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15
Q

what group are the alkali metals in?

A

1

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16
Q

what group are the halogens in?

A

17

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17
Q

what group are the noble gases in?

A

18

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18
Q

what block are the transition metals in?

A

d block

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19
Q

what are the physical and chemical properties of the alkali metals?

A

•shiny
•soft-high ductility
-excellent conductivity of electricity and heat
•silvery
•highly reactive at standard temperature and pressure
•readily lose their outermost electron to form cations with a charge of +1
-low melting points,

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20
Q

what are the physical and chemical properties of the halogens?

A 
low melting points and boiling points
gas to liquid to solid down the group
highly reactive
high electronegativity
poor thermal and electrical conductors
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21
Q

what are the physical and chemical properties of the noble gases?

A

odorless, colorless, monatomic
very low chemical reactivity
low boiling points

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22
Q

what are the common properties of transition metals?

A

coloured ions, multiple stable ions, use as catalysts

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23
Q

what factors affect position of equilibrium + rate at which equilibrium is achieved?

A

concentration+amount of reactants and products
catalyst
temperature
pressure

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24
Q

what is STP?

A

standard temp and pressure-273 K (0° C) and 1 atmosphere.

different to RTP

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25
Q

how many dm3 does a gas occupy at STP?

A

22.4

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26
Q

how do you calculate solubility?

A

Divide the mass of the compound by the mass of the solvent and then multiply by 100 g to calculate the solubility in g/100g

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27
Q

why is % yield never 100%?

A

other, unexpected reactions occur which don’t produce the desired product, not all of the reactants are used in the reaction, or perhaps when the product was removed from the reaction vessel it was not all collected, or it was an equilibrium reaction

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28
Q

on a basic level, oxidation is…

A

gain of oxygen or removal of hydrogen

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29
Q

on a basic level, reduction is…

A

gain of hydrogen or removal of oxygen

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30
Q

what are the 2 disproportionation reactions?

A

Cl2 + H20—> HOCl +HCl

Cl2 + NaOH—> NaCl + NaOCl + H2O

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31
Q

what is disproportionation?

A

a reaction in which the same element is both oxidised and reduced.

32
Q

in terms of electrons, what is oxidation?

A

loss of electrons

33
Q

in terms of electrons, what is reduction?

A

gain of electrons

34
Q

what is a metal?

A

electron donors producing cations

35
Q

how reactive are group 1 metals?

A

h i g h l y

36
Q

what are the physical properties of group 1 metals?

A

soft

low melting + boiling points (for a metal)

37
Q

how are group 1 metals stored and why?

A

under oil, so they don’t react with moist air

38
Q

what does reactivity do down group 1?

A

increases

39
Q

what happens when group 1s react with water?

A

metal hydroxide and hydrogen are formed, gets more vigorous down the group. effervescence and they float and disappear

40
Q

what happens when group 1s up to potassium react with oxygen?

A

burn to form metal oxides

lithium: red flame
sodium: orange
potassium: purple

41
Q

what happens when group 1s after potassium react with oxygen?

A

form superoxide compounds:

M(s)+O2(g)→MO2(s)

42
Q

what happens when group 1s react with halogens?

A

react vigorously to form salts.

43
Q

what is a nonmetal?

A

acceptor of electrons, forming anions

44
Q

what is the reactivity of the halogens like?

A

they’re the most reactive nonmetals.

45
Q

how do you test for bromide, chloride, and iodide ions?

A

add silver nitrate and then dilute then conc ammonia:

chloride: white ppt, dissolves in dilute
bromide: cream ppt, dissolves in conc
iodide: yellow ppt, doesn’t dissolve in either.

46
Q

what is the reactivity of the noble gases like?

A

least reactive of the periodic table.

47
Q

how do chemical procedures separate compounds?

A

by chemical reactions, eg displacement or electrolysis

48
Q

what are mixtures?

A

substances that may be mixed together but are not chemically joined.

49
Q

how are miscible liquids separated?

A

by fractional distillation, because of the differences in boiling points, or (for non volatile liquids) paper chromatography.

50
Q

how are immiscible liquids separated?

A

using a separating funnel.

51
Q

how are soluble solids mixed with insoluble solids separated?

A

dissolving, filtering, evaporating/distilling, crystallisation.

52
Q

what are monoprotic acids + examples?

A

acids which give a single proton or hydrogen ion in aqueous solution, eg HCl, CH3COOH, HNO3

53
Q

what are diprotic acids + examples?

A

acids which release two hydrogen ions in aqueous solution, eg H2SO4, H2CO3

54
Q

what are triprotic acids and examples?

A

acids which release three hydrogen ions in aqueous solution, eg H3PO4

55
Q

what are polyprotic acids?

A

capable of losing more than a single proton per molecule in acid-base reactions.

56
Q

what is a base?

A

lone pair donor/proton acceptor

57
Q

what are acids?

A

species that donate a proton (H+)/ electron pair acceptors

58
Q

what are the properties of acids?

A

conduct electricity
corrosive
produce H+ ions in solution
sour taste

59
Q

what are the properties of bases?

A

bitter taste
conduct electricity
slippery/soapy feel

60
Q

what affects rate of reaction?

A 
concentration
temp
particle size
catalyst
pressure
61
Q

how can rate of reaction be found?

A

by measuring loss of reactant or gain of product over time.

62
Q

what is a catalyst?

A

a substance which alters rate of reaction without being used up.

63
Q

why are alkanes chemically unreactive?

A

the stability of the C-C + C-H bonds

64
Q

what is a condensed formula?

A

when you write it like CH3CH2CH3

65
Q

what is the test for unsaturation?

A

the ability to decolourise bromine water

66
Q

what can addition reactions of alkenes take place with?

A

hydrogen
halogens
hydrogen halides
steam (to form alcohol)

67
Q

what type of reaction is polymerisation?

A

addition reaction

68
Q

what are polymers>

A

giant molecule$

69
Q

what are biodegradable polymers?

A

a specific type of polymer that breaks down after its intended purpose to result in natural byproducts such as gases (CO2, N2), water, biomass, and inorganic salts.

70
Q

what are non biodegradable polymers?

A

polymers that are resistant to environmental degradation + microbes can’t break it down

71
Q

what are the problems with burning polymers?

A

Carbon dioxide is produced, which adds to global warming. Toxic gases are also produced, unless the polymers are incinerated at high temperatures.

72
Q

what are the problems with landfilling polymers?

A

uses up valuable land which then can’t be used for agriculture, natural habitat and development.
the decomposition releases large quantities of dangerous gases, including methane
soil pollution-Chemicals can leak into the soil from the accumulation of waste, and may eventually end up in the water supply.
eyesore, diseases. noise, smelly for local people.

73
Q

what are some common uses of carboxylic acids?

A

production of soft drinks
manufacture of additives
pharmaceuticals, eg manufacture of vitamin C-based medicines
Manufacture of toothpaste

74
Q

what are some common uses of alcohols?

A

fuel
perfumes and cosmetics.
industrial feedstocks
alcoholic drinks

75
Q

what are the chemical properties of alcohols?

A

soluble in water
boiling point of an alcohol is always much higher than the boiling point of the corresponding alkane with the same hydrocarbon chain
sweet odor

76
Q

what are the chemical properties of carboxylic acids?

A

weak acids
react with metals to liberate hydrogen
In aqueous solution, the carboxylic acids undergo self ionization and exist in equilibrium

BMAT (4 decks)

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