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eoy > s3 chem > Flashcards

s3 chem Flashcards

1
Q

what is the Si Unit of time?

A

second (s)

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2
Q

what is the Si Unit of temperature?

A

kelvin (K)

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3
Q

temperature in K (kelvin) = temperature in degree celcius + ?

A

273

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4
Q

what is the Si Unit of length?

A

metre (m)

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5
Q

what is the Si Unit of mass?

A

kilogram (kg)

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6
Q

what is the Si Unit of volume?

A

cubic metre (m^3)

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7
Q

1m = ?dm

A

10

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8
Q

1m^3 = ?dm^3

A

? = 1000

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9
Q

what is the degree of accuracy of a pipette?

A

10.0 cm ^3 or 25.0cm^3 (e.g : 10, 20, 30)

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10
Q

what is the degree of accuracy of a volumetric flask?

A

100 cm^3 or 250cm^3

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11
Q

what is the degree of accuracy of a measuring cylinder?

A

a range of volumes to the nearest 0.5cm^3 (e.g: 31.5 cm^3 or 23.0 cm^3)

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12
Q

what is the degree of accuracy of a burette?

A

a range of volumes to the nearest 0.05 cm^3. (e.g: 31.55 cm^3 or 23.00 cm^3)

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13
Q

what kind of apparatus can we use to measure the volume of a gas?

A

gas sringe

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14
Q

what can a magnet be used to separate in the separation of solid-solid mixtures?

A

a magnet can be used to separate magnetic solids from non-magnetic solids

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15
Q

name 3 different ways/techniques to separate solid-solid mixtures.

A

magnetic attraction, sieving, and suitable solvents.

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16
Q

how does sieving work?

A

in a mixture of bigger and smaller particles, we can use a sieve of the right pore size to separate the components. The pore size tells us how big the holes in the filter are. Bigger pores let bigger particles through.

  • a sieve can be used to separate solids with different particle sizes
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17
Q

how does using suitable solvents to separate solid-solid mixtures?

A

a suitable solvent can be used to separate solid-solid mixtures in which only one of the solids is soluble in the solvent.

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18
Q

name 4 different ways/techniques to separate solid-liquid mixtures

A

filtration, evaporation to dryness, crystallisation, simple distillation

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19
Q

what is evaporation to dryness used for?

A

to separate a dissolved solid from its solvent by heating the mixture until all the solvent has vaporised.

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20
Q

what is crystallisation used for?

A

to obtain a pure solid from its saturated solution. (saturated solution = one in which no more solute can be dissolved.

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21
Q

what is simple distillation used for?

A

to separate a pure solvent (liquid) from a solution.

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22
Q

what are 2 ways/techniques to separate liquid-liquid mixtures?

A

chromatography, fractional distillation

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23
Q

what is chromatography used for?

A

to separate a mixture of substances which have different solubilities in a given solvent.

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24
Q

what is fractional distillation used for?

A

to separate miscible liquids with different boiling points

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25
Q

how can the purity of substances be determined?

A

a pure substance has a specific melting/boiling point under fixed conditions.

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26
Q

define the kinetic particle theory

A

all matter is made up of tiny particles and these particles are in constant random motion.

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27
Q

define the kinetic particle theory

A

all matter is made up of tiny particles and these particles are in constant random motion.

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28
Q

define sublimation

A

the process by which a solid changes directly into a gas

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29
Q

define an atom

A

an atom is the smallest particle that can still have the chemical characteristics of an element.

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30
Q

does the no. of protons in an atom equate to the no. of electrons in an atom?

A

yes

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31
Q

define a ion

A

an ion is the particle formed when an atom or group of atoms gains or loses electrons. (no. of protons and neutrons remain the same)

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32
Q

define a ion

A

an ion is the particle formed when an atom or group of atoms gains or loses electrons. (no. of protons and neutrons remain the same)

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33
Q

what are isotopes?

A

isotopes are atoms of the same element that have the same proton(atomic) number but different nucleon(mass) numbers. (diff numbers of neutrons)

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34
Q

what gases are monoatomic? (single atoms & chemically un-reactive)

A

noble gases. as the have a noble gas electronic configuration

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35
Q

what are positive ions?

A

positive ions have more protons than electrons and have a net positive charge,

36
Q

what are negative ions

A

negative ions (anions) have a net negative charge and usually have a noble gas electronic configuration.

37
Q

define ionic bonding

A

an ionic bond is the mutual electrostatic attraction between ions of opposite charges

38
Q

what are ionic structures?

A

an ionic compound forming a structure called a giant ionic crystal lattice.

39
Q

define covalent bonding/valency

A

when 2 non-metal gases share electrons to form a noble gad configuration

40
Q

ionic compounds have ? melting and boiling points

A

high

41
Q

what is the hardness of ionic compounds?

A

ionic compound are physically hard but brittle

42
Q

what is the solubility in ionic compounds?

A

ionic compounds are often soluble in water but insoluble in organic solvents

43
Q

when can ionic compounds conduct electricity?

A

ionic compounds conduct electricity when molten or in aqueous solution, but not in the solid state.

44
Q

what are the usual structural properties of covalent substances at room temperature and pressure?

A

simple covalent substances are usually gases or liquids at room temperature and pressure.

45
Q

why do simple covalent substances have low melting and boiling points?

A

as the molecule gets larger , the melting and boiling points are usually higher.

46
Q

why do simple covalent substances have low melting and boiling points?

A

as the molecule gets larger , the melting and boiling points are usually higher.

47
Q

what is the solubility of simple covalent substances?

A

simple covalent substances are usually insoluble in water and soluble in organic solvents.

48
Q

what is the electrical conductivity of simple covalent substances?

A

simple covalent substances do not conduct electricity.

49
Q

what is an alloy

A

an alloy is a mixture of a metal with one of more other elements.

50
Q

what are the structural properties of pure metals?

A

pure metals are malleable and ductile.

51
Q

do pure metals have high or low melting or boiling points?

A

pure metals have high melting and boiling points. they are good conductors of heat

52
Q

do pure metals have high or low melting or boiling points?

A

pure metals have high melting and boiling points. they are good conductors of heat

53
Q

what is the electrical conductivity of metals and alloys?

A

metals and alloys are good conductors of electricity

54
Q

what is the relative atomic mass of an element?

A

the relative atomic mass of an element is the average mass of one atom of that element reletive to 1/12 the mass of an atom of carbon-12 (standard atom)

55
Q

what is the relative molecular mass of a molecular substance?

A

the relative molecular mass of a molecular substance is the average mass of one molecule of that substance relative to 1/12 the mass of an atom of carbon-12.

56
Q

what is the relative formula mass of an ionic compound?

A

the relative formula mass of an ionic compound is the average mass of one unit of that compound relative to 1/12 the mass of an atom of carbon-12

57
Q

how do we calculate the number of moles in a gas?

A

volume / 24dm^3

58
Q

what is a acid?

A

an acid is a substance that produces hydrogen ions, H+, in aqueous solutions

59
Q

acids react with reacting metals to form ?

A

a salt and hydrogen gas

60
Q

acids react with bases to form ?

A

a salt and water

61
Q

acids react with bases to form ?

A

a salt and water

62
Q

acids react with carbonates to form ?

A

a salt, water, and carbon dioxide gas

63
Q

what is a base?

A

a base is any metal oxide or hydroxide. They can contain either the oxide ion or the hydroxide ion.

64
Q

what is an alkali?

A

an alkali is a substance that produces hydroxide ions, OH-, in aqueous solutions

65
Q

alkalis react with acids to form ?

A

a salt and water

66
Q

name 4 properties of alkalis

A
  • they taste bitter
  • feel slippery and soapy
  • dissolve in water to form solutions that can conduct electricity
  • turns red litmus paper blue
67
Q

what is the ionic equation for any neutralisation reaction between an acid and alkali?

A

H+ (aq) + OH- (aq) — Hsmall 2 O(l)

68
Q

what is the ionic equation for any neutralisation reaction between an acid and alkali?

A

H+ (aq) + OH- (aq) — Hsmall 2 O(l)

69
Q

alkalis when heated with ammonium salts, give off ?

A

ammonia gas

70
Q

define oxidation

A
  • gain of oxygen
  • loss of hydrogen
  • loss of electrons
  • oxidation number/state will increase
71
Q

define reduction

A
  • loss of oxygen
  • gain of hydrogen
  • gain of electrons
  • oxidation number/state will decrease
72
Q

what is the periodic table?

A

a list of elements arranged in order of increasing proton(atomic) numbers

73
Q

what are groups in the periodic table?

A

the vertical column of elements

74
Q

what are periods in the periodic table?

A

the horizontal row of elements

75
Q

the number of electron shells an element has is the same as its ?

A

period number

76
Q

what are the metallic properties of elements across a period?

A

there is a decrease in metallic properties and an increase in non-metallic properties across a period.

77
Q

what are the metallic properties of elements when going down a group?

A

going down a group, there is an increase in metallic properties and a decrease in non-metallic properties

78
Q

what happens in a displacement reaction?

A

in a displacement reaction, on element takes the place of another element in the compound.

79
Q

how are metals arranged in the reactivity series?

A

in the reactivity series, metals are arranged from the most reactive to the least reactive.

80
Q

what are the conditions for rusting to occur

A

the presence of both oxygen(in air) and water are necessary for rusting to occur.

81
Q

what is an acid?

A

substances that dissolve in water to produce H+ ions

82
Q

what are strong acids?

A

strong acids are acids that dissolve completely when dissolved in water to produce a high concentration of H+ ions. Thus, pH of strong acids are very low

83
Q

what are weak acids?

A

weak acids are acids that only partially dissolve in water and produce a low concentration of H+ ions. Thus, pH of weak acids are not very low

84
Q

acids + metals = ?

A

salt + H2

85
Q

acids + metals = ?

A

salt + H2

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