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chemistry paper 1 > whole of chemistry 1 > Flashcards

whole of chemistry 1 Flashcards

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1
Q

define a compound

A

two or more elements chemically bonded together

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2
Q

mendeleev

A

he arranged elements by mass, similar patterns and left gaps for unknown elements

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3
Q

what do groups show?

A

how many electrons in the final shell

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4
Q

what do periods show?

A

how many shells there are

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5
Q

where are metals on the periodic table and what do they do?

A

they’re on the left hand side
they lose electrons which gives them a positive charge

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6
Q

where are non-metals on the periodic table and what do they do?

A

they’re on the right hand side
they gain electrons giving them negative charge

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7
Q

define ionic bonding

A

the transfer of electrons between a metal and non metal

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8
Q

what is the structure of an ionic compound?

A

giant lattice structure, high mp/bp, conduct when molten/dissolved as the ions are free to move

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9
Q

define covalent bonding

A

the sharing of electrons between two non-metals

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10
Q

formula for carbon dioxide

A

CO2

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11
Q

formula for water

A

H2O

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12
Q

formula for oxygen gas

A

O2

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13
Q

formula for hydrogen gas

A

H2

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14
Q

formula for nitrogen gas

A

N2

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15
Q

formula for ammonia

A

NH3

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16
Q

formula for hydrochloric acid

A

HCl

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17
Q

formula for sulfuric acid

A

H2SO4

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18
Q

characteristics of simple covalent bonds

A

low mp/bp
do not conduct electricity

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19
Q

characteristics of giant covalent bonds

A

high mp/bp
do not dissolve
do not conduct electricity

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20
Q

structure of diamond

A

made of carbon atoms- each carbon makes 4 bonds
very hard
can be used for cutting tools

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21
Q

structure of graphite

A

made of carbon atoms- each carbon makes 3 bonds
soft
conducts electricity
made in sheets
used in pencils

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22
Q

structure of fullerene

A

made of carbon atoms- each carbon makes 3 bonds
very hard
can be used as a lubricant

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23
Q

define polymer

A

a large molecule made up of repeated subunits known as monomers

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24
Q

what happens when polymers with cross links are heated

A

they will stay fixed in place and burn

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25
Q

what happens when polymers without cross links are heated

A

they will melt because they can slide over each other

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26
Q

acid + metal —> ___ + ___

A

acid + metal —> salt + hydrogen

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27
Q

define moles

A

units for the amount of a substance

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28
Q

equation for moles

A

moles = mass/mR

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29
Q

what is avagadro’s constant

A

6 x 10^23

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30
Q

equation for concentration

A

concentration (mol/dm^3) = amount (mol) / volume (dm^3)

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31
Q

what are metals made up of?

A

positive ions in a sea of delocalised electrons allowing them to conduct electricity

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32
Q

what is an alloy made up of?

A

positive ions in a sea of delocalised electrons but also containing a metal or non-metal
they have distorted layers that cannot slide meaning they’re hard

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33
Q

what is it called to go from:
solid —> liquid —> gas

A

solid —> liquid = melting
liquid —> gas = evaporating/boiling
gas —> liquid = condensing
liquid —> solid = freezing
solid —> gas/gas —> solid = sublimation

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34
Q

energy from different states

A

solid —> liquid —> gas = energy in
gas —> liquid —> solid= energy out

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35
Q

liquid + liquid —> solid (___)

A

liquid + liquid —> solid (cloudy)

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36
Q

liquid + solid —> gas (___)

A

liquid + solid —> gas (bubbles)

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37
Q

liquid + liquid —> gas (___)

A

liquid + liquid —> gas (bubbles)

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38
Q

equation for Rf

A

Rf= distance moved by spot / distance moved by solvent

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39
Q

equation for atom economy

A

atom economy= mR of atoms in required products / mR of reactants

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40
Q

how to purify water

A

remove the salt (desalination)
remove dirt/bacteria/unwanted ions
add chlorine/fluorine

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41
Q

bond for:
hydrogen + chloride —> hydrogen chloride

A

H—Cl

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42
Q

bond for:
hydrogen (H2)

A

H—H

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43
Q

bond for:
ammonia (NH3)

A

H — N — H
|
H

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44
Q

bond for:
chlorine (Cl2)

A

Cl—Cl

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45
Q

bond for:
methane (CH4)

A

H
|
H — C — H
|
H

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46
Q

bond for:
oxygen (O2)

A

O = O

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47
Q

bond for:
nitrogen (N2)

A

N ≡ N

48
Q

what does each line on the bonds show?

A

how many pairs of electrons being shared

49
Q

pH scale: acid

A

pH of 1-6
H+ hydrogen ions

50
Q

pH scale: neutral

A

pH of 7

51
Q

pH scale: alkali

A

pH of 8-14
OH- hydroxide ions

52
Q

what is the neutralisation equation?

A

H+ + OH- ⇌ H2O
acid + alkali —> salt + water

53
Q

what colour does phenolphthalein go in an alkali and an acid?

A

acid= colourless
alkali= pink

54
Q

what colour does methyl orange go in an acid and alkali?

A

acid= red
alkali= yellow

55
Q

which type of acids fully dissociate?

A

strong acids

56
Q

which acids partially dissociate?

A

weak acids

57
Q

acid + metal —> ?

A

acid + metal —> salt + hydrogen

58
Q

acid + metal oxide —> ?

A

acid + metal oxide —> salt + water

59
Q

acid + metal hydroxide —> ?

A

acid + metal hydroxide —> salt + water

60
Q

acid + metal base —> ?

A

acid + metal base —> salt + water

61
Q

acid + metal carbonate —> ?

A

acid + metal carbonate —> salt + water + carbon dioxide

62
Q

what happens when hydrogen gas is present?

A

squeaky pop

63
Q

what happens when oxygen gas is present?

A

relight glowing splint

64
Q

what happens when carbon dioxide gas is present?

A

turns limewater cloudy

65
Q

what happens when chlorine gas is present?

A

bleach damp litmus paper

66
Q

OILRIG

A

Oxidation
Is
Loss
Reduction
Is
Gain

67
Q

PANIC

A

Positive
Anode
Negative
Is
Cathode

68
Q

Reactivity Series

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold

69
Q

calculation for moles

A

mols= concentration x volume
OR
mols= mass/mR

70
Q

calculation for percentage yield

A

percentage yield= actual yield/ theoretical yield

71
Q

in electrolysis what does sodium chloride produce?

A

H2
Cl2
NaOH

72
Q

in electrolysis what does sodium sulfate produce?

A

H2
O2

73
Q

in electrolysis what does copper chloride produce?

A

Cu
Cl2

74
Q

in electrolysis what does copper sulfate produce?

A

Cu
O2

75
Q

process of making a pure salt:

A

heat sulfuric acid
stir in copper oxide until it is in excess
let it cool
filter solution to remove excess copper oxide
evaporate away the liquid

76
Q

titration method:

A

• pipette 250cm3 of alkali into a conical flask, add a phenolphthalein indicator
• fill a burette with an acid of known concentration
• take initial reading on burette and record it
• while swirling the flask, use the tap to slowly add the acid to the alkali
• when it changes from pick to colourless stop adding the acid
• record final volume in the burette
• repeat until titres are within 0.05cm3

77
Q

properties of transition metals:

A

• hard
• shiny
• conductors of electricity

78
Q

equation for rusting:

A

iron + oxygen + water —> iron oxide

79
Q

how do you stop rusting?

A
  • use a sacrificial metal
  • exclusion of oxygen
  • exclusion of water
80
Q

titration calculations:

A

• calculate the number of mols of acid used
• use this to find num of H+ ions involved in reaction, this is equal to the number of OH- ions
• calculate num of moles of alkali used
• calculate the concentration of alkali

81
Q

why are alloys stronger than metals?

A

they contain metals in different sizes and an irregular strangely meaning they can’t slide over each other easily

82
Q

what are the strengths and weaknesses for fuel cells?

A

strengths:
- water is the only product
- less maintenance required
- quieter than petrol/diesel engines

weaknesses:
- H2 needs to be stored in a tank
- constantly needs to be supplied with fuel
- H2 is produced by steam

83
Q

what do fertilisers promote and what do they replace?

A

they promote plant growth and they replace mineral ions

84
Q

what are the two types of fertilisers and what are they both also known as?

A
  • ammonium nitrate
  • ammonium sulfate
    these are both salts
85
Q

formula for nitric acid:

A

HNO3

86
Q

what is the haber process?

A

where ammonia is formed from nitrogen

87
Q

what is the equation for the haber process?

A

N2 + (3)H2 ⇌ (2)NH3

88
Q

what are the conditions that the haber process takes place is?

A

450 degrees
pressure of 200 atmospheres
iron catalyst

89
Q

compare the making of ammonium sulfate in an industry and lab

A

industry:
- large scale
- continuous
- the method is in several stages

lab:
- small scale
- only create a batch at a time
- the method used is titration

90
Q

define dynamic equilibrium

A

when the forwards and backwards reaction are happing at the same rate

91
Q

define reversible reactions

A

where the forwards and backwards reaction happen at the same time, not the same rate

92
Q

which 3 things can shift the equilibrium?

A
  • temperature
  • pressure
  • concentration
93
Q

how does pressure affect the equilibrium?

A

higher pressure means that the equilibrium moves to the side with fewer molecules (the number infront of the symbol when balancing)

94
Q

how does concentration affect the equilibrium?

A

higher concentration of reactants means you are making more products as the equilibrium moves to that side

95
Q

how does temperature affect the equilibrium?

A

higher temperatures means it moves to the endothermic direction
lower temperatures means it moves to the exothermic direction

96
Q

what is the equation for volume of gas?

A

volume of gas = amount of gas x molar volume (always 24dm3)

97
Q

what are the charges and masses of protons, neutrons and electrons?

A

proton: charge= +1 mass= 1
neutron: charge= 0 mass= 1
electron: charge= -1 mass= 1/1836

98
Q

how do you calculate r.a.m?

A

(mass of isotope x %) + (mass of isotope x %) + (mass of isotope x %) / 100

99
Q

what colour does litmus go in an alkali and an acid?

A

alkali= blue
acid= red

100
Q

Investigate the change in pH on adding powdered calcium hydroxide or calcium oxide to a fixed volume of dilute hydrochloric acid

A
  • add​ ​dilute​ ​HCl​ ​to​ ​the​ ​beaker​ ​and​ ​measure​ ​pH
  • add​ ​weighed​ ​mass​ ​of​ ​calcium​ ​hydroxide​ ​and​ ​stir​ ​then​ ​record​ ​pH
  • keep​ ​adding​ ​weighed​ ​masses​ ​of​ ​calcium​ ​hydroxide​ ​until​ ​there​ ​is​ ​no​ ​more
    change​ ​to​ ​the​ ​pH
101
Q

what does it mean if something is concentrated?

A

large amount of substance in the given volume

102
Q

what does it mean if something is dilute?

A

lesser amount of substance in a given volume of a solution

103
Q

what does it mean if something is a strong acid?

A

it fully dissociates in an aqueous solution releasing more H+ ions

104
Q

what does it mean if something is a weak acid?

A

it partially dissociates in an aqueous solution releasing less H+ ions

105
Q

what is the definition of electrolysis?

A

using electricity to split a substance

106
Q

in electrolysis, where do the positively charged ions (cations) move?

A

to the negative electrode (cathode)

107
Q

in electrolysis, where do the negatively charged ions (anions) move?

A

to the positive electrode (anode)

108
Q

what happens at the anode and what happens at the cathode?

A

anode= oxidation
cathode= reduction

109
Q

draw and label the diagram for electrolysis

A
110
Q

state the reactivity series

A

potassium
sodium
calcium
magnesium
aluminium
carbon
zinc
iron
tin
led
hydrogen
copper
silver
gold

111
Q

how do things above carbon in the reactivity series get extracted?

A

electrolysis

112
Q

how do things below carbon in the reactivity series get extracted?

A

displacement reaction with carbon

113
Q

how do you extract silver and gold?

A

mining

114
Q

what is an ore?

A

a mineral that can be extracted

115
Q

give 5 reasons why we should recycle metals?

A
  • burning less fossil fuels
  • less space needed for landfill sites
  • doesn’t destroy habitats
  • saves energy
  • saves money
116
Q

what are the 4 stages of a life cycle assessment?

A
  • making the material
  • manufacturing the product
  • using the product
  • disposing the product

chemistry paper 1 (1 decks)

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