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Chemistry Flashcards - OCR 21st Century > Chemistry Mock Exam 2021 > Flashcards

Chemistry Mock Exam 2021 Flashcards

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1
Q

Metal consist of a _____ structure of atoms arranged in a _______ pattern.

A

giant, regular

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2
Q

Metals have….

  • _______ metal ____
  • _________ electrons
A

Positive metal ions

Delocalised electrons

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3
Q

The electrons on the ______ shell of metals are _______ ( they are free to _____ around)

A

outer, delocalised, move

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4
Q

The strong forces of ________ _______ between the ______ metal ____ and the “sea” of shared negative _______ electrons hold the atoms _____ together in a ______ structure.

This is known as _______ bonding. - It is very ______ in strength

A

electrostatic attraction, positive metal ions, delocalised electrons, closely, regular

metallic bonding, strong

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5
Q

Substances held together by metallic bonding include _______ elements and ______.

A

metallic elements, alloys

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6
Q

Metals have high _______ and _______ points because lots of ______ is required to overcome the _____ number of strong _______ ______.

A

melting, boiling, energy, large, metallic bonds

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7
Q

Metals are very _____ since the _____ metallic structure is strongly ____ ________.

A

strong, giant, held together

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8
Q

Metals are both _______ (able to change shape) and ductile (can be drawn into ____ ______ or _____) because layers of metal ions can _____ over each other when ______ are applied

A

malleable, thin sheets, wires, slide, forces

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9
Q

Metals are good conductors of _____ and ________ as they have ________ electrons which are free to _____ and are able to carry _______ and _____ whilst moving.

A

heat, electricity, delocalised, move, current, heat

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10
Q

ionic bonding is caused by the ______ of electrons between ______ and ___-______

A

transfer, metals, non-metals

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11
Q

In Ionic bonding, the metal atom _____ electrons to form a _______ ion, and the non-metal _____ these electrons to form a _______ ion.

These oppositely _____ ions are strongly attracted to one another by _______ _____. - This attraction is called an _____ bond.

A

loses, positive, gains, negative

charged, electrostatic forces, ionic bond

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12
Q

The net overall charge of any ionic compound is __. So all negative ______ in the compound must balance all the _______ ______. - This can be used to find out the ______ of the ionic compound

A

0, charges, positive charges, formula

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13
Q

E.g. find out the chemical formula of Magnesium Bromide.

Mg has a ___ charge
Br has a __ charge
To balance the 2+ charge from Mg, you need ___ Br- ions.

Therefore the chemical formula is ______.

A

2+, -, 2

MgBr2

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14
Q

Ions formed in groups 1,2,3,5,6 and 7.

Group 1 = \_\_\_ ions
Group 2 = \_\_\_ ions
Group 3 = \_\_\_ ions
Group 5 = \_\_\_ ions
Group 6 = \_\_\_ ions
Group 7 = \_\_\_ ions
A 
Group 1 = 1+ ions
Group 2 = 2+ ions
Group 3 = 3+ ions
Group 5 = 3- ions
Group 6 = 2- ions
Group 7 = 1- ions
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15
Q

Negative ions form when atoms ____ electrons - they have more _______ than ______

Positive ions form when atoms _____ electrons - they have more _______ than ______

A

gain, electrons, protons

lose, protons, electrons

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16
Q

The number of electrons lost or gained is the same as the ______ on the ion.

E.g. if 2 electrons are lost the charge is ___.
If 3 electrons are gained the charge is ___.

A

charge

2+, 3-

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17
Q

Ionic compounds always have _____ _____ ______ structures.
The ions form a closely packed ______ ______.
There are very strong _______ _____ of attraction between _______ charged ____, in ____ directions

A

giant ionic lattice, regular lattice, electrostatic forces, oppositely charged ions, all directions

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18
Q

Ionic compounds have high _______ and ______ points due to the strong _______ _____ of attraction between the ____, which takes lots of ______ to overcome this attraction.

A

melting, boiling, electrostatic forces, ions, energy

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19
Q

Solid ionic compounds don’t conduct _______ because the ____ are fixed in _____ and can’t _____.
But when the compound _____, the ___ are able to ____ and can carry an ________ ______.

A

electricity, ions, place, move

melts, ions, move, electrical charge

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20
Q

Many ionic compounds dissolve easily in _____ because their ______ allow them to interact with the ______ molecules.

The ions separate and are all free to _____ in the solution, so they can carry an _______ _____.

A

water, charges, water

move, electrical charge

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21
Q

A homologous series is a family of molecules which share the same g______ f______ and f_______ g_____, as well as similar c______ ________.

Examples include _______ and _______

A

general formula, functional group, chemical properties

Alkanes and Alkenes

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22
Q

As the carbon chain length gets longer…

  • ________ (thickness) increases
  • __ and __ point increases
  • They become less f_______
A
  • Viscosity increases
  • BP and MP increases
  • Become less flammable
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23
Q

The _______ of these compounds (as seen before) affect how they’re used for ____.

e.g. compounds with short carbon chain lengths have lower ___, so they are used as bottled gases - stored under _______ as ______ in bottles

A

properties, fuels

BPs, pressure, liquids

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24
Q

Alkanes all have s____ _______ b____ (especially C___ bonds)

General formula is _____.

Are all ________ - compounds containing only ______ and ______.

First 4 alkanes are ______, ______, ______ and ______.

A

single covalent bonds, C-C,

General formula - CnH2n+2

All hydrocarbons, hydrogen, carbon

Methane, Ethane, Propane, Butane

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25
Q

The displayed formula is a drawing that shows all the _____ and ____ in a molecule.

Go search an image of one.

A

atoms, bonds

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26
Q

Complete combustion occurs when there is plenty supply of _______

Formula - _____-based compound + _______ –> ______ ______ + ______ (and ______)

Both c_____ and h______ are _______ in the reaction.

A

oxygen

Carbon-based compound + oxygen —> Carbon dioxide + Water (and energy)

carbon and hydrogen are oxidised in the reaction

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27
Q

Carbon-based compounds are used as fuels due to the amount of _____ they release when _______ ________.

A

energy, combust completely

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28
Q

A functional group is a group of ____ within a molecule that determines how a molecule _____.

Remember, particular ________ series contain the same _______ group.

A

atoms, reacts

homologous series, functional group

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29
Q

Alkanes are s______ - all their bonds are currently ____.

Alkenes however are ___ _______. (see later)

A

saturated, full

not saturated

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30
Q

Alkanes don’t have a ________ group so they only easily take part in ________ reactions.

Alkenes have a ____ d_____ bond ______ group - this allows alkenes to take part in a greater range of _______.

A

functional group, combustion reactions

C=C double bond functional group - Alkenes.

greater range of chemical reactions

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31
Q

Alkenes

The C=C double bond in ______ means that they have ___ fewer _______ atoms compared with alkanes with the same number of _______ atoms.

The C=C double bond can ____ up to ____ with other atoms - this makes alkenes far more ______ than alkanes and shows that alkenes are u_______.

A

alkenes, two fewer hydrogen atoms, carbon

open up, react with, reactive, unsaturated

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32
Q

Alkenes have the general formula ______ and contain ____ C=C double bond.

The first four alkenes are ______ (with ___ carbon atoms), _______, ______ and _______.

Search the display formulas

A

CnH2n, one

Ethene, two, Propene, Butene, Pentene

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33
Q

Complete combustions of alkenes when there is plenty of ______.

Formula Alkene + ______ –> ______ ______ + ________ (+ _______)

A

oxygen

Alkene + Oxygen –> Carbon Dioxide + Water (+energy)

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34
Q

Alkenes can react via _______ reactions - this is when the ____ double bond will ____ up to leave a _____ bond and a new ____ to added to the previous ____ bond.

These reactions can be used to make useful _______, such as _______.

Check cgp

A

addition, C=C, open yp, single, atom, C=C

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35
Q

Alkenes will also react in ______ reactions with h_______ such as bromine, c_____ and iodine.

The ___ d_____ bond opens up so that each of the ____ carbons bond to a _______ atom.

A

addition reactions, with halogens, chlorine

C=C double bond, C=C, halogen

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36
Q

The addition of bromine to a double bond can be used to test for _______.

  • When ______ bromine water is added to a compound with no _____ bond, like an alkane, no ______ will happen and it’ll stay bright ______.
A

alkenes

orange, double bond, no reaction, bright orange

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37
Q
  • If ______ water is added to an alkene, the bromine will add across the ______ ____, making a _______ solution.
A

bromine water, double bond, colourless

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38
Q

Alkene molecules can also react with other alkene molecules by ______ up their ______ bonds and forming _____ bonds between themselves.

When lots of alkene molecules ____ together, they form an ________ polymer. (eg poly(ethene) )

A

opening, double, single

join, addition polymer

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39
Q

Crude oil is a _______ of lots of different _______, most of which are alkanes. The different compounds in crude oil are separated by _______ _______.

A

mixture, hydrocarbons, fractional distillation

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40
Q

Fractional distillation

1) The oil is _____ till it turns into ____ state. The gases enter a ________ ______ (and the liquid bit is drained off).

A

heated, gas, fractionating column

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41
Q

Fractional distillation

2) The fractionating column is a ___ column which has _______ coming off at various points

A

tall column, condensers

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42
Q

Fractional distillation

3) The column is heating from the bottom so there’s a temperature ______ (it’s hot at the _______ and gets cooler the more ___ you go).

A

temperature gradient, hot at the bottom, cooler as you go up

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43
Q

Fractional distillation

4) The longer hydrocarbons have ___ BP. They condense back into ______ and drain out of the column early on, when they’re near the ______.
The shorter hydrocarbons have ____ BP so they condense and drain out much later on, near the ____ of the column where it is _______.

A

long chain - high BP, liquid, near the bottom

short chain - low BP, top of the column - cooler

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44
Q

Fractional distillation

5) You end up with the crude oil ______ separated out into the different ______.
Each fraction contains a mixture of mainly _____ that have similar number of ______ atoms, so have similar ____.

A

mixture, fractions, mainly alkanes, similar number of carbon atoms, similar BPs

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45
Q

Explaining how the hydrocarbons change state.

The heat supplies the molecules with extra _____, which causes them to _____ more.
Soon, there will be enough _____ to overcome the ________ ______ that keep it with the other molecules, so it can turn into a ____.

A

extra energy, move more, enough energy to overcome intermolecular forces, turn into gas

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46
Q

Short-chain hydrocarbons have weaker ______ _______ and so they have lower ____

A

Short chain, weaker IMF, lower BPs

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47
Q

Long-chain hydrocarbons have stronger _______ _______ and so they have high _____.

A

Long-chain, stronger IMF, higher BPs

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48
Q

Check CGP for fractional distillation experiment

A

Yes sir!

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49
Q

Polymers are ____ molecules made up of lots of small molecules called _______ which are ____ together.

A

long molecules, monomers, joined together

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50
Q

Polymerisation - When lots of _______ join together to form a _______.

A

monomers, polymer

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51
Q

To make polymers synthetically, a high ______ and a ______ are normally needed

A

synthetic polymers, high pressure, catalyst

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52
Q

Plastics are made up of ______. They’re usually _____-based and their monomers are often ______.

The alkenes used to make polymers usually come from ________ crude oil.

A

polymers, carbon-based, alkenes

cracking

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53
Q

Addition Polymers are made from _______ monomers. These monomers have a _____ ______ bond functional group. (Alkenes)

A

unsaturated monomers, C=C carbon double bond functional group

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54
Q

Lots of alkenes can _____ __ their ______ bonds and join together to form ______ chains. This is called _______ polymerisation

Check cgp for more info

A

open up double bonds, polymer chains

Addition polymerisation

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55
Q

Drawing the displayed formula of addition polymers

  • First draw two alkene carbons, replace the ______ bond with a ______ bond and add an extra single bond to each of the _______.
  • Then fill in the rest like normal, Finally, stick a pair of ______ around the repeating bit, and put “_” after it (to show that there a lots of monomers) CGP
A

replace double bond with single bond, carbons

brackens, n

56
Q

Displayed formula of polymer —-> just do the reverse.
Draw out the _______ bit of the polymer, get rid of the two bonds going through the _____, and put a _____ bond between the carbons CGP

A

repeating bit, brackets, double

57
Q

The name of the polymer comes from the type of _______ it’s made from

You just put poly first and then the name of the _______ in brackets

eg poly(propene)

A

monomer

monomer in brackets

58
Q

Condensation polymers usually involves two different types of ______ which contain different _______ ______.

A

2 different monomers with different functional groups

59
Q

The monomers react together and forms ___ between them, making ______ chains

Each _______ _____ can react with the functional group of another ______, creating long chains of ________ monomers.

A

forms bonds between them, polymer chains

functional group, monomer, long chains of alternating monomers

60
Q

The repeating unit of a condensation polymer always contain the _____ chains of both _______ and the link that forms between them. CGP

A

carbon chains of both monomers

61
Q

Two types of Condensation polymers are

  • Poly_____
  • Polya____
A

Polyesters

Polyamides

62
Q

Polyesters form when ________ ____ monomers and ____ monomer react together

CGP

A

dicarboxylic acids, diol

63
Q

Polyester fibres are used to make ______. They can replace ______ fibres such as wool and silk.

A

make clothes, replace natural fibres

64
Q

Formula of monomers used to make the CP from it’s repeating unit

First find the _____ (HN-CO) or ester (__-_) link, Break it down the ______.

Then add an __ or ___ to both ends of both molecules to find the monomers CGP.

A

Amide (HN-CO), Ester (CO-O), middle

Add an H or OH

65
Q

Repeating unit of CP from formulas of a pair of monomers.

Draw out the two ______ molecules next to each other

Remove an ___ from the dicarboxylic acid, and an H from the -____ group of the diamine or the -OH group of the ___ —- that gives you a _____ molecule

A

monomer molecules

OH, -NH2, diol, water molecule

66
Q

Continued

Join the __ (from the C=O of the ________ acid) to the __ from the amide or the __ from the diol.

Take another __ and ___ off the ____ of your molecule CGP Freesciencelesson

A

C, dicarboxylic acid, N, O

67
Q

Naturally occurring polymers

  • ____
  • ________
  • _____ ____
A

DNA
Carbohydrates
Amino acids

68
Q

DNA is a complex molecule that contains ______ info

It contains two ______ made of monomers called _________ that bond together in a ________ reaction

A

genetic info

strands, nucleotides, polymerisation reactions

69
Q

There are 4 different nucleotide monomers in DNA, referred to by letters __, __, __ and __.

Short sequences of these ________ monomers in DNA are called ____. These allow organisms to ______ and develop.

A

A, G, C, T

nucleotide monomers, genes, allow organisms to function and develop

70
Q

Carbohydates are molecules containing c____, o_____ and h______, used by living organisms to store _____.

A

carbon, oxygen and hydrogen, store energy (i.e. they are a source of energy).

71
Q

S____ and C_____ are large complex carbohydrates, which are made up of many _____ units of carbohydrates, known as ______, joined together in a ____ chain.

A

Starch and cellulose, smaller units, sugars, long chain

72
Q

Amino acids form polymers known as ______ via ________ polymerisation.

Proteins have many important uses in the human body, like for _____ and re___ in organisms.

A

proteins, condensation polymerisation

growth and repair

73
Q

Polymers are held together by _______ bonds and ________ forces.

A

covalent bonds, intermolecular forces

74
Q

In polymers, all atoms in the chain are joined by ______ _______ bonds.

There are ________ forces between the _____.

A

strong covalent bonds

intermolecular forces, chains

75
Q

The _________ forces between polymer molecules are stronger than ______ molecules, so more ______ is needed to break them. This means most polymers are _____ at room temp.

A

intermolecular forces, simple molecules, energy, solid

76
Q

The intermolecular forces are still weaker than _____ or _______ bonds, so polymers generally have _____ MP than ____ or ____ ______ compounds.

A

ionic, covalent bonds, lower MP, ionic, giant covalent

77
Q

Before polymers melt, they become ____. The weaker the forces between the chains, the _____ the so______ point of a polymer.

A

Weaker forces, lower softening point

78
Q

Polymers have different properties depending on their _______ and the _____ between the chains

A

structure, forces

79
Q 
Low density (LD) poly(ethene) is made from \_\_\_\_\_\_\_. 
There's lots of space between the polymer chains, so the \_\_\_\_\_ between the chains are relatively \_\_\_\_.

This means LD is ______ and so is used for bags and _______.

A

ethene

lots of space, weak forces

LD is flexible

80
Q

High density (HD) poly(ethene) is also made from ______. The chains are packed ______ together, so the forces between them are ______.

So it’s ____ and is used for water tanks and ______/

A

ethene, closely together, stronger forces

stiff, drainpipes

81
Q

As well as intermolecular forces between the chains, some polymers also form _______ or _____ crosslinks.

A

covalent or ionic crosslinks

82
Q

Polymers with IM forces only between the chains are made up of individual ______ _____ that can ____ over each other.

The forces between the chains can be overcome, so the polymers can be _____.

A

individual tangled chains, slide over each other

overcome forces, polymer can be melted

83
Q

An electrolyte is a _____ or ______ _____ compound.

A

Molten or dissolved ionic compund

84
Q

Cathode is the ______ electrode

A

negative electrode

85
Q

Anode is the _______ electrode

A

positive electrode

86
Q

Electrolysis

1) An electric _____ is passed through an _______.
The ____ move towards the electrode, where they react, and the compound ________.

A

current, electrolyte

ions move to electrodes, compound decomposes

87
Q

Electrolysis
2) The positive _____ or ________ ions in the electrolyte will move towards the ______ (______ electrode) and ____ electrons (they are _______)

A

positive metal or hydrogen ions, cathode (negative electrode), gain electrons, they are reduced

88
Q

Electrolysis
3) The negative ___-____ ions in the electrolyte will move towards the _____ (_______ electrode) and ____ electrons (they are ______)

A

negative non-metal ions, anode (negative electrode), lose electrons, they are oxidised

89
Q

Electrolysis

4) As ions travel to _______, it creates a flow of ______ through the _______

A

electrodes, flow of charge through the electrolyte

90
Q

Electrolysis

5) As ions gain or lose _______, they form the ______ element and are _______ from the electrolyte.

A

electrons, uncharged, discharged

91
Q

An ionic solid can’t be _________ because the ____ are in ____ ______ and so can’t _____.

A

Solid no electrolysed, ions are fixed in place, can’t move

92
Q

Molten ionic compounds can be ________ because the ___ can ____ freely and conduct _______.

A

Molten yes electrolysed, ions can freely move, and can conduct electricity

93
Q

Molten ionic liquids, e.g. lead bromide, are always broken up into their _______.

At the cathode: Pb2+ + ____ —-> Pb

At the anode: ____ —> Br2 + ____.

A

elements

At the cathode: Pb2+ + 2e- —> Pb

At the anode: 2Br- —> Br2 + 2e-

94
Q

During electrolysis, the electrodes should be _____ so they don’t react with the _______.

______ and ______ are commonly used to make _____ electrodes

A

inert (unreactive), electrode

Graphite and Platinum, inert electrodes

95
Q

If a metal is too _____ to be reduced with _____ or reacts with ______, then electrolysis can be used to ______ it.

A

reactive, reduced with carbon, reacts with carbon, electrolysis can be used to extract it

96
Q

Extracting metals via electrolysis is very _______ as lots of ______ is required to ____ the ore and product the required _______.

A

expensive, lots of energy needed to melt ore and produce current

97
Q

Electrolysis is the _________ of an electrolyte by an electric _______.

A

decomposition, current

98
Q

Electrolysis needs:

  • a ___ electrical power supply
  • a negative _______, called a ______
  • a positive _______, called an ______
A

DC power supply

negative electrode - cathode

positive electrode - anode

99
Q

During electrolysis

  • Positive ions , _____ , move to the ______
  • Negative ions, _____, move the the ______.
A

+ ions - cations - move to cathode

  • ions - anions - move to anode
100
Q

Oxidation and Reduction of electrons

Oxidation is ____ of _______

Reduction is ____ of ________

A

OILRIG

Oxidation is loss of electrons

Reduction is gain of electrons

101
Q

Reduction happens at the _______ c_____ because this is where ______ ions ____ electrons.

A

Reduction - negative cathode, positive ions gain electrons

102
Q

Oxidation happens at the ______ _____ because this is where ______ ions ____ electrons.

A

Oxidation - positive cathode, negative ions lose electrons

103
Q

Half equations include ___ and _______, and are used to describe the process happening at an ________.

A

ions and electrons, electrode

104
Q

Half equations

  • Electrons are shown as ___
  • Same number of ____ of each _______ on ____ sides of the equation
  • The total _____ on each side must be the _____ (usually 0)
A

Electrons - e-

same number of atoms, element, both sides

total charge on each side must be equal

105
Q

For all half equations, you must show the ______ of _______

e.g. 2Cl- → Cl2 + 2e-
Pb2+ + 2e- → Pb

Both add e-

A

addition of electrons

106
Q

If a metal is too _____ to be reduced with _____ or reacts with ______, then electrolysis can be used to ______ it.

A

reactive, reduced with carbon, reacts with carbon, electrolysis can be used to extract it

107
Q

Extracting metals via electrolysis is very _______ as lots of ______ is required to ____ the ore and produce the required _______.

A

expensive, lots of energy needed to melt ore and produce current

108
Q

Electrolysis of Alu Oxide

1) Aluminium is extracted from the ore ______ by ______. ______ contains _______ ______ (Al2O3)

A

ore - bauxite, electrolysis.

Bauxite contains Alu Oxide

109
Q

Electrolysis of Alu Oxide

2) Alu oxide is heated to a very ____ _________ to form ______ Alu Oxide

_______ can be added to _______ the ___.

A

high temperature, molten Alu Oxide

Cryolite - lowers MP significantly

110
Q

Electrolysis of Alu Oxide

3) The molten mixture contains ____ ions, so it’ll conduct ________.

A

molten mixture - free ions - can conduct electricity

111
Q

Electrolysis of Alu Oxide

4) The positive ____ ions are attracted to the _______ ______ where they each pick up __ electrons to form ______ aluminium _____.

These then sink to the ______ of the electrolysis ____.

A

Al3+. negative electrode (cathode), gain 3 electrons, form neutral Al atoms

112
Q

Electrolysis of Alu Oxide

5) The negative ____ ions are attracted to the _______ ______ where they each lose __ electrons.

The ______ oxygen atoms _______ to form ___ molecules (Oxygen is d_____)

A

negative O2- ions, positive electrode (cathode), lose 2 electrons

neutral oxygen atoms combine to form O2

Oxygen is diatomic

113
Q

At the cathode

Process - ______ - ____ of electrons

____ + ____ –> Al

Aluminium is produced at the _______

A

Reduction - Gain of electrons

Al3+ + 3e- —> Al

Produced at the cathode

114
Q

At the anode

Process - _______ - ____ of electrons

2O2- —> ____ + _____

Oxygen is produced at the ______

A

Oxidation - Loss of electrons

2O2 —> O2 + 4e-

Oxygen is produced at the cathode

115
Q

Overall equation for the electrolysis of Alu Oxide

_______ ______ —> ______ + _______

_____ –> ____ + ____

A

Aluminium Oxide —> Aluminium + Oxygen

2Al2O3 –> 4Al + 3O2

116
Q

Electrolysis of Alu oxide

The electrodes are made up of _______.
The ______ needs to be ______ regularly as it reacts with ______ to product ______ _______

A

electrodes - carbon

electrode, replaced, O2 reacts with it to form CO2

117
Q

Electrolysis of Aqueous solutions

Ions from the _____ compounds are present, but there will also be ________ ions (H+) and ________ ions (___) from the water.

A

ion

118
Q

Electrolysis of Aqueous solutions

At the Cathode:
- Hydrogen will be produced at the ______ if the _____ is ____ reactive than _______

A

cathode, metal is more reactive than hydrogen

Metal more reactive than H, H is produced

119
Q

Continued Aq Electro

  • The ____ metal will be produced at the ______ if it is ____ reactive than ________.
A

pure metal, cathode, less reactive than H

Metal less reactive, pure metal produced

120
Q

Aq Electro

At the anode:
______ is produced (from hydroxide ions) at the anode UNLESS _____ ions (chlroride, ______ etc) are present.

A

Anode - Oxygen produced, unless halogen ions present

121
Q

Balanced half equation for the formation of oxygen from _______ ions is:

4OH- → 2H2O + __ + __

A

4OH- → 2H2O + O2 + 4e-

122
Q

Reactivity series from most to least

\_\_\_\_\_\_\_\_
Sodium 
\_\_\_\_\_\_
Calcium
\_\_\_\_\_\_\_\_\_
Aluminium 
CARBON
\_\_\_\_
Iron
HYDROGEN
\_\_\_\_\_\_
Silver
\_\_\_\_
A 
Potassium
Sodium 
Lithium
Calcium
Magnesium
Aluminium 
CARBON
Zinc
Iron
HYDROGEN
Copper
Silver
Gold
123
Q

Mass number is located in the ___-___ corner of its symbol.

The mass number tells us the no. of ______ + no. of ______ in an atoms _________.

A

Mass number - top left corner of symbol

Mass number = no. of protons + no. of neutrons

124
Q

Sometimes, relative atomic mass will be on the ___-___ instead, which is the _______ mass of all the _______ of that element.

Noted by ____.

A

Relative Atomic mass - Also top-left corner instead
Relative Atomic Mass - The average mass of all the isotopes of that element

Ar

125
Q

Example of relative atomic mass

Chlorine has 2 _______, which are Chlorine 35 and Chlorine 37

The Ar of these is the _______ of the two isotopes masses when we consider how ________ each one is.

So chlorine Ar = 35.5

A

Chlorine - 2 Isotopes Cl 35, Cl 37

Ar - average of the isotopes when considering how common each one is

126
Q

An Isotope is an atom of an element with the same number of ______, but different number of ______ in their nuclei.

A

Isotope - Same no. protons, different no. neutrons

127
Q

Relative Formula Mass (___)

Found by ______ together the atomic _____ of all the ____ in that compounds _______ formula.

A

Relative Formula Mass (Mr)

Adding together Ar of each atom of each element in the compounds molecular formula

E.g. MgCL2 = 24 + 35.5 + 35.5 = Mr = 95

128
Q

Calculate the percentage mass of a particular element in a compound

Formula = (___ of atom n x ____ of atom) / Mr of the compound

Then multiply ANS of this by _____ to turn into %

A

Percentage mass = (Ar of atom x No. of atom)/Mr of compound) = ANS

ANS x 100 gives %

E.g. %mass of S in H2SO4 = (32x1)/98 = 0.327
0.327x100 = 32.7%

129
Q

Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH₄NO₃

A

14+4+14+(16x3)=80 = Mr of ammonium nitrate

130
Q

A mole is a name given to a certain _______

Just like a dozen = ___, a mole is equal to a certain _______

A

A mole - name for a certain number

Dozen = 12

131
Q

A mole is given by _______ _______ - its value is ______ x10^__

A

A mole is given by Avogadro’s constant = 6.02 x 10^23

132
Q

A mole/_______ constant shows the number of _____ in ___g of ______-12.

This is also the same number of atoms or ________, that are in any ______ or _________. CGP

A

Mole/Avogadro’s constant shows the no. of atoms in 12g of Carbon -12.

Also the same no. of atoms or molecules in any element or compound

133
Q

Moles

One mole of particles (atoms, ___, ________ etc) of any _________ will have a _____ in grams equal to the ___ or ___ for that substance.

A

One mole of particles (atoms, ions, molecules etc) of any substance will have a mass in grams =to the Ar or Mr for that substance

CGP

134
Q

Examples of moles

Neon has a Ar of 20.2 The mass of 1 mole of neon is __

Nitrogen gas N2 has an Mr of 28 The mass of 1 mole of N2=___

Hexane C6H14 has Mr of 86 The mass of 1 mole of hexane is ____

A

Mass of 1 mole of neon = 20.2g (same as Ar)

Mass of 1 mole of N2 = 28g (same as Mr)

mass of 1 mole of hexane = 86g (same as Mr)

So 12g of Carbon, 28g of N2 and 86g of hexane all contain the same number of PARTICLES, namely ONE MOLE or 6.02x10^23

135
Q

Moles

The mole tells us the number of _______ (atoms or molecules) in any _______ or ________.

A

Mole - No. of particles in any element or compound

Chemistry Flashcards - OCR 21st Century (9 decks)

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