Chemistry Mock Exam 2021 Flashcards
(135 cards)
1
Q
Metal consist of a _____ structure of atoms arranged in a _______ pattern.
A
giant, regular
2
Q
Metals have….
- _______ metal ____
- _________ electrons
A
Positive metal ions
Delocalised electrons
3
Q
The electrons on the ______ shell of metals are _______ ( they are free to _____ around)
A
outer, delocalised, move
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
5
Q
Substances held together by metallic bonding include _______ elements and ______.
A
metallic elements, alloys
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
7
Q
Metals are very _____ since the _____ metallic structure is strongly ____ ________.
A
strong, giant, held together
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
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
10
Q
ionic bonding is caused by the ______ of electrons between ______ and ___-______
A
transfer, metals, non-metals
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
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
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
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
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
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-
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
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
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
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
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
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
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
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
25
The displayed formula is a drawing that shows all the _____ and ____ in a molecule.
Go search an image of one.
atoms, bonds
26
Complete combustion occurs when there is plenty supply of _______
Formula - _____-based compound + _______ --> ______ ______ + ______ (and ______)
Both c_____ and h______ are _______ in the reaction.
oxygen
Carbon-based compound + oxygen ---> Carbon dioxide + Water (and energy)
carbon and hydrogen are oxidised in the reaction
27
Carbon-based compounds are used as fuels due to the amount of _____ they release when _______ ________.
energy, combust completely
28
A functional group is a group of ____ within a molecule that determines how a molecule _____.
Remember, particular ________ series contain the same _______ group.
atoms, reacts
homologous series, functional group
29
Alkanes are s______ - all their bonds are currently ____.
Alkenes however are ___ _______. (see later)
saturated, full
not saturated
30
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 _______.
functional group, combustion reactions
C=C double bond functional group - Alkenes.
greater range of chemical reactions
31
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_______.
alkenes, two fewer hydrogen atoms, carbon
open up, react with, reactive, unsaturated
32
Alkenes have the general formula ______ and contain ____ C=C double bond.
The first four alkenes are ______ (with ___ carbon atoms), _______, ______ and _______.
Search the display formulas
CnH2n, one
Ethene, two, Propene, Butene, Pentene
33
Complete combustions of alkenes when there is plenty of ______.
Formula Alkene + ______ --> ______ ______ + ________ (+ _______)
oxygen
Alkene + Oxygen --> Carbon Dioxide + Water (+energy)
34
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
addition, C=C, open yp, single, atom, C=C
35
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.
addition reactions, with halogens, chlorine
C=C double bond, C=C, halogen
36
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 ______.
alkenes
orange, double bond, no reaction, bright orange
37
- If ______ water is added to an alkene, the bromine will add across the ______ ____, making a _______ solution.
bromine water, double bond, colourless
38
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) )
opening, double, single
join, addition polymer
39
Crude oil is a _______ of lots of different _______, most of which are alkanes. The different compounds in crude oil are separated by _______ _______.
mixture, hydrocarbons, fractional distillation
40
Fractional distillation
1) The oil is _____ till it turns into ____ state. The gases enter a ________ ______ (and the liquid bit is drained off).
heated, gas, fractionating column
41
Fractional distillation
2) The fractionating column is a ___ column which has _______ coming off at various points
tall column, condensers
42
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).
temperature gradient, hot at the bottom, cooler as you go up
43
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 _______.
long chain - high BP, liquid, near the bottom
short chain - low BP, top of the column - cooler
44
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 ____.
mixture, fractions, mainly alkanes, similar number of carbon atoms, similar BPs
45
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 ____.
extra energy, move more, enough energy to overcome intermolecular forces, turn into gas
46
Short-chain hydrocarbons have weaker ______ _______ and so they have lower ____
Short chain, weaker IMF, lower BPs
47
Long-chain hydrocarbons have stronger _______ _______ and so they have high _____.
Long-chain, stronger IMF, higher BPs
48
Check CGP for fractional distillation experiment
Yes sir!
49
Polymers are ____ molecules made up of lots of small molecules called _______ which are ____ together.
long molecules, monomers, joined together
50
Polymerisation - When lots of _______ join together to form a _______.
monomers, polymer
51
To make polymers synthetically, a high ______ and a ______ are normally needed
synthetic polymers, high pressure, catalyst
52
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.
polymers, carbon-based, alkenes
cracking
53
Addition Polymers are made from _______ monomers. These monomers have a _____ ______ bond functional group. (Alkenes)
unsaturated monomers, C=C carbon double bond functional group
54
Lots of alkenes can _____ __ their ______ bonds and join together to form ______ chains. This is called _______ polymerisation
Check cgp for more info
open up double bonds, polymer chains
Addition polymerisation
55
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
replace double bond with single bond, carbons
brackens, n
56
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
repeating bit, brackets, double
57
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)
monomer
monomer in brackets
58
Condensation polymers usually involves two different types of ______ which contain different _______ ______.
2 different monomers with different functional groups
59
The monomers react together and forms ___ between them, making ______ chains
Each _______ _____ can react with the functional group of another ______, creating long chains of ________ monomers.
forms bonds between them, polymer chains
functional group, monomer, long chains of alternating monomers
60
The repeating unit of a condensation polymer always contain the _____ chains of both _______ and the link that forms between them. CGP
carbon chains of both monomers
61
Two types of Condensation polymers are
- Poly_____
- Polya____
Polyesters
| Polyamides
62
Polyesters form when ________ ____ monomers and ____ monomer react together
CGP
dicarboxylic acids, diol
63
Polyester fibres are used to make ______. They can replace ______ fibres such as wool and silk.
make clothes, replace natural fibres
64
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.
Amide (HN-CO), Ester (CO-O), middle
Add an H or OH
65
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
monomer molecules
OH, -NH2, diol, water molecule
66
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
C, dicarboxylic acid, N, O
67
Naturally occurring polymers
- ____
- ________
- _____ ____
DNA
Carbohydrates
Amino acids
68
DNA is a complex molecule that contains ______ info
It contains two ______ made of monomers called _________ that bond together in a ________ reaction
genetic info
strands, nucleotides, polymerisation reactions
69
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, G, C, T
nucleotide monomers, genes, allow organisms to function and develop
70
Carbohydates are molecules containing c____, o_____ and h______, used by living organisms to store _____.
carbon, oxygen and hydrogen, store energy (i.e. they are a source of energy).
71
S____ and C_____ are large complex carbohydrates, which are made up of many _____ units of carbohydrates, known as ______, joined together in a ____ chain.
Starch and cellulose, smaller units, sugars, long chain
72
Amino acids form polymers known as ______ via ________ polymerisation.
Proteins have many important uses in the human body, like for _____ and re___ in organisms.
proteins, condensation polymerisation
growth and repair
73
Polymers are held together by _______ bonds and ________ forces.
covalent bonds, intermolecular forces
74
In polymers, all atoms in the chain are joined by ______ _______ bonds.
There are ________ forces between the _____.
strong covalent bonds
intermolecular forces, chains
75
The _________ forces between polymer molecules are stronger than ______ molecules, so more ______ is needed to break them. This means most polymers are _____ at room temp.
intermolecular forces, simple molecules, energy, solid
76
The intermolecular forces are still weaker than _____ or _______ bonds, so polymers generally have _____ MP than ____ or ____ ______ compounds.
ionic, covalent bonds, lower MP, ionic, giant covalent
77
Before polymers melt, they become ____. The weaker the forces between the chains, the _____ the so______ point of a polymer.
Weaker forces, lower softening point
78
Polymers have different properties depending on their _______ and the _____ between the chains
structure, forces
79
```
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 _______.
ethene
lots of space, weak forces
LD is flexible
80
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 ______/
ethene, closely together, stronger forces
stiff, drainpipes
81
As well as intermolecular forces between the chains, some polymers also form _______ or _____ crosslinks.
covalent or ionic crosslinks
82
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 _____.
individual tangled chains, slide over each other
overcome forces, polymer can be melted
83
An electrolyte is a _____ or ______ _____ compound.
Molten or dissolved ionic compund
84
Cathode is the ______ electrode
negative electrode
85
Anode is the _______ electrode
positive electrode
86
Electrolysis
1) An electric _____ is passed through an _______.
The ____ move towards the electrode, where they react, and the compound ________.
current, electrolyte
ions move to electrodes, compound decomposes
87
Electrolysis
2) The positive _____ or ________ ions in the electrolyte will move towards the ______ (______ electrode) and ____ electrons (they are _______)
positive metal or hydrogen ions, cathode (negative electrode), gain electrons, they are reduced
88
Electrolysis
3) The negative ___-____ ions in the electrolyte will move towards the _____ (_______ electrode) and ____ electrons (they are ______)
negative non-metal ions, anode (negative electrode), lose electrons, they are oxidised
89
Electrolysis
| 4) As ions travel to _______, it creates a flow of ______ through the _______
electrodes, flow of charge through the electrolyte
90
Electrolysis
| 5) As ions gain or lose _______, they form the ______ element and are _______ from the electrolyte.
electrons, uncharged, discharged
91
An ionic solid can't be _________ because the ____ are in ____ ______ and so can't _____.
Solid no electrolysed, ions are fixed in place, can't move
92
Molten ionic compounds can be ________ because the ___ can ____ freely and conduct _______.
Molten yes electrolysed, ions can freely move, and can conduct electricity
93
Molten ionic liquids, e.g. lead bromide, are always broken up into their _______.
At the cathode: Pb2+ + ____ ----> Pb
At the anode: ____ ---> Br2 + ____.
elements
At the cathode: Pb2+ + 2e- ---> Pb
At the anode: 2Br- ---> Br2 + 2e-
94
During electrolysis, the electrodes should be _____ so they don't react with the _______.
______ and ______ are commonly used to make _____ electrodes
inert (unreactive), electrode
Graphite and Platinum, inert electrodes
95
If a metal is too _____ to be reduced with _____ or reacts with ______, then electrolysis can be used to ______ it.
reactive, reduced with carbon, reacts with carbon, electrolysis can be used to extract it
96
Extracting metals via electrolysis is very _______ as lots of ______ is required to ____ the ore and product the required _______.
expensive, lots of energy needed to melt ore and produce current
97
Electrolysis is the _________ of an electrolyte by an electric _______.
decomposition, current
98
Electrolysis needs:
- a ___ electrical power supply
- a negative _______, called a ______
- a positive _______, called an ______
DC power supply
negative electrode - cathode
positive electrode - anode
99
During electrolysis
- Positive ions , _____ , move to the ______
- Negative ions, _____, move the the ______.
+ ions - cations - move to cathode
- ions - anions - move to anode
100
Oxidation and Reduction of electrons
Oxidation is ____ of _______
Reduction is ____ of ________
OILRIG
Oxidation is loss of electrons
Reduction is gain of electrons
101
Reduction happens at the _______ c_____ because this is where ______ ions ____ electrons.
Reduction - negative cathode, positive ions gain electrons
102
Oxidation happens at the ______ _____ because this is where ______ ions ____ electrons.
Oxidation - positive cathode, negative ions lose electrons
103
Half equations include ___ and _______, and are used to describe the process happening at an ________.
ions and electrons, electrode
104
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)
Electrons - e-
same number of atoms, element, both sides
total charge on each side must be equal
105
For all half equations, you must show the ______ of _______
e.g. 2Cl- → Cl2 + 2e-
Pb2+ + 2e- → Pb
Both add e-
addition of electrons
106
If a metal is too _____ to be reduced with _____ or reacts with ______, then electrolysis can be used to ______ it.
reactive, reduced with carbon, reacts with carbon, electrolysis can be used to extract it
107
Extracting metals via electrolysis is very _______ as lots of ______ is required to ____ the ore and produce the required _______.
expensive, lots of energy needed to melt ore and produce current
108
Electrolysis of Alu Oxide
1) Aluminium is extracted from the ore ______ by ______. ______ contains _______ ______ (Al2O3)
ore - bauxite, electrolysis.
Bauxite contains Alu Oxide
109
Electrolysis of Alu Oxide
2) Alu oxide is heated to a very ____ _________ to form ______ Alu Oxide
_______ can be added to _______ the ___.
high temperature, molten Alu Oxide
Cryolite - lowers MP significantly
110
Electrolysis of Alu Oxide
3) The molten mixture contains ____ ions, so it'll conduct ________.
molten mixture - free ions - can conduct electricity
111
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 ____.
Al3+. negative electrode (cathode), gain 3 electrons, form neutral Al atoms
112
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_____)
negative O2- ions, positive electrode (cathode), lose 2 electrons
neutral oxygen atoms combine to form O2
Oxygen is diatomic
113
At the cathode
Process - ______ - ____ of electrons
____ + ____ --> Al
Aluminium is produced at the _______
Reduction - Gain of electrons
Al3+ + 3e- ---> Al
Produced at the cathode
114
At the anode
Process - _______ - ____ of electrons
2O2- ---> ____ + _____
Oxygen is produced at the ______
Oxidation - Loss of electrons
2O2 ---> O2 + 4e-
Oxygen is produced at the cathode
115
Overall equation for the electrolysis of Alu Oxide
_______ ______ ---> ______ + _______
_____ --> ____ + ____
Aluminium Oxide ---> Aluminium + Oxygen
2Al2O3 --> 4Al + 3O2
116
Electrolysis of Alu oxide
The electrodes are made up of _______.
The ______ needs to be ______ regularly as it reacts with ______ to product ______ _______
electrodes - carbon
electrode, replaced, O2 reacts with it to form CO2
117
Electrolysis of Aqueous solutions
Ions from the _____ compounds are present, but there will also be ________ ions (H+) and ________ ions (___) from the water.
ion
118
Electrolysis of Aqueous solutions
At the Cathode:
- Hydrogen will be produced at the ______ if the _____ is ____ reactive than _______
cathode, metal is more reactive than hydrogen
Metal more reactive than H, H is produced
119
Continued Aq Electro
- The ____ metal will be produced at the ______ if it is ____ reactive than ________.
pure metal, cathode, less reactive than H
Metal less reactive, pure metal produced
120
Aq Electro
At the anode:
______ is produced (from hydroxide ions) at the anode UNLESS _____ ions (chlroride, ______ etc) are present.
Anode - Oxygen produced, unless halogen ions present
121
Balanced half equation for the formation of oxygen from _______ ions is:
4OH- → 2H2O + __ + __
4OH- → 2H2O + O2 + 4e-
122
Reactivity series from most to least
```
________
Sodium
______
Calcium
_________
Aluminium
CARBON
____
Iron
HYDROGEN
______
Silver
____
```
```
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
CARBON
Zinc
Iron
HYDROGEN
Copper
Silver
Gold
```
123
Mass number is located in the ___-___ corner of its symbol.
The mass number tells us the no. of ______ + no. of ______ in an atoms _________.
Mass number - top left corner of symbol
Mass number = no. of protons + no. of neutrons
124
Sometimes, relative atomic mass will be on the ___-___ instead, which is the _______ mass of all the _______ of that element.
Noted by ____.
Relative Atomic mass - Also top-left corner instead
Relative Atomic Mass - The average mass of all the isotopes of that element
Ar
125
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
Chlorine - 2 Isotopes Cl 35, Cl 37
Ar - average of the isotopes when considering how common each one is
126
An Isotope is an atom of an element with the same number of ______, but different number of ______ in their nuclei.
Isotope - Same no. protons, different no. neutrons
127
Relative Formula Mass (___)
Found by ______ together the atomic _____ of all the ____ in that compounds _______ formula.
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
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 %
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
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH₄NO₃
14+4+14+(16x3)=80 = Mr of ammonium nitrate
130
A mole is a name given to a certain _______
Just like a dozen = ___, a mole is equal to a certain _______
A mole - name for a certain number
Dozen = 12
131
A mole is given by _______ _______ - its value is ______ x10^__
A mole is given by Avogadro's constant = 6.02 x 10^23
132
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
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
Moles
One mole of particles (atoms, ___, ________ etc) of any _________ will have a _____ in grams equal to the ___ or ___ for that substance.
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
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 ____
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
Moles
The mole tells us the number of _______ (atoms or molecules) in any _______ or ________.
Mole - No. of particles in any element or compound
