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Chemistry > Core + Paper 1 > Flashcards

Core + Paper 1 Flashcards

1
Q

what is an element?

A

a substance made from atoms that have the same number of protons in the nucleus

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2
Q

what is an atom?

A

the smallest particle of an element that still has its chemical properties

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3
Q

what is a molecule?

A

a molecule consists of 2 or more of the same atoms that are chemically bonded together

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4
Q

what is a compound?

A

a compound consists of two or more different elements chemically joined together

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5
Q

what is an ion?

A

an ion is an electrically charged particle

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6
Q

How is an Ion formed?

A

an ion is formed when an atom or group of atoms loses or gains electrons

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7
Q

who were the 5 scientist that helped discover the structure of the atom

A

Dalton
Thomson
Rutherford
Borh
Chadwick

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8
Q

what did Dalton think the atom was

A

dalton thought that the atom was the smallest think and could not be broken into anything smaller

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9
Q

what was Thompsons discover

A

Thompson created the plum pudding model where the atom was a sphere of positive with negative electrons dotted around

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10
Q

what did Rutherford discover and what was his model

A

Rutherfurd discovered the nucleus(gold foil experiment) and it was a solar system model where there was a positively charged nucleus surrounded by negative electrons in orbit

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11
Q

what did Bohr discover about the atom?

A

that the electrons were laid out in shells/ energy levels

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12
Q

what did Chadwick discover

A

neutrons

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13
Q

what does the (aq) state symbol mean

A

in solution

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14
Q

are metal atoms more likely to lose or gain electrons?

A

lose electrons

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15
Q

what is the relative mass of an electron?

A

1/1836

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16
Q

what is an isotope?

A

An atom with the same number of protons but different amounts of protons

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17
Q

who developed the modern periodic table?

A

Mendeleev

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18
Q

how did Mendeleev order the periodic table?

A

order of atomic mass

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19
Q

What pair of elements did Mendeleev swap

A

tellurium and iodine

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20
Q

what were the horizontal rows on the periodic table called?

A

periods

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21
Q

what are periods

A

the number of shells that an atom has

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22
Q

what were the vertical columns called?

A

groups

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23
Q

what did the groups show

A

The number of electrons on the last shell

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24
Q

what side are the metals on the periodic table

A

the left side

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25
Q

what do you call a positively charged ion?

A

cation

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26
Q

what do you call a negatively charged ion

A

anion

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27
Q

how does the name of a non-metal element change when it becomes a negative ion

A

add -ide to end

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28
Q

How does the name of a negatively charged ion change when it becomes a negative ion that also contains oxygen

A

add -ate to the end

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29
Q

what are ionic bonds?

A

strong electromagnetic forces of attraction between oppositely charged ions

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30
Q

what do you call the structure formed in an ionic compund

A

lattice

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31
Q

do ionic compounds have high or low melting/boiling points?

A

high melting point

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32
Q

why do ionic compounds have high melting and boiling points?

A

because there are many strong ionic bonds and a large amount of energy must be transferred to the lattice structure to break these bonds

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33
Q

do ionic compounds dissolve in water?

A

yes

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34
Q

state why sodium chloride does not conduct electricity in a solid state

A

the charged particles are not free to move around and carry a current

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35
Q

what is a covalent bond?

A

a bond formed when a pair of electrons are shared between 2 atoms

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36
Q

give 3 properties of covalent bonds

A
  • are strong
  • formed between non-metal atoms
  • often produce molecules which can be compounds or elements
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37
Q

how do we model covalent bonds

A

dot and cross diagrams

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38
Q

what are simple molecular substances in terms of their bonding

A

consist of just a few atoms joined together by strong molecular bonds

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39
Q

why do simple molecular substances have low boiling/melting points?

A

even though there are strong covalent bonds, the molecules are joined together by weak intermolecular forces that are broken during state changes

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40
Q

what state are simple molecular substances in at room temp

A

liquid or gas

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41
Q

do simple molecular substances conduct electricity?

A

no, because their molecules are not electrically charged and there are no electrons that are free to move

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42
Q

name a simple molecular substance that dissolves in water

A

chlorine, carbon dioxide, sulfur dioxide

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43
Q

what are giant covalent bonds in terms of their bonding

A

they consist of many atoms, that are joined by strong covalent bonds and are arranged in a regular lattice structure

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44
Q

why do giant covalent bonds have a high boiling temperature?

A

it is because of how a lot of energy must be transferred to break the many strong covalent bonds during melting and boiling.

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45
Q

give 2 examples of giant molecular substances

A

Diamond and Graphite

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46
Q

why does graphite conduct electricity but diamond doesn’t

A

this is because carbon has the ability to form 4 covalent bonds. but in graphite, carbon only forms 3 which means that there is a delocalised electron that is free to move around and carry the current

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47
Q

what are some other forms of carbon?

A

graphene’s and fullerenes

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48
Q

what is the structure of graphene?

A

graphene is a giant molecular substance that resembles a single layer of carbon. each atom is connected to three other atoms.

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48
Q

what are the 3 properties of graphene?

A
  • graphene conducts electricity because of delocalised electron
  • graphene is very strong and flexible due to its strong covalent bonds
  • graphene is almost transparent because it is only one atom thick
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49
Q

what are the 2 types of fullerenes?

A

buckyballs and nanotubes

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50
Q

give 3 properties of buckyballs

A

-have delocalised electrons so they can conduct electrons
-the carbon atoms are arranged in pentagons and hexagons
-they are soft when in the solid state because they have weak intermolecular forces

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51
Q

give 3 properties of nanotubes

A

-have closed ends or open ends
-can conduct electricity because they have delocalised electron
-are very strong because the structure has many strong covalent bonds

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52
Q

how does the appearance vary on metals to non-metals

A

metals are shiny
while non-metals are dull

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53
Q

how do electrical and conduction vary on metals and non-metals

A

metals can conduct electricity and are good conductors of heat

while some non-metals are also good conductors but cannot conduct electrical

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54
Q

how do density and meting points compare on non-metals and metals?

A

metals have high melting points and density while

non-metals have low melting points and have a low density

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55
Q

what is the opposite of malleable

A

brittle

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56
Q

describe the structure and bondings of metal

A
  • made up of a large lattice of positively charged metal ions and surrounded by a sea of delocalised electrons
  • metallic bonds are strong electrostatic forces of attraction between positive metal ions and delocalised electrons
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57
Q

why are metals malleable?

A

layers of ions have the ability to slide over each other and change the shape of the metal without shattering

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58
Q

what does ductile mean

A

the ability to be stretched into a thin wire without shattering

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59
Q

what are the five models that can be used to represent atom structure?

A
  • written formulae
  • drawn structures
  • ball-and-stick diagrams
  • space-filling models
  • Dot and cross diagrams
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60
Q

what are the empirical formulae?

A

the simplest whole number ratio of atoms of each element

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61
Q

what is the symbol for relative atomic mass?

A

Mr

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62
Q

write down the 6 steps to calculating the empirical formula using grams

A
  1. write down the symbol of each element as a header
  2. write down the mass of each element (given)
  3. write down the atomic mass of each element
  4. for each element calculate mass / atomic mass
  5. divide each answer by the smallest answer.
  6. then multiply the numbers to remove fractions and write down the empirical formulae
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63
Q

what is the conservation of mass?

A

the total mass of reactants and products stays constant during a chemical reaction. The total mass before and after a reaction is the same.

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64
Q

what is a closed system?

A

a closed system is a situation where no substance can enter or leave during a reaction

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65
Q

what is the stoichiometry of a reaction?

A

it has to do with the ratio of the amounts of reactants and products involved when you balance a chemical equation you are finding the stoichiometric equation

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66
Q

what is a solution?

A

a solution is a mixture of a solute in a solvent

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67
Q

what is the solvent?

A

the solvent is the substance that the solute dissolves in

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68
Q

what is the solute?

A

the solute is the substance that dissolves

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69
Q

what does dm3 stand for

A

cubic decimetres

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70
Q

what do you need to calculate the concentration of a solution?

A

the mass of the solute in grams and the volume of the solution in cubic decimetre

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71
Q

how many cm cubes is a dm

A

1000cm3

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72
Q

what is the unit of measurement for concentration?

A

dm-3

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73
Q

what is a mole

A

a mole is the unit for the amount of a substance

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74
Q

what is Avagadro’s constant?

A

6.02 * 10^23

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75
Q

what is the mass of 1 mole of carbon?

A

12g

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76
Q

what is the formula for moles?

A

amount(mol) = mass(g)/Mr

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77
Q

what is the arrangement of particles like in solids?

A

close together, regular pattern

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78
Q

what is the arrangement of particles like in liquids?

A

close together, random

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79
Q

what is the arrangement of particles like in gases?

A

far apart, random

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80
Q

what is the movement of particles like in solids?

A

vibrate around a fixed position

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81
Q

what is the movement of particles like in liquids?

A

move around each other

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82
Q

what is the movement of particles like in gases?

A

fast in all direction

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83
Q

order the different states of matter. from which has the least stored energy to the most

A

solids - least
liquid
gasses - most

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84
Q

what do call gas to liquid?

A

condensing

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85
Q

what do call liquid to solid?

A

freezing

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86
Q

what do you call solid to liquid?

A

melting

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87
Q

what do call liquid to gas?

A

boiling./evaporating

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88
Q

what do you call gas to solid?

A

deposition

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89
Q

what do you can solid to gas?

A

sublimation

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90
Q

what is an element?

A

it is a substance that consists only of atoms with the same atomic number

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91
Q

what is a compound?

A

a compound is a substance that consists of two or more different atoms(different elements) that are chemically joined together

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92
Q

what 2 structures can elements exist as

A

atoms or molecules

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93
Q

what is a pure substance?

A

a substance that only contains one element or compound

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94
Q

what is a mixture?

A

a substance that contains different elements and/or compounds that are not chemically joined together

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95
Q

what is the difference between impure and pure substances based on their melting point?

A

pure substances will have a sharp melting point while impure substances will not because it has many different impurities that will each have different melting points

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96
Q

what is fractional distillation used for

A

to separate liquids from a mixture of miscible liquids

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97
Q

what is simple distillation used for?

A

to separate a solvent from a solution

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98
Q

explain simple distillation

A

simple distillation works because the solute will have a higher boiling point than the solvent. so when the solution is heated the solvent will boil, pass into the condenser, cool and collect in the other container while the solute is left.

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99
Q

explain fractional distillation

A

fractional distillation works because the liquids that need to be separated will all have different boiling points. so by heating the mixture up:
- the mixture boils
- hot vapour rises up the column
- vapour condenses when it hits the cool surfaces of the column it condenses and drips back down
- the fraction with the lowest boiling point will reach the top of the column first
- its vapour will then pass into the condenser where it is cooled and transferred into a different container
- if you carry on heating, the vapours from the fractions with higher boiling points pass into the condenser

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100
Q

what do you use filtration for

A

you use filtration to separate an insoluble substance from a liquid or a solution.

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101
Q

what do you call the material left in the filter after filtration

A

residue

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102
Q

what do you call the solution created from filtration

A

filtrate

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103
Q

what do you produce with crystallisation?

A

solid crystals

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104
Q

what are the 3 steps to crystallisation?

A
  1. the solution is heated to remove enough solvent to make the solution saturated
  2. as the solution cools crystals will form
  3. The crystals are then separated from the liquid and dried
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105
Q

why do we use a water bath in crystallisation?

A

to give you more precise control over the temperature

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106
Q

why does filtration work?

A

because the filter paper has tiny pores that are large enough to let dissolved substances through while also being small enough to stop insoluble solid particles going through

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107
Q

why does crystallisation work

A

This is because the solubility of a solvent is higher the higher the temperature. so when a saturated solution cools down the excess solute forms crystals.

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108
Q

what is paper chromatography used for

A

to separate the mixture of soluble substances

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109
Q

explain the process of setting up chromatography

A
  1. put spots of the samples you want to separate onto the paper and label them with a pencil.
  2. put the paper into liquid, but make sure it does not reach the level of the inks.
  3. as the water moves up the sheet of paper the water will dissolve the samples.
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110
Q

explain how chromatography works

A

chromatography works as the more soluble compounds are carried up the paper faster than less soluble ones, which makes the compounds separate.

111
Q

what are the 2 phases of chromatography?

A
  • stationary phase
  • mobile phase
112
Q

what is the stationary phase in chromatography?

A

a substance that does not move

113
Q

what is the mobile phase in chromatography?

A

a substance that moves through the stationary phase - the solvent

114
Q

what can the Rf be used for

A

identify different substances

115
Q

how do you know if a substance is pure or not using chromatography?

A

a pure substance will only have 1 spot while a compound will have more than one spot

116
Q

what are the formulae for finding the RF value?

A

distance travelled by spot/distance travelled by solvent

117
Q

what are two features that potable drinking water must have

A

low levels of contaminating substances
low levels of microbes

118
Q

what are the 3 phases of water treatment?

A

sedimentation
filtration
chlorination

119
Q

what happens in the sedimentation stage of water treatment

A

the water is left to rest so that the large insoluble particles sink to the bottom of the tank

120
Q

what happens in the filtration stage of water treatment

A

small insoluble particles are removed by filtering through sand and gravel

121
Q

what happens in the chlorination stage of water treatment

A

chlorine gas is bubbled through water to kill microbes

122
Q

what process can be used in seawater treatment?

A

simple distillation

123
Q

what are the 2 positives of treating seawater?

A
  • there is plenty of seawater
  • produces pure water by killing microbes
124
Q

what is a negative of using distillation for the treatment of seawater?

A

needs a lot of energy to heat the water

125
Q

what are the 3 properties of acids?

A
  • have a PH less than 7
  • they are a source of hydrogen ions (Hydrochoric acid produces h+ ions)
  • the higher the concentration of H+ the lower the PH of the acidic solution
126
Q

what are the 3 properties of alkalis?

A
  • the PH is greater than 7
  • they are a source of hydroxide ions (sodium hydroxide releases OH- ions)
  • the higher the concentration of OH- ions the higher the pH of the solution
127
Q

what is the range of the PH scale?

A

0-14

128
Q

what colour does the universal indicator go if the solution is acidic

A

red

129
Q

what colour does the universal indicator go if the solution is alkaline

A

blue/purple

130
Q

what colour does litmus paper go if the solution is acidic?

A

red

131
Q

what colour does litmus paper go if the solution is alkaline?

A

blue

132
Q

what colour does phenolphthalein go if the solution is acidic?

A

colourless

133
Q

what colour does phenolphthalein go if the solution is alkaline?

A

pink

134
Q

what colour does methyl orange go if the solution is acidic?

A

red

135
Q

what colour does methyl orange go if the solution is alkaline?

A

yellow

136
Q

how can you change a concentrated solution to a dilute solution?

A

by adding more water

137
Q

how can change a dilute solution into a concentrated solution?

A

add more solute
evaporate some of the water

138
Q

1cm cubed of 2 mol dm-3 is added to 4sm cubed of water what is the new concentration

A

1/5 * 2 = 0.4 mol dm-3

139
Q

why are hydrochloric acid and sulfuric acid strong acids

A

because they fully dissociate into ions when added to the solution, and since the concentration of H+ ions is what determines the strength of the solution they are both strong acids.

140
Q

what does dissociation mean

A

the process in which molecules separate into ions

141
Q

why is ethanoic acid weak?

A

because it only partially dissociated into ions in solution. and since the concentration of H+ ions is what determines the strength of an acid, it is weak

142
Q

what does it mean when it says that alkali metals have a soluble base?

A

one that dissolves in water

143
Q

what is a base (acids and alkali topics)

A

any substance that reacts with acids to form salt and water only

144
Q

what are bases normally (acids and alkali topics)

A

they are usually metal hydroxides

145
Q

what is the simple word equation for a reaction between a base and an alkali.

A

base + acid –> salt + water

146
Q

how do salts form (acids and alkali topics)

A

they form when hydrogen ions in an acid are replaced by metal ions or ammonium ion

147
Q

how do we name salts?

A

metal in base + acid name
sodium hydroxide + hydrochloric acid —> sodium chloride

148
Q

what does a metal + acid make

A

metal + acid —> salt + hydrogen

149
Q

what does a metal carbonate and an acid make

A

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

150
Q

what test do we use to test for hydrogen?

A

hydrogen splint pop test, the lighted splint will ignite the hydrogen and make a pop sound

151
Q

how do we test for carbon dioxide?

A

carbon dioxide will turn lime water milky or cloudy white

152
Q

what are the 3 steps for the practical use of making salts from insoluble bases?

A
  1. add an excess base to the acid
  2. filter the excess base from the solution
  3. slowly evaporate solution to get crystals
153
Q

what are the 3 steps for the practical use of making salts from soluble bases?

A
  1. use titration to find the exact volume of the soluble base that is needed to react it with the acids
  2. mix the acid and the soluble in the correct proportions to produce a perfectly saturated solution
  3. warm the solution to evaporate the water and leave salt crystals behind
154
Q

what are the 6 steps of titration?

A
  1. put acid into the burette
  2. use a pipette to put a known volume of alkali into the conical flask
  3. put a few drops of indicator into the conical flask
  4. record the amount of acid in the burette
  5. add acid to the alkali until the colour changes
  6. record the end amount of acid left and calculate how much acid was needed to neutralise the acid
155
Q

what is the Titre

A

the tire is the exact volume needed to exactly neutralise an acid

156
Q

what are the 6 different chemical types that will form a soluble solution?

A
  • common sodium salts
  • common potassium salts
  • common ammonium salts
  • all nitrates
  • common chlorides
  • common sulfates
157
Q

what 3 hydroxides that are soluble

A

sodium hydroxide
potassium hydroxide
ammonium hydroxide

158
Q

what 3 carbonates that are soluble

A

sodium carbonate
potassium carbonate
ammonium carbonate

159
Q

what are 2 chloride exceptions that are insoluble?

A

silver chloride
lead chloride

160
Q

what are 3 sulfate exceptions that are insoluble?

A

lead sulfate
barium sulfate
calcium sulfate

161
Q

what are 2 chemical types that produce insoluble salts?

A

common hydroxides
common carbonates

162
Q

what is electrolysis used for

A

it is used to decompose ionic compounds in the molten state or dissolved in water

163
Q

what is an electrolyte?

A

an ionic compound in a molten or dissolved state

164
Q

what is the definition of electrolysis?

A

a process in which electrical energy from a direct current supply decomposes an electrolyte

165
Q

what is an anion?

A

negatively charged ions that move to the positively charged electrode (anode)

166
Q

what is a cation?

A

positively charged ions that move the (cathode)

167
Q

what is the charge of the cathode

A

negative

168
Q

what is the charge of the anode?

A

positive

169
Q

what happens to the anion during electrolysis

A

oxidised

170
Q

what happens to the cation during electrolysis

A

reduced

171
Q

what ions does water change into

A

H+ and HO-

172
Q

what happens at the cathode when electrolysis happens in a solution

A

at the negative electrode, hydrogen will be produced unless the compound contains ions from a metal less reactive than hydrogen, in which case a metal is produced

173
Q

give 2 metals that are below hydrogen in the reactivity series

A

copper and silver

174
Q

what happens at the anode when electrolysis happens in a solution

A

oxygen is produced unless the compund contains halides in which case the anode will make a halide molecule with 2 of the halide

175
Q

what are the products when a metal with a reactivity higher than hydrogen reacts with water

A

metal + water –> metal hydroxide + hydrogen

176
Q

what is produced when a metal reacts with an acid

A

metal + acid –> salt + hydrogen

177
Q

true or false “The rate of reaction is greater in a metal if the acid is cold,”

A

false

178
Q

give an exception for metals that don’t react with water even though they are more reactive than hydrogen and give a reason

A
  • aluminium = It has a layer of aluminium oxide that stops the water from reaching the metal below
179
Q

give an exception for metals that surprisingly slowly react with water even though they are more reactive than hydrogen and give a reason

A
  • magnesium = a layer of sparingly soluble magnesium hydroxide forms which slows the reaction
180
Q

give an exception for metals that don’t react with acid even though they are more reactive than hydrogen and give a reason

A

in the reaction of calcium with dilute sulfuric acid

181
Q

give the reactivity series in order from most to least reactive

A

(Please Stop Calling Me A Zebra I,ll Her Calling Me A Super Powerful Giraffe)

-potassium
-sodium
-calcium
-magnesium
-aluminium
-zinc
-Iron
-hydrogen
-copper
-mercury
-Silver
-platinum
-gold

182
Q

what happens in a metal displacement reaction

A

a more reactive metal will displace a less reactive metal from its salt

183
Q

explain how metal displacement reactions are redox

A
  • the atoms of the more reactive metal are oxidised - lose electron
  • the metal cations of the less reactive metal are reduced - they gain electrons
184
Q

how does a metal form a cation

A

metal atoms lose electrons to form cation

185
Q

metals react with water to form :

A

metal hydroxides

186
Q

metals react with dilute acids to form

A

salts

187
Q

why are some metals more reactive than other

A

because the more reactive metal gives away its outer electron easier to form a cation

188
Q

what is an ore?

A

an ore is a rock that contains a metal that can be extracted

189
Q

how can reduce a metal oxide to just a metal?

A

heat it with carbon or hydrogen to create metal + carbon dioxide

190
Q

name a way to extract metal from ores

A

electrolysis

191
Q

why is electrolysis not used to extract all metals?

A

because it requires constant electricity which is expensive

192
Q

name 5 metals that are extracted from ores by electrolysis

A

potassium
sodium
calcium
magnesium
aluminium

193
Q

give the 3 methods that are used to extract metals from ores

A

electrolysis
reduction
displacement reaction

194
Q

what methods of extraction are used to extract elements less reactive than carbon

A

reduction

195
Q

how can you use reducing to extract ores?

A

by reducing metal oxide to metal and carbon dioxide

196
Q

what is a biological method of extracting metal from ores?

A

phytoextraction
bioleaching

197
Q

how does phytoextraction work

A

by getting plants to absorb the metal compounds through it’s roots and then burning the plants the ash will contain metal compounds

198
Q

what are the 3 disadvantages of extracting metals from ores?

A

uses up limited resources
uses a lot of energy
damages the environment

199
Q

what are the 4 advantages of recycling metals?

A

metal ores will last longer
less energy is needed
fewer quarries and mines are needed
less noise and dust are produced
less land is needed

200
Q

what are the 3 negatives of recycling metals?

A

used metal items must be collected and transported to the recycling centre

different metals must be removed from used items and sorted

recycling saves different amounts of energy depending on the metal involved

201
Q

what is a life cycle assessment?

A

is a cradle-to-grave analysis of the impact of an item on the environment

202
Q

what are the 4 stages of a life cycle assessment?

A
  • obtaining raw materials
  • manufacturing the product
  • using the product
  • disposing of the product
203
Q

what are the 6 factors that a LCA will need?

A

an LCA is likely to need data on these factors at most or all stages;
- the use of energy
- the release of waste materials
- transport and storage

an LCA is also likely to need data on
- whether the raw materials needed are renewable or non-renewable
- whether any of the products can be reused or recycled
- how the product is disposed of

204
Q

where are transitional metals found?

A

they are placed between groups 2 and 3

205
Q

what are 2 typical physical properties of transitional properties?

A

high melting point
high density

206
Q

what are 2 chemical properties of transitional properties?

A

formation of coloured compounds
can be catalysts

207
Q

what are 4 chemical and physical properties of group 1 and 2 metals?

A

relatively low melting points
relatively low density
formation of white or colourless compounds
lack of catalytic activity

208
Q

which process is iron a catalyst for

A

the Haber process

209
Q

what does the oxidisation of metals result in

A

corrosion

210
Q

what is the name given to the corrosion of iron and steel?

A

rusting

211
Q

what 2 things does iron need to rust

A

oxygen and water

212
Q

what are the 4 prevention methods used to stop the rusting of iron? (keeping water + oxygen away from it)

A

painting
using oil and grease
coating with plastic
coating with another metal

213
Q

give one way to keep oxygen away from iron to prevent rust

A

store the iron in a vacuum

214
Q

give one way to keep water away from iron to prevent rust

A

put the item in a container with a desiccant

215
Q

what is desiccant

A

something that absorbs water vapour

216
Q

what are the benefits of electroplating iron/steel?

A

improves its appearance
improves its resistence to corrosion

217
Q

what happens in electroplating

A

a thin layer of unreactive metal such as nickel, silver or gold is deposited on the surface of the metal object to keep air and water out

218
Q

what is the name of the process of coating iron/steel objects with a thin layer of zinc to prevent them from rusting

A

galvanising

219
Q

how does galvanising work

A

by coating iron or steel with a more reactive metal the oxygen and water will corrode the zinc instead of the iron/steel

220
Q

what is an alloy?

A

a mixture of metal with one or more other elements, these elements are usually other metals or carbons

221
Q

what is steel made out of

A

iron mixed with carbon

222
Q

what is stainless steel made out of

A

iron and chromium

223
Q

how does stainless steel resist corrosion?

A

the layer of chromium will form an invisible thin layer of chromium oxide that forms on the surface of the steel and prevents air and oxygen from reaching the iron

224
Q

what is magnalium made out of

A

aluminium and magnesium

225
Q

what are some properties of magnalium?

A

low density

226
Q

what is magnalium used for

A

cars and aeroplanes

227
Q

what is jewellery gold made out of

A

gold and copper

228
Q

what are some typical properties of jewellery gold?

A

attractive, resistant to corrosion

229
Q

what is brass made out of

A

copper and zinc

230
Q

what are some typical properties of brass?

A

hard
resistant to corrosion
good electrical conductor

231
Q

what is brass used for

A

electrical plugs and coins

232
Q

why does adding carbon to iron make it stronger

A

the larger carbon atoms will stop the layers of pure iron from sliding over each other relatively as the large carbon atoms will disrupt the layers and prevent the layers from sliding over each other

233
Q

what is the formula for calculating the concentration?

A

concentration = amount of solute/volume of solution

234
Q

what is the unit for measuring concentration?

A

mol/dm-3

235
Q

how do you convert from mol dm-3 to g/dm3

A

multiply by Mr

236
Q

what is the yield in chemistry?

A

the mass of the product made in a chemical reaction

237
Q

what are the 3 types of yields in chemistry?

A

theoretical yield
actual yield
percentage yield

238
Q

what is the theoretical yield?

A

the maximum amount of product that can be made

239
Q

what is the actual yield?

A

the mass of the product that you really get at the end of a reaction, this is always less than the theoretical yield

240
Q

what are 3 reasons why the yield in chemical reactions is less than usual

A

incomplete reactions if the reaction reaches an equilibrium

practical losses during the experiment

side reaction

241
Q

what is the formula for percentage yield?

A

(actual yield / theoretical yield) * 100

242
Q

what is atom economy?

A

a way of measuring the atoms wasted when making a substance

243
Q

what 2 things do you need to know to calculate the atom economy?

A

the relative formula masses of the products

the balanced equation for the reaction

244
Q

what is the formula to calculate atom economy?

A

total Mr(formula masses) of useful product
—————————————————-*100
total Mr of all products

245
Q

what is Avagadro’s law on molar gases?

A

it states that equal volumes of gas at the same temperature and pressure will have the same number of molecules

246
Q

what are the 3 factors that affect the volume occupied by a gas?

A
  • the number of particles present
  • the temperature of the gas
  • the pressure of the gas
247
Q

what does the molar volume mean in terms of gas?

A

the amount of volume occupied by one mole of a gas at room temp and atmospheric pressure or 24 dm3/mol

248
Q

what is the formula for the volume of gas?

A

molar volume * amount

249
Q

what is the equation for finding the mass of a gas?

A

Mr * amount

250
Q

what are reversible reactions?

A

the direction of some reversible meaning that the direction of the reaction can be altered by changing the conditions

251
Q

what is a dynamic equilibrium?

A

when the forward rate of a reversible reaction is the same as the backward rate of a reaction.

252
Q

what is the Haber process?

A

is a reversible reaction between nitrogen and hydrogen that forms ammonia. n2+ 3h2 –> 2nH3

253
Q

what are some conditions needed for the Haber process?

A

iron catalyst
200 atmosphere
450 temperature

254
Q

what 4 factors affect the position of the equilibrium in a chemical reaction

A

temperature
pressure
the concentration of the reacting substance
catalyst added

255
Q

what happens to the position of the equilibrium and the rate at which it will be reached if temperature is increased

A

it will move in the direction of the endothermic reaction
and the rate is increased

256
Q

what happens to the position of the equilibrium and the rate at which it will be reached if pressure is increased

A

the equilibrium will move in the direction of the fewest molecules of gas and the rate will be increased

257
Q

what happens to the position of the equilibrium and the rate at which it will be reached if concentration is increased

A

will move in the direction away from the reacting substance and the rate is increased

258
Q

what happens to the position of the equilibrium and the rate at which it will be reached if a catalyst is added

A

no change in the position of equilibrium but the rate is increased

259
Q

what factors affect the conditions chosen for industrial processes

A

the availability of raw materials and energy supplies.

the control of temperature and pressure

the use of a suitable catalyst

260
Q

what 3 chemicals help plants grow

A

nitrogen
phosphorus
potassium

261
Q

what soluble compund is added to fertilisers to supply nitrogen

A

nitrate and ammonium salts

262
Q

what soluble compund is added to fertilisers to supply phosphorus

A

phosphate salts

263
Q

what soluble compund is added to fertilisers to supply potassium

A

potassium salts

264
Q

why is ammonium used in fertilisers?

A

they are a source of soluble nitrate

265
Q

how is ammonium sulfate created in labs?

A

ammonium solution and dilute sulfuric acid are brought from chemical manufacturers. the process involves only a few stages (titration then crystallisation) but only every little product is made

266
Q

how is ammonium sulfate created in factories?

A

will use natural gas, air and water (raw materials needed to make ammonia)
sulfur, air and water will be used to make sulfuric acid
this process will involve many stages but a lot of produce will be made

267
Q

what are 2 ways that can be used to create a voltage?

A

chemical cells and fuel cells

268
Q

what are the steps to make a simple chemical cell?

A

make one beaker with zinc dipped in zinc sulfate solution and another with copper dipped in copper sulfate solution. connect the 2 metals with crocodile clips wired to a voltmeter. connect the 2 solutions with filter paper soaked in KCl

269
Q

how does a chemical cell work

A

electrons will flow through the zinc and copper because zinc is more reactive. Ions will pass through the filter paper completing the circuit.

270
Q

what is a hydrogen-oxygen fuel cell?

A

where hydrogen and oxygen are used to make a voltage. and where water vapour is the only product.

271
Q

what are 2 advantages of chemical cells?

A

suitable for portable devices
are cheap to manufacture

272
Q

what are 2 disadvantages of chemical cells?

A

may contain harmful substances
do not produce voltage when one of the reactants run out

273
Q

what are 2 advantages of hydrogen-oxygen fuel cell?

A

produce water as only waste product

produce a voltage as long as the fuel and air are supplied

274
Q

what are 2 disadvantages of hydrogen-oxygen fuel cell?

A

are not suitable for portable devices

are expensive to manufacture

Chemistry (11 decks)

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