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BMAT Section 2 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Relative mass of an electron

A

1/1870

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2
Q

Relative mass of a proton

A

1

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3
Q

Relative mass of a neutron

A

1

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4
Q

Relative charge of a neutron

A

0

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5
Q

Relative charge of a proton

A

+1

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6
Q

Relative charge of an electron

A

-1

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7
Q

Atomic number

A

Same as the number of electrons

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8
Q

Number of electrons in positively charges ions =

A

Atomic number - charge on ion

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9
Q

Number of electrons for negatively charged ions =

A

Atomic number + charge on ion

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10
Q

Does the number of protons in an atom change during a chemical reaction?

A

No, the nucleus isn’t involved in chemical reactions

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11
Q

Mass spectra show the relative abundance against the mass/ charge ratio, what does this show?

A

The abundance of isotopes

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12
Q

Reactivity down group 1

A

Increases

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13
Q

Ammonia

A

NH3

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14
Q

Carbon Dioxide

A

CO2

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15
Q

Carbon monoxide

A

CO

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16
Q

Methane

A

CH4

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17
Q

Nitrogen dioxide

A

NO2

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18
Q

Nitrogen monoxide

A

NO

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19
Q

Sulfur dioxide

A

SO2

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20
Q

Sulfur trioxide

A

SO3

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21
Q

Water

A

H2O

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22
Q

Ammonium

A

NH4+

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23
Q

Carbonate

A

CO32−

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24
Q

Hydroxide

A

OH-

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25
Q

Nitrate

A

NO3−

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26
Q

Sulfate

A

SO42−

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27
Q

Ethanoic acid

A

CH3COOH

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28
Q

Buckminsterfullerene

A

C60

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29
Q

Acid + Alkali

A

Salt + water

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30
Q

Acid + Carbonate

A

Salt + water + carbon dioxide

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31
Q

Acid + Ammonia

A

Ammonium salt

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32
Q

Acid + metal

A

Salt + hydrogen

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33
Q

Dynamic equilibrium

A

No chemicals can get in or out, reversible reactions can reach a state of dynamic equilibrium. At this point, both the forwards and reverse reaction are taking place simultaneously and at the same rate

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34
Q

More reactants

A

Moves eqm to the right

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35
Q

More products

A

Equilibrium moves to the left

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36
Q

Increase temperature on an exothermic reaction

A

Moves reaction to the endothermic direction (to the left) to lower the temperature

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37
Q

Increasing temperature on an endothermic reaction

A

Moves reaction to exothermic side (to the right) to increase the temperature

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38
Q

Increase pressure

A

Moves to sides with fewer particles

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39
Q

Isotope definition

A

Variations of elements that differ only in neutron number - abundance from mass spectrometer

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40
Q

RAM definition

A

Average atomic mass of a chemical element found relative to 1/12th the mass of a sample of C12

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41
Q

How are elements grouped?

A

According to electron number - which results in similar chemical properties

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42
Q

How to construct an ionic equation

A

Split up (aq) ions and remove the spectator ions (solids and liquids can be present but only if not on both sides of the equation)

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43
Q

Reversible reaction

A

Reaction that doesn’t go to completion as not all the reactants turn into products (closed system) - Eqm is reached when the forward rate = the backward rate

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44
Q

Avogadro’s number

A

6.02 x10^23 = number of particles in 1 mole of a substance

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45
Q

% composition by mass =

A

(mass/ total mass) x 100

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46
Q

How to calculate masses of products which reagent do you use?

A

Limiting

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47
Q

Ideal gas occupies…

A

24dm^3 at a given temperature and pressure

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48
Q

Volume (dm^3) when given moles =

A

n (moles) x Vm (24dm^3)

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49
Q

Number of moles given conc. and volume =

A

Concentration (mol dm^-3) x Volume (dm^3)

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50
Q

How to perform a titration calcuation

A

Use conc. and reacting ratios from a balanced equation

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51
Q

Oxidation is…

A

Gain of oxygen, loss of hydrogen or loss of electrons

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52
Q

Reduction is…

A

Loss of oxygen, gain of hydrogen or gain of electrons

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53
Q

Oxidation state of O

A

-2

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54
Q

Oxidation state of H

A

+1

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55
Q

Oxidation state of G1 Metals

A

+1

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56
Q

Oxidation state of G2 Metals

A

+2

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57
Q

Oxidation state of Cl

A

-1

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58
Q

Disproportionation

A

Reduction and oxidation occur to the same element in the same equation

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59
Q

Oxidising agent

A

Thing being reduced

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60
Q

Reducing agent

A

Thing being oxidised

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61
Q

Element definition

A

Primary constituent of matter, distinguished by it’s atomic number

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62
Q

Compound definition

A

Composed of 2 or more elements - inseparable

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63
Q

Mixture definition

A

2 or more elements - separable

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64
Q

How are ions formed?

A

By the transfer of electrons from metals to non-metals (ions of opposite charge attract to form ionic compounds)

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65
Q

Group 1 and 2 form what ions?

A

+1 and +2 respectively

66
Q

Group 6 and 7 form what ions?

A

-2 and -1 respectively

67
Q

Common features of ionic compounds

A

High melting/ boiling points (strong oppositely charged electrostatic forces of attraction), electrical conductor when melted or aqueous (charged particles can move) and giant ionic lattice structure

68
Q

Covalent bond

A

Atoms share 1 or more pairs of electrons

69
Q

Small covalent examples

A

H2O, NH3 and CH4

70
Q

Giant covalent examples

A

Diamond, graphite and silicon dioxide

71
Q

Simple covalent properties

A

Low mpts and bpts (weak intermolecular forces of attraction) and don’t conduct (no free electrons to carry charge)

72
Q

Giant covalent properties

A

Very high mpts and bpts (strong covalent bonds must be broken) and variable electrical conductivity (depends on availability of free electrons)

73
Q

Structure in metals

A

Giant structure of positively charged cations surrounded by free moving delocalised electrons

74
Q

Properties of metals

A

High mpt and bpts (lattice structure with electrostatic forces) and conduct electricity (free moving electrons to carry charge)

75
Q

What cause physical properties of substances

A

Structure AND bonding

76
Q

Properties and common reactions of Group 1

A

Silvery, soft, highly reactive, low melting points that decrease down the group, react with water to form metal hydroxides and H2

77
Q

Properties of Group 7 elements

A

Get darker down the group, low melting and boiling points that increase down the group (larger atoms)

78
Q

Properties of Group 8 elements

A

Low boiling points that increase down the group, inert because of full outer shell

79
Q

How do displacement reactions occur?

A

More reactive displace elements with lower reactivities (result of the ability to attract valence electrons)

80
Q

What does a pure substance give on a chromatogram?

A

1 single spot

81
Q

Acid definition

A

Substance that can form H+ ions in solution or is an H+ donor

82
Q

Acid + Metal ->

A

Salt + Hydrogen

83
Q

Acid + Carbonate ->

A

Salt + water + CO2

84
Q

Acid + metal hydroxide ->

A

Salt + water

85
Q

Acid + Base ->

A

Salt + Water

86
Q

Acid + metal oxide ->

A

Salt + Water

87
Q

Strong

A

Completely dissociate into ions in solution

88
Q

Weak

A

Partially dissociate into ions in solution

89
Q

Dilute

A

Low conc. of ions

90
Q

Concentrated

A

High conc. of H+ ions

91
Q

pH is a measure of…

A

H+ ion concentration on a logarithmic scale

92
Q

What is a di/tri/polyprotic acid?

A

Can donate more than 1H+ ion

93
Q

Base definition

A

Forms OH- ions in solution and/ or accept H+ ions

94
Q

Acid + Base ->

A

Salt + Water (neutralisation) and normally exothermic

95
Q

Increase concentration on rate of reaction

A

Faster - more reactant particles

96
Q

Increase temp on reaction rate

A

Faster - more energy and collisions

97
Q

Increase particle size on rate

A

Slows - surface area

98
Q

Add a catalyst to the rate

A

Faster - more collisions

99
Q

Increase pressure on rate

A

Faster - more collisions

100
Q

Collision theory

A

Reaction progression dependent on the correct collision and alignment of the particles

101
Q

Exothermic diagram

A

Products lower than reactants

102
Q

Endothermic diagram

A

Products higher than reactants

103
Q

Catalysts key features

A

Not used up, chemically unchanged by the end of a reaction, provide and alternate reaction mechanism with a lower Ea - Don’t affect position of EQM

104
Q

Exothermic reaction H =

A

-ve

105
Q

Endothermic reaction H =

A

+ve

106
Q

Bond breaking

A

Endothermic

107
Q

Bond forming

A

Exothermic

108
Q

H from bond energies =

A

Reactants - Products

109
Q

Electrode

A

Solid electrical conductor that carries current into a non-metallic compound

110
Q

Cathode

A

Negative electrode

111
Q

Anode

A

Positive electrode

112
Q

Electrolyte

A

Substance that produces an electrically conducting solution when dissolved in a polar solvent (eg. H2O)

113
Q

Why is AC not used in electrolysis

A

Would constantly switch the anode and the cathode - leading to an uneven deposition of ions

114
Q

Anode formation

A

Anions (-) loose electrons to form atoms/ molecules (oxidation)

115
Q

Cathode formation

A

Cations (+) receive electrons to form atoms/ molecules (reduction)

116
Q

Electrons on half equations for OX/ RED

A

Left side for RED

Right side for OX

117
Q

What is formed at electrodes?

A

Aq solutions can attract more than one ion at an electrode (one rules) and molten binary compounds only contain 2 elements

118
Q

Longer carbon chain properties

A

More viscous, higher bpt/ mpts and smokier flames

119
Q

Homologous series definition

A

Species with the same functional group that exhibits similar chemical properties

120
Q

Br2 test

A

Decolourises in an alkene

121
Q

Alcohol + Na ->

A

Sodium ethoxide and H2

122
Q

Carboxylic ACID

A

Weak acids - don’t fully dissociate

123
Q

COOH + OH

A

Produce an ester

124
Q

Reactivity series mnemonic

A

Please Stop Calling Me A Careless Zebra Instead Try Learning How Copper Saves Gold

125
Q

Electrolysis separates…

A

Most reactive metals from their compounds

126
Q

Alloy

A

Metal combination

127
Q

Metal ore

A

Always involve reduction (they are metal OXIDES)

128
Q

Transition metal properties

A

Stable ions in variable oxidation states, coloured compounds and often used as ion/ atom catalysts

129
Q

State changes overcome

A

Forces of attraction

130
Q

H2 gas test

A

Squeaky pop with a lit splint

131
Q

O2 test

A

Relights a glowing splint

132
Q

CO2 test

A

Turns limewater cloudy

133
Q

Chlorine test

A

Damp blue litmus turns red then bleaches

134
Q

Carbonate ion test

A

Bubbles when in presence of dilute acid

135
Q

X- ion test

A

Aq solution of silver nitrate and dilute nitric acid gives white for Cl, cream for Br and yellow for I

136
Q

Sulphate ion test

A

Barium chloride in presence of dilute HCl - white sulfate of barium sulfate is +ve result

137
Q

Metal cation test in NaOH for Al3+, Ca2+ and Mg2+

A

White ppt

138
Q

Metal cation test in NaOH for Cu2+

A

Blue ppt

139
Q

Metal cation test in NaOH for Fe2+

A

Green ppt

140
Q

Metal cation test in NaOH for Fe3+

A

Brown ppt

141
Q

Flame test for Li

A

Crimson red

142
Q

Flame test for Na

A

Yellow/ orange

143
Q

Flame test for K

A

Lilac

144
Q

Flame test for Ca

A

Red/orange

145
Q

Flame test for Cu

A

Green

146
Q

Test for presence of H2O

A

Anhydrous Copper (II) Sulfate gives a white to blue colour change

147
Q

Dangers of CO2

A

Global warming (traps IR - UV) + acid rain

148
Q

Dangers of CO

A

Toxic to haemoglobin

149
Q

Dangers of SO2

A

Respiratory problems + acid rain

150
Q

Dangers of NOx

A

Ecosystem damage + breathing problems

151
Q

Electrolysis definition

A

Ionic substances are broken down into simpler substances as an electric current is passed through them

152
Q

Covalent cannot act as electrolytes because…

A

They don’t contain ions, but neutral atoms

153
Q

Ions in electrolysis must be …

A

Free to move - so when an ionic substance if dissolved in water of when it is melted

154
Q

Positively charged ions move to the

A

Negative electrode (cathode) during electrolysis. They receive electrons and are reduced

155
Q

Negatively charged ions move to the…

A

Positive electrode (anode) during electrolysis. They lose electrons and are oxidised. The substance that is broken down is called the electrolyte

156
Q

Where is the metal and non-metal found in electrolysis

A

the metal is formed at the negative electrode because that is where the positive metal ions are attracted
the non-metal element is formed at the positive electrode where the negative non-metal ions are attracted

157
Q

What is formed at the negative electrode?

A

The metal if it is less reactive than H2 (Copper, Silver or Gold) - otherwise H2 is produced

158
Q

At the positive electrode

A

If the negative ion is simple - then that element will be produced (eg: Bl- or Cl-) otherwise it is O2

159
Q

Charge transferred during electrolysis can be calculated from the mean current used and time taken:

A

Charge (Q (C)) = Current x Time

160
Q

One faraday is 1 mole of electrons and equal to

A

96500 Coulombs

161
Q

When should you use an inert electrode?

A

An inert electrode is needed to conduct the electrons but it is not part of the redox reaction. You only need an inert electrode (like Pt) if your reactants cant function as an electrode (like I2 and Ce ions). If you have a metal like Zn, Cu or Ag involved you can just use the metal

Copper, zinc, lead, and silver can all be used as participatory electrodes

162
Q

How does electroplating work?

A

The negative electrode should be the object to be electroplated.
The positive electrode should be the metal that you want to coat the object with.
The electrolyte should be a solution of the coating metal, such as its metal nitrate or sulfate.

BMAT Section 2 (4 decks)

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