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Chemistry Paper 1 > Module 2 > Flashcards

Module 2 Flashcards

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1
Q

What is the relative mass of a proton? (1 mark)

A

1

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2
Q

What is the relative mass of a neutron? (1 mark)

A

1

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3
Q

What is the relative mass of an electron? (1 mark)

A

1/2000

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4
Q

What charge does a proton have? (1 mark)

A

1+

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5
Q

What charge does an electron have? (1 mark)

A

1-

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6
Q

What charge does a neutron have? (1 mark)

A

0

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7
Q

Why is an atom neutral? (2 marks)

A

There are the same number of protons and electrons,
so the charges cancel out.

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8
Q

What identifies an element, makes all the atoms of that element the same element? (1 mark)

A

The atomic number, aka the number of protons

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9
Q

State two differences in chemical properties between water and heavy water. (2 marks)

A

Heavy water has:
Higher melting and boiling points
Higher density

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10
Q

What is heavy water? (1 mark)

A

A form of water with an isotope of H in it (known as deuterium, 2,1H).

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11
Q

What is an isotope? (2 marks)

A

Atoms of an element with different numbers of neutrons, but the same number of protons.

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12
Q

What is an ion? (2 marks)

A

An ion is a charged atom.
It has a different number of protons from electrons.

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13
Q

Define relative isotopic mass. (2 marks)

A

Relative isotopic mass is the mass of an isotope relative to 1/12th of the mass of a carbon-12 atom.

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14
Q

Define relative atomic mass. (3 marks)

A

Relative atomic mass is the weighted mean mass of an atom relative to 1/12th of the mass of a carbon-12 atom.

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15
Q

How is the relative atomic/isotopic mass determined? (1 mark)

A

Using a mass spectrometer.

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16
Q

What ions to metals form? (1 mark)

A

Positive ions/cations

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17
Q

What ions do non-metals form? (1 mark)

A

Negative ions/anions

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18
Q

What is a binary compound? (1 mark)

A

A compound that only contains two elements.

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19
Q

What is a polyatomic ion? (1 mark)

A

An ion that contains atoms of more than one element bonded together.

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20
Q

What is the overall charge of an ionic compound? (1 mark)

A

0

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21
Q

Explain Avagadro’s constant. (1 mark)

A

The number of particles contained in one mole of any substance.

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22
Q

How do you calculate the number of moles something? (1 mark)

A

moles= mass/Mr or molar mass

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23
Q

What is molar mass? (1 mark)

A

The mass (in grams) in each mole of a substance.

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24
Q

What is a molecular formula? (1 mark)

A

The number of atoms of each element in a molecule.

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25
Q

What is an empirical formula? (1 mark)

A

The simplest whole number ratio of atoms of each element in a compound.

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26
Q

Define relative molecular mass (Mr). (2 marks)

A

Relative molecular mass is the mass of a molecule relative to 1/12th of the mass of a carbon-12 atom.

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27
Q

Define relative formula mass. (2 marks)

A

Relative formula mass is the mass of a formula unit relative to 1/12th of the mass of a carbon-12 atom.

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28
Q

What does it mean if a salt is hydrated? (1 mark)

A

Water molecules are part of their crystalline structure.

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29
Q

What are two assumptions that decrease the accuracy of experimental formula of hydrated salts? (2 marks)

A

All the water has been lost
No further decomposition of the salt

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30
Q

What are the two equations for concentration?

A

conc= mol/vol
conc=mass/vol

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31
Q

What is a standard solution? (1 mark)

A

A solution of known concentration.

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32
Q

What is molar gas volume? (2 marks)

A

The volume that a mole of gas molecules occupies, at a stated temperature and pressure.

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33
Q

State the ideal gas equation. (2 marks)

A

pV=nRT

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34
Q

What are the units for the ideal gas equation? (3 marks)

A

p- Pascals (Pa)
V- Metres cubed (m3)
n- Moles (mol)
R- 8.31 Jmol-1K-1 (the ideal gas constant)
T- Kelvin (K)

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35
Q

What are the values of room temperature and pressure (RTP)? (2 marks)

A

293K/298K or 20/25 degrees celcius
101kPa or 1atm

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36
Q

Explain what the term stoichiometry means. (1 mark)

A

The ratio of the amount, in mol, of each substance in an equation.

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37
Q

What is the equation for percentage yield? (1 mark)

A

= (actual yield/theoretical yield) x 100

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38
Q

What is the limiting reagent? (1 mark)

A

Th reactant that is not in excess.

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39
Q

What is the equation for atom economy? (1 mark)

A

= (Mr of desired products/Mr if all products) x 100

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40
Q

How is relative formula mass calculated? (1 mark)

A

By adding together the relative atomic masses of the elements in the empirical formula.

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41
Q

How do you convert between mol/vol and mass/vol? (1 mark)

A

mol/vol= (mass/vol)/Mr

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42
Q

Identify a compound of calcium that could be used to convert a soil pH from 5.8 to 7.5. (1 mark)

A

Ca(OH)2
or CaO

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43
Q

A salt has empirical formula H4N2O3, suggest the formulae of the ions present in this salt. (2 marks)

A

NH4+
NO3-

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44
Q

What element do all acids contain? (1 mark)

A

Hydrogen

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45
Q

What does an acid release when dissolved in water? (1 mark)

A

H+ ions

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46
Q

What is a strong acid? (2 marks)

A

A strong acid releases all its hydrogen atoms into solution as H+ ions
and completely dissociates in aqueous solution.

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47
Q

What is a weak acid? (2 marks)

A

A weak acid only releases a very small proportion of its available hydrogen atoms into solution as H+ ions.
A weak acid only partially dissociates.

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48
Q

Define the term ‘base’. (1 mark)

A

A base is a substance which readily accepts H+ ions.

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49
Q

What is an alkali? (2 marks)

A

An alkali is a base that dissolves in water
releasing OH- ions into the solution.

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50
Q

What does an alkali release when dissolved in water? (1 mark)

A

OH- ions

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51
Q

Describe what happens when an acid is neutralised. (2 marks)

A

The H+ ions from acid react with OH- ions from base to form a salt and neutral water.

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52
Q

What is formed when an acid reacts with a metal hydroxide? (2 marks)

A

Water and a salt

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53
Q

What is formed when an acid reacts with a metal oxide? (2 marks)

A

Water and a salt

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54
Q

What are formed when an acid and alkali react? (2 marks)

A

Water and a salt

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55
Q

What are formed when an acid and metal carbonate react? (2 marks)

A

Water, carbon dioxide, and a salt

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56
Q

Explain the statement ‘Sulphuric acid is a strong acid, but this is true only for one of the two hydrogen atoms. (3 marks)

A

When sulphuric acid is mixed with water each H2SO4 molecule dissociates, releasing just one of its two hydrogen atoms as an H+ ion.
This means HSO4 - ions are formed, which behave as a weak acid.

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57
Q

Finish the sentence:
A burette reading is recorded to the nearest…. (1 mark)

A

Half division

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58
Q

What is a concordant result, in titration, and what are they used for? (2 marks)

A

Titres within 0.10cm3 of each other.
They are used to calculate the mean titre.

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59
Q

What is the oxidation number of an element? (1 mark)

A

0

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60
Q

Where is the sign placed for an oxidation number? (1 mark)

A

BEFORE the number

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61
Q

What is the oxidation number of hydrogen in metal hydroxides? (1 mark)

A

-1
e.g. NaH or CaH2

62
Q

What is the oxidation number of oxygen in peroxides? (1 mark)

A

-1
e.g H2O2

63
Q

What is the oxidation number of oxygen when bonded to fluorine? (1 mark)

A

+2
e.g. F2O

64
Q

What is a redox reaction? (1 mark)

A

Redox reactions involve reduction and oxidation.

65
Q

What is oxidation in terms of electrons? (1 mark)

A

The loss of electrons.

66
Q

What is reduction, in terms of electrons? (1 mark)

A

The gain of electrons.

67
Q

What is oxidation, in terms of oxygen? (1 mark)

A

Gain of oxygen.

68
Q

What is reduction, in terms of oxygen? (1 mark)

A

Loss of oxygen.

69
Q

What is oxidation, in terms of oxidation number? (1 mark)

A

Increase in oxidation number.

70
Q

What is reduction, in terms of oxidation number? (1 mark)

A

Decrease in oxidation number.

71
Q

What is the significance of oxidation number in equations? (1 mark)

A

The changes in oxidation number balance out in an equation.

72
Q

What is the shell number called? (1 mark)

A

The principle quantum number (n)

73
Q

When n is the number of the shell, what is the formula for the number of electrons in a shell? (1 mark)

A

2n^2

74
Q

What are shells made up of? (1 mark)

A

Atomic orbitals

75
Q

How many electrons does an atomic orbital hold, and what direction do they spin? (2 marks)

A

2
opposite directions

76
Q

What are the types of atomic orbital? (4 marks)

A

s-orbitals
p-orbitals
d-orbitals
f-orbitals

77
Q

How many s-orbitals are in a shell from n=1? (1 mark)

A

1

78
Q

How many p-orbitals are in a shell from n=2? (1 mark)

A

3

79
Q

How many d-orbitals are in a shell from n=3? (1 mark)

A

5

80
Q

How many f-orbitals are in a shell from n=4? (1 mark)

A

7

81
Q

How many electrons are in an s-orbital? (1 mark)

A

2

82
Q

How many electrons are in a p-orbital? (1 mark)

A

6

83
Q

How many electrons are in a d-orbital? (1 mark)

A

10

84
Q

How many electrons are in a f-orbital? (1 mark)

A

14

85
Q

How many electrons are in shell 1? (1 mark)

A

2

86
Q

How many electrons are in shell 2? (1 mark)

A

2 + 6= 8

87
Q

How many electrons are in shell 3? (1 mark)

A

2 + 6 + 10= 18

88
Q

How many electrons are in shell 4? (1 mark)

A

2 + 6 + 10 + 14= 32

89
Q

What order are orbitals filled in? (1 mark)

A

In order of increasing energy.

90
Q

What is an electron orbital? (2 marks)

A

A region around the nucleus that can hold up to 2 electrons with opposite spins.

91
Q

What are the two exceptions to the 3d, 4s rule? (2 marks)

A

Chromium
Copper

92
Q

What is ionic bonding? (1 mark)

A

The electrostatic attraction between positive and negative ions.

93
Q

What is the structure of ionic compounds? (1 mark)

A

Giant ionic lattice

94
Q

Why do ionic compounds dissolve in water? (2 marks)

A

Water is polar, the polar water molecules break down the lattice and surround each ion in solution.

95
Q

What is covalent bonding? (2 marks)

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

96
Q

What is dative covalent bond? (1 mark)

A

A covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only.

97
Q

What is the correlation between bond enthalpy and bond strength? (1 mark)

A

The larger the value of the average bond enthalpy, the stronger the covalent bond.

98
Q

What does isoelectronic mean? (1 mark)

A

Two molecules have the same number of electrons.

99
Q

What shape is an s-orbital? (1 mark)

A

Spherical

100
Q

What shape is a p-orbital? (1 mark)

A

Dumb-bell

101
Q

Does a lone pair or bonded pair repel more strongly? (1 mark)

A

Lone pair

102
Q

Why does a lone pair repel more strongly than a bonded pair? 2 marks)

A

A lone pair is slightly closer to the central atom, and occupies more space.

103
Q

What is the bond angle decreased by for each lone pair? (1 mark)

A

2.5 degrees

104
Q

What is the bond angle and shape of methane? (2 marks)

A

Tetrahedral
109.5

105
Q

What is the bond angle of a tetrahedral molecule? (1 mark)

A

109.5

106
Q

What is the shape of a molecule with bond angle 109.5?

A

Tetrahedral

107
Q

What is the shape and bond angle of a molecule with 4 bonded pairs and no lone pairs? (2 marks)

A

Tetrahedral 109.5

108
Q

What is the shape and bond angle of ammonia? (2 marks)

A

Pyramidal
107

109
Q

What is the bond angle of a molecule with a pyramidal shape? (1 mark)

A

107

110
Q

What is the shape of a molecule with bond angle 107? (1 mark)

A

Pyramidal

111
Q

What is the shape and bond angle of a molecule with 2 bonded pairs and 2 lone pairs? (2 marks)

A

Non- linear
104.5

112
Q

What is the shape of a molecule with bond angle 104.5? (1 mark)

A

Non-linear

113
Q

What is the shape and bond angle of a molecule with three bonded paired and one lone pair? (2 marks)

A

Pyramidal
107

114
Q

What is the bond angle of a molecule with a non-linear shape? (1 mark)

A

104.5

115
Q

What is the shape and bond angle of water? (2 marks)

A

Non-linear
104.5

116
Q

What is the shape of a molecule with 2 electron regions? (2 marks)

A

Linear

117
Q

What is the bond angle of a linear molecule? (1 mark)

A

180

118
Q

What is the bond angle and shape of carbon dioxide? (2 marks)

A

Linear
180

119
Q

What is the shape of a molecule with bond angle 180? (1 mark)

A

Linear

120
Q

What is the shape and bond angle of a molecule with 3 electron pairs/regions?

A

Trigonal planar
120

121
Q

What is the shape of a molecule with bond angle 120? (1 mark)

A

Trigonal planar

122
Q

What is the shape and bond angle of BF3? (2 marks)

A

Trigonal planar
120

123
Q

What is the bond angle of a molecule with a trigonal planar shape? (1 mark)

A

120

124
Q

What is the bond angle and shape of sulphur hexafluoride? (2 marks)

A

Octahedral
90

125
Q

What is the bond angle of a molecule with an octahedral shape? (1 mark)

A

90

126
Q

What is the bond angle and shape of a molecule with 6 electron pairs/regions? (2 marks)

A

90
Octahedral

127
Q

What is the shape of a molecule with bond angle 90? (1 mark)

A

Octahedral

128
Q

What is electronegativity? (1 mark)

A

The attraction of a bonded atom for the pair of electrons in a covalent bond.

129
Q

How is electronegativity measured? (1 mark)

A

The Pauling scale

130
Q

Describe electronegative on the periodic table. (2 marks)

A

The top right of the periodic table contains the most electronegative elements. With Florine being in the corner (ignore group 0).

131
Q

Is an ionic or covalent bond more electronegative? (1 mark)

A

Ionic

132
Q

What does a bond being non-polar mean? (1 mark)

A

The bonded electron pair is shared equally between the bonded atoms.

133
Q

What does it mean when a bond is described as polar? (1 mark)

A

The bonded electron pair is shared unequally between the bonded atoms.

134
Q

Why is carbon dioxide non-polar even though it contains two C=O bonds with permanent dipoles? (1 mark)

A

The two dipoles act I’m opposite directions and exactly oppose each other (due to a linear shape).

135
Q

What are the three main catagories of intermolecular forces? (3 marks)

A

Induced dipole-dipole interactions
Permanent dipole-dipole interactions
Hydrogen bonding

136
Q

Which intermolecular force is the strongest? (1 mark)

A

Hydrogen bond

137
Q

Which intermolecular bond is the weakest? (1 mark)

A

Induced dipole-dipole interactions

138
Q

Where are induced dipole-dipole interactions? (2 marks)

A

Exist between all molecules.
They act between induced dipoles in different molecules.

139
Q

Describe the origin of induced dipole-dipole interactions. (3 marks)

A

Movement of electrons produces a changing dipole in a molecule.
At any instant, an instantaneous dipole will exist (position is alway shifting).
This instantaneous dipole induces a dipole on a neighbouring molecule.
Etc.

140
Q

Describe the strength of the induced dipole-dipole interactions in a molecule with more electrons. (3 marks)

A

Larger instantaneous and induced dipoles
Greater the induced dipole-dipole interactions
The stronger the attractive forces between molecules.

141
Q

Where are permanent dipole-dipole interactions? (2 marks)

A

They act between the permanent dipoles in different polar molecules.

142
Q

Describe the bonding and intermolecular forces in a simple molecular lattice. (2 marks)

A

Strong covalent bonds
Weak intermolecular forces.

143
Q

What happened when a simple non-polar molecular substance is added to a non-polar solvent? (3 marks)

A

Intermolecular forces form between the molecules and the solvent.
The interactions weaken the intermolecular forces in the simple molecular lattice.
The intermolecular forces break.
The compound dissolves.

144
Q

Why are non-polar simple molecular substances insoluble in polar solvents? (2 marks)

A

The intermolecular bonding within the polar solvent is too strong to be broken, so there is little interaction between the molecules keep s in the lattice and the solevent molecules.

145
Q

What is the solubility of a polar simple molecular substance dependent on? (1 mark)

A

The strength of the dipole.

146
Q

Describe the electrical conductivity of simple molecular structures. (2 marks)

A

There are no mobile charge carriers, so they do not conduct electricity.

147
Q

What three elements can form a hydrogen bond with H? (3 marks)

A

Oxygen
Nitrogen
Fluorine

148
Q

Why is ice less dense than water? (2 marks)

A

Hydrogen bonds hold water molecules apart in an open lattice structure in ice.

149
Q

Why does water have a relatively high melting and boiling point? (2 marks)

A

Hydrogen bonds are really strong, require more energy to be broken.

150
Q

What is the bond angle of a molecule with a square planar shape? (1 mark)

A

90 degrees

151
Q

How many lone/bonded pairs of electrons does a molecule with a square planar shape have? (2 marks)

A

4 bonded
2 lone

152
Q

Which elements form a square planar shape? (3 marks)

A

Au
Pt
Pd

Chemistry Paper 1 (3 decks)

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