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9701 > physical chem > Flashcards

physical chem Flashcards

1
Q

isotopes

A

atoms of the same element with different number of neutrons

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2
Q

Relative atomic mass (Ar)

A

the average mass of the atoms of the naturally occuring isotopes of an element relative to 1/12th the mass of a C-12 atom

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3
Q

relative isotopic mass

A
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4
Q

relative molecular mass (Mr)

A
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5
Q

Relative formula mass

A
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6
Q

Mole

A
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7
Q

Avagadros constant

A

6.02*10^23

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8
Q
A
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9
Q
A
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10
Q
A
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11
Q

gdm-3 -> moldm-3

A

divide by mr

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12
Q

n=

A

m/Mr
v/24
M*V

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13
Q

M(gmdm-3)

A

m/V

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14
Q

denisty=

A

m/v

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15
Q

atoms consist of

A

a nucleus surrounded by electron shells

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16
Q

the nucleus is made up of

A

protons, which are +ve charged and neutrons which are neutral and hence have no charge

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17
Q

the electron shells are composed of

A

electrons that revolve around the nucleus, electrons are -vely charged

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18
Q

in an atom the number of protons =

A

number of electrons

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19
Q

the proton number is

A

the atomic number

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20
Q
A
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21
Q

ions

A

atoms that attain a charge after gaining or loosing electrons

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22
Q

cations

A

+ve

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23
Q

anions

A

-ve

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24
Q

an idead gas is a gas that obeys

A

pV=nRT

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25
Q

in an ideal gas,

A

there are no IMF, the volume of particles is negligible compared to the volume of a gas

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26
Q

all collisions of ideal gas particles are

A

elastic

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27
Q

ideal gas particles move

A

rapidly and randomly

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28
Q

how does a gas approach ideal gas behaviour

A

as the temperature of the gas increases, as pressure of a gas decreases

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29
Q

pV=nRT units

A

p is pressure in pascals
V is volume in m^3
n is number of moles
R is 8.31
T is temperature in kelvin

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30
Q

pressure is inversely proportional to volume

A
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31
Q

when pressure increases

A

temperature increases

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32
Q

he is the

A

closest ideal gas

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33
Q

when we heat a solid the particles gain

A

energy hence they vibrate more strongly and the solid expands, when a solid is heated further beyond a certain point, the energy is enough to break the bonds or IMF in the solid and hence the particles move further apart and start sliding over each other forming a liquid, this is called melting

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34
Q

when we cool a liquid

A

the particles loose energy and hence come closer together as they move slowly the forces of attraction between the particles increase, bringing the particles even closer hence forming a solid, this is called freezing

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35
Q

when we heat a liquid

A

the particles start gaining energy and start moving faster, the liquid expands

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36
Q

evaporation

A

the particles with most energy at the surface tend to form a vapour and escape

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37
Q

boiling

A

when a liquid is heated further , there us enough energy to break the bonds or intermolecular forces inside the liquid so the particles move apart, forming a gas or a vapour the temp at which this takes place is called boiling point

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38
Q

enthalpy change of vaporisation

A

the energy needed to change one mole of liquid to one mole of gas

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39
Q

condensation

A

when we cool a gas, the particles loose energy and hence, they move closer to each other and move more slowly, this I because of increases forces of attraction between the particles, condensation also takes place at the boiling point

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40
Q

vapour pressure

A

when we heat a liquid in a closed container, some of it evaporates and moves up to the lid, on the lid as the particles are closer together, they experience increased forces of attraction, which results in the vapour turning back to the liquid on the lid, over time a dynamic equilibrium is established between the liquid and the vapour the pressure of the vapour at this equilibrium is called vapour pressure

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41
Q

vapour pressure increases as

A

temperature increases because the particles gain energy and move faster and hence collide more frequently and with more energy withe the balls of the container

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42
Q

the temp at which vapour pressure = atmospheric pressure is called the

A

boiling point

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43
Q

alloys are _ of metals

A

mixture

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44
Q

alloys are _ and __ than metals that they are composed of

A

harder and more rigid

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45
Q

why are alloys harder and more rigid than the metals that they are composed of

A

metals have atoms of different sizes so it becomes difficult for the metal layers to move

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46
Q

graphite is

A

a giant molecular structure

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47
Q

graphite is an _ of carbon

A

allotrope

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48
Q

allotropes are

A

different form of the same element

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49
Q

giant molecular structure

A

has continuous network of covalent bonds

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50
Q

in graphite each carbon

A

atom is covalently bonded to 3 other carbon atoms forming hexagonal rings, these rings are stacked on top of each other

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51
Q

graphite has _ MP

A

high because it is difficult to break the covalent bonds within the rings

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52
Q

graphite uses

A

it is slipperly and is used as lubricant because the layers can slide over each other as the forces between the layers are weak van der waals forces

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53
Q

graphite conducts

A

electricity because each carbon atom has one free electron and these free electrons form an electron cloud over the rings which allows electricity to be conducted thus graphite is used in electrodes

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54
Q

graphite is _

A

INERT

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55
Q
A

GRAPHITE, red lines are covalent bonds and blue lines are vander waals forces

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56
Q

diamond has a

A

giant molecular structure

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57
Q

diamond is _ of carbon

A

allotrope

58
Q

in diamond each carbon atom

A

is covalently bonded to four other carbon atoms forming a giant 3D network structure thus diamond has a very high MP because a lot of energy is needed to break the covalent bond

59
Q

diamond is amonth the _ known substance on earth

A

hardest

60
Q

diamond does not

A

conduct electricity because it does not have any free electrons

61
Q

diamond is

A

INERT

62
Q
A

DIAMOND

63
Q

SiO2 has

A

a giant molecular structure

64
Q

SiO2

A

Silicon (IV) oxide

65
Q

in SIO2 each silicon atom

A

is covalentlty bonded to 4 oxygen atoms and each oxygen atom is covalently bonded to 2 silicon atoms forming a giant 3D network structure like diamond SiO2 has a high MP and is very hard

66
Q

fullerenes have

A

simple molecular structures

67
Q

fullerenes have

A

simple molecular structures

68
Q

fullerenes are _ of carbon

A

allotropes

69
Q

fullerenes are

A

ball like or tube like structures with hexagonal and pentagonal rings of carbon atoms, each carbon atom is covalently bonded to 3 other carbon atoms

70
Q

C60 has a low MP and BP

A

because there are weak van der waals forces between the ball like molecules for the same reason, they are quite soft they conduct electricity but to a lesser extent than graphite and are quite reactive

71
Q

nanotubes are tubes of hexagonal rings of

A

carbon atoms, electricity is conducted over the long axis of the tubes

72
Q

metals lose electrons to gain

A

stability

73
Q

non metals gain electrons to gain

A

stability

74
Q

in ionic bonding

A

a metal looses its valence electrons to a non metal

75
Q

ionic bond

A

results in the formation of a strong electrostatic force of attraction between the metal cation and nonmetal anion

76
Q

dot and cross diagrams of NaCl

A
77
Q

a lattice

A

alternating arrangement of oppositely charged ions, held together by strong ionic bonds

78
Q

properties of ionic compounds

A
  • they are solid at room temperature
  • high MP
  • high BP
  • high enthalpy change of vaporisation
79
Q

ionic compounds are generally soluble in water

A

this is because when the ionic compound is added to water, water molecules form bonds with the ions on the surface of the lattice, these bonds replace the bonds within the lattice thus ions go into the solution

80
Q

ionic compounds do not conduct electricity in solid state because

A

the ions are immobile in the lattice however when the compound is molten or dissolved in water, the ions are mobile so currents pass through

81
Q

the larger the charge on the ion

A

stronger the bond , thats why MgO is stronger than NaCl

82
Q

when 2 non metals react

A

both need to gain electrons to attain stability they do this by sharing electrons

83
Q

covalent bonds

A

force of attraction between the nucleus and the shared pair of electrons

84
Q

a single bond is formed when

A

one pair of electrons is shared between the covalently bonded atoms

85
Q

a double bond is formed when

A

2 pairs of electrons are shared between the covalently bonded atoms

86
Q

a triple bond is formed when

A

3 pairs of electrons are shared between the covalently bonded atoms

87
Q

dot and cross of Cl2

A
88
Q

dot and cross of O2

A
89
Q

dot and cross of N2

A
90
Q

electronegativity

A

the extent to which an atom covalently bonded to another atom attracts the bonded pair of electrons

91
Q

electronegativity increases

A

across a period

92
Q

electronegativity decreases

A

down the group

93
Q

bond polarity

A

the unequal sharing of electron pairs between covalently bonded atoms, the centres of positive and negative charge do not coincide, the bond is said to be asymmetric

94
Q

in a polar bond

A

one atom has a partial positive charge and one atom has a negative charge

95
Q

dipole

A

when both atoms have a partial charge in polar bond

96
Q

no difference in electronegativity

A

non polar bonds, electrons equally shared

97
Q

AlCL3 is a

A

covalent compound

98
Q

dot and cross of AlCl3

A
99
Q

2 types of IMF

A

van der waals forces
hydrogen bonds

100
Q

2 types of van der waals forces

A

instantaneous dipole induced dipole forces
permanent dipole-dipole forces

101
Q

instantaneous dipole- induced dipole forces

A

these forces exist between non-polar molecules
they are the weakest type of IMF
the larger the molecule the stronger the ID-ID forces due to more surface contact points
the more the number of electrons in the molecule, the stronger the id-id forces

102
Q

permanent dipole-dipole forces

A

these forces exist between polar molecules
these are stronger than id-id forces

103
Q

hydrogen bonds

A

there are the strongest type of IMF
they only exist between molecules that have -OH, -NH groups and if the HF molecule is present

104
Q

C-H

A

non dipole

105
Q

most electronegative elements

A

F,O anf then N

106
Q

covalent bonds result in the formation of

A

a simple molecular structure which are held together by IMF

107
Q

Molecules that are held together by Vander Waals forces are usually

A

gases and have low MP, BP and entalpies of vaporisation

108
Q

Molecules that are held together by hydrogen bonds are usually

A

have high MP, BP and entalpies of vaporisation

109
Q

molecules that are held together by ID-ID forces are

A

insoluble in H2O but highly soluble in non polar solvents

110
Q

molecules that are held together by Permanent induced - dipole dipole forces are

A

weakly soluble in water, weakly soluble in non polar solvents but highly soluble in polar solvents

111
Q

molecules that are held together by hydrogen bonds are

A

highly soluble in water

112
Q

simple molecular compounds do not

A

conduct electricity because they have neither mobile ions nor mobile electrons

113
Q

water has a

A

high surface tension compared to other liquids because of hydrogen bonds

114
Q

ice is less dense than water because

A

of longer hydrogen bonds between molecules of water than in the liquid itself, give ice a more open structure

115
Q

in a molecule, there is repulsion between

A

pairs of electrons

116
Q

the repulsion between the lone pairs is the

A

maximum

117
Q

the repulsion between lone pairs and bond pairs is

A

slighty smaller

118
Q

repulsion between bond pairs is

A

the smallest

119
Q

linear

A
120
Q

trigonal planar

A

like AlCl3

121
Q

bent or angular

A
122
Q

tetrahedral

A

like CH4

123
Q

trigonal pyramidal

A

like NH3

124
Q

H2O

A
125
Q

TRIGONAL BIPYRAMIDAL

A

LIKE PCl5

126
Q

octahedral

A

like SF6

127
Q
A

sp^3 hybridised orbitals in tetrahedral, 109.5 degree

128
Q
A

sp^2 hybridised orbitals in trigonal planar 120 degree

129
Q
A

sp hybridised orbitals in 180 degree

130
Q

bond energy

A

the energy needed to break one mole of a bond in gaseous state

131
Q

as bond length increases

A

bond energy decreases

132
Q

coordinate bond

A

one species provides both the electrons for the formation of a covalent bond, this type of covalent bond

133
Q

coordinate bonds are AKA

A

dative covalent bonds

134
Q

the strength of a coordinate bond is the same as that of a

A

covalent bond

135
Q

NH4+ DATIVE COVALENT

A
136
Q

AlCl3 and Al2Cl6 are

A

dimers

137
Q

Al2Cl6 dot and cross

A
138
Q

AlCl3 exists at

A

high temp

139
Q

Al2Cl6 exists at

A

low temp

140
Q
A

9701 (5 decks)

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