PAST PAPER CONTENT Flashcards
1
Q
Fc6Would Ions with a greater charge be deflected more in a Mass Spectrometer
A
Yes !
Ions with a greater charge would be more deflected in a Mass Spectrometer
Because there is a greater force
2
Q
Dative Covalent Bonding Definition?
A
A Two center, Two Electron covalent bond in which these two electrons derive from the same atom
3
Q
How to Draw Carbon Monoxide ?
A
Diagram
4
Q
Polar vs Non-Polar
A
Hydrocarbons are non-polar
Symmetry = Polar
Polar>0.5 EN
5
Q
Examples of Polar Molecules?
A
H- N,O,F
H20, NH3, HF
6
Q
What line is it on the EM if an electron emits energy to N=1, N=2, N=3 ?
A
UV-Radiation n=1
Visible Light Transition n=2
Infrared Radiation Transition n=3
7
Q
Is Combustion exothermic or endothermic
A
exothermic
8
Q
Is Decomposition endo or exo?
A
endo
9
Q
Is neutralisation exo or endo?
A
exo
10
Q
What three processes go on in Mass Spectrometry?
A
Ionization, Acceleration and Deflection
11
Q
Outline the three processes in Mass Spectrometry.
A
ionization: sample bombarded with high-energy or high-speed
electrons/OWTTE;
acceleration: electric field/oppositely charged plates;
deflection:
(electro)magnet/magnetic field;
12
Q
Electrolytic Cell Diagram?
A
See Answer
13
Q
Define the term activation energy
A
the minimum quantity of energy which the reacting species must possess in order to undergo a specified reaction.
14
Q
Distinguish between a strong and a weak acid
A
Weak Acid- Partially Ionizes in Solution
15
Q
Enthalpy Change
A
The Enthalpy change is independent of the route taken
16
Q
The definition of the standard enthalpy of formation, ΔHf, is:
A
The enthalpy change when 1 mole of a compound is formed from its elements; [1]
In their standard states; [1]
17
Q
The equation for the formation of the following compounds are?
Methanol
Carbon Dioxide
Ethane
A
C (s) + ½O2 (g) + 2H2 (g) → CH3OH (l)
C (s) + O2 (g) → CO2 (g)
2C (s) + 3H2 (g) → C2H6 (g)
18
Q
Which properties increase as you go down group 1?
A
Atomic Radius
Electronegativity
First Ionization Energy
19
Q
Which properties decrease as you go down group 1?
A
Melting Point
20
Q
What does the strength of Metallic Bonding depend on?
A
Ionic radius and charge
Smaller Ionic Radius –> Stronger Bonding
Greater Charge –> Stronger Bonding
21
Q
Are enthalpy changes accurate and how do they compare to enthalpy change of formation?
A
Bond Enthalpies are not specific to compounds - averages are taken from the data booklet
Enthalpy Changes of Formation are specific
22
Q
Equation for Equilibrium Constant?
A
[C}X{D}/[A}X[B]
23
Q
Does a weak acid have poor conductivity?
A
Yes
24
Q
Are neutralisation reactions redox?
A
Neutralisation reactions are not redox
25
Describe the reaction between halogen and ethane?
Free radical substitution and homolytic
26
In the equation Pv = nRT, what is the relationship between n and T?
Inverse Relationship
27
S,P,D,F on the periodic table?
SEE
28
What is true about Strong Acids
They are good proton donors and they have weak conjugate bases
29
What Compund is the exception to the rule that O2 has a -2 Oxidation number?
H2O2 - Hydrogen Peroxide where it has an oxidation number of -1
30
Suggest two reasons why atoms are no longer regarded as the indivisible units of matter.
subatomic particles «discovered»
OR
particles smaller/with masses less than atoms «discovered»
OR
«existence of» isotopes «same number of protons, different number of neutrons»✔
charged particles obtained from «neutral» atoms
31
Lewis Structure for Ammonia
See?
32
Suggest why the Bond enthalpy might not be right?
«N-H» bond enthalpy is an average «and may not be the precise value in NH3»
33
Suggest an experiment to show that one metal is more reactive than the other
MG and ZN
Alternative 3
construct a cell with Mg and Zn electrodes ✔
bulb lights up
OR
shows (+) voltage
OR
size/mass of Mg(s) decreases <>
OR
size/mass of Zn increases <>
34
Brønsted–Lowry acid.
fully ionizes/dissociates ✔
proton/H+ «donor »✔
35
Explain the trend of ionisation energy across a period
Left to right
Ionisation energy increases
36
Ionisation Energy
Minimum energy required to remove the most loosely bound electron of an isolated gaseous atom, positive ion, or molecule
37
do Metallic Bonds have low ionisation energies?
Yes - low Ionisation energies
They lose electrons so removing them is a tough one for them!
38
State the trend between ionisation energy and group number?
Going down a group the ionisation energy decreases
39
Do Metallic Bonds have a large atomic radii?
Yes - Metallic Bonds have laerg atomic radii
40
Do Metallic Bonds have high EM values?
No - on the lower end
41
Can you arrange the electron configuration in a periodic table?
SEE
42
State the trend between Atomic Radius and a group and explain the reason why?
As you go down the group the Atomic Radius increases
This is because there are more Shells
Although there may be greater nuclear charge --> effect counteracted due to a greater number of protons
43
State the trend between Atomic Radius and the period number? and explain why?
Atomic radius decreases across a period
BECAUSE
Nuclear charge increases with no significant change in shielding
Shielding remains approximately constant --. Atoms in the same period have the same number of inner shells
44
Compare the size of ionic and atomic radii?
Ionic radii of positive ions are smaller than their atomic radii
Ionic radii of negative ions are greater than their atomic radii
45
Why is Na larger than Na+?
Na has one extra shell
They both have the same nuclear charge
Greater amount of electron repulsion --> Greater amount of e-
Larger e- cloud in Na because there are more electrons repelling for the same nuclear charge
46
How does charge change with ionic radius?
Positive ions --> Decrease in radius as the charge increases
Negative --> Increase in radius as the charge increases
47
How Volatile are Ionic Compounds?
Low volatility
Strong electrostatic forces of attraction
48
How soluble are Ionic Compounds in Water?
Often soluble in water.
Water is a polar solvent and energy is released when the ions are hydrated by being surrounded by water molecules.
Energy pays back energy required to break apart the ionic lattice
49
How soluble are Ionic Compounds in non-Polar solvents?
Great deal of energy required to break apart the ionic lattice
Energy is not paid back by the energy released when the non-polar solvent forms interactions with ions
50
Metal Oxide + Water
Metal Hydroxide
51
Metal + Base
Salt + Hydrogen
52
Acid + Metal + Carbonate
Salt + Water + Hydrogen
53
Are Metal Oxides basic or acidic?
Are Non Metal Oxides basic or acidic?
Basic
Acidic - non Metal
54
Outline the electron configuration of a Hydrogen Emission spectrum?
E- occupy discrete energy levels
Energy Levels converge
55
BOND ANGLE DIAGRAM
SEE
56
4 E- Pair and 1 lone pair
Trigonal Pyramidal
57
rate of reaction def
the increase in the concentration of product per unit time.
58
metalloid?
Elements with a mixture of metallic and non-metallic physical properties
59
Closed system
A system in which neither matter nor energy can be lost or gained. An equilibrium can never occur in a system that is not closed
60
Homogeneous reaction
A reaction in which all the species involved are in the same phase.
61
Le Chatelier’s principle
If an equilibrium is subjected to a stress, the equilibrium will shift to minimize the effect of the stress.
62
Amphoteric and Amphriprotic
Amphiprotic species specifically refer to species that can donate or accept a proton (H+ ion). So, a molecule or ion that is amphiprotic must have at least one hydrogen atom that can be ionized, allowing it to act as an acid or a base.
On the other hand, amphoteric species refers to substances that can react with both acids and bases, not necessarily by donating or accepting a proton. This means that an amphoteric species can act as an acid in the presence of a base, and as a base in the presence of an acid.
63
Orbital:
A region of space around the nucleus of an atom that is occupied by a maximum of two electrons at any given time.
63
Orbital:
A region of space around the nucleus of an atom that is occupied by a maximum of two electrons at any given time.
64
Electronegativity
Relative measure of the ability an atom has to attract a shared pair of electrons.
65
Allotropes
Occur when an element can exist in different crystalline forms, such as in carbon, which can exist as graphite, fullerene and diamond.
66
Allotropes
Occur when an element can exist in different crystalline forms, such as in carbon, which can exist as graphite, fullerene and diamond.
67
Electron affinity
Enthalpy change when an electron is added to an isolated atom in the gaseous state.
67
Electron affinity
Enthalpy change when an electron is added to an isolated atom in the gaseous state.
68
Buffer
A solution that resists changes in pH when small amounts of acid or alkali are added to it.
69
Enthalpy of Combustion
The energy released when one mole of a compound is burned in excess oxygen.
70
Standard enthalpy of formation
The energy change when one mole of a compound is formed under standard conditions from its constituent elements in their standard states.
71
Standard enthalpy of solution
: The energy change when one mole of a substance is dissolved in an infinite amount of water under standard conditions.
72
Aufbau principle
The principle that states that lowest energy levels are filled first.
73
Aufbau principle
The principle that states that lowest energy levels are filled first.
74
Ionic Radius trends down the group?
- As the number of shells filled
- Valence electrongs less strongly attracted
- Due to Greater Shielding
- Distance from the nucleus
- Increase in Atomic Radius
75
Atomic Radius Trends across a period?
- As the number of proton increases
- increasing nuclear charge attracts the valence electrons more strongly
- Decrease in Atomic radius
76
Ionization Energy definition?
- Minimum energy required
- to eject an electron
- out of a neutral atom
- in its ground states
77
Factors that affect ionization energy?
- Force of attraction between the valence electron and the nucleus
- The stronger the force, the more energy is required to pull it away
78
Ionization Energy trend across Period?
- As the number of protons increases
- The increasing nuclear charge attracts the valence electrons more strongly
79
Ionization Energy trends going down the group?
- As the number of filled shells increases
- The valence elctrons are less strongly attracted
- Due to greater shielding and distance from the nucleus
80
Electronegativity trends across period?
- As the number of protons increases
- Increasing Nuclear charge attracts the electrons more strongly
81
How does Electronegativity vary going down the group?
Greater Atomic Radius and shielding weakens the attractive force on the electron
82
Amphoteric?
A chemical species that behaves as both an acid and a base
83
Reactions of the Oxides period 3 with Water?
Na2O + H2O --> 2NaOH(aq)
MgO + H2O --> Mg(OH)2 (s)
Al2O3 + H2O --> no reaction
SiO2 + H2O --> no reaction
P4O6 + 6H2O --> 4H3PO3
SO2 + H2O --> H2SO3
Cl2O + H2O --> 2HClO
84
Allotropes?
Allotropes are different molecular or crystalline structures of an element
85
Graphite characteristics?
**Conductivity - High **
Only 3 electrons used in bonding - the fourth electron is found in a delocalised sea of electrons
**Geometry - 2-dimensional**
**Hardness - Very Soft**
2 dimension sheets slide over each other because of van der Waals' forces between the sheets
86
Fullerence characteristics?
**Conductivity - Intermediate**
Surface of the "ball" is conductive
**Geometry**
2 dimensonal folded into a sphere
**Soft**
87
How do you determine if something is an London Forces?
Non-polar molecules
Any molecular element like Cl2, Br2, O2, P4, S8
Hydrocarbons
88
How do you do you know something is a Dipole-Dipole IMF?
- A covalent molecule that has different non-metals, not symmetrically oriented
89
Physical properties of Solids
Giant Ionic
- High Boiling Point
- Low Volatility
- High Delta H vap
90
Giant Metallic Physical Properties?
High Boiling Point
Low Volatility
High Delta H vap
91
Giant Covalent Physical Properties?
High Boiling Point
Low Volatility
High Delta H vap
92
Molecular Covalent Physical Properties of Solids?
low boiling point
high volatility
low delta H vap
93
Assumptions in Calorimetry?
- Specific Heat Capacity of the solution is the same as pure water
- Zinc in the reaction mixture did not absorb some of the energy
- Density of the solution was 1.0g/cm3
- The Calorimeter itself did not absorb any heat
- Heat Loss
94
Equilibrium definition?
Equilibrium is achieved when the forward rate of reaction and the reverse rate of reaction are equal
95
How does the Removal of a Species changes its equilibrium constant?
Shifts towards that species to maintain its concentration
Usualy accomplished by adding something else that reacts with only that species
96
Continuos Spectrum?
contains all wavelengths of electromagentic radiation
97
Line spectrum?
contains only certain energies of electromagnetic radiation
98
Line spectrum?
contains only certain energies of electromagnetic radiation
99
Shapes of orbitals?
S - spherical
p - dumbell
d - 4-leaf clover
f - pointing to corners of a cube
100
Electronic structure of the Periodic Table?
**Group 1 **
1s1 --> 5s1
**Group 2 **
2s2 --> 5s2
**Transition metals **
1st row: 3d1 --> 3d10
2nd row: 4d1 --> 4d10
Group 3:
2p1 --> 5p1
**Group 4:**
2p2 --> 5p2
Group 5:
2p3 --> 5p3
Group 6:
2p4 --> 5p4
Group 7:
2p5 --> 5p5
Group 8:
1s2 --> 5p6
101
Where does oxidation and reduction take place in Voltaic cell electrolysis?
Anode - where oxidation occurs (negative)
Cathode - where Reduction occurs (positive)
102
Voltaic Cell Drawing Check List?
- electrodes labelled with metal type
- external circuit
- salt bridge
- half reactions
- anode/cathode labelled
- electrode polarity labelled
- electron flow in external circuit shown
103
Purpose of salt bridge?
- Salt bridge completes the circuit
- allows for the conduction of ions
- allows for the balancing of ionic charge
104
Common mistakes made with the salt bridge?
- Electrons flow through the wire in the external circuit
- Ions flow through the salt bridge
105
Dynamic Equilibrium?
The rate of the forward reaction is equal to the rate of the backwards reaction
106
What characteristics do equilibrium reactions have?
- Forward and Reverse reactions occur at the same rate (see graph)
- The concentration of reactants and products are equal
- Equilibrium requires a closed system
- There is no change in macroscropic properties
107
What does the value of Kc determine?
To which side the reaction has gone/
108
Values of Kc and what they mean?
Forward reaction hardly proceeds - Kc < 10^-10
Reactants dominant at equilibrium - 0.01
Equal - 1
Products predominant at the reaction - 100
Reaction - almost goes to completion - Kc > 10^10
109
If a reaction is reversed, what will the reciprocal of the reaction be equal to?
If the forward reaction value of Kc = 500, the reverse reaction would be equal to 1/500
110
If the reaction is doubled then what happens to the Kc?
The Kc is also doubled
111
Le Chatleiers Principle
- When a system at equilibrium is subject to change, the system will react to minimise the effect of that change
112
Which factors affect Kc?
ONLY temp
113
Why do catalysts not effect the rate of reaction?
A catalyst increases the rate of the forward and backward reactions equally
tHEY INCREASE THE RATE OF REACTION WITHOUT BEING CHEMICALLY CHANGED as they offer a lower activation energy
114
Functional Groups
SEE
115
Factors affecting Volatility
- Low volatility = High Boiling Point
- The more polar the molecule
116
Equilibrium Constant equation?
[D]^x/[A]^x [B]^x
117
What side will the equilibrium shift if the temp is increased?
When temp increases --> Moves to endothermic side --> Moves Forward/Backwards (depending on the reaction)
118
First Ionisation Eneegry
the energy required to remove one mole of the most loosely held electrons from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+
119
What is the difference between Electron Domain and Molecular Geometry?
Electron domain geometry describes the arrangement of electron domains (either bonding pairs or lone pairs) around a central atom in a molecule, regardless of the positions of the atoms. In other words, electron domain geometry is based solely on the number and arrangement of electron pairs around the central atom, and it determines the overall shape of the molecule. The electron domain geometry is usually determined by counting the number of electron pairs around the central atom and using that to identify the molecular shape.
On the other hand, molecular geometry describes the actual arrangement of atoms in a molecule, taking into account the positions of the atoms and not just the electron pairs. Molecular geometry is also known as the "shape" of the molecule, and it is often used to explain the properties of the molecule, such as polarity, reactivity, and intermolecular forces. Molecular geometry is determined by the electron domain geometry and the positions of the atoms around the central atom.
120
Collision Theory
- Particles myst collide in their correct orientation
- Particles require sufficient activation energy
- Sufficient Energ y> Actyivation Energy
121
Reactions of Electroolysis of Copper Bromide at the Anode and the Cathode?
2Br - + 2e- --> Br2
Cu --> Cu 2+ + 2e-
122
Orbital Diagram of Scandium?
SeeS
123
SPDF ON THE PERIODIC TABLE
SEE
124
Electronic configuration of Co
and Co2+
1S2 2S2 2P6 3S2 3P6 3D7 4S2: ATOM
1S2 2S2 2P6 3S2 3P6 3D7 4S2: ION
125
FUNCTIONAL GROUP OF ALKYNE
- C (TRIPLE BOND) C -
(Alkynes)
CnH2n - 2
126
General formula of Halogenalkanes?
- Cn H2n+1X
127
Formula group of Aldehydes?
R-CHO
(-al)
Cn H2n + 1 CHO
128
Ketones Functional group?
R-CO-R
carbonyl (-one)
Cn H2n + 1 COC x H2x+1
129
Ether Functional group?
R-O-R
(alkoxy)
Cn H2n+1O CmH2m+1
130
Ester
R–COO–R'
ester
CnH2n+1CO2CmH2m+1
131
Amines Functional group?
R–NH2
amine or amino
CnH2n+1NH2
132
Amides
R–CONH2
carboxamide or amido
CnH2n+1CONH2
133
Nitriles
R–CN
nitrile
CnH2n+1CN
–C≡N
134
What does Volatility mean?
The measure of how easily a substance evaporates is referred to as its volatility
135
What is the relationship between melting point and volatility?
The higher the volatility the lower the boiling point
136
Factors affecting Volatility?
- Boiling Point
- Is it branched chained?
- Shape of the molecule
137
How does the nature of the functional group affect the volatility?
- Polar functional groups --> Strong dipole-dipole interactions between the molecules and higher boliling points
138
Functional groups in order of boiling point?
Alkanes, Halogenalkane, Aldehyde, Ketone, Amine, Alcohol, Carboxylic Acid
139
Factors affecting the solubility of organic compounds?
Depends on their ability to form hydrogen bonds with water molecules
Compunds that are able to form hydrogen bonds in the water wiull be soluble
The first three alcohols - methanol, ethanol and propanol - are considered to be completely soluble in water.
As the length of the hydrocarbon chain increases, however, the solubility decreases. Alcohols with 10 or more carbon atoms, such as decanol (CH3(CH2)9OH), are considered to be insoluble in water.
This is due to the increasing size of the hydrocarbon chain, which increases the hydrophobic character of the molecule, decreasing its solubility in polar solvents such as water.
140
How to classify primary, secondary and tertiary?
- Alcohols and Halogenalkanes --> Refers to the nmber of carbon atoms that are bonded to the carbon atom with the Functional group
- Amines --> Number of alkyl groups that are bonded to the Amine
141
Why should you not innhale benzene?
Vapours are quite hazardous --> Benzen is a carcinogen
142
Write the equations for the initian, propogation and termination of Free Radical substitution between Clhorine and Methane?
(- represents the dot)
Cl2 --> 2Cl' (Initiation)
**Propogation**
CH4 + Cl' --> 'CH3 + HCl
'CH3 + Cl2 --> CH3Cl + Cl'
**Termination**:
Cl' + Cl' --> Cl2
'CH3 + 'Cl --> CH3Cl
143
Can you explain what happens in the initiatoon step of free-radical substituion?
- Bond between Cl2 atoms breaks in the presence of UV light
- Homolytic Bond fission --> forms free radicals
144
Propogation
- Chlorine free radical + Molecule of methane
- Makes a chlorine free radical and Hydrogen Chloride
145
What is the theoretical enthalpy change in combustion equation?
Sum of reactants - Sum of products
1- You take big (number of moles ) into account
2- Tink about each indivudal bond
146
Why does Mg have a higher ionisation energy than Na?
- Mg has a greater number of protons
- greater attraction by Mg for valence electrons --> Lower Atomic Radius
147
Why does Calcium have a greater melting point than K
Ca2+ > K+
- greater attraction between delocalised e
148
Why is the boiling point of Na2O > SO3?
Sodium oxide is ionic whereas SO3 is covalent
Na2O has SEFoA whereas SO3 has weak IMF's
Forces more easily broken than in ionic bonds
149
Definition of enthalpy bond change?
Enenrgy needed to break one mole of a bond in a gaseous molcule; averaged over similar compounds
150
How soluble are Alchohol?
- Alcohols are soluble in water as they can form H bonds in Water
151
How soluble are Alchohol?
- Alcohols are soluble in water as they can form H bonds in Water
152
Partial oxidation of Primary Alcohols?
Catalyst - Potassium Dichromate
Aldehyde
If the aldehyde is the desired product, it can be removed as it forms by distillation
. This is possible because the boiling point of the aldehyde is lower than that of both the alcohol and the carboxylic acid
153
Complete Oxidation of primary alcohols?
Carboxylic Acid
Conditions: heat under reflux + excess oxidising agent
If Carboxylic acid is wanted --> heat mixture
154
Oxidation of Secondary Alcohols
Only produces 1 product for both partial and complete oxidation
Ketone
Conditions: Potassium Dichromate and heat under reflex
155
Oxidation of tetiary alcohols
Tertiary alcohols have no hydrogen atoms bonded to the carbon atom that is directly bonded to the hydroxyl group. Therefore, they do not undergo oxidation reactions
156
Examples of giant covalent structures?
Diamond, graphite Silicon, Silicon Dioxide
157
Examples of Molecular covalent structures?
H2O, CO2, C6H12O6
158
aRE TWO IDENTICAL NON-METALS POLAR?
No, two non-polar covalent bonds for two identical molecules (also for C-H)
159
Scale for electronegativity?
0 - 0.4 (Pure covalent)
0.4-1.7 (Polar covalent)
1.7 - xyz (Iionic)
160
Ncl3 VESPR
4 Electron Domain
Electron Domain Geometry Tetrahedral
3 Bond Pairs and 1 lone pairs
Molecular Geometry (no lone pairs) Trigonal Pyramid
Bond Angle - 107
161
Cl2O VESPR
4 Electron Domain --> Electron Domain Geometry Tetrahedral
Bond pairs - 2
Lone Pairs - 2
Molecular Geometry - Bent
Bond Angle - 104.5
162
Properties of Diamond
Conductivity: None - all electrons are used in localised bonds
Geometry: 3-dimensional
Hardness: Very hard - all atoms are held together in the lattice by strong covalent bonds
163
Properties of Graphite
Conductivity - High only 3 electrons used in bonding - fourth found in a delocalised electron sea
Geometry - 2 dimensional
Hardness - Very soft - 2 dimeonsional sheets slide over each other because of weak van der Waals' forces between the sheets
164
Properties of Fullerene
Conductivity - No
Hardness - Soft imagine the molecular form of the ball room at Mcdonalds
165
does sulfur trioxide have a simple molecular structure
Sulfur trioxide (SO3) has a simple molecular structure.
166
What does the IHD mean?
- Gives the number of molecules of the H2 needed to convert organic compounds to the corresponding saturated, non-cyclic molecule
167
What does the IHD mean?
- Gives the number of molecules of the H2 needed to convert organic compounds to the corresponding saturated, non-cyclic molecule
168
IHD equation
IHD = 2X + 2-Y/2
169
rules for IHD
O2 + Sulfur atoms are not counted
Halogen atoms are treated like H atoms
For each N atom --> add 1 C + 1 H
Each double bond = 1IHD
One Benzen Ring = 1
170
Magnesium Oxide
Dot and cross for ionic compounds
SEE
171
Maxwell BoltzmannCurve
see
172
If you ae finding the IHD of a coumpound and you know the molecular formula, check the mr table and see if it corresponds with the exact mr value
If you ae finding the IHD of a coumpound and you know the molecular formula, check the mr table and see if it corresponds with the exact mr value
173
How to calculate IHD
SEE
174
Outline the concept of relative abundance.
Relative abundance is the percent abundance in nature of a particular isotope.
✓
✓
175
What are the following requirements for a reaction to occur?
- Correct orientation
- Reactant particles must collide with sufficient energy --> Ea needed
176
Diagram of Activation Energy on the effect of the Rate of Reaction
See
177
Draw a Maxwell - Boltzmann Distrbution graph
SEE
178
Draw a Maxwell - Boltzmann Distribution diagram when there is an increase in temperature?
SEE
179
Describe how a catalyst increases the rate of reaction
- Provides an alternative pathway
- Lower Ae
- Greater proportion of particles now have energy equal to, or greater, than the og AE
- Greater frequency of succesful collisions
180
What is the pH of unpolluted H2O
5.6
181
What is the pH of acidic H2O
5.0
182
What are the two types of Acid Deposition?
Wet Deposition and Dry Deposition
Wet - Acid rain, snow and fog
Dry - Acid, gases and solid particles
183
How are SO2 and Oxides of Nitrogen formed?
1.) Lightnings
2.) Internal combustion in engines
3.) Volcanic Eruptions
184
Draw the Equilibrium constant of
2NH3(g) + 2O2(g) ⇌ N2O(g) + 3H2O(g)
Squared always goes along the bottom
