Key definitions etc. Flashcards
1
Q
What is a radical
A
Atoms with an unpaired electron. They are formed from CFCs and by using UV Radiation and high energy radiation. Molecules can undergo homolytic fission and create radicals.
2
Q
Explain why you cannot measure the enthalpy bond of formation of 2 reactants?
A
Because they don’t react together under standard conditions. There will be side products formed.
3
Q
What is the CO bond in CO2?
A
A DOUBLE BOND (this is important for calculating bond enthalpy)
4
Q
What is one main thing about concentrated acids?
A
They create a greater change in oxidation states.
5
Q
How to obtain a more accurate value for the enthalpy change of combustion? (PAG related)
A
Insulate the can.
Burn the material in oxygen to ensure it is fully oxidised.
6
Q
Explain Le Chatelier’s principle
A
There will be an equilibrium shift in an reaction to minimise the effects of a change in a condition
7
Q
Define the enthalpy change of combustion
A
The enthalpy change for the complete combustion of 1mol of a substance under standard conditions (100kPa and 298K)
8
Q
Define the enthalpy change formation
A
The enthalpy change when 1 mol of substance is formed from its elements under standard conditions.
9
Q
If they ever ask you to calculate the enthalpy change of combustion, what is one thing to remember ?
A
ENTHALPY CHANGE OF COMBUSTION IS ALWAYS NEGATIVE
10
Q
How can you identify for Fe?
A
Add NaOH and if it creates a green precipitate, Fe is present.
11
Q
How can you identify non-polar and polar molecules?
A
If there is a lone pair of electrons on the central atom, then the molecule is polar.
12
Q
Where is electronegativity the highest?
A
Generally, F is the highest in electronegativity. It increases from left to right, and from the bottom up.
13
Q
What difference in electronegativity makes a bond polar?
A
0.4 - 1.7 means it is polar covalent
14
Q
What is electronegativity?
A
An atom’s ability to attract a pair of electrons in a covalent bond.
15
Q
Tests for halide ions
A
Add some drops of nitric acid.
Then some silver nitrate solution.
Observe the colour of the precipitate.
16
Q
Testing for sulfate ions
A
Add barium chloride (or barium nitrate).
If a white precipitate is formed, then sulfate ions are present (as it create Barium sulfate)
17
Q
Testing for carbonate ions
A
Add dilute HCl. Put any gas being formed to lime-water. If it turns cloudy, then the gas being formed is carbon dioxide.
18
Q
How can you obtain an accurate value for the ethalpy change of combustion?
A
Insulate the can.
Put a lid of the can.
Burn the fuel in oxygen to ensure full oxidation.
19
Q
How can you differentiate between alcohols?
A
Add acidified potassium dichromate (VI) annd tertiary alcohols will stay the same colour. But pirmary and secondary ones will change their colour (turn green)
20
Q
Markownikoff’s Rule
A
When a HX reacts with an assymetrical alkene, the X will bond to the Carbon bonded to the most Carbons. Because a tertiary carbocation is more stable than a secondary one.
21
Q
What are the 4 main stages in a simple generalised model of heterogeneous catalysis.
A
Stage 1 reactant(s) adsorbed/bond to surface of catalyst
Stage 2 (reactant) bonds (weaken) and break
Stage 3 (product) new bonds form
Stage 4 product(s) desorbed from surface of catalyst
22
Q
What colour is iodine in cyclohexane
A
Purple
23
Q
What colour is bromine in cyclohexane
A
Orange
24
Q
What colour is chlorine in cyclohexane
A
Colourless
25
Are hydrogen bonding stronger than dipole-dipole interactions
Yes, they are. This means that they require more heat to break.
26
Difference between absorption and emission spectrum
The difference between absorption and emission spectra are that absorption lines are where light has been absorbed by the atom thus you see a dip in the spectrum whereas emission spectra have spikes in the spectra due to atoms releasing photons at those wavelengths.
27
How does the salt form in this reaction?
The hydrogen ion of the acid has been replaced by a metal ion
28
What is the one thing u should remember when you are writing equations for ionisation energies?
INCLUDE STATE SYMBOLS (always gases)
29
Why is a molecule polar?
Because the molecule is non-symmetrical and so the dipoles don’t cancel out. This means there is a net dipole on the molecule
30
What is the difference between a base and an alkali
A base is a substance that readily accepts H+ ions.
An alkali is a substance that releases OH- ions into aqueous solutions
31
What is a homologous series?
Same functional group
Same general formula
Each successive member differs by the addition of a CH2 group.
Same physical and chemical properties.
32
Name the 2 stages that'll turn an alkane into an ethene.
fractional distillation and cracking.
33
What does "average bond enthalpy" mean
Average enthalpy change when one mole of bonds of gaseous covalent bonds is broken
34
Properties of a gas in an aerosol:
```
Low reactivity
Non-flammable
Volatile
Low boiling point
Non-toxic.
```
35
What happens to a molecule when IR is absorbed?
The bond will vibrate and bend more.
36
Why may your value of Energy change be smaller than expected?
Incomplete combustion
Non-standard conditions
Evaporation of water or alcohol
Count towards the SHC of beaker.
37
Describe the relative energies of the 2s orbital and each of the three 2p orbitals in a
nitrogen atom.
p-orbitals have greater energy than s-orbitals
| (three) p-orbitals have equal energy
38
Solid chlorine and solid bromine have a similar structure.
| Name this structure.
Simple covalent
39
Main points in:
Explain the differences in the melting points of sodium and magnesium, using the model of
metallic bonding.
Just remember that the Mg has a greater attraction between the ions and the delocalised electrons.
40
Give the formula and the name of the compound formed between fluorine and sulfur
which has octahedral molecules.
SF6.
| Called sulfurhexafluoride.
41
If you are going to produce X(OH)2 as a product, then the H20 you are reacting with, needs to be what state?
The H20 needs to be in a liquid state.
| Otherwise, it will produce XO, when the H20 is in a gaseous state.
42
What shape is a F20?
Bent/ non-linear.
| It has bond angles of 104.5
43
On a F20, what is the dipole?
Negative on the F, positive on the O.
44
In F20, what is the oxidation state of the O?
+2
45
Where are the ionisation numbers the highest?
It increases from right to left, and from bottom to top.
| So the highest, is top right.
46
Define the second ionisation energies
It is the energy needed to remove a second electron from each ion in 1 mole of gaseous 1+ ions to give gaseous 2+ ions.
47
What is hydrolysis
When you break something down by adding water.
48
How carbon monoxide and nitrogen monoxide is made in catalytic converters, and emitted from cars.
Generally, they are formed due to incomplete combustion, so incomplete combustion equations for the reactions/ pollutants mentioned.
Then, talk about how a catalytic converter works.
Reactnats are absorbed onto surface, then the bonds are weakened. Then, the reaction takes place (the 2 pollutants react together, to form usually CO2 and N2). They desorb from the surface.
49
Structural isomers definition
Same molecular formula, but a different structural formula
50
Stereoisomers definition
Same molecular, and structural formula, but a different spacial arrangement
51
State two ways that the use of catalysts helps chemical companies to make their
processes more sustainable and less harmful to the environment.
Lower temperatures, lower pressures can be used.
Lower energy demand
Greater atom economy, so less waste, less use of toxic reactants
52
When drawing isomers from a peak on a mass spectrum
make sure to put charges (usually +)
53
State and explain the features of a hex-2-ene molecule that lead to E and Z isomers.
(carbon-carbon) double bond does not rotate
OR has restricted rotation
Each carbon atom of the double bond attached to (two)
different groups/atoms
54
With E=mc Change in T questions...
if they ever give you a density, then you should ALWAYS ALWAYS ALWAYS USE THE VOLUME TO CALCULATE THE MASS!!!
55
dm3 to m3
multiply by 10^ -3
56
Difference between pi-bonds and sigma bonds
Sigma bond is between bonding atoms/nuclei AND pi- bond is above and below the bonding atoms/nuclei.
sigma bond has direct/head-on overlap of orbitals AND pi- bond has sideways overlap. sigma bond has a lower bond enthalpy / is weaker than a pi-bond.
Sigma bond has electron density between bonding atoms AND Pi- bond has electron density above and below bonding atoms
57
When drawing OH bonds
never make it a horizontal OH bond!!
58
When naming isomers
make sure to put the Z/E in front of the isomer.
59
What is the formulae of vinegar?
CH3COOH
60
During a titration:
Suggest one assumption that the student has made that might mean that their calculated
concentration of ethanoic acid in the vinegar is invalid.
Predict, with a reason, how the experimental result would differ from the actual
concentration of CH3COOH if the assumption were not correct.
That the vinegar is pure, and contains no other acids. Otherwise the result would be greater.
61
Whenever calculating the Kc
always multiply the concentrations.
| And it's products/ reactants.
62
In any transition element questions
The 4S ELECTRONS ARE LOST FIRST!
63
How to calculate the EMF of a cell?
Reduction value - oxidation value.
64
Advantages of using fuel cells rather than fossil fuels
Only water is created- so there are no toxic products.
| Has a greater efficiency
65
Disadvantages of using fuel cells rather than fossil fuels
H2 is difficult to store
| H2 is difficult to manufacture initially.
66
Define the term "standard electrode potential"
The EMF of an electrochemical cell comprising a half cell combined with a standard hydrogen electrode at 1 atm, 298K, and all solutions at 1 moldm-3
67
Complete the diagram to show how the standard electrode potential of xyz can be measured.
Draw 2 half cells, connected by a salt bridge. In one, put a beaker thing with Hydrogen feeder inside it. That solution should be labelled as 1 moldm-3 H+ (aq). Put inside the hydrogen feeder, a platinum electrode.
In the other half cell, put in the normal electrode (AND LABEL THE IONS AND ELECTRODES!! WITH STATES!)
Connect the electrode together using a voltmeter.
68
Give one use for Chromium
Used for stainless steel because it can resist corrosion.
69
How to determine which half cell is reduction or oxidation?
Whichever is more positive is the reduction.
| YOU HAVE TO SAY MORE POSITIVE!!! NOT HIGHER!!!
70
What are standard conditions for a electrochemical cell
Temperature of 298K, solutions at 1 moldm-3, and 100kPa pressure.
71
If they ask you about the oxidising ability of a specific chemical
Say that it's EMF is more positive than the others, so it is a better oxidising agent.
72
When labelling an electrochemical diagram
PUT ALL IONS AND THEIR STATES!!!
| it costs marks.
73
If they ask you what is oxidised and what is reduced
You have to say that xyz ION is oxidised, and xyz ION is reduced.
74
What colour is an acid on the pH scale?
Red
75
What colour is an alkali on the pH scale?
Violet/ blue
76
What colour is neutral on the pH scale?
Green
77
What is an aromatic compound?
They have a benzene ring in it.
78
What is an aliphatic compound?
No benzene ring.
79
When writing the equation of formation
The reactants are the elements itself, ALONE. You can’t have NaCl, but you can have Na + Cl2.
80
Hess’s law
The enthalpy change of any chemical change is independent of the route by which the chemical reaction occurs.
81
Equation for chlorine + NaOH to form bleach
2NaOH + Cl2 -> NaCl + NaClO + H20
| Conditions: cold and dilute NaOH.
82
Equation for glucose + yeast:
C6H12 O6 -> 2C2H5OH + 2CO2
| Has to occur in anaerobic conditions and betwen 20-45 degrees.
83
Catalytic converter reaction:
2NO + 2CO -> 2CO2 + N2
84
Describe how London forces arise
The random movement of electrons causes an uneven distribution of negatvie charge, which creates an instantaneous dipole on a molecule. Then, this interacts with other neighbouring molecules to induce a dipole on them too.
85
If you have a solution of NaI and another of NaCl. THen, you add in bromine water into each, and some cyclohexane, then what colour change will you see, what are the reactions that'll tkae place and what does this tell you about the trend in reactivity?
Reactivity of the halogens decreases down the group. This is because the electron shielding increases down the group, and the nuclear attraction becomes smaller, making it harder to gain an electron and react. A halogen that is more reactive can take the place of a halogen that is less reactive.
When you add the Bromine water to the NaI, then the bromine will take place of the iodine. This is because bromine is more reactive than iodine. This means that you will gain Br- ions, and I2. There will be 2 layers in the test tube, where the organic laer will be a purple colour due to the I2.
(give ionic reaction)
When you add the bromine water to the NaCl, then no reaction will take palce. This is because chlorine is more reactive than bromine. There will be Br2 and Cl- ions, which means that in the test tube, there will be a colour change to orange due to the bromine.
86
How could the student obtain a sample of magnesium phosphate after reacting magnesium with phosphoric acid?
Filter to obtain the solid and then evaporate the water (or dry the solid)
87
Equation to find the EMF of a cell:
E = E(reduction) - E(oxidation)
88
How to find the sign of an electrode:
It's the same as the EMF value for each half cell.
89
How does platin act in the treatment of cancer patients.
Platin binds to the DNA of cancer cells and stops them replicating.
90
What is meant by one mole of substance?
(The amount of substance which contains) as many
| particles as there are carbon atoms in 12g of 12C (atoms)
91
Reasons for the order of anions test
Carbonates test is done first, because the barium ions will react with the carbonate ions to precipitate, giving a false positive.
Also, you add nitric acid before testing for halides because the solutions can easily absorb CO2 to form carbonate ions, which if reacting with Ba2NO3, then it will easily show a false positive for halides.
92
If they ever ask for the molecular formula
Give it as "C4H802", rather than "C3H7COOH", because the second one is more structural formula.
93
Whenever they ask you about boiling point of one being greater than the other
Refer to forces between them. As in x has hydrogen bonding, and y has permanent dipole-dipole interactions.
So x is harder to break, and requires more energy.
94
What is stronger, hydrogen bonding or PD-PD?
Hydrogen bonding is a lot stronger.
95
How do you know that all the impurity from a reaction has been removed/ the reaction has finished?
There will be no more fizzing, precipitation formed, or colour change etc.
96
Whenever they talk about breaking things down
Say how they break (eg- by hydrolysis) and into their monomer units.
97
If they ever ask you to draw optical isomers
Draw 3D diagrams
98
Whenever talking about chiral centres?
Say that they are attached to 4 different groups, this allows it to produce mirror images of a compound, and create 2 enantiomers.
99
When do you use cis/trans
For cis/trans, each Carbon on the double bond needs to be attached to another carbon or alkyl chain
100
Disadvantages of producing a chiral drug as a mixture of stereoisomers. Then state some solutions to make only a single optical isomer
Disadvantages:
- Cost/ difficulty in separating.
- one stereoisomer might have harmful) side effects
- reduces the (pharmacological) activity/effectiveness
Synthesis of a single optical isomer
- using enzymes or bacteria
- using a chiral catalyst
OR transition metal complex/transition metal catalyst
- using chiral synthesis
OR chiral starting material
OR natural amino acid
101
How can you manufacture ethanol
```
Ethane
Add phosphoric acid
And steam
300 degrees C
60-70 atm pressure
```
102
Why does xyz not show optical isomerism
Because it doesn’t have a chiral carbon and so there is no asymmetry in the molecule
103
What happens at the isoelectric point
A zwitterion is formed and the net charge is 0.
104
Suggest an advantage of synthesising something starting form a natural steroid
It ensures that you create the correct isomer. So that way, you have to only make one and don’t need to spend money separating isomers.
105
State ways polyester can be degraded
UV or photodegradable
| Or hydrolysis
106
Write the formula of H2N(CH2)4NH2 mixed with excess HCl
ClH3N(CH2)4NH3Cl
107
Why would something be in zero order
Because it is in excess or it’s concentration doesn’t change.
108
How does the ionisation energies change across a group
The number of electrons increases, increasing the atomic radius, and therefore the electron shielding.
The nuclear attraction on the outer electron decreases as well, and therefore the first ionisation energies decrease.
109
How does the ionisation energies change across a period
Nuclear charge increases, shielding doesn't increase, so that the nuclear attraction increases on the outermost electrons, leading to the atomic radius decreasing. This means that the first ionisation energy increases.
110
Graphs of the first ionisation energies
It gradually increases across a period, but then goes all the way down for the next period, and starts increasing again.
111
Weird cases for the first ionisation energies
2p4 is easier to remove than 2p3.
This is because there is electron repulsion between the 2 electrons, leading to a smaller energy required to separate them.
Why is it easier to remove a 2p electron than a 2s electron? Because the 2p is a higher energy electron,
112
A proposed mechanism for this reaction takes place in several steps.
Suggest two reasons why it is unlikely that this reaction could take place in one step.
The rate equation doesn't match the overall equation. Collision is unlikely with more than 2 ions.
113
Whenever there is a compound, and they ask you why it is only x% effective/ thinking of isomers-
Write down how many chiral carbons there are and so how many enantiomers are made.
2 to the power of no. of chiral carbons.
114
Why is a certain fatty acid more likely to be concerned with heart diseases?
Because it is a saturated.
115
State 2 features that allow alkenes to show cis-trans isomerism
They have restricted rotation around the C=C double bond.
| Each Carbon on the C=C double bond must be attached to 2 different groups or atoms.
116
When something has a pH of 2.77 and it is put into a something with a high pH, how does the zwitterion change
You get COO- groups forming.
High pH means more alkaline- meaning you produce more OH-, so you have to remove the H+ ion from the COOH, and produce water, but you are left behind with COO-.
117
What does a cyclic dieter look like?
It has 6 C atoms, and there are 2 ester bonds in the circle.
118
Does C2O4 have a charge?
YES. -1
119
What is Iodate(V) ions
IO3 -
120
If I- is produced, and you want to check for the end point in a titration, what can you add
You should add starch.
| It will turn a blue black solution to colourless.
121
What causes the colour change from orange to green in the oxidation of alcohols?
Reduction of Cr 6+ to Cr 3+.
122
Suggest why the reaction causes a mixture of products
Because substitution can occur on any of the positions on the ring, forming different isomers.
123
How does amine act as a base
There is a lone pair of electrons on the Nitrogen atom, so it can accept a proton.
124
How to write reduction equation
4[H]
125
How can we use GC-MS to analyse a compound?
You can separate the compounds using the GC.
| Then, you can compare the results using a database. You can also identify using the fragmentation ions.
126
Define a nucleophile
The are electron pair donors
127
Name common nucleophiles
OH-
H20-
NH3-
128
Which C-X bonds are the strongest? The weakest?
The C- F bond is the strongest, and the C-I bond is the weakest. Therefore, the iodoalkanes react the fastest with nucleophiles, and the fluroalkanes react the slowest with nucleophiles.
129
What can esters be used for?
Perfumes, flavouring.
130
Difference between optical isomerism and stereoisomerism
Stereoisomerism is only used in alkenes.
| Optical isomerism is when there are chiral carbon existing, and the carbon is connected to 4 different groups or atoms.
131
If there are ever a LOT of peaks in a Carbon 13 NMR, but not too many in a Proton NMR
There is likely a benzene ring in there somewhere.
132
How is NMR used in medicine?
NMR Imaging.
133
How can you test for OH- ions?
Red litmus paper turns blue in the presence of OH- ions.
134
Order of tests:
Carbonates -> hydroxides -> sulfates -> halides
135
How many lone pairs of electrons are on the Oxygen in H2O?
There are 2 lone pairs.
136
Alkene + water
Alcohol
137
Which groups are 2,4 directing?
Don't begin with C-
138
Which groups are 3 directing?
Begin with C-
| NO2 and C-N.
139
Whenever dealing with amide /amine?
RTFQ!
| DOES IT SAY AMIDE OR AMINE?
140
Which compound is used as a standard for NMR chemical shift measurements?
Si(CH3)4
141
What is an alicyclic compound
NO BENZENE RINGS
142
Alkene + steam
Alcohol at the double bond.
143
Amides bond breaking down - draw the structure of the salts
You can't leave the charge alone. Salts should always have a net zero charge. So add NA+ etc. or as said in the question.
144
How to go from g/dm3 -> mol/dm3
Divide by the Mr.
145
Which of these organic compounds is more likely to be formed?
The element which is more electronegative will attach itself to the C bonded to the most Carbons. This is because the carbocation formed in this compound is more stable that the other one.
Then, show structures for both the compounds, saying one is more likely, and the other is less likely.
146
NaOH + compound with OH and COOH
Turns into COO-Na+ and O-Na+.
147
Na2CO3 + compound with OH and COOH
COO-Na+
148
How to prepare a organic solid?
Recrystallise- dissolve in a minimum amount of hot solvent.
Then cool and filter under reduced pressure.
Scratch with a glass rod.
Wash with cold water or solvent
And then dry.
If needed to find purification- then find melting point and compare to known values using a database.
149
CaCO3 + CH3COOH
2CH3COOH + CaCO3 → (CH3COO)2 Ca + CO2 + H2O
150
What is the product when CH3COCl is attached onto benzene ring?
Phenylethanone
151
What is a product with 2 COOH groups called
ex: Ethandioic acid
152
Which is stronger polyamides or polyester
Polyester has a permanent dipole-dipole interactions.
| Polyamides has Hydrogen bonding, which is stronger, so polyamides are stronger.
153
Why is acyl chlorides better than COOH
A faster reaction
154
Why are Anhydrides better than Acyl chlorides
They aren't as violent of reactions.
155
Is (CH3)NH more basic than ammonia?
Yes!!!
Because the alkyl group pushes the electron density towards the nitrogen atom- making it more attractive to electrophiles.
156
What is the reaction where you turn a primary amine into a secondary amine by using a haloalkane?
A nucleophilic substitution
157
Solubility of group 2 sulfates down the group
Decreases down the group
158
Solubility of group 2 hydroxides down the group
Increases down the group
159
Are alcohols polar?
Yes, they are polar. They have the -OH Bonding which makes it polar.
160
How to show hydrogen bonding
Make a bond from the Oxygen of the alcohol to a hydrogen of the H2O molecule. AND- Always put 2 pairs of electrons on the Oxygen atom.
161
Alcohol to alkene
Reflux with H3PO4.
Called a dehydration reaction or elimination.
Here, you may get isomers, as you can't control where the double bond will go.
162
What can be used as a drying agent?
Anhydrous MgSO4.
163
What is a redox reaction/ what to look for when identifying a redox reaction?
Look at the oxidation states.
| For a redox reaction, you should have an oxidation reaction and a reduction reaction.
164
Which of the following is the correct procedure for rinsing glassware before beginning a titration?
1. Rinse the burette with acid before filling with the acid solution.
2. Rinse the pipette with distilled water before filling with alkali.
3. Rinse the conical flask with alkali before adding a measured volume of the solution.
Only 1.
2. is wrong because the pipette should be rinsed with the alkali that will be used, and not distilled water.
165
Should you rinse the burette with acid before filling with the acid solution
Yes.
166
How do group 2 metals react with water?
X(OH)2 + H2.
167
How does the reactivity of group 2 metals change as you go down the group?
Increases- because they form 2+ ions.
168
How does the alkalinity of group 2 hydroxides change as you go down the group?
The solubility of the hydroxides in water increases.
Therefore, the pH increases.
And so, the alkalinity increases.
169
In terms of bond breaking, explain why this reaction is exothermic.
Bond breaking is exothermic, and bond making is endothermic.
Bond breaking absorbs energy and bond making releases energy.
In this reaction, more energy is released than absorbed.
170
How to calculate the enthalpy change
Bond breaking - bond making.
171
Enthalpy diagrams- which way is exothermic
Go down
172
Why is the boiling point of AsH3 higher than PH3?
They both have a charge of -3.
As has more electron shielding, so it has a greater negative attraction, therefore it requires more energy to break than P.
173
Note for explaining in equilibrium why something doesn’t have a high temperature despite it reaches a higher yield?
It is because high temperatures can use up a large amount of energy and fuel, not because it’s expensive.
174
How to represent Partial pressure (used for gases only)
p(X)
175
In a heterogeneous reaction, what states ARE included?
ONLY GASES AND AQUEOUS.
176
Note for why does the group 2 elements Mg- Ba increase down the group
Don’t say that it is easier to remove the electrons, say that as you go down the groups, it requires less energy to react
177
Proper definition of a disproportionate reaction
A reaction in which the same element is both oxidised and reduced.
178
How to write an equation for the enthalpy change of atomisation of X
It MUST PRODUCE 1MOL OF THE PRODUCT!
| ONLY 1 MOL OF PRODUCT
179
What happens o Cu2+ in NH3
It forms Cu(OH)2.
| Only in EXCESS nh3, it forms the complex ion with 4 NH3 and 2 H2P
180
Uses of hydrogen
```
Fuel cells
Hydrogenation of alkenes
Haber process
Making of HCl
Making of methanol
```
181
How can an aqueous solution of an acid contain hydroxide ions?
Because the water also dissociates
182
Reaction of CaCO3 and CH3COOH
```
It produces (CH3COO)2Ca
If you will use ions, and signs, make sure to put the symbols on both the ions. OR just don't put them at all.
```
183
Transition elements as catalysts
Haber process- iron catalyst.
Contact process- Vanadium(V) Oxide
Hydrogenation of margarine- Nickel.
Decomposition of hydrogen peroxide- MnO2.
184
Features of Transition elements
- Elements can act as catalysts
- Different oxidation states
- Have colourful compounds
185
Weird cases for the electron configuration of transition elements
Copper and chromium:
They have 3d5 4s1 or 3d10 4s1.
It is better to have this than a nearly full or nearly half full 3d shell.
186
Transition metals and oxygen
Each haem group has a Fe2+ ion.
| The oxygen binds to this.
187
Explaining why the temperature of a reaction is lower than it should be for an equilibrium reaction
Because a high temperature requires more energy and fuel.
188
How to represent partial pressure of a substance
p(X)
189
What states are included for the Kc expression of a heterogenous reaction?
Only gases and aqueous compounds
190
Proper definition of a disproportionate reaction
A reaction in which the same ELEMENT is both oxidised and reduced.
191
Explain why the reactivity of group 2 elements increases down the group
At the end, you have to say that there is less energy required for the reaction to occur.
192
Why does As have a higher boiling point than P
Both have a charge of 3-.
| As has more electron shielding. Therefore, it has a greater attraction, so more energy is required to break the bonds.
193
How to write the reaction of Standard enthalpy change of atomisation
YOU MUST PRODUCE 1 MOL OF THE PRODUCTS.
| ONE ONLY!!!
194
Why should you always calibrate pH meters before using?
Because they can be affected by temperature changes.
195
How to show the enthalpy change of reaction in a enthalpy profile diagram
Make sure to add the arrow to show which way the enthalpy change is.
196
Chlorate (I)
ClO-
197
Chlorate (VI)
ClO3 -1.
198
How is the periodic table arranged?
Increasing proton number.
In periods, showing repeating trends in physical and chemical properties.
In groups, having similar chemical properties.
199
What is metallic bonding
Strong electrostatic attraction between cations and delocalised electrons.
All metals have this giant metallic lattice structure.
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Use of Group 2 metals
Ca(OH)2 in agriculture to neutralise acidic soils.
| Mg(OH)2 and CaCO3 as antacids in treating indigestion.
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Why can't we use Ka to calculate the pH of stronger acids
Because the concentration of the acid at equilibrium may no longer be equal to the concentration of the acid at the beginning. (because it is for the weak acids)
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Example of a square planar complex ion
Pt(Nh3)2Cl2
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If you are told to react Mg (or any other metal with the charge of more than 1+) in an existing buffer solution, and are told to calculate the pH, what should you do?
Calculate the moles of the metal.
Multiply it by the magnitude of its charge (because then it creates a balanced reaction).
Then, add that moles onto the moles of the conjugate base (as you produce more), and take it away from the moles of the acid (as it will be used up instead).
Then, use the Ka to calculate the H+ concentration and eventually, the pH.
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What is the difference between the endpoint of a titration and the equivalence point?
The endpoint is when the colour changes, but the equivalence point is when the added titrant is chemically equivalent to the base.
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What does the stability of a compound based on?
A tertiary carbocation is more stable than a secondary carbocation. Also, the more alkyl groups attached to the Carbon atom, the more stable it is.
