Chemistry Conditions/Reactions Flashcards
1
Q
Addition of Water to Alkene
A
Phosphoric or sulfuric acid (conc) 330C 6MPa
2
Q
Addition of Hydrogen to Alkene
A
140C Nickel Catalyst
3
Q
Elimination of Haloalkane
A
Haloalkane + NaOH(eth) = Alkene + Salt + Water
NaOH(ethanolic)
4
Q
Elimination Dehydration of Alcohol
A
Alcohol = Water + Alkene Hot Aluminium Oxide or Sulfuric Acid
5
Q
Haber Process Condition
A
450C 350 Atm (similar to the temperature of the addition of water to alkene) Iron Catalyst
6
Q
Nucleophilic addition of CN- to Aldehyde/Ketones
A
NaCN and dilute sulfuric acid to produced HCN HCN is the catalyst
7
Q
Contact Process
A
450C Vanadium Pentoxide
8
Q
Increase in IE across Period 3
A
Increase in proton number AND similar shielding from the electrons underneath. There is a increased nuclear attraction of outer electrons.
9
Q
Why do giant covalent molecules not conduct
A
Because there are no mobile electrons to carry charges and they are fixed in covalent bonds
10
Q
Why a major product forms
A
Primary carbocations are LESS STABLE that teritiary or secondary carboncations and there produced more frequently. This is because of the POSITIVE INDUCTIVE EFFECT of ALKYL GROUPS and the tertiary or secondary carbocations have more alkyl groups.
11
Q
Standard enthalpy change of combustion
A
Enthalpy change when 1 mole of a SUBSTANCE is burnt in excess oxygen under stp
12
Q
Standard enthalpy change of formation
A
Enthalpy change when 1 mole of a compound is formed from it elements under stp
13
Q
Why giant covalent has higher BP than simple covalent with respect to SiO2 and SO3
A
SiO2 has a network of strong bonds. SO3 has weak VDW forces from induced dipoles. Higher energy is required to break bonds between SiO2 than to overcome the VDW forces of SO3 between molecules
14
Q
Amphoteric
A
A substance that reacts wtih an acid or base
15
Q
Acidic Hydrolysis of Nitrile to Carboxylic Acid
A
Dilute acid Reflux
eg propanenitrile + HCl + Water = Propanoic acid + ammonium chloride
16
Q
Shape of PCl5
A
Trigonal bipyramidal 120 and 90 degrees dsp3 hybridisation
17
Q
Weak Alkali versus Strong Alkali
A
Weak Alkali (like Mg(OH)2) do not fully disociate in water. Strong Alkali (like Na(OH)2 fully disociate in water and thus there are more OH- ions and hence are more alkali.
18
Q
Magnesium and Steam and speed of reaction compared to with water
A
Magnesium + steam= Magnesium oxide + hydrogen gas. Reacts vigorously as opposed to Mg + water which is slow
19
Q
Hess’ Law
A
The total enthalpy change chemical reation is independent of the route by which the chemical reaction takes place as long as the initial and final conditions are the same.
20
Q
Nucleophile
A
A donator of a pair of electrons
21
Q
Electrophile
A
An acceptor of a pairs of electrons
22
Q
Substitution of Alcohol with PCl5
A
Alcohol + PCl5 = POCl3 + Halogenoalkane + Hydrogen Halide
23
Q
Substitution of Alcohol with PCl3
A
Alcohol + PCl3 = Halogenoalkane + H3PO4
24
Q
Substitution of Alcohol with SOCl3
A
Alcohol + SOCl3 = Halogenoalkane + SO2 + HCl (SO2 and HCl are gases)
25
Lattice Structure
A uniform repeating arrangement
26
Acid Base Reaction with Halide Salt and H2SO4
NaCl + H2SO4 = NaHSO4 + HCl
27
Difference between Neutralisation Reaction and Acid Base
Neutralisation happens when 1 mol of water forms from a hydroxide ion and a hydrogen ion. Acid base reaction is when one molecule gives a hydrogen ion to another.
28
How bonding is affected by electronegativity
It depends on the DIFFERENCE IN ELECTRONEGATIVITY of the atoms involved in the bond. If the difference is larger there is the transfer of electrons to form an ionic bond. If the difference is small there is the sharing of pairs of electrons.
29
With relation to electronegativity why does NaCl have different bonding that SiCl4
There is a difference in electronegativity between the Na Cl and the Si and Cl. Because the difference in electronegativity of the Na and the Cl is so large, there is the transfer of electrons forming an ionic bond. Because the difference of the Si and Cl is smaller, there is the sharing of pairs of electrons forming a covalent bond.
30
Relative atomic mass
The average mass of an atom relative to 1/12 of the mass of a C-12 atom
31
Relative molecular mass
It is the ratio of the sum of all the relative atomic masses of the atoms in a molecule to 1/12 the mass of a C-12 atom
32
Aluminium Oxide with HCl
Al203 + 6HCl = 2AlCl3 + 3H20 It does not form Al2Cl6
| Aluminium Chloride behaves like a normal aluminium salt when it is aqueous
33
Explain why a disproportionation ocurrs
X atom has both lost and gained electrons
34
Conditions for Nucleophilic Substitution of Halogenoalkanes to make an amine
Ethanolic ammonia. Refluxed. Heated in a sealed tube.
35
Conditions for Nucleophilic Substitution of Halogenoalkanes to make a nitrile
Ethanolic CN- and refluxed. Heated in a sealed tube
36
Oxidation of primary alcohols to form aldehydes
DILUTE Acidified Potassium dichromate or acidified potassium manganate. WARMED NOT REFLUXED. DISTILLED
37
The equation and conditions for the formation of NO in the atmosphere
N2 + O2 = 2NO Extreme conditions required because a high activation energy is required because the triple covalent bond requires a lot of energy to break
38
Formation of NO2 in the atmosphere
Further oxidation 2NO + O2 = 2NO2 Brown gas
39
Formation of nitric acid from moist air and during a lightning storm
2NO2 + 1/2O2 + H2O = 2HNO3
40
Formation of ammonium salts to make fertilizers
NH3 (aq) + HNO3 (aq) = NH4NO3 (aq)
| NH3 (aq) + H3PO4 (aq) = (NH4)3PO4 (aq)
41
Ammonium Salt reacting with a hydroxide
Ammonium salt + metal hydroxide = Metal salt + water + ammonia.
NH4Cl (s) + Ca(OH)2 (s) = CaCl2 (aq)+ H2O (l) + NH3 (g)
Used to test for the presence of an ammonium salt. Add sodium hydroxide and heat and NH3 is released turning red litmus blue.
42
How to make nitric acid ammonia then fertilizers
N2 + O2 = 2NO
2NO + O2 =2NO2
2NO2 + H2O + 1/2 O2 = 2HNO3
N2 + 3H2 = 2NH3
NH3 + HNO3 = NH4NO3
43
The reactions for how acid rain is made worse by NO
SO2 + NO2 = SO3 + NO
2NO + O2 = 2NO2
SO3 + H2O = H2SO4
44
How is NO2 a catalyst
It increases the rate of reaction of SO2 to form SO3, it lowers it activation energy (hence why there is the contact process which is equilibrium) It ican be regenerated easily by oxidising again with O2 in the air
45
How are catalytic converters used to reduce acid rain/ the amount of NO which speeds up the producing of acid rain
2CO + 2NO = 2CO2 + N2
| Platinum hot catalyst in cars
46
Standard enthalpy change of atomisation
The standard enthalpy change when ONE mole of gaseous atoms is formed from its elements under standard condition.
47
Standard enthalpy change of neutralisation
The enthalpy change when one mole of water is formed by the reaction of an acid with an alkali under standard condition in their standard states
48
Standard enthalpy change of reaction
The enthalpy change when the amount of reactants skwon in the equation react to give products under standard conditions. The reactants and prodcuts must be in their standard states
49
Standard enthalpy change of solution
the enthalpy change when one mole of solute is dissolved in a solvent to form an infinitely dilute solution under standard conditions
50
Standard enthalpy change of hydration of an anhydrous salt
The enthalpy change when one mole of a hydrated salt is formed from 1 mole of the anhydrous salt under standard condition
51
Homogeneous Catalyst
When the catalyst is in the same state as the reactants eg when the catalyst is in a aqueous state and the reactants are in an aqueous state
52
Electron Configuration for Cu
[Ar] 3d10 4s1
Rather than [Ar] 3d9 4s2
Extra stability of fully d orbitals
53
Electron Configuration for Cu+
[Ar] 3d10
10 should be smaller and above the d
Removes electron from 4s1 because it is the least stable and easiest to remove
54
Electorn Configuration for Cu2+
[Ar] 3d9
| 9 should be smaller and above the d
55
Electron Configuration for Cr
[Ar] 3d5 4s1
| Rather than [Ar] 3d4 4s2
56
Electron Configuration for Cr2+
1s2 2s2 2p6 3s2 3p6 3d4
| First removes the 4s1 because it is the least stable then an electron from 3d5 to go to 3d4
57
Electron Configuration for Cr3+
1s2 2s2 2p6 3s2 3p6 3d3
58
Electron Configuration for Ti
[Ar] 3d2 4s2
| GENERALLY electrons fill up from the 4s orbital and then start to fill up 3d orbitals
59
Electron Configuration for Fe
1s2 2s2 2p6 3s2 3p6 3d6 4s2
Write the configuration with the higher number energy levels are the end because that is the order that the electrons are removed
60
Electron Configuration for Fe2+
1s2 2s2 2p6 3s2 3p6 3d6
61
Electron Configuration for Fe3+
1s2 2s2 2sp6 3s2 3p6 3d5
62
Trend in Thermal Decomposition of Nitrates and Carbonates
The temperature at which the thermal decomposition occurs increases going own Group 2 for both carbonates and nitrates of Group 2. In some cases, the more reactive the element, the stronger the bond.
63
pH of Period 3 Chlorides with water
NaCl 7 MgCl2 6.5 Al2Cl6 3 SiCl4 2 PCl5 2 SCl2 2
64
Thermal Decompostion of calcium nitrate
Calcium nitrate = Calcium oxide + nitrogen dioxide + oxygen
65
Thermal Decomposition of calcium carbonate
Calcium carbonate = calcium oxide + carbon dioxide
66
Trend in thermal stability of hydrogen halides
HF is most thermally stable and HI is the least thermally stable because the bond energies decrease as you go down the group. It is because iodine has a large molecule are larger and thus a larger bond length thus less energy is required to break it. Less overlap of electrons
67
Trend in displacement reactions with halogen
The more reactive halogen displaces a less reactive halogen
68
Why Cl2 displaces Br in NaBr
Chlorine atoms are more electronegative than Bromine tom so have a stronger tendency to form negatively charged ions.
69
Use for cyclohexane with respect to Halogens
During displacement reactions is it difficult to identify the halogen that is displaced out. Adding the non polar solvent dissolves the diatomic molecule present in the solution and gives a colour corresponding to the halogen that has been dissolved.
70
How diols are made from alkenes
Alkene + WATER + [O] = Diol
Cold dilute Manganate solution
eg ethene + H2O + [O] = ethane- 1,2 - diol
71
Alcohol and Sodium Metal
| Ethanol and Sodium
Sodium Ethoxide/ Alkoxide + H2 gas
| Similar to sodium and water reaction
72
Allotrope Definition
Different crystalline or molecular FORMS that exist of the an element
73
Colour of Group 2 Flames when heated in O2
| Magnesium and Calcium
Calcium flame. Brick-red
| Magnesium flame. Bright white flame
74
Colour of flame when Strontium and Barium are heated in O2
Strontium scarlet red flame
| Barium green flame
75
Colour of Group 2 Metal Oxides when heated in O2
White solid White oxide
76
Explain the trend in reactivity of Group 2 Metals with O2
Reactivity increases down the group. It is because atoms get larger and larger down the group and hence the 1st and 2nd ionisation energies for the metals decreases down the group and hence lose their outer electrons more easily
77
Trend in reactivity of Group 2 Metals with H2O
As you go down the group, the reactivity with water increase and gets more vigorous
78
Trend in reactivity of Group 2 Metal oxides with water to form a hydroxide
As you go down the group, the reactivity of group 2 metal oxides with water increase and gets more vigorous
79
Reactivity of Period 3 when heated with O2
```
Na reacts vigorously
Mg reacts vigorously
Al burns
Si reacts slowly
P reacts vigorously
S burns gently and can be further oxidised with V2O5
```
80
Observations when Period 3 is heated with O2
Na bright yellow flame white solid
Mg bright white flame white solid
Al bright white flame less bright that Mg
Si burns slowly
P yellow-white flame cloud of white phosphorous oxide
S powder burns gently with blue flame
81
Reactivity of Period 3 with Chlorides
Na Mg Al all react vigorously
Si reacts slowly to form SiCl4
P reacts slowly to form PCl5
82
Use for CaCO3 and CaOH2
Neutralise Soil
83
Use for CaCO3
Cement
84
What reacts with 2,4 -DNPH
The carbonyl group of only aldehydes and ketones nothing else
85
Explain how fertilisers cause harm to animal and plant life
Nitrate fertilisers dissolve and are leached into waterways/ground water.
Promotes an algae bloom
Sunlight is blocked because algae grows on the surface of the water and plants cannot photosynthesise
Those plants and the algae die and abcteria in the water feed on dead organisms
Decrease in O2 concentration in water and fish can die
86
Vapour Pressure and high vapour pressure and low vapour pressure
It is the pressure exerted by a vapour in equilibrium with its liquid. It is caused by the gas particles hitting the walls of the container. A closed system
At a high vapour pressure there is a greater proportion of gas particles than liquid particles in the equilibrium
At a low vapour pressure there is a greater proportion of liquid particles than gas particles in the equilibrium
87
What 3 factors that increase vapour pressure
The kinetic energy of the gas particles is high
The gas particles move faster and so are able to overcome intermolecular forces of attraction more easily
The strength of the intermolecular forces that occur between each gas molecule
88
Boiling Point in relation to vapour pressure
The temperature at which the vapour pressure is equal to the atmospheric pressure is the boiling point of the liquid
89
Colour change when Cr2O72- is reduced or when it oxidises something
Orange to Green
90
Groups that react with iodine and aqueous NaOH
CH3CO group with aldehyde and ketones. Methyl ketones. Only ethanal reacts. CH3CHOH. Secondary Alcohol group. Only ethanol reacts.
91
Avogadro's hypothesis
At room temperature and pressure, one mole of any gas has a volume of 24dm3
92
Hydrolysis of Nitriles with H2O
CH3CN to CH3CONH2 to CH3COONH4 very slow
93
Hydrolysis of Nitriles with Acid
CH3CH + H2O + HCl = NH4Cl + CH3COOH
| The carboxylic acid is a very weak acid so carboxylate ions do not form readily
94
Hydrolysis of Nitriles with Alkali
CH3CH + H2O + NaOH = CH3COONa + NH3
| Sodium carboxylate is more soluble so it produces a lots of CH3COO- ions.
95
Why isotopes have the same chemical properties
They have the same number of electrons
96
Where are electrons found in the atom
In the shells
97
SO2 and the environment
Forms acid rain Kills plant life
98
Properties of ideal gases
Particles have volume but the volume is NEGLIGIBLE compared to the volume of the container
Collisions between particles are perfectly elastic
No interactions between particles except when they collide
Particles are in constant random motion
Kinetic energy of particles is proportional to the temperature
KNoT REN
99
Optical Isomers
Molecules are that non-superimposable mirror images of each other and have a central chiral carbon atom
100
What do more alkyl groups do to a carbocation
Because of more alkyl groups there is a greater positive inductive effect. It STABILISES THE CHARGE of the carbocation and makes the carbocation more stable/ spreads the charge across the molecule
101
Problems with PTFE
Releases toxic gases like HCl when burnt . Nonbiodegradable
102
Enhanced greenhouse effect
HUMAN ACTIVITY that creates a thicker layer of greenhouse gases and has an impact on climate change
103
Problems with CFCs
Contribute to ozone depletion. Greenhouse gas that warms contributes to global warming and climate change.
104
Substition of Alcohol with SOCl2
alcohol + SOCl2 = SO2 + HCl + Chloroalkane
105
Reduction of carboxylic acids to alcohol and catalysts
CH3COOH + 4[H] = CH3CH2OH + H2O
Aqueous alkali NaBH4
LiAlH4 in dry ether
106
Use for MgOH2 or MgO
Antacids
