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Chemistry Conditions/reactions > Chemistry Conditions/Reactions > Flashcards

Chemistry Conditions/Reactions Flashcards

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1
Q

Addition of Water to Alkene

A

Phosphoric or sulfuric acid (conc) 330C 6MPa

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2
Q

Addition of Hydrogen to Alkene

A

140C Nickel Catalyst

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3
Q

Elimination of Haloalkane

A

Haloalkane + NaOH(eth) = Alkene + Salt + Water

NaOH(ethanolic)

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4
Q

Elimination Dehydration of Alcohol

A

Alcohol = Water + Alkene Hot Aluminium Oxide or Sulfuric Acid

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5
Q

Haber Process Condition

A

450C 350 Atm (similar to the temperature of the addition of water to alkene) Iron Catalyst

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6
Q

Nucleophilic addition of CN- to Aldehyde/Ketones

A

NaCN and dilute sulfuric acid to produced HCN HCN is the catalyst

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7
Q

Contact Process

A

450C Vanadium Pentoxide

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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.

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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

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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.

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11
Q

Standard enthalpy change of combustion

A

Enthalpy change when 1 mole of a SUBSTANCE is burnt in excess oxygen under stp

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12
Q

Standard enthalpy change of formation

A

Enthalpy change when 1 mole of a compound is formed from it elements under stp

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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

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14
Q

Amphoteric

A

A substance that reacts wtih an acid or base

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15
Q

Acidic Hydrolysis of Nitrile to Carboxylic Acid

A

Dilute acid Reflux

eg propanenitrile + HCl + Water = Propanoic acid + ammonium chloride

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16
Q

Shape of PCl5

A

Trigonal bipyramidal 120 and 90 degrees dsp3 hybridisation

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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.

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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

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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.

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20
Q

Nucleophile

A

A donator of a pair of electrons

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21
Q

Electrophile

A

An acceptor of a pairs of electrons

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22
Q

Substitution of Alcohol with PCl5

A

Alcohol + PCl5 = POCl3 + Halogenoalkane + Hydrogen Halide

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23
Q

Substitution of Alcohol with PCl3

A

Alcohol + PCl3 = Halogenoalkane + H3PO4

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24
Q

Substitution of Alcohol with SOCl3

A

Alcohol + SOCl3 = Halogenoalkane + SO2 + HCl (SO2 and HCl are gases)

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25
Q

Lattice Structure

A

A uniform repeating arrangement

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26
Q

Acid Base Reaction with Halide Salt and H2SO4

A

NaCl + H2SO4 = NaHSO4 + HCl

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27
Q

Difference between Neutralisation Reaction and Acid Base

A

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.

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28
Q

How bonding is affected by electronegativity

A

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.

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29
Q

With relation to electronegativity why does NaCl have different bonding that SiCl4

A

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.

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30
Q

Relative atomic mass

A

The average mass of an atom relative to 1/12 of the mass of a C-12 atom

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31
Q

Relative molecular mass

A

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

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32
Q

Aluminium Oxide with HCl

A

Al203 + 6HCl = 2AlCl3 + 3H20 It does not form Al2Cl6

Aluminium Chloride behaves like a normal aluminium salt when it is aqueous

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33
Q

Explain why a disproportionation ocurrs

A

X atom has both lost and gained electrons

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34
Q

Conditions for Nucleophilic Substitution of Halogenoalkanes to make an amine

A

Ethanolic ammonia. Refluxed. Heated in a sealed tube.

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35
Q

Conditions for Nucleophilic Substitution of Halogenoalkanes to make a nitrile

A

Ethanolic CN- and refluxed. Heated in a sealed tube

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36
Q

Oxidation of primary alcohols to form aldehydes

A

DILUTE Acidified Potassium dichromate or acidified potassium manganate. WARMED NOT REFLUXED. DISTILLED

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37
Q

The equation and conditions for the formation of NO in the atmosphere

A

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

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38
Q

Formation of NO2 in the atmosphere

A

Further oxidation 2NO + O2 = 2NO2 Brown gas

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39
Q

Formation of nitric acid from moist air and during a lightning storm

A

2NO2 + 1/2O2 + H2O = 2HNO3

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40
Q

Formation of ammonium salts to make fertilizers

A

NH3 (aq) + HNO3 (aq) = NH4NO3 (aq)

NH3 (aq) + H3PO4 (aq) = (NH4)3PO4 (aq)

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41
Q

Ammonium Salt reacting with a hydroxide

A

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.

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42
Q

How to make nitric acid ammonia then fertilizers

A

N2 + O2 = 2NO
2NO + O2 =2NO2
2NO2 + H2O + 1/2 O2 = 2HNO3

N2 + 3H2 = 2NH3

NH3 + HNO3 = NH4NO3

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43
Q

The reactions for how acid rain is made worse by NO

A

SO2 + NO2 = SO3 + NO

2NO + O2 = 2NO2

SO3 + H2O = H2SO4

44
Q

How is NO2 a catalyst

A

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
Q

How are catalytic converters used to reduce acid rain/ the amount of NO which speeds up the producing of acid rain

A

2CO + 2NO = 2CO2 + N2

Platinum hot catalyst in cars

46
Q

Standard enthalpy change of atomisation

A

The standard enthalpy change when ONE mole of gaseous atoms is formed from its elements under standard condition.

47
Q

Standard enthalpy change of neutralisation

A

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
Q

Standard enthalpy change of reaction

A

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
Q

Standard enthalpy change of solution

A

the enthalpy change when one mole of solute is dissolved in a solvent to form an infinitely dilute solution under standard conditions

50
Q

Standard enthalpy change of hydration of an anhydrous salt

A

The enthalpy change when one mole of a hydrated salt is formed from 1 mole of the anhydrous salt under standard condition

51
Q

Homogeneous Catalyst

A

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
Q

Electron Configuration for Cu

A

[Ar] 3d10 4s1
Rather than [Ar] 3d9 4s2
Extra stability of fully d orbitals

53
Q

Electron Configuration for Cu+

A

[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
Q

Electorn Configuration for Cu2+

A

[Ar] 3d9

9 should be smaller and above the d

55
Q

Electron Configuration for Cr

A

[Ar] 3d5 4s1

Rather than [Ar] 3d4 4s2

56
Q

Electron Configuration for Cr2+

A

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
Q

Electron Configuration for Cr3+

A

1s2 2s2 2p6 3s2 3p6 3d3

58
Q

Electron Configuration for Ti

A

[Ar] 3d2 4s2

GENERALLY electrons fill up from the 4s orbital and then start to fill up 3d orbitals

59
Q

Electron Configuration for Fe

A

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
Q

Electron Configuration for Fe2+

A

1s2 2s2 2p6 3s2 3p6 3d6

61
Q

Electron Configuration for Fe3+

A

1s2 2s2 2sp6 3s2 3p6 3d5

62
Q

Trend in Thermal Decomposition of Nitrates and Carbonates

A

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
Q

pH of Period 3 Chlorides with water

A

NaCl 7 MgCl2 6.5 Al2Cl6 3 SiCl4 2 PCl5 2 SCl2 2

64
Q

Thermal Decompostion of calcium nitrate

A

Calcium nitrate = Calcium oxide + nitrogen dioxide + oxygen

65
Q

Thermal Decomposition of calcium carbonate

A

Calcium carbonate = calcium oxide + carbon dioxide

66
Q

Trend in thermal stability of hydrogen halides

A

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
Q

Trend in displacement reactions with halogen

A

The more reactive halogen displaces a less reactive halogen

68
Q

Why Cl2 displaces Br in NaBr

A

Chlorine atoms are more electronegative than Bromine tom so have a stronger tendency to form negatively charged ions.

69
Q

Use for cyclohexane with respect to Halogens

A

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
Q

How diols are made from alkenes

A

Alkene + WATER + [O] = Diol

Cold dilute Manganate solution

eg ethene + H2O + [O] = ethane- 1,2 - diol

71
Q

Alcohol and Sodium Metal

Ethanol and Sodium

A

Sodium Ethoxide/ Alkoxide + H2 gas

Similar to sodium and water reaction

72
Q

Allotrope Definition

A

Different crystalline or molecular FORMS that exist of the an element

73
Q

Colour of Group 2 Flames when heated in O2

Magnesium and Calcium

A

Calcium flame. Brick-red

Magnesium flame. Bright white flame

74
Q

Colour of flame when Strontium and Barium are heated in O2

A

Strontium scarlet red flame

Barium green flame

75
Q

Colour of Group 2 Metal Oxides when heated in O2

A

White solid White oxide

76
Q

Explain the trend in reactivity of Group 2 Metals with O2

A

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
Q

Trend in reactivity of Group 2 Metals with H2O

A

As you go down the group, the reactivity with water increase and gets more vigorous

78
Q

Trend in reactivity of Group 2 Metal oxides with water to form a hydroxide

A

As you go down the group, the reactivity of group 2 metal oxides with water increase and gets more vigorous

79
Q

Reactivity of Period 3 when heated with O2

A 
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
Q

Observations when Period 3 is heated with O2

A

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
Q

Reactivity of Period 3 with Chlorides

A

Na Mg Al all react vigorously
Si reacts slowly to form SiCl4
P reacts slowly to form PCl5

82
Q

Use for CaCO3 and CaOH2

A

Neutralise Soil

83
Q

Use for CaCO3

A

Cement

84
Q

What reacts with 2,4 -DNPH

A

The carbonyl group of only aldehydes and ketones nothing else

85
Q

Explain how fertilisers cause harm to animal and plant life

A

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
Q

Vapour Pressure and high vapour pressure and low vapour pressure

A

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
Q

What 3 factors that increase vapour pressure

A

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
Q

Boiling Point in relation to vapour pressure

A

The temperature at which the vapour pressure is equal to the atmospheric pressure is the boiling point of the liquid

89
Q

Colour change when Cr2O72- is reduced or when it oxidises something

A

Orange to Green

90
Q

Groups that react with iodine and aqueous NaOH

A

CH3CO group with aldehyde and ketones. Methyl ketones. Only ethanal reacts. CH3CHOH. Secondary Alcohol group. Only ethanol reacts.

91
Q

Avogadro’s hypothesis

A

At room temperature and pressure, one mole of any gas has a volume of 24dm3

92
Q

Hydrolysis of Nitriles with H2O

A

CH3CN to CH3CONH2 to CH3COONH4 very slow

93
Q

Hydrolysis of Nitriles with Acid

A

CH3CH + H2O + HCl = NH4Cl + CH3COOH

The carboxylic acid is a very weak acid so carboxylate ions do not form readily

94
Q

Hydrolysis of Nitriles with Alkali

A

CH3CH + H2O + NaOH = CH3COONa + NH3

Sodium carboxylate is more soluble so it produces a lots of CH3COO- ions.

95
Q

Why isotopes have the same chemical properties

A

They have the same number of electrons

96
Q

Where are electrons found in the atom

A

In the shells

97
Q

SO2 and the environment

A

Forms acid rain Kills plant life

98
Q

Properties of ideal gases

A

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
Q

Optical Isomers

A

Molecules are that non-superimposable mirror images of each other and have a central chiral carbon atom

100
Q

What do more alkyl groups do to a carbocation

A

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
Q

Problems with PTFE

A

Releases toxic gases like HCl when burnt . Nonbiodegradable

102
Q

Enhanced greenhouse effect

A

HUMAN ACTIVITY that creates a thicker layer of greenhouse gases and has an impact on climate change

103
Q

Problems with CFCs

A

Contribute to ozone depletion. Greenhouse gas that warms contributes to global warming and climate change.

104
Q

Substition of Alcohol with SOCl2

A

alcohol + SOCl2 = SO2 + HCl + Chloroalkane

105
Q

Reduction of carboxylic acids to alcohol and catalysts

A

CH3COOH + 4[H] = CH3CH2OH + H2O
Aqueous alkali NaBH4
LiAlH4 in dry ether

106
Q

Use for MgOH2 or MgO

A

Antacids

Chemistry Conditions/reactions (1 decks)

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