Chemistry Chemical Reactions Flashcards
Group 1 metal nitrate heated
—> metal nitrile + oxygen
2MNO3(s) —> 2MNO2(s) + O2(g)
Group 1 metal carbonate heated
Does not undergo thermal decomposition as too thermally stable. (Except lithium carbonate)
Group 2 metal oxide + water
—> metal hydroxide
MO(s) + H2O —> M(OH)2
Group 2 metal oxide + dilute acid
—> salt
MO(s) + 2HCl(aq) —> MCl2(aq) + H2O(l)
Group 2 metal hydroxide + water
—> aqueous metal hydroxide
M(OH)2(s) ——> M(OH)2(aq)
—————H2O——————
Group 2 metal hydroxide + dilute acid
—> salt
M(OH)2(aq) + 2HCl(aq) —> MCl2(aq) + 2H2O(l)
Group 2 metal + water
—> metal hydroxide + hydrogen
M(s) + 2H2O(l) —> M(OH)2(aq) + H2(g)
Group 2 metal + oxygen
—> metal oxide ( white ppt )
2M(s) + O2(g) —> 2MO(s)
Group 2 metal + chlorine
—> metal chloride (white precipitate)
M(s) + Cl2(g) —> MCl2(s)
Decomposition of group 2 metal carbonate
—> metal oxide + carbon dioxide
MCO3(s) —> MO(s) + CO2(g)
Decomposition of lithium carbonate
Li2CO3(s) —> Li2O(s) + CO2(g)
Decomposition of group 2 nitrates
—> metal oxide + nitrogen dioxide + oxygen
2M(NO3)2(s) —> 2MO(s) + 4NO2(g) + O2(g)
Decomposition of lithium nitrate
4LiNO3(s) —> 2Li2O(s) + 4NO2(g) + O2
What is nitrogen dioxide
A brown toxic gas
REDOX: Halogen + G1
—> halide salt
2M(s) + X2(s) —> 2MX(s)
—0——0———- +1– -1–
REDOX: Halogen + G2
—> halide salt
M(s) + X2(s) —> MX2(s)
-0——-0———+2– -1——
Hydrogen halide + water
HX(g) ——> X-(aq) + H+(aq)
Properties of HX(g)
Acidic gases—> turn damp blue litmus paper red
Hydrogen halide + ammonia
—> ammonium halide (white fumes)
HX(g) + NH3(g) —> NH4X(g)
Chlorine + cold dilute alkali
—> sodium chlorate (I)- bleach + sodium chloride + Water
Cl2 + 2NaOH(aq) —> NaOCl + NaCl + H2O
Chlorine + hot dilute alkali
—> sodium chlorate (V) + sodium chloride + water
3Cl2 + 6NaOH —> NaClO3 + 5NaCl + 3H2O
Chlorine + water
—> hydrochloric acid + hypochlorous acid
Cl2(g) + H2O(l) <=> HCl(aq) + HClO(aq)
HClO + water
—> chlorate (I) ion (kills bacteria)
HClO + H2O <=> ClO- + H3O+
Free radical substitution of methane overall equation
CH4 + Cl2 —(UV)—> CH3Cl + HCl
Free radical substitution of methane: initiation
Cl2 —-(UV)—> 2Cl*
Free radical substitution of methane: propagation
CH4 + Cl* —> *CH3 + HCl
CH3 + Cl2 —> CH3Cl + Cl
Free radical substitution of methane: termination
Cl* + Cl* —> Cl2
*CH3 + *CH3 —> C2H6
CH3 + Cl —> CH3Cl
Complete combustion of alkanes ( ethane )
2C2H6(g) + 7O2(g) —> 4CO2(g) + 6H2O(g)
Incomplete combustion of alkanes (ethane)
C2H6(g) + 2O2(g) —> CO(g) + C(s) + 3H2O(g)
Main reactions alkenes undergo
Electrophilic addition
Alkene + hydrogen
(Products, conditions, reaction)
—> alkane
Nickel catalyst, 150°C
H2C=CH2 + H2(g) —-> CH3CH3
Alkene + halogen
—> dihalogenoalkane
H2C=CH2 + X2 —> CH2XCH2X
Which dihaloalkane is colourless
Dibromoalkane
Alkene + hydrogen halide
—> haloalkane
H2C=CHCH3 + HX —> CH3CHXCH3
Steam hydration of alkenes
(Product, conditions, reaction)
Alkene + steam —> alcohol
- Phosphoric (V) acid catalyst, 300°C, 60atm
H2C=CH2(g) + H2O(g) <=> CH3CH2OH
Oxidation of alkenes
(Product, conditions, reaction, observation)
—> diol
- acidified potassium manganate (VII)
H2C=CH2 —(H+/MnO4-)—> CH2(OH)CH2(OH) ethane-1,2-diol
Purple- colourless solution
Elimination of haloalkanes
(Products, conditions, reaction)
Haloalkane + OH- —> alkene
- Reflux, warm ethanolic KOH
RX + KOH —> RC=C + H2O + KX
What does the OH- act as in elimination of haloalkanes
Acts as a base, removing H+ from the haloalkane
Main reaction of haloalkanes
Nucleophilic substitution
Haloalkane + water
—> alcohol
RX + H2O —> ROH + H+ + X-
Haloalkane + OH- (SN)
(Conditions, reaction, products)
—> alcohol
- reflux, warm KOH(aq)
RX + KOH —> ROH + KX
Haloalkane + CN-
(Products, reaction, conditions, use)
—> nitrile
- reflux, KCN in ethanol (ethanolic)
RX + CN- —> R-C=-N + X-
- used to increase length of the carbon chain
Haloalkane + ammonia
(Products, conditions, reaction, observation)
—> amines
- warm with excess, ethanolic ammonia
RX + NH3 —> R-NH2 + NH4+
- R-NH2 has a fish smell
Combustion of alcohols (ethanol)
C2H5OH + 3O2 —> 2CO2 + 3H2O
Oxidation of primary alcohol to final product
(Reaction, products, conditions, observation)
P1—(distillation)—> aldehyde
P1—(reflux)—> carboxylic acid
ROH + 2[O] —> RCOOH + H2O
[O] = acidified potassium dichromate
Colour change orange - green
Oxidation of secondary alcohol
—> ketone
ROHR + [O] —> RCO + H2O
[O] = acidified potassium dichromate
Colour change orange-green
Acyl chloride + water
—> carboxylic acid + HCl(g)
CH3COCl + H2O —> CH3COOH + HCl
Acyl chloride + alcohol
—> ester + hydrogen chloride gas
CH3COCl + CH3CH2OH —> CH3C=OOCH2CH3 + HCl
Acyl chloride + amine (methylamine)
—> n-methylethanamide + Hydrogen chloride gas
CH3COCl + CH3NH2 —> CH3C=ONHCH3 + HCl
Acyl chloride + ammonia
—> acylamide + Ammonium chloride
CH3COCl + NH3 —> CH3C=ONH2 + HCl
NH3 + HCl —> NH4Cl
Overall: CH3COCl + 2NH3 —> CH3CONH2 + NH4Cl
——————————————ethanamide————
Main reaction of arenes
Electrophilic substitution
Formation of nitrobenzene conditions + type of reaction
- concentrated H2SO4 (catalyst)
- concentrated HNO3
- <50°C
- Electrophilic substitution
Adding a halogen to a benzene
(Type of reaction, conditions + formation of catalyst)
- electrophilic substitution
- halogen (e.g Br2)
- halogen carrier (FeBr3/AlCl3)
AlCl3 + Cl2 —> AlCl4- + Cl+
Acylation of a benzene conditions + type of reaction
- Acyl chloride
- AlCl3
- electrophillic substitution
Alkylation of benzene conditions + type of reaction
- electrophillic substitution
- AlCl3
- RCl (with methyl or ethyl group etc..)
Carbonyl + HCN
Products, conditions, type of reaction
—> hydroxynitrile
- HCN in the presence of KCN
RCOR + HCN —> RCOHCNR
Reduction of nitrobenzene
(Products, conditions)
—> phenylamine (C6H5NH2)
1. Sn, Conc HCl, reflux
2. OH-
Bromination of phenol (products, reactant)
- 3/2 Br2
- 2,4,6-tribromophenol
Hydrolysis of nitriles
(Products, conditions, reaction)
—> carboxylic acid + ammonium chloride
- reflux with dilute HCl, distil off COOH
CH3CN + 2H2O + HCl —> CH3COOH + NH4Cl
Carboxylic acid + aqueous base
—> salt + water
CH3COOH +NaOH —> CH3COONa + H2O
Carboxylic acid + carbonate/hydrogen carbonate
—> salt + water + carbon dioxide
2CH3COOH + Na2CO3(s) —> 2CH3COONa(aq) + CO2 + H2O
CH3COOH + NaHCO3(s) —> CH3COONa(aq) + CO2 + H2O
