Chemistry As reactions

ideal gas equation

pV\=nTR

1 atm

101325 Pa

m^3

1000 dm^3

273 K

0 C

R

8.314

moles 2

concentration x volume

moles 1

mass / mr

solid

s

solid

s

aqueous solution

aq

gas

g

moles 3

v/24

percentage yield

actual amount in mole/theoretical mount in mole x100

Atom economy

molecular mass of desired product/molecular mass of all products x100

sulfuric acid

H2SO4

hydrochloric acid

HCl

nitric acid

HNO3

sodium hydroxide

NaOH

Potassium hydroxide

KOH

ammonia

NH3

Neutralisation reaction

H+ + OH- \= H2O

Dissolved ammonia

NH3 + H2O \= NH4+ + OH-

acid + carbonate

salt + water + carbon dioxide

acid + metal oxides

salt + water

acid + alkali

salt + water

acid + metal

salt + hydrogen

ammonia and nitric acid NH3 + HNO3

NH4NO3

methyl orange in acid

red

methyl orange in alkali

yellow

methyl orange end point

orange

Phenolphthalein in acid

Colourless

Phenolphthalein in alkali

pink

Phenolphalein end point

pale pink

bromothymol blue in acid

yellow

bromothymol blue in alkali

blue

bromothymol blue end point

green

oxidation number uncombined element

0

oxidation combined oxygen

-2

oxidation combined oxygen in peroxides

-1

oxidation combined hydrogen

+1

oxidation combined hydrogen in metal hydrides

-1

simple ion

charge on ion

combined fluorine

-1

electrons in first shell

2

electrons in second shell

8

electrons in third shell

18

electrons in fourth shell

32

electrons in an orbital

2

number of s orbitals

1

number of p orbitals

3

number of d orbitals

5

number of f orbitals

7

giant ionic lattice

high mp and bp, conduct electricity when molten or dissolved, soluble in polar solvents

simple molecular

low mp and bp, dont conduct electricity, soluble in non-polar substances

giant covalent lattice

high mp and bp, dont conduct electricity, soluble in polar and non-polar substances

linear

2 bonding pairs 0 lone pairs 180 CO2

non linear

2 bonding pairs 2 lone pairs 104.5 H20

trigonal planar

3 bonding pairs 0 lone pairs 120 BF3

trigonal pyramidal

3 bonding pairs 0 lone pairs 107 NH3

Tetrahedral

4 bonding pairs 0 lone pairs 109.5 CH4

Trigonal Bypyramidal

5 bonding pairs 0 lone pairs 120 90 PCl5

Octahedral

6 bonding pairs 0 lone pairs 90 SF6

Giant metallic lattice

high mp and bp, conduct electricity, malleable and ductile

1st oxidation of G2 elements

M -\> M+ + e-

2nd oxidation of G2 elements

M+ -\> M2+ + e-

G2 and oxygen

2M + O2 -\> 2MO

G2 and water

M + 2H2O -\> M(OH)2 + H2

G2 and dilute acids - HCl

M + 2HCl -\> MCl2 + H2

neutralising acidic soils

Ca(OH)2

Indigestion remedies

Mg(OH)2

Building and construction

CaCO3

Halogen in water
Cl2
Br2
I2

pale green
orange
brown

Halogen in cyclohexane

pale green
orange
violet

Water purification reaction

Cl2 + H2O -\> HClO + HCl

Bleach formation equation

Cl2 + 2NaOH -\> NaCl + NaClO + H2O

carbonate ions CO3 2- test

add strong acid, collect gas, pass through limewater, turns limewater cloudy

sulfate ions SO4 2- test

Add dilute HCl, add BaSO4, white precipitate formed

Halide ions test

dissolve in water, add aqueous silver nitrate, precipitate formed, add aqueous ammonia dilute then concentrated

halide ions result

Cl2 - white, soluble in dilute
Br2 - cream, soluble in concentrated
I2 - yellow, insoluble

silver and chloride reaction

Ag+ + Cl\- -\> AgCl

Ammonium ions test NH4 +

Add sodium hydroxide and warm, test gas with red litmus paper, paper turns blue and distinctive smell

Enthalpy change

reactant - product

exothermic

making -

endothermic

breaking +

standard conditions

100 kPa
273 K

Enthalpy change of reaction

The energy change associated with a given reaction

enthalpy change of formation

the enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions

enthalpy change of combustion

The energy change that takes place when 1 mole of a substance is completely combusted

enthalpy change of neutralisation

The energy change associated with the formation of 1 mole of water from a neutralisation reaction.

energy equation

q \= mct

homogeneous catalyst

same phase as reactants

Hetrogeneous catalyst

different phase as reactants

Kc

\[products]/[reactants]

Homologous series

A series of organic compounds with the same functional group but with each successive member differing by CH2

aliphatic hydrocarbon

hydrocarbon consisting of a linear chain of carbon atoms

Alicyclic hydrocarbon

A hydrocarbon with carbon atoms joined together in a ring structure.

aromatic hydrocarbon

Contain a benzene ring

functional group

group of atoms responsible for the characteristic chemical reactions of a compound

structural isomers

same molecular formula but a different structural formula

sterioisomers

Compounds with the same structural formula but with a different arrangement of the atoms in space.