CHEM 1

Frage	Antworten
First Ionisation Energy equation	X(g)>>>>X+(g) +e-
Mass Spectrometer stages	Vapourise Ionise Accelerate Deflect Detect
Atomic Radius ACROSS	DECREASES Nuclear charge increases but electrons are added to the same energy level, therefore, greater EFA between nucleus and outermost electrons
Atomic Radius DOWN	INCREASES Electrons are added to different energy levels further from the nucleus, reducing EFA and shielding of charge also increases
First Ionisation Energy DOWN	DECREASES
First Ionisation Energy ACROSS	INCREASES GENERALLY
First Ionisation Energy blips	Electrons in higher energy subshells OR Spin pair repulsion between paired negative electrons
Relative mass of an electron	1/1840
Moles in solution	Moles= volume x concentration
Moles in solid	Moles = mass / mr
Ideal Gas Equation	pV = nRT p in pa v in m^3 t in K
Degrees to Kelvin	+273
Empirical formula	% or mass / by Ar / by smallest use ratio
Empirical to molecular	n = mr of molecule / mr of empirical empirical x n = molecular formula
Atom economy	mass of product / mass of all reactants x 100
Yield	actual mass / theoretical mass x 100
Ionic bond	Strong EFA between oppositely charged ions
Ionic are soluble in water	Polar solvent molecules attract ions out of the lattice into solution
Metallic bond	Strong EFA between positive metal ions and delocalised electrons
Covalent bond	A shared pair of electrons between two atoms
Giant covalent structures	Silicon dioxide Graphite Diamond
Dative covalent bond	A covalent bond where both of the shared electrons are donated from one of the atoms
Van der Waal's depends on...	Size of molecules - more electrons means larger dipoles which are harder to overcome which INCREASES mbp Branching - more branching decreases surface contact area and vdw which DECREASES mbp
Hydrogen bond	H bonded to an O, N or F with at least one lone pair
2 Bonding Pairs	Linear 180°
3 Bonding Pairs	Trigonal Planar 120°
4 Bonding Pairs	Tetrahedral 109.5°
5 Bonding Pairs	Trigonal Bipyramidal 120° and 90°
6 Bonding Pairs	Octahedral 90°
1 Lone Pair 2 Bonding Pairs	Angular 117.5°
1 Lone Pair 3 Bonding Pairs	Pyramidal 107°
2 Lone Pairs 2 Bonding Pairs	Bent 104.5°
2 Lone Pairs 4 Bonding Pairs	Square Planar 90°
Structural Isomers	Chain Isomerism Position Isomerism Functional Group Isomerism
Fractional Distillation	Separates alkanes into chain lengths by bp HOT BOTTOM and COLD TOP LONG BOTTOM and SHORT TOP
LPG	Camping gas
Naptha	Petrochemicals
Kerosene	Jet fuel
Diesel	Central heating fuel
Mineral oil	Lubricant
Fuel oil	Power station fuel
Wax, grease	Candles
Bitumen	Road surfacing
What is Cracking?	Breaking C-C alkane bonds to form an alk-1-ene and shorter chained alkane
Thermal Cracking conditions	ONE ALKENE PRODUCT 1000K 7000KPa No catalyst
Catalytic Cracking	BRANCHED ALKANES (burn smoothly as fuels), CYCLOALKANES AND AROMATICS 720K Just above atmospheric pressure Zeolite catalyst
Complete alkane combustion	Alkane + Oxygen>>>> Carbon Dioxide + Water
Incomplete alkane combustion	Alkane + Oxygen >>>> Carbon Monoxide + Water Alkane + Oxygen >>>> Carbon + Water
Nitrogen Oxides	Formed as air petrol mixture sparks and explodes Nitrogen + Oxygen >>>> Nitrogen Monoxide
Catalytic Converter	PLATINUM, PALLADIUM, RHODIUM Spread thinly over ceramic honeycomb to give large surface area 2CO + 2NO >>>> N2 + 2CO2 NO + Alkane >>>> CO2 + Water + N2
Sulphur dioxide pollutant	Under UV SO2 + 1/2 O2 >>>> SO3 SO2 OR SO3 + Water >>>> Acid Rain NOT REMOVED IN CATALYTIC CONVERTER
Flue Gas Desulphurisation	Use Calcium Carbonate (limestone) to neutralise SO2

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