Chemistry Flashcards by A D

Relative Formula Mass (Mr)

sum of relative masses of atoms in a compound

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Relative Atomic Mass (Ar)

average mass of one atom of an element

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Isotopes

atoms of the same element that contain the same number of protons but different numbers of neutrons
have different mass number
have same atomic number

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Molecular Formula

gives the actual numbers of atoms of each element in a molecule

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Concentration

amount of solute in a certain volume of solution
g/dm^3
mass (g) / volume (dm^3)

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Empirical Formula

gives the smallest whole number ratio of atoms of each element in a compound

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Mole

Mass / Mr

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Avogadro’s Number

6.02 x 10^23

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Acid

A substance with a pH lower than 7 and produces H+ ions when dissolved in water

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Limiting Reactant

Reactant used up in a reaction

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Alkali

A soluble base that releases OH- ions when dissolved in water

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Base

A substance with a pH greater than 7 which only produces a salt and water during neutralisation

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Indicator

A substance with changes colour when added to an acidic or alkaline solution

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Neutral Solution

A solution that is neither acidic nor alkaline and has a pH of 7

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Hydrocarbon

Compound made of hydrogen and carbon only

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Crude oil

A finite resource made from plant and animal remains from millions of years ago found in rocks
A complex mixture of different compounds including hydrocarbons

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Deposition

When a gas becomes a solid without becoming a liquid

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Sublimation

When a solid becomes a gas without becoming a liquid

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Formulation

Useful mixtures composed of specific amounts of each compound

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% of nitrogen in early atmosphere

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% of nitrogen in current atmosphere

78%

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% of oxygen in early atmosphere

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% of oxygen in current atmosphere

21%

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% of carbon dioxide in early atmosphere

70%

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% of carbon dioxide in current atmosphere

0.04%

% of water vapour in early atmosphere

10%

% of water vapour in current atmosphere

0.06%

% of methane in early atmosphere

20%

% of methane in current atmosphere

Alkane Formula

Cn H2n+2

Methane

CH4

Ethane

C2H6

Propane

C3H8

Butane

C4H10

Alkene Formula

Cn H2n

Ethene

C2H4

Propene

C3H6

But-1-ene

C4H8

But-2-ene

C4H8

What is gas used for?

heating and cooking

What is petrol used for?

fuel for cars

What is kerosene used for?

fuel for aircrafts

What is diesel oil used for?

fuel for cars and trains

What is fuel oil used for?

fuel for ships

What is bitumen used for?

road and roof surfacing

All common ammonium salts

soluble in water

All common potassium salts

soluble in water

Most sulfates

soluble in water

Lead chloride

INsoluble in water

Silver chloride

INsoluble in water

Most chlorides

soluble in water

Sodium carbonate

soluble in water

Calcium sulfate

INsoluble in water

Barium sulfate

INsoluble in water

Lead sulfate

INsoluble in water

Sodium hydroxide

soluble in water

Most carbonates

INsoluble in water

potassium carbonate

soluble in water

ammonium carbonate

soluble in water

Sodium carbonate

soluble in water

Most hydroxides

INsoluble in water

ammonium hydroxide

soluble in water

potassium hydroxide

soluble in water

All common sodium salts

soluble in water

1 mole contains ____ particles

6.02 x 10^23

NO of molecules =

moles x 6.02 x 10^23

NO of atoms =

NO of molecules x NO of atoms in a molecule

Mass (g) of 1 mole =

(Ar) relative atomic mass of element

Percentage mass of element in compound =

Mr of element/Mr of compound x 100

acid + metal

salt + hydrogen

acid + metal oxide

salt + water

acid + metal hydroxide

salt + water

acid + metal carbonate

salt + water + carbon dioxide

Energy change =

Bonds broken - Bonds formed

Exothermic

A reaction that transfers energy to the surroundings

Endothermic

A reaction that takes in energy from the surroundings

Rate of reaction =

(amount of reactants used up / products produced) / time taken

Physical properties of fluorine

Yellow gas

Physical properties of chlorine

Poisonous green gas

Physical properties of bromine

Poisonous red-brown liquid, gives off orange vapour

Physical properties of iodine

Black solid, gives off purple vapour

Reaction of lithium with water

Fizzes on surface of water

Reaction of sodium with water

Fizzes, melts, yellow flame

Reaction of potassium with water

Fizzes, melts, purple flame

Retention Factor (Rf Value) =

distance travelled by substance / distance travelled by solvent

Reaction of metal with steam

Metal + steam → metal oxide + hydrogen

Reaction of metal with cold water

Metal + water → metal hydroxide + hydrogen

Neutralisation Reaction

Metal + acid → salt + hydrogen

Oxidation Reaction

Metal + oxygen → metal oxide

Ore

a rock that contains a high enough amount of metal to make it worthwhile extracting

Carbon reduction formula

Metal oxide + carbon –heat—> metal + carbon monoxide (may be CO2 if indicated)

Electrolysis

The splitting of ionic substances using electricity

Electrolyte

The liquid/solution that conducts electricity

Electrodes

Solids placed in the electrolyte that conduct electricity

Anode

positive electrode

Cathode

negative electrode

Malleable

Can be shaped easily without breaking

Ductile

Can be easily drawn into wires

Alloy

Mixture of two or more elements, where at least one is a metal

Bronze

Copper + Tin alloy Medals, decorative ornaments, statues

Brass

Copper + Zinc alloy low friction situations (eg door hinges)

Magnalium

Magnesium + aluminium alloy 5% magnesium: stronger, lighter and more resistant to corrosion than aluminium Car and aeroplane parts 50% magnesium: highly reactive, burns brightly and more stable than magnesium Fireworks

Gold alloys

Gold + zinc, copper, silver… alloy Jewellery (pure gold too soft and malleable)

Steel

Iron + carbon [+ chromium + nickel] alloys Low carbon steels: malleable Sheeting High carbon steels: hard Cutting tools Stainless steels [+ chromium + nickel]: resistant to corrosion Cutlery

Atom economy

Mr of desired product / Sum of Mr of all products x 100%

Percentage yield

Actual yield / Theoretical yield x 100%

Concentration

(g/dm^3) mass (g) / volume (dm^3)

Concentration

(mol/dm^3) mole (mol) / volume (dm^3)

Gas volume

dm^3 moles (mol) x molar volume (dm^/mol) [24 at RTP]

mol/dm^3 →g/dm^3

x Mr

g/dm^3 →mol/dm^3

/ Mr