Mole
1 _____ of a substance is 6.022�10�� atoms of that substance.
g/mol
The unit used to measure molar mass.
Molar Mass
The mass of an entire molecule.
Relative Atomic Mass
The mass of an individual atom.
Moles
_____ = Mass � Molar Mass
Conserved
Mass is _____ during a reaction.
Reactants
The substance(s) on the left of the arrow.
Products
The substance(s) on the right of the arrow.
Thermal Decomposition
The breaking down of a substance under heat.
Empirical Formula
The simplest way of writing a ratio of each type of atom in a molecule.
Moles
The amount of _____ of each element is divided by the amount of _____ of the element least moles present in one molecule is .
2
The number of hydrogen atoms in the empirical formula for glucose.
Percentage Mass
_____ _____ of Element = Total mass of Element in Compound � Formula Mass of Compound) x 100
Molar Mass
_____ _____ = Mass � Moles
Concentration
The amount of solute in 1dm� of solution.
g
Concentration is measured in __/dm�
Dilute
If more solvent is added, the solution will become more _____.
Concentrated
If more solute is added, the solution will become more _____.
1000
To convert from cm� to dm�, multiply by _____.
Moles
_____ = Concentration x Volume
Volume
_____ = Moles � Concentration
GDA
_____ is the recommended amount of a nutrient which should be ingested each day.
Guideline Daily Allowance
GDA stands for _____ _____ _____.
Sodium Chloride
The scientific name for salt.
Sodium Ions
_____ _____ are mainly sourced from salt and are used in nerve impulse transfer & water balance.
Titration
The method of finding the concentration of a reactant by slowly adding a substance.
Acids
_____ have low pHs.
Alkalis
_____ have high pHs.
Alkali
A soluble base is an _____.
High
Bases have _____ pHs.
Universal Indicator
The substance which changes colour in a substance, dependent on the pH.
Litmus
_____ paper will change to blue in an alkali and red in an acid.
Phenolphthalein
_____ will be pink in an alkali and colourless in an acid.
Salt
Acid + Alkali -> _____ + Water
Hydrogen
Acid + Metal -> Salt + _____
Metal Oxide
Acid + _____ _____ -> Salt + Water
Carbon Dioxide
Acid + Metal Carbonate -> Salt + Water + _____ _____
Neutralisation
The process of adding enough alkali to acid (or vice versa) to result in a neutral substance.
Pipette
A small tube with a bulb at the top which can be pressed to form a vacuum, allowing liquids to be sucked into it.
Burette
A tall cylinder with measurements along it and a tap at the end to slowly let a liquid out.
Acid Concentration
Number of Moles of Alkali = _____ _____ x Volume in dm�
Alkali Concentration
Number of Moles of Acid � Number of Moles of Alkali = _____ _____
24
Number of Moles = Volume of Gas in dm� � __
Limiting Reactant
The substance which is used up first.
Explosion
The rapid expansion of gas.
Gas Syringe
Gas volume can be measured using a _____ _____.
Steeper
The _____ the gradient, the faster the reaction.
Reversible Reaction
A reaction in which both the forward and backward reaction occur at the same time.
Equilibrium
The state at which the rate of reaction for both the forward and backward reactions is equal.
Left
If the concentration of the reactants increase, the equilibrium will be on the _____.
Right
If the forward reaction is exothermic and the temperature is increased, the equilibrium will be on the _____.
Exothermic
A reaction which gives out more energy than it takes in is _____.
Endothermic
A reaction which takes in more energy than it gives out is _____.
Catalyst
A _____ does not change the equilibrium, instead increasing the rate of reaction for both the forward and backward reactions.
Contact Process
The series of reactions used to produce sulfuric acid.
1
Stage __ of the Contact Process is "S + O? -> SO?
2
Stage __ of the Contact Process is "2SO? + O? ? 2SO?
3
Stage __ of the Contact Process is "SO? + H? -> H?SO?
450
Stage 2 of the Contact Process is carried out at approximately __�C
Sulfuric Acid
The name for H?SO?
Vinegar
_____ is a good example of a commonly used weak acid.
Battery Acid
_____ _____ is a good example of a commonly used strong acid.
Lower
Strong acids have a _____ pH than weak acids.
Strong
_____ Acid -> Hydrogen Ions + Other Ions
Weak
_____ Acid ? Hydrogen Ions + Other Ions
Water
When an acid or an alkali is added to _____, it ionises.
H
Acids contain __+ ions.
OH
Alkalis contain __- ions.
Stronger
_____ acids contain more H+ ions.
Precipitate
A solid substance formed when one liquid is poured into another liquid.
Ionic Lattices
Compounds containing metal and non-metal ions form _____ _____.
Spectator Ions
_____ _____ are left out from an equation as they do not change through the reaction.
Silver Nitrate
The substance used to test for halide ions.
Barium Chloride
The substance used to test for sulphate ions.
Evaporating
Solid salts can be separated from a solvent by _____ the solvent.