PAPER 1 CONTENT

reactivity series

Potassium

Sodium

Calcium

Magnesium

Aluminium

Carbon

Zinc

Iron

Tin

Lead

Hydrogen

Copper

Silver

Gold

Platinum

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change In terms of oxygen In terms of hydrogen In terms of electrons

Oxidation Gaining oxygen Losing hydrogen Loss of electrons

(OIL)

Reduction Losing oxygen Gaining hydrogen Gain of electrons

(RIG)

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Acid used Second part of salts name

Hydrochloric acid Chloride

Sulfuric acid sulfate

Nitric acid nitrate

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Group 7

• Reaction decreases going down the group

• All halogens have 7 electrons in their highest occupied energy levels

• Form covalent bonds by sharing electrons with other non- metals

• Non metallic elements

• Poor conductors of electricity and thermal energy

• Form ionic compounds with metals

• Halide ions charge -1

• A more reactive halogen is able to displace a less reactive H from aq solution

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Group 1

• All soluble in water, colourless solution with high ph. turns purple

• Form +ve ions with a charge of 1+ in reactions- ionic compounds

• Usually white or colourless crystals that dissolve in water produce colourless solutions

• React with water to produce hydrogen gas

• Low densities

• Very reactive metals

• Low melting and boiling points that decrease going down the group

• React quickly with O2 in the air------ layer of oxide forms on the surface of the metal.

A solution forms when a solute dissolve in a solvent. The concentration of a solution is a measure of how 'crowded' the solute particles are. The more concentrated the solution, the more particles it contains in a given volume.

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Calculating concentration

The concentration of a solution can be calculated using:

• the mass of dissolved solute in grams, g

• the volume of solution (or solvent) in cubic decimetres, dm3

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Worked example

8 g of sodium hydroxide is dissolved in 2 dm3 of water. Calculate the concentration of the sodium hydroxide solution formed.

concentration = mass of solute in g volume in dm3

concentration = 8 g 2 dm3

concentration = 4 g/dm3

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covalent bonding

covalent bonding is shared pair of electrons between atoms

covalent bonds occur in non- metallic elements

atoms are shared -complete outer shell

covalent bonds are very strong

negative electrons in a sea of positive charge

ionic bonding

ions are formed when atoms gain or lose electrons giving them an overall charge.

Ions have a complete outer shell of electrons

Ionic bonding involves a transfer of electrons from metal to non-metal atoms

The metal atoms lose electrons to become +ve charged

The non-metals gain electrons to become -ve charged