paper 1

They have weak intermolecular forces. these do not require very much to overcome.

they have no free electrons or ions to carry a charge through a substance.

they have many strong electrostatic attractions between oppositly charged ions. this requires a lot of energy to overcome.

when molten or dissolved. this is because ions are free to move and carry charge.

many strong electrostatic attraction between positively charged ions and a sea of delocalised electrons requies a lot of energy to overcome.

They conduct electricity because electrons in a sea of delocalised ions are free to move and carry charge through the structure.

beause elections in the sea of delocalised electrons are free to move.

pure metals are malleable. if we introduced another atom/ion that's a different size. the layered structure is disrupted meaning that the layers can no longer slide over each other.

is made of layers of carbon atoms which has weak bonds between they layers. the layers can slide over each other easily, this gives graphite the property of being slippery.

there are many strong covalent bonds. which requires a lot of wnergy to overcome.

each carbon atom has three bonds, this means there is a spare electron per carbon atom. this can carry a charge through the structure.

diamonds are used in cutting tool as its strong and hard - interlocking structure of carbon atom is bonded to each other. doesn't conduct electricity- every carbon atom is bonded to each other. so it has no free electrons to move and carry charge. has ahigh melting point- there are many strong covalent bonds which requires a lot of energy to overcome.

1) cations (+) are discharged at the calthode (-) where they gain electrons. 2) Anions (-) are dishcharged at the anode (+) where they lose electrons 3) If you have a solution (aq) the electrolyte contains H+ ions and OH- ions as well as the elements in a formula 4) In a solution, the least reactive postive ion is the one discharged that the electrode 5) In a solution if you have a halide ion (group 7) it will be the one discharged at the anode 6) if you have a solution and no halide ion, oxygen will be formed from the OH- ion.

2Cl‐ – 2e‐ —> Cl 2 or Na+ + e- —> Na

remains of plankton from million of years ago

a mixture of different hydrocarbons

a compound made of hydrogen and carbon atoms alone

at the top it is cold = flamable, low bioling point, volitile

it is hot = long hydrocarbons, high boiling point, viscous, not flammable

incomplete compution

it is toxic

compustion

causes global warm exaple increasing sea levels

buring coal with sulphur impuritice

it causes acid rain

inside high temperature of a car engines (diesel)

causes acid rain, corrosin

incomplete combination

it causes global dimming

Methane, Ethane, Propane and Butane

high temperature, catalyst = thermal decomposition

have a pH scale is red/ orange. the pH is between 1-6. All the acids contain a H+ ion.

HCl, HNO3, H2SO4

apart of group 1- Alkali metals. Have a pH scale of blue/ purple. pH 8-14. All alkalis conatin an OH- ion

NaOH, NH4OH

a strong acids can fully dissociate in water and weaker acids partically dissociate in water

• hydrochloric acid will always make something chloride. • hydrochloric acid —> _____ Chloride. • Sulfuric acid —> _____ Suphate. • nitric acid —> _____ nitrate.

•Metal + acid —> slat + hydrogen (not a neutralisation) • metal carbonate + acid —> salt + water + carbon dioxide • metal oxide/ hydroxide + acid —> salt + water

water = neutralisation reaction

• add alkali to acid drop by drop till neutral - test with Universal indicator paper. • heat gently till crystalising • Leave to crystallise • flture, wash and dry

•add base to acid until in exess. • filter the exess. • heat gently until cystalstaion • leave to crystallise • filter, wash and dry.

• electrolysis • temp change in solutions • making salts

a substance containing one type of atom

a substance containing two or more different types of atoms chemically bonded

consists of a differnet substances NOT chemically bonded

mass = 1 and charge = +1

mass = 1 and charge =0

mass = 0 and change = -1

the same element that has different numbers of neutrons but the same number of electrons