States of Matter

Draw a particles (circles) diagram

Heating and cooling curvesLabel the graph with the state at each point.

Why does the temperature not change when something changes state _______________________ _______________________ _______________________

DiffusionDefine diffusion __________________________________________ _______________________ ________________________________

The smoke forms nearer

to the ammonia end –

why?.________________

___________________-PressureDefine pressure __________________________________________ _______________________ ________________________________

State 4 ways to increase pressure________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________

Separation techniques – draw a labelled diagram for the following and give an example of each filtering Chromatography

Distillation Fractional distillation

Crystallisation Purity testing

Define Solvent _________________________________________ Define Solute _________________________________________Define insoluble _________________________________________Define dissolve_________________________________________Define solution_________________________________________

Chemical reactions Give 4 signs that a chemical reaction has taken place•______________________________________________•______________________________________________•______________________________________________•______________________________________________

Element/compound or mixtureCan contain any number of substances in a different ratio A/B/C/D Element/compound or mixtureContains one type of atom A/B/C/D Element/compound or mixtureContains more than one type of atom chemically bonded A/B/C/D lement/compound or mixture

Metallic/Ionic/Covalent Bonding

Ionic Bonding – Draw the ions for the followingCovalent Bonding – Draw on the electrons to show bonding

HydrogenChlorine

WaterOxygen

Methane (CH4)

Carbon dioxide (CO2)

Diamond Graphite

Use

Bonding(diagram)

Properties

Subatomic particle

Mass Charge

+1

-1

0

Match the pictures above with the words below and define the wordsElement

Compound

Mixture

Name the 3 parts of the atom.

a__________________

b__________________

c__________________

Complete the sentences with the following words. (some are red herrings!) Ionic elementsodium electron covalent chlorine chlorine sodium Na+ Na- Cl+ compoundCl-

Sodium chloride NaCl is a ____________. There are __________ bonds between the two elements _________ and _________. When these atoms bond one ____________ from the ___________ atom is donated to the _____________ atom. This results in 2 ions : _______ and _______.

ion Lost/ gained?

Number of electrons

Mg 2+ lost 2

Cl -

Li +

O 2-

Fe 3+

Complete the electron arrangement of a boron atom

Complete the electron arrangement of a boron ion

Colour on the Periodic table • non-metals • unreactive gases • alkali metals are found (very reactive)Atoms in the same group have similar properties because they have the same number of _____________ in the outer shell.The mass number is the total number of ________ and _______.The atomic number is the number of __________.

Isotopes• Isotopes are atoms of the same element with

the same/different numbers of protons. Isotopes are atoms of the same element with the same/ different numbers of electrons.

• Isotopes are atoms of the same element with the same/ different numbers of neutrons.

Alkali MetalsWhat do they look like?

______________________________________

Why are they stored under oil?

_______________________________________

Why does reactivity increase down the group?

_______________________________________

_______________________________________Write the equation for sodium with water produces sodium hydroxide and hydrogen

______________________________________

Subatomic particle

Mass Charge

+1

-1

0

Name the 3 parts of the atom.

a__________________

b__________________

c__________________

Colour on the Periodic table • non-metals • unreactive gases • alkali metals are found (very reactive)Atoms in the same group have similar properties because they have the same number of _____________ in the outer shell. The nucleon number is the total number of ________ and _______. The proton number is the number of __________which is equal to the number of ________________.

Periodic Table LabelNucleon number and Proton number (LHS)Protons neutrons Electrons (RHS)

HalogensGive two examples of halogens

______________________________________

Describe what they look like

_______________________________________

Why does reactivity decrease down the group?

_______________________________________

_____________________________________

Transition metals

What are their physical properties? _________________________ _________________________

What are their chemical properties? _________________________ _________________________

What are their uses? __________________________________________________

Moles

Atom calculations

How many atoms of carbon are in a 10 g diamond Moles = mass/RMM = 10/12= 0.833 moles 1 moles = 6.02x1023 0.833 x 6.02x1023 = 5.02x1023

Q1 What mass of silicon contains 1.25x1022 silicon atoms

Q2 What mass of titanium contains 1.204x1024 atoms

Avagadro’s constant is 6.02x1023

What mass of aluminium oxide is produced when 135 g of aluminium is burned in oxygen?

2 Al + 3 O2 Al2O3

 

What mass of iodine is produced when 7.1 g of chlorine reacts with excess potassium iodide?

Cl2 + 2 KI 2 KCl + I2

Gas CalculationsWhat volume does 0.25moles of a gas occupy at rtp?1 mole occupies 24 dm3 so 0.25 moles occupies 0.25 x 24 dm3 = 6 dm3

So 0.25 moles of any gas occupies 6dm3 at rtp.

Q 3 What volume of nitrogen reacts with 10 kg of hydrogen to form ammonia?

N2(g) + 3 H2(g) ® 2 NH3(g) Q4 What volume of oxygen reacts with 510 g of ammonia? 4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6 H2O(g)

ConcentrationsSolution A contains 2.5g copper sulphate in 1dm3 of waterSolution B contains 125g copper sulphate in 0.5dm3 waterChange the mass to moles.Mr of copper sulphate is 250

Solution A : 2.5g = 0.01 moles 1dm3 there are 0.01 moles/dm3

Solution B : 125g in 0.5dm3, which is 250g in 1dm3 =1 moles/dm3 = 1M

Q5 What is the concentration of a solution containing.a) 4 moles in 2 dm3 of solutionb) 0.3 moles in 200cm3 of solution

Q6 The Mr of sodium hydroxide is 40. How many grams of sodium hydroxide are inc) 500cm3 of a molar solutiond) 25cm3 of a 0.5M solution

For each of the following compounds the Mr and the empirical formula is shown. Work out the molecular formula of each compound. 1. empirical formula = CH3 Mr = 302. empirical formula = NH3 Mr = 173. empirical formula = CH2 Mr = 984. empirical formula = CH Mr = 78Calculate the percentage of the elements shown in the following compounds: C in CO N in (NH4)2SO4

O in Al(OH)3 O in Na2CO3.10H2O

Acids and Bases Zinc reacts with oxygen. Zinc oxide is made.What are the reactants?________ ________What is the product?_____________Complete the word equation for this reaction___________+ ____________ __________ ________

2Zn + O2 2ZnOHow many Zinc and Oxygen atoms are on the left-hand side?Zn ______ 0_______How many Zinc and Oxygen atoms are on the right-hand side?Zn ______ O______Is this equation balanced? Yes/No

Acids have pHs of _____ to _____Bases (soluble alkalis) have pHs of _______ to ______.Neutral is pH _______Indicators are used to….

Complete the equation for a neutralisation reaction:Acid+ Alkali ________ + _________

Tick which of the following are real uses of neutralisation reactions. Indigestion tablets (neutralising stomach acid) In cars (neutralising battery acid) On fish and chips (vinegar is an acid) In Gardening (Neutralising acidic soils) In Lakes (Neutralising lakes which have become acidic due to acid rain

pH

2

7

8

14

Colour with Universal indicator

Acid Alkali, neutral?

Purple Strong Alkali

Red

Blue

Green

Reactions with Acids. Complete the equationsAcid+ metal salt + hydrogenHydrochloric acid + _________ magnesium chloride + hydrogen_________ acid + zinc zinc sulfate + HydrogenAcid + metal oxide salt + waterAcid + metal hydroxide salt + waterNitric acid + copper oxide- ___________ ___________ + waterSulphuric acid + ________ _______ zinc sulfate + water___________acid + sodium hydroxide sodium chloride + ______Acid+ metal carbonate salt + water + carbon dioxideHydrochloric acid + sodium carbonate ______ ________ + water + ___________ ____________

Which gas What do you do? What happens?

Gives a squeaky pop

Bubble through limewater

Oxygen

Organic Chemistry CrackingWhat is cracking? __________________________________________ _______________________ ________________________________What conditions are needed for cracking? ________________________________________________________What is a hydrocarbon? _____________________________________

CombustionWhat is combustion? ________________________________________

Equation for Complete Combustion ________________________________________________________Equation for Incomplete Combustion ________________________________________________________

Difference between alkanes and alkenes __________________________________________________ __________________________________________________What can you use to test if something is an alkane or alkene? __________________________________________________

Two ways to make alcohol __________________________________________________ __________________________________________________ Fractional Distillation

The crude oil enters the column at the _________ where it is extremely ________. Here the different fractions _________ and evaporates. The higher they rise the _________ they become. When they _________ enough they will turn back to _________. The fractions can be collected at the __________ of the column. Fractions with ___________ boiling points are found at the bottom. Ones with _________ boiling points are found at the top.

Polymers Match up the following

5 uses of plastics ____________________________________________________________________________________________________ 5 properties of plastics _____________________________________________________________________________________________________________________________

How can plastics be disposed of __________________________________________________

Rates of Reaction What FOUR things cause a reaction to increase? Explain using particle theory!

1. ______________________________________________________

2. ______________________________________________________

3. ______________________________________________________

4. ______________________________________________________

Draw the apparatus to investigate the rate of reaction

Define Rate of Reaction _______________________________________

Two reasons a reaction stops?

______________________________________________________________________________What 2 things need to occur for a reaction to happen

______________________________________________________________________________

Describe the role of light in photochemical reactions and the effect on the rate (speed)

____________________________________________________________________________________________________________________________________________________________________________________________________________________________

Behaviour of Metals

Iron reduces copper oxide (OIL RIG)

EquationFe (s) + CuO (s) FeO (s) + Cu(s)

Half equations __________________________________ _________________________________

Ionic equations _________________________________

Where are metals found in the periodic table? __________________

Name 5 properties of metals _________________________________ _________________________________________________________

Chemical properties of metals________________________________ ________________________________________________________

Draw a picture of an alloy What is an alloy? ___________________

______________________

Thermal Decomposition Reactions _____________ Oxide + carbon dioxide (except Na &K)

_____________ Oxide + Water (except Na & K)

_____________ Oxide + nitrogen dioxide + oxygen (except Na & K)

Why does aluminium not rust? ______________________________ _______________________________________________________Explain 2 ways you can protect iron from rusting? _______________________________________________________ _______________________________________________________ ______________________________________________________

REDOX

OILRIG stands for

O_________ I__ L_______ o __ e_________

R__________ I__ G_______ o__ e_________

Rules

Oxidation state of an element is 0

Ionic compounds oxidation state is its charge

Hydrogen = +1

Oxygen = -2

Oxidation states in a compound = 0

Work out the oxidation states :2Mg + O2 2MgOMg = ______O = _____MgO ______Has the Mg been oxidised/reduced?Has the O been oxidised/reduced?

This reaction takes place in the blast furnace: Fe2O3 (s) + 3CO ( g) 2Fe (l) + 3CO2( g)

The word equation for the reaction is:

……………………………………………………………………………………………

It is a redox reaction, because

……………………………………………………………………………………………

The reducing agent in this reaction is ………………………………....

Which is being oxidised and which is being reduced?

a) Mg + 2HCl → MgCl2 + H2

b) 2CO + O2 → 2 CO2

c) 3H2 + N2 → 2NH3

d) 4Na + O2 → 2Na2O

What is the oxidation state of:

Cu in CuO ___________

Cu in Cu2O ___________

Fe in FeCl2 ___________

Fe in FeCl3 ___________

Electrolysis What is a conductor? ____________________________What is an insulator? ___________________________Why are the only solids that conduct are metals and graphite ___________________________________ ________________________________________________Why do ionic substances only conduct when molten/dissolvedElectrolysisDefine electrolysis _______________________ ______________________________________4 uses of electrolysis _____________________ ______________________________________

RULES FOR ELECTROLYSISAt cathode (-), either a metal/hydrogen forms• If a metal is more reactive than hydrogen its ions stay in

solution and hydrogen bubbles off• If the metal is less reactive than hydrogen the metal forms.

At anode (+) a non-metal other than hydrogen forms.• If it is a concentrated solution of a halide then halogens

form.• If the halide solution is dilute /no halide oxygen forms.

Match the keyword Electrolysis of copper with copper electrodes

Ionic equation at cathode

___________________________

Ionic equation at anode

___________________________

Electrolysis of copper with inert electrodes

Ionic equation at cathode

___________________________

Ionic equation at anode

___________________________

Anode

Cathode

Anions

Cations

Electrolyte

negative ions

liquid which conducts electricity

positive electrode

Positive ions

Negative electrode

Chemical Uses

Sodium chloride

Chlorine

Hydrogen

Sodium hydroxide

Test for chlorine _______________

Electrolysis of Brine

Ionic equation at cathode

___________________________

Ionic equation at anode

___________________________

USES of METALS Extraction of metals from the oresLabel on the right Which ones are extracted by

electrolysis, which are found naturally and which are burnt with carbon and reduced

Name two uses of aluminium? ______________________________ _______________________________________________________

Two uses of copper ? _____________________________________

Two uses of zinc? _____________________________________

Name the uses of mild steel ________________________________

Name the uses of stainless steel _____________________________ _______________________________________________________

Name the uses of copper related to its properties ______________ _______________________________________________________

Label the blast furnaceName an iron ore used in the blast furnace._________________________ Name two substances that are mixed with iron ore__________________________________________________Name one of the gases leaving the blast furnace. _________________________________________________________________________________ Name two substances which react together to produce most of the energy required to heat the furnace to 1400C ________________________________________________ What impurities are found and how are they removed._________________________________________________________________________________

Extracting zincHow do you extract zinc from zinc blende? _______________________________________ _______________________________________ _______________________________________

OresWhat is haematite ? ______________________What is bauxite? _________________________

Equilibrium & Breaking BondsDefine exothermic reaction _______________________ _______________________________________________Define endothermic reaction ______________________ _________________________________________________Define equilibrium _______________________________ _________________________________________________Define Dynamic ___________________________________ _________________________________________________

Increasing ConcentrationIncreasing PressureIncreasing temperature

Exothermic/endothermic?Amount of energy needed to break bonds less than amount of energy released. Exothermic/endothermic

If the energy taken in to break bonds is more than the energy released Exothermic/endothermicBurning a fuel in air Exothermic/endothermic

Hydrogen Biofuel Nuclear fuel

2 pros

2 cons

AIR and WATER Seperation of airYou can separate gases from air by fractional distillation.________________________________________________________ ________________________________________________________2 uses of oxygen _______________________________________2 uses of nitrogen _______________________________________2 uses of noble gases _______________________________________

What is the equation for respiration _______________________________________________________

What is the equation for combustion

_______________________________________________________

What is the equation for photosynthesis

_______________________________________________________

What is thermal decomposition?

_______________________________________________________

Name 4 pollutants in air _______________________________ _____________________________________________________________

What is the composition of air?

Complete the pie chart for oxygen, nitrogen, carbon dioxide and other gases

RustingWhat 2 conditions are needed for rusting? _______________________

Write and equation __________________________________________

How can you stop rusting _____________________________________ __________________________________________________________ __________________________________________________________

Define solution_________________________________Define solvent _________________________________Define soluble_________________________________2 tests for water?________________________________________________________ ________________________________________________________

Water treatmentAdd the labels chlorination (kill bacteria) coagulant sand filters and charcoal add air

Non-Metals Y11

Haber Process What does the Haber process make? ______________________What is the equation ? __________________________________

Where does the nitrogen come from? ______________________Where does the hydrogen come from? _____________________

3 conditions for the Haber Process? _______________________ _____________________________________________________

LimestoneFormula of Limestone? ___________________________________2 uses of limestone _____________________________________Formula of Lime _______________________________________2 uses of lime ________________________________________Formula of Slaked Lime ___________________________________2 uses of Slaked Lime ____________________________________

Thermal decomposition Define Thermal decomposition ______________________________

2 Uses of Calcium oxide ____________________________________What is the equation for calcium oxide when it reacts with water? ________________________________________________________

Equations for making fertilisers

Ammonia + nitric acid __________________

________ + Sulphuric acid ammonium _________

Ammonia + ___________ acid _________ phosphate

Potassium hydroxide + nitric acid potassium ____ +water

Ammonium chloride + calcium hydroxide calcium chloride + water + _______

Making fertilisers

Element What it is used for?

Nitrogen _______________________________________

Phosphorous _______________________________________

Potassium _______________________________________

In the Lab I on tested Solution added colour Barium chloride + dilute

hydrochloric acid

Chloride (Cl–)

A white precipitate

Copper

zinc

Sodium hydroxide White precipitate in NaOH, which dissolves in excess

Sodium hydroxide with aluminium foil and heat

I ron(I I I ), (Fe3+(aq))

Hydrochloric acid Bubbles of carbon dioxide are given off . I ron(I I ) (Fe2+(aq))

Colourless precipitate

I odide (I –)

Barium chloride + dilute hydrochloric acid

A white precipitate of barium sulf ate is f ormed.

Metal Colour of flame

Copper

Lilac

Lithium

Brick-red

Sodium

Barium

Metal Colour of flame

Carbon dioxide

Damp litmus gets bleached

Oxygen

Hydrogen