States of Matter Draw a particles (circles) diagram Heating and cooling curves Label the graph with...
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Transcript of States of Matter Draw a particles (circles) diagram Heating and cooling curves Label the graph with...
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