Temperature
By heating chemicals, we raise the energy levels of the molecules involved in the reaction. Increasing the temperature means the molecules move faster and the reaction rate increases.
I can
- state that the alkanes are a subset of the set of hydrocarbons
- state what is meant by a homologous series
- identify an alkane from the -ane ending
- explain that the alkane family is an example of a homologous series
- state the name for each alkane up to octane
- give examples of uses of alkanes
- for straight chain alkanes, (C1 to C8), work out the names from molecular formulae, shortened and full structural formulae
- for straight chain alkanes (C1 to C8), construct full and shortened structural formulae and molecular formulae given the name
- for alkanes, use the general formula to work out the molecular formulae derive a general formula for alkanes
- explain in terms of increasing molecular size why the boiling point increases as the number of carbon atoms in an alkane increases
- state the name of each cycloalkane up to cyclohexane
- explain that the cycloalkane family is an example of a homologous series
- state what is meant by isomers
- state that the alkanes are a subset of the set of hydrocarbons
- identify an alkene from the – ene ending
- state the name for each alkene up to hexene
- explain that the alkene family is an example of a homologous series
- for alkenes, (C1 to C6), work out names from molecular, shortened or full structural formulae
- for alkenes, C1 to C6 construct full and shortened structural formulae and molecular formulae given the name
- for alkenes, us a general formula to work out molecular formulae
- derive a general formula for alkenes
- identify from a structural formula the following types of compound: alkanes and alkenes
- for simple organic molecules, including alkanes, alkenes and clycloalkanes, construct appropriate isometric forms, given a molecular formula
- state what is meant by a saturated hydrocarbon
- explain that the alkanes are saturated hydrocarbons
- state what is meant by an unsaturated hydrocarbon
- explain that the alkenes are a sub-set of the set of unsaturated hydrocarbons
- state that it is possible to distinguish an unsaturated hydrocarbon from a saturated hydrocarbon using bromine (solution)
- state the name of the alkane formed by the reaction of an alkene with hydrogen
- state what is meant by an addition reaction
- explain that the reactions of alkenes with bromine and hydrogen are addition reactions
- state that fractional distillation of crude oil yields more long chain hydrocarbons than are useful for present-day industrial purposes
- state that cracking is an industrial method for producing smaller, more useful molecules
- state that the catalyst allows the reaction to take place at a lower temperature
- state that the cracking produces smaller hydrocarbons, some of which are unsaturated
- explain why cracking produces a mixture of saturated and unsaturated products.
Topic 7 : Properties of Substances
Topic 9 : Reactions of Acids
Topic 6 : Hydrocarbons
Topic 10 : Making Electricity
The only non-metal which conducts is carbon in the form of graphite.
In graphite, the atoms are arranged in overlapping rings, held by strong covalent bonds and other electrons can move easily from one ring to the next throughout the structure.
I can
- state that metal elements and carbon (graphite) are conductors of electricity and that most non-metal elements are non-conductors of electricity
- state that covalent compounds (solid, liquid, solution) do not conduct electricity
- state that compounds made from metal elements do not conduct electricity in solid state, and that these compounds do conduct electricity when dissolved in water or when molten
- state that electric current is a flow of charged particles
- state that electrons flow through metals and that ions flow through solutions
- state that electrical energy chemically changes a solution which conducts
- state that a d.c. supply must be used if the products are to be identified
- describe the formation of ions in terms of atoms losing and gaining electrons
- state that solid compounds can be ionic or covalent and that compounds which exist as liquids or gases at room temperature are covalent
- state that ionic solids exist as networks/lattices of oppositely charged ions
- explain why ionic and covalent network substances are solid, and why covalent substances can be solid, liquid or gas
- give examples of covalent substances which are insoluble in water but which dissolve in other solvents
- state that when ionic compounds dissolve in water, the lattice breaks up completely
- identify the elements which are formed when an ionic solution is changed by electrical energy, explaining the products at each electrode, in terms of positive metal ions being attracted to the negative electrode and negative non-metal ions being attracted to the positive electrode
- explain the formation of atoms/molecules at each electrode in terms of positive ions gaining electrons and negative ions losing electrons
- state that electrical energy chemically changes a molten ionic compound
- explain why the melt conducts but the solid does not
- state what is meant by an electrolyte
- state what is meant by electrolysis
- relate the colour of an ionic compound to the colour of the positive and/or negative ions
- explain why the process is only applicable to ionic compounds.
- explain the results of experiments involving the migration of coloured ions
I can
- state that neutralisation is the reaction of acids with neutralisers
- give everyday examples of neutralisation, including:
- reducing acidity in soil by adding lime
- the use of lime to reduce acidity in lakes caused by rain
- treatment of acid indigestion
- state that neutralisation moves the pH of an acid toward 7
- tate that the reaction of acids with alkalis is an example of neutralisation
- tate that neutralisation moves the pH of an alkali towards 7
- tate that the reaction of H+(aq) to form water is an example of neutralisation
- tate that the reaction of hydrogen ions and hydroxide ions form water
- name the products formed in the reaction of a neutraliser with dilute hydrochloric, nitric or sulphuric acid
- define a salt as a substance in which the hydrogen ion of an acid has been replaced by a metal ion (or the ammonium ion).
- state that an acid reacts with a metal carbonate to give off carbon dioxide
- state that the reaction of hydrogen ions and carbonate ions forms water and carbon dioxide
- explain why, in the preparation of a given salt, it is often easier to use an insoluble metal carbonate or metal oxide as the neutraliser
- explain the effect of acid rain on buildings and carbonate rocks
- define a base as a substance which neutralises an acid
- state that bases which dissolve in water form alkalis
- state that an acid reacts with some metals to give off hydrogen gas
- state that in the reaction, hydrogen ions form hydrogen molecules
- name the products formed when dilute hydrochloric or sulphuric acid reacts with a metal
- explain the effect of acid rain on structures made from iron
- state that precipitation is the reaction of two solutions to form an insoluble product called a precipitate
- state that insoluble salts can be formed by precipitation
- name the insoluble product formed by the reaction of two solutions
- carry out calculations to find the concentration of acids/alkalis from volumetric titration.
I can
- state that, in a battery, electricity comes from a chemical reaction
- state that electricity passing along metal wires is a flow of electrons
- explain the need to replace batteries in terms of the chemicals being used up in the reaction
- state that some batteries are rechargeable, eg the lead-acid battery
- explain that ammonium chloride in a cell is an example of an electrolyte
- explain that the purpose of the electrolyte is to complete the circuit
- state that electricity can be produced by connecting different metals together (with an electrolyte) to form a cell
- state that the voltage between different pairs of metals varies and that this leads to the electrochemical series
- use an electrochemical series showing metals only to explain why displacement reactions occur and describe the experimental observations
- use an electrochemical series to predict whether or not displacement reactions occur; and predict the experimental observations
- state that the reactions of metals with acids can establish the position of hydrogen in an electrochemical series
- state that electricity can be produced in a cell by connecting two different metals in solutions of their metal ions
- state that electricity can be produced in a cell when at least one of the half-cells does not involve metal atoms
- state that the purpose of the “ion bridge” is to complete the circuit
- explain that the movement of ions in the ion bridge is to provide ions to complete the circuit
- compare batteries and mains electricity sources in relation to ease of transport, safety, costs and uses of finite resources
- state that a metal element reacting to form a compound is an example of oxidation
- state that oxidation is a loss of electrons by a reactant in any reaction
- state that a compound reacting to form a metal element is an example of reduction
- state that reduction is a gain of electrons by a reactant in any reaction
- state that, in a redox reaction, reduction and oxidation go on together
- apply terms oxidation and reduction to more complex ion-electron equations, eg SO42-/SO32-.
Examples – Finding the mass
What is the mass of one mole of water?
What is the mass of 2 moles of calcium carbonate?
What is the mass of 0.5 moles of sulphuric acid?
What is the mass of 0.1 moles of nitric acid?
What is the mass of 4 moles of sodium hydroxide?
Examples – Finding the number of moles.
How many moles are present in 104g of magnesium oxide?
How many moles are present in 9.8g of sulphuric acid?
How many moles are present in 67g of methane?
How many moles are in 10.6g of sodium carbonate?
Topic 8 : Acids & Alkalis
Do these examples in your classwork jotter. Double underline your final answer and SHOW YOUR WORKING!
Calculate the number of moles in 1 litre of a 6 mol/l solution
Calculate the number of moles in 0.4 litres of a 2 mol/l solution
Calculate the number of moles in 50cm3 of a 0.1 mol/l solution
Calculate the number of moles in 750cm3 of a 0.25 mol/l solution
What is the concentration of 9 moles of solute dissolved in 2 litres of solution?
What is the concentration of 0.5 moles of solute dissolved in 250cm3 of solution?
What is the concentration of 2 moles of solute dissolved in 3 litres of solution?
What is the concentration of 0.05 moles of solute dissolved in 75cm3 of solution?
Recap : The experiment
40g of H2SO4 dissolves in half a litre of water to form sulphuric acid. What is the concentration? 0.82 mol/l
Calculate the mass of calcium carbonate required to prepare 2 litres of a 0.2 mol/l solution. 40g
What volume of 0.5mol/l solution will be created when 8g of sodium hydroxide dissolves? 0.4l
Current that flows in one direction and so allows identification of product
Passing a current through a substance to break it up into its elements.
A substance containing free ions so conducting electricity.
Current that flows in one direction and so allows identification of product
pH Scale
I can
- state that non-metal oxides which dissolve in water produce acid solutions
- state that sulphur dioxide reacts with water in the atmosphere to produce acid rain
- give examples of the damaging effects of acid rain on buildings, other structures, soils and plant and animal life
- state that the pH scale is a continuous range
- state that:
- acids have a pH of less than 7
- alkalis have a pH of more than 7
- pure water and neutral solutions have a pH equal to 7
- give examples of common acids and alkalis used in the laboratory and in the home
- state that:
- ions are present in an acid solution
- ions are present in an alkali solution
- the concentration of ions in water is small
- state that in water and a neutral solution, the concentration of H+(aq) and OH-(aq) ions is the same
- state the test for hydrogen
- state that an acidic solution is one which contains hydrogen ions (H+(aq))
- explain that an acidic solution contains more H+(aq) ions than does pure water
- state that an alkaline solution is one which contains hydroxide ions (OH-(aq))
- explain that an alkaline solution contains more OH-(aq) ions than does pure water
- state that metal oxides or hydroxides which dissolve in water produce alkaline solutions
- for an acid and an alkali, describe the effect of dilution on:
- the acidity or alkalinity
- the pH
- explain dilution in terms of the decreasing concentration of hydrogen and hydroxide ions
- calculate the formula mass of a substance
- state that the gram formula mass of any substance is known as one mole
- state that the concentration of a solution is expressed in mo1/1 (mo1/dm³)
- calculate moles to mass and masses to moles
- carry out calculations involving mass from mo1/1 and mass per volume for a requested concentration.
The pH scale is a continuous range
Used to measure the acidity or alkalinity of a solution.
Below 0 to above 14.
Below 7 - acidic
Above 7 - alkaline
Topic 5 : Fuels
Formation of Coal
Millions of years ago, the Earth was covered in swamps and trees.
When the trees died they fell into the swamps and started to rot.
Over time, layers of rotting plants and earth built up.
The weight of the earth compressed the layers : this pressure, along with heat and a lack of oxygen, formed coal.
Formation of Crude Oil
Test for Oxygen
Millions of years ago the seas were filled with microscopic marine organisms.
When they died, they sank to the bottom of the sea.
A combination of pressure, heat and a lack of oxygen caused the decaying organisms to turn into oil and gas.
Oxygen gas relights a glowing splint.
Universal Indicator and the pH scale
Topic 12 (Not required for prelim)
Some facts about acids and alkalis
Topic 11 : Metals
I can
- state that a fuel is a chemical which burns giving out energy
- state that combustion is a reaction of a substance with oxygen, giving out energy
- state the test for oxygen
- state that the main components of air are oxygen and nitrogen in proportion of 1:4
- state that an exothermic reaction is one in which energy is released
- state what is meant by finite resource and fuel crisis in relation to the amount of coal, oil and natural gas in the earth
- state what is meant by a fossil fuel
- describe the formation of coal, oil and natural gas
- give examples of the pollution problems associated with oil and coal and explain their occurrence
- state that crude oil is a mixture of compounds
- state that substances have specific melting points and boiling points
- state that a fraction is a group of compounds with boiling points within a given range
- state that fractional distillation is the process used to separate crude oil into fractions
- explain why fractions can be separated by distillation
- state what is meant by: flammability; viscosity
- give examples of how the products of fractional distillation of crude oil can be used
- state the typical ranges of chain length of the molecules in each fraction and relate this to their use
- describe how each of the following varies for fractions of different boiling points: evaporationflammabilityviscosity
- explain in terms of molecular size the change in each of the following: boiling pointflammabilityviscosity
- state that the chemical compounds which are found in oil and natural gas are mainly hydrocarbons
- state that a hydrocarbon is a compound which contains hydrogen and carbon only
- state the tests for carbon dioxide and water
- state that hydrocarbons burn completely to produce only carbon dioxide and water
- explain why the production of carbon dioxide and water, on burning, indicates the presence of carbon and hydrogen in the original fuel
- state that carbon, and carbon monoxide, a poisonous gas, are produced when the hydrocarbons burn in a supply of oxygen which is insufficient for complete combustion
- state that the burning of some fuels releases sulphur dioxide, a poisonous gas, to the atmosphere
- state that removing sulphur compounds reduces air pollution
- state that nitrogen and oxygen from the air react inside a car engine to form nitrogen oxides (poisonous gases)
- state that lead compounds which are added to petrol cause pollution
- state that air pollution from the burning of hydrocarbons can be reduced by special exhaust systems or by altering the fuel to air ratio
- explain that transition metal catalysts can convert the pollutant gases to harmless gases
- explain that decreasing the fuel to air ratio improves the efficiency of combustion thus decreasing pollution.
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http://www.kgsorkney.co.uk/cmsmadesimple/uploads/chemistry/SG%20Chem%20Notes/Topic%205%20notes%20PC.pdf
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http://www.kgsorkney.co.uk/cmsmadesimple/uploads/chemistry/SG%20Chem%20Notes/Topic%205%20notes%20PC.pdf
BOTTOM
Highest boiling point,
hard to evaporate,
least flammable,
most viscous,
largest molecules.
A comparison
TOP
Lowest boiling point,
evaporates easiest,
most flammable,
least viscous,
smallest molecules.
I can
- state that metals conduct electricity when solid or liquid
- relate specific properties of metals, eg density, thermal and electrical conductivity, malleability, strength, to their uses
- explain the need for recycling metals in terms of the finite nature of the metal resources
- describe the reactions of different metals with oxygen, water and dilute acid
- state that these reactions give an indication of the reactivity of the metal
- state that ores are naturally-occurring compounds of metals
- state that the less reactive metals are found uncombined in the earth’s crust and that the more reactive metals have to be extracted from ores
- explain that the extract of a metal from its ore is an example of reduction
- explain why the inactive metals were among the first to be discovered
- give examples of social and industrial factors which resulted in large scale extraction of more reactive metals
- state that some metals can be obtained from metal oxides by heat alone; some by heating with carbon; and some need other methods
- explain in terms of the reactivity of the metal why some metals can be obtained from metal oxides by heat alone; and why some metal oxides need to be heated with other substances, eg carbon or carbon monoxide; and why some metals cannot be obtained by these methods
- state that iron is produced from iron ore in the blast furnace
- state the two key reactions which take place in the blast furnace:
- production of carbon monoxide
- reduction of iron oxide
- state that an alloy is a mixture of metals or of metals with non-metals
- give examples of the important uses of alloys, eg brass, solder, “stainless” steel
- work out empirical (or molecular) formulae from masses or percentage composition
- work out percentage masses of elements in compounds from their names or formulae
A Complete Revision Guide
Covalent Bonding
When non-metal atoms combine by sharing electrons in a covalent bond, this is called a molecule.
Definition to learn
A covalent bond is the attraction each nucleus has for shared pair(s) of electrons.
The attraction of the two nuclei for the same shared electrons hold the two atoms together.
Topic 4 : How Atoms Combine
Methane CH4
Ammonia NH3
Water H2O
Hydrogen has a valency of 1
Oxygen has a valency of 2
Hydrogen has one outer electron.
To become stable it needs to share an electron with another hydrogen atom.
Hydrogen
Topic 13 (Not required for prelim)
This prezi contains :
Complete learning outcomes to the course
Links to helpful websites / videos
Past Paper Examples.
E-mail ssmith332@gryffehigh.renfrewshire.sch.uk if you have any problems.
Happy studying :)
I can
- state that atoms can be held together by bonds
- state that atoms can achieve a stable electron arrangement
- describe the covalent bond in terms of atoms sharing pairs of electrons
- state that a molecule is a group of atoms held together by covalent bonds
- explain the covalent bond as a situation in which two positive nuclei are held together by their common attraction for the shared pair of electrons
- state that the chemical formula gives the number of atoms of each element in a molecule of a covalent substance
- state that (usually) only atoms of non-metal elements bond to form molecules
- state that a diatomic molecule is made up of two atoms
- give examples of elements which exists as diatomic molecules
- draw a diagram to show how the outer electrons form a covalent bond
- draw diagrams to show the shape of simple two element molecules.
Topic 3 : Atoms and the Periodic Table
Name of subatomic particle
Dmitri Mendeleev
Proton
Neutron
Electron
Topic 14 (Not required for prelim)
I can
- classify elements in different ways, eg naturally occurring/made by scientists; solid/liquid/gas; metal/non-metal
- state that chemists have classified elements by arranging them in the Periodic Table
- state that a group is a column of elements in the Periodic Table
- state that elements in one group of the Periodic Table show similar chemical properties
- identify the following families of elements: the halogens, the alkali metals, the noble gases, the transition metals
- state that noble gases are a family of very unreactive elements
- state that every element is made up of very small particles called atoms
- describe the atom as having a vary small positively charged nucleus with negatively charged electrons moving around outside the nucleus
- describe the location and charge of the proton, neutron and electron
- state the relative masses of the proton, neutron and electron
- state that an atom is neutral because the positive charge of the nucleus is equal to the sum of the negative charges of the electrons
- state that an atom is neutral because the numbers of protons and electrons are equal
- state that atoms of different elements are different and have a different number on the Periodic Table called the atomic number
- state that atoms of different elements have a different number of protons, called the atomic number
- state that the electrons in an atom are arranged in energy levels
- state the electron arrangements of the first 20 elements
- explain the structure of the Periodic Table in terms of the atomic number and chemical properties of the elements
- state that elements with the same number of outer electrons have similar chemical properties
- state that an atom has a mass number which equals the number of protons plus neutrons
- calculate the number of n, p and e from the mass number and atomic number, and vice versa
- calculate the number of n, p and e from nuclide notation, including ions
- state that most elements exist as a mixture of isotopes
- state what is meant by isotopes
- state that atoms of different elements vary in size and in mass
- state what is meant by relative atomic mass
- explain why the average atomic mass of an element is rarely a whole number.
Isotopes
They have the same numbers of protons and electrons.
Chlorine – 37 has two more neutrons than Chlorine – 35
This means that Chlorine -37 is heavier.
Atoms with the same atomic number but different mass numbers are called isotopes.
Protons = 6
Neutrons = 6
Electrons = 6
Relative Atomic Mass
Most elements are made up of a mixture of isotopes.
The relative atomic mass of an element is the average mass of all the isotopes.
For this reason, the relative atomic mass is rarely a whole number.
Topic 2 : Speed of Reactions
I can
- describe how the following affect the speed of a reaction: particle size, concentration, temperature
- give examples of reactions (both laboratory and everyday) affected by the following: particle size, concentration, temperature
- state that catalysts are substances which: speed up some reactions, are not used up during the reaction, can be recovered chemically unchanged
- give everyday examples of uses of catalysts, eg transition metals in car exhaust systems.
Standard Grade Chemistry
NOTE : Catalysts
Some reactions can be speeded up by the use of a special chemical called a CATALYST.
Hydrogen peroxide decomposes (breaks up) slowly releasing oxygen gas. If manganese dioxide is added the reaction is much faster and oxygen gas is given off quickly. Manganese dioxide is a catalyst for this reaction. At the end of the reaction all of the manganese dioxide can be recovered (by filtration) and used again.
Catalysts in living things are called ENZYMES e.g. an enzyme in saliva called amylase helps your body digest food into smaller pieces. Enzymes are used in some washing powders, beer and wine making and in making sweets.
NOTE : Speed of Reactions
The speed of a chemical reaction is the time it takes for the reactants to be converted to the products.
In order for a reaction to proceed, the reactant particles must collide.
The more collisions that there are, the faster the reaction will be.
Concentration
Changing the concentration means that there is more chance that the molecules will collide. The frequency of the collisions will be greater as we increase the concentration, and the reaction rate will increase.
Quizlet
SQA Past Papers
Evans2Chemweb
Topic 15 (Not required for prelim)
NOTE : factors affecting reaction rate continued…
http://www.sqa.org.uk/pastpapers/findpastpaper.htm?subject=Chemistry&level=SC
Factors affecting reaction rate
Particle Size
Smaller reactant particles provide a greater surface area which increases the chances for particle collisions so the reaction rate increases.
Great revision website.
Username is gryffe and password is boron
Topic 1 : Chemical Reactions
Past Papers and Marking Schemes
Download flashcards onto your iPhone, iPod Touch or iPad using apps like 'Flashcardlet' or you can use the flashcards online.
Definitions : http://quizlet.com/_6hjys
Questions : http://quizlet.com/_6j0qp
http://www.evans2chemweb.co.uk/
I can
- identify a chemical reaction by a change in appearance of substance
- identify a chemical reaction by a detectable energy change
- state that all chemical reactions involve the formation of one or more new substances
- give examples of chemical reactions which occur in our day-to-day lives
- state that everything in the world is made from about 100 elements
- state that each element has a name and a symbol
- state that compounds are formed when elements react together
- state that mixtures occur when two or more substances come together without reacting
- state that a solution is formed when a solute dissolves in a solvent
- apply the general rules: the compounds with the name ending in “ide” contain the two elements indicated, and that the ending “ite” or “ate” indicates the additional element oxygen.
Revision Guide
The solute dissolves in the solvent to create a solution
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Mixture
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How do we know a reaction has occurred?
In a mixture, the substances have not reacted together.
Mixtures can be separated.
Add more crystals
We have to look for signs of a change
Effervescence
Look for a fizzing or bubbles to show that a gas has been produced.
Precipitate Forms
Look for a solid forming from two solutions.
Colour Change
Remember the difference between ‘colourless’ and ‘clear/transparent’
Energy change
Heat, light, electricity.
dilute
concentrated
saturated
Compounds
Compounds are formed when elements react together.
A compound contains two or more elements that are chemically joined together.
Separating Mixtures
Filtration
Separates an insoluble solid from a liquid
Distillation
Separates two liquids
Chromatography
Separates mixtures of colours.
Elements
An element is made up of only one type of atom.
Each element has a name and a symbol.