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Name a metal found un combined in the Earth’s crust. Gold, silver or copper.
Give a property of metals. Ductile Strong Malleable Conducts heat Conducts electricity
Which metal is extracted from it’s ore in a Blast Furnace? IRON
What is produced when metal reacts with oxygen? Metal oxide
Name a metal obtained from its ore by electrolysis? Mg, Al, Na, K, Li
Name the products of the reaction between zinc and sulphuric acid. Zinc Sulphate + Hydrogen
Name the products of the reaction between sodium and water. Sodium Hydroxide + Hydrogen
What is an alloy? Mix of difference metals or a mix of metals and non metals.
Which type of reaction takes place when a metal is extracted from its compound (ore)? Reduction
Identify the two alloys from the list: brass, iron, copper and steel. Brass and Steel.
Calculate the percentage mass of potassium in potassium sulphide. gfm K = 39 G Gfm K 2 S = 2 x 39 + 32 = 110 % mass= (39/ 110) x 100 = 35.5 %
Name a metal which does NOT react with dilute acid Gold, silver or copper.
What is the name of group 1 metals? Alkali Metals.
What is a displacement reaction ? A metal high in the electrochemical series displaces ( takes its place) ions of a metal lower in the series from it solution.
Is this ion electron equation an example of reduction or oxidation? Cu 2+ + 2e - Cu Reduction.
Is this ion electron equation an example of reduction or oxidation? 2Cl - Cl 2 + 2e - Oxidation
Electricity is the flow of ? Electrons.
Why do batteries run out? The chemicals get used up.
State an advantage of batteries over mains electricity Batteries are portable.
What is the purpose of the ion (salt) bridge? To complete the circuit.
What is the relationship between the position of metals in the electrochemical series and the voltage of a cell? The further away they are from each other the larger the voltage.
What is the purpose of an electrolyte? To complete the circuit.
What directions will the electrons flow in a zinc / copper cell? Zinc to Copper.
What is oxidation? Loss of electrons.
What is reduction? Gain of electrons.
Name the type of chemical reaction taking place. Mg + CuCl 2 Cu + MgCl 2 Displacement.
What is corrosion? A chemical reaction involving metals changing from element to a compound.
What are the two conditions required for rusting to take place? Water and oxygen.
What type of reaction takes place when a metal corrodes? Oxidation
How can you test to see if Iron has corroded? Will change from an element to an ion, Fe 2+ and Fe 2+ can be detected as it turns Ferroxyl indicator blue.
Which terminal of a battery protects iron from rusting? Negative
Why does salt speed up corrosion? As salt is an electrolyte.
How does a physical barrier protect iron against rusting? Prevents water and oxygen ( air).
What metal is used to galvanise Iron? Zinc
Why does scratched tin plated iron rust faster then non – plated iron? Electrons flow from Iron to Tin because Tin is below Iron in the electrochemical series.
Magnesium provides Iron with sacrificial protection. In which direction do electrons flow? From Magnesium to Iron.
Give examples how Iron can be physically protected? Layer of Paint Layer of Grease Layer of plastic Tin plating Electroplating Galvanising
eymmcl eymmcl Are metals finite or infinite resources? answer finite.
Metals, Making Electricity and Corrosion. Metals The job that a metal is used for is determined by its physical and chemical properties. Physical properties.
eymmcl eymmcl Why does scratched, tin plated iron rust faster than non-plated iron? answer Electrons flow from.
Revision Quiz Corrosion 1 1.Define corrosion? 2.Define rusting? 3.What is the cause of rusting? 4.How can the initial stages of rusting be detected? 5.Write.
Standard Grade Chemistry Topic 12 - Corrosion. Corrosion Corrosion is the changing of the surface of the metal from an element into a compound. This natural.
Calderglen High School Calderglen High School 1 Are metals finite or infinite resources? answer finite.
Calderglen High School What is corrosion? A chemical reaction involving a metal changing from an element to a compound answer.
Corrosion is when metals react with substances in the Air to produce compounds. The metal is changing from an atom to an ion. The metal atom looses electrons.
TOPIC 12 Corrosion Corrosion When a metal corrodes it loses electrons and forms positive metal ions. When a metal corrodes it loses electrons and forms.
Intermediate 1 Unit 2a Metals
Corrosion Intermediate 2 Unit 3(c). WHAT IS CORROSION? When the surface of a metal changes from being an element into a compound The surface goes from.
3.17 Uses of electrolysis Purification of copper: Impure copper extracted from its ore by heating the ore with carbon (smelting) – a mixture of copper.
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Metal Corrosion 1. The structure of metals The arrangement of the atoms Metals are giant structures of atoms held together by metallic bonds Metallic.
CHEMISTRY DEPARTMENT WAID ACADEMY Standard Grade Topic 12.
Calderglen High School Calderglen High School 1 Electricity is a flow of …..? answer electrons.
By – Miss Kiran Rathod. Metals Metals are solids. (except mercury) Metals are hard. (except Lithium, Potassium, Sodium) Metals have metallic lustre.
Properties of metals Metals physical properties includes: they are; Ductile; they can be drawn into wire, Malleable; they can be hammered into sheets.
Metals and their Properties Metals have distinctive properties such as: 1. Electrical Conductivity 2. Good Thermal Conductivity 3. Strength 4. Malleability.
Preventing Corrosion. Corrosion can be prevented in a number of ways: Corrosion can be prevented in a number of ways: Physical protection Physical protection.
29/05/2014 Reactivity of Metals. 29/05/2014 Reactions of metals with oxygen When a metal reacts with oxygen it will form a METAL OXIDE. This is what happens.
Topic 7 - Corrosion. Topic 7 Corrosion Lesson 1/2 These outcomes relate to the PowerPoint Slides 1-4 on Corrosion.
IGCSE CHEMISTRY SECTION 2 LESSON 4. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.
Do Now! Describe how aluminium can rust, and how it’s different to rusting iron (use the information found in the “Iron and Aluminium” worksheet) Aluminum.
Metals. Learning Objectives Use reactivity data to determine a reactivity series Relate extraction method to reactivity of metals Write word/symbol equations.
Standard Grade Chemistry Topic 11 - Metals. Properties of Metals Density – this is the mass of a substance in a given volume. A high density material.
Created by C. Ippolito March 2007 Updated March 2007 Chapter 22 Electrochemistry Objectives: 1.describe how an electrolytic cell works 2.describe how galvanic.
How are metals extracted from their ores? How are metals prevented from reverting to their oxides? Reactivity series How to extract metals IRON Electrolysis.
Corrosion of metals and their protection. What is corrosion? A) The reaction of a metal with oxygen in the air, moisture or other substances in the environment.
Topic 3 Metals and their uses. Extracting metals Metals are found in the Earth’s crust They are often chemically combined with other elements – this is.
More Protection Techniques. Direct Electrical Protection When a metal corrodes it loses electrons (oxidation). If electrons could be ‘pushed’ back onto.
Metals and their Properties TOPIC 11 Metals and their Properties Metals have distinctive properties such as: 4. Malleability. 3. Strength 2. Good Thermal.
Patterns of Reactivity. Properties of metals and non-metals Metals have very high melting points (which means that they are usually _____) whereas non-metals.
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Standard Grade Revision Unit 10 Q1. Pairs of metals are used to produce a cell. Standard Grade Chemistry (a)What is the purpose of the filter paper soaked.
Electrochemistry Chapter 20. Electrolysis Electrolysis is the use of electricity to bring about a chemical reaction. Redox reactions occur at the electrodes.
CHAPTER - 4 MATERIALS : METALS AND NON METALS. 1) Occurrence of metals and non metals :- Out of the 92 naturally occuring elements 70 are metals and about.
Write down the Reactivity Series from Potassium to Gold. Potassium Sodium Lithium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Hydrogen Copper.
Metals. Learning Objectives Order metals in order of reactivity Relate extraction method to reactivity Write word/symbol equations for reduction of metal.
Engineering Chemistry 14/15 Fall semester Instructor: Rama Oktavian Office Hr.: M.13-15, Tu , W , Th ,
Electrochemistry. Electrochemical Cells Electrons are transferred between the particles being oxidized and reduced Two types –Spontaneous = Voltaic.
Cell potential is related to concentrations Electrodes can be used that are sensitive to specific ions They measure concentrations of specific ions which.
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CHAPTER - 3 METALS AND NON METALS CLASS :- X MADE BY :- MANAS MAHAJAN SCHOOL :- K.V. GANESHKHIND PUNE-7.
ELECTROLYSIS. What is a redox reaction? Oxidation is the addition of oxygen to a substance and reduction is the removal of oxygen from a substance. lead.
By Miss Buicke Metals and Non-metals. What we need to know from the syllabus : OC45 understand that rusting is a chemical process that changes iron into.
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