Last lesson 2g) Hydrogen. acid + metal salt + hydrogen Hydrochloric acid + magnesiummagnesium chloride + hydrogen Nitric acid + ironiron nitrate + hydrogen.

Slides:

Advertisements

Similar presentations

Topic 5 Acids in Action.

Advertisements

TESTING FOR CATIONS QUALITATIVE ANALYSIS.

Reactivity Series of Metals

Calderglen High School

CHEMISTRY DEPARTMENT WAID ACADEMY Standard Grade Topic 9.

Making Salts Soluble salt Insoluble salt Acid + excess insoluble solid

ACIDS AND BASES. Acids  Acidic solutions contain water and hydrogen ions (H+)

Do now! Can you talk to your partner about what we learned last lesson?

Introduction to Chemical Reactions Learning Reaction Types and Their Patterns.

Ammonia (NH3) Metal oxides Metal hydroxides

Making Changes Topic overview. The topic can be conveniently split into six interrelated sections  Oxidation/Reduction  Salts  Preparation of gases.

11/10/2015 Reactions of metals and metal compounds.

Balancing chemical equations. WRITING CHEMICAL EQUATIONS Chemical equations should show : (a) formulas of the reactants & products (b) their states of.

H 2 SO 4 + Zn  1) Sulphuric acid + zinc 3) Nitric acid + sodium thiosulphate 2) Hydrochloric acid + magnesium 4) Hydrogen peroxide with catalyst Popular.

Say we start with a strong alkali containing Universal indicator, and gradually add acid The alkali will gradually get.

Preparation for Practical chemistry Exercise on Chemistry Paper 4= 2014= form 5.

pH What is the pH of an ACID? Which type of OXIDE forms an ALKALI? Which type of OXIDE forms an ACID? What happens to the pH of an ACID when it is diluted?

1. Write down everything you can remember about: 2. Do you remember any properties of an acid?

Salts By Amy Badger.

Preparation of Salts.

Acid reactions. Metals and acid reaction Example Magnesium Metal (Mg) reacts with Hydrochloric acid (HCl) to produce Hydrogen Gas and Magnesium Chloride.

Acid and bases Bases.

“Chemical Reactions”. All chemical reactions…  have two parts: 1.Reactants = the stuff you start with 2.Products = the stuff you end up with  The reactants.

2j Preparing and analysing. Last lesson - Precipitation reactions Reactions that produce an INSOLUBLE SALT.

2j Preparing and analysing

Lab Tests, results, and Sulphuric acid Tes lab, hasil, dan asam sulfat

C5 lesson 4. Learning objective: To understand how unknown compounds can be identified. Must: Explain what a precipitate is – E Should: Be able to use.

Common precipitation reactions with hydroxide ions. When sodium or ammonium hydroxide is added to a solution of metal ions an insoluble metal hydroxide.

Revision Quiz Acids 1 1.What is the pH scale? 2.What numbers on the pH scale show an acid? 3.What is an indicator? 4.What number is neutral? 5.What colour.

Acids and Alkalis Year 11. CONTENTS Acidity and alkalinity Indicators pH Acids General methods for making salts Making salts from metal oxides Making.

Chemical Reactions. Reactions involve chemical changes in matter resulting in new substances Reactions involve rearrangement and exchange of atoms to.

Colour changes for simple indicators IndicatorColour in acidColour in alkali litmusredblue methyl orangeredyellow phenolphthaleincolourlessred.

Properties of Metals and Non-Metals Done By: Sherrell Mungal.

IGCSE CHEMISTRY SECTION 2 LESSON 3. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

TESTS FOR GASES & WATER.

Reactions of Metals. Metal Oxides Salts and hydrogen React with oxygen to giveReact with acids to give.

Acids and Bases and Salts Revision IGCSE 620. Which ions are definitely given out from an acid? and alkali? when mixed with water Acid H+ ions (hydrogen.

A cids Bases & Salts (Bases) an e-learning series by ycs.

IGCSE CHEMISTRY SECTION 2 LESSON 5. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

AS Revision Lessons Identification tests.

Core Chemistry Smart Teach 3: Acids and electrolysis.

Learning Objectives By the end of the lesson, you should be able to: a)Give the definition of a strong and weak acid, and the properties of it. b)Identify.

 Most carbonates are insoluble (can not be dissolved in water) except those containing sodium or potassium ions.

Naming Salts, state symbols and writing equations

Chemical Changes and Structure

Tests for Oxidising / Reducing Agents

Reactions of metals and metal compounds

Acids and Alkalis Grade 10.

Reactions of Acids.

Topic 1 – Qualitative testing.

Qualitative Analysis Reactions that produce an INSOLUBLE SALT.

Reactions of metals and metal compounds

19/09/2018 Chemistry in Action W Richards The Weald School.

Lab Tests, results, and Sulphuric acid

Testing for ions and gases

Reactions of Metals Displacement Reactions:

Transition elements Copper

Reactions of Acids.

Transition elements Nickel

Transition elements Cobalt

Transition elements Iron

Transition metal ions All transition metals lose electrons when they react, and so form positive ions. Some transition metals only make one type of ion,

Week 6 – Acids and Alkalis

Presentation transcript:

Last lesson 2g) Hydrogen

acid + metal salt + hydrogen Hydrochloric acid + magnesiummagnesium chloride + hydrogen Nitric acid + ironiron nitrate + hydrogen Sulphuric acid + zinc zinc sulphate + hydrogen In general, hydrochloric acid makes a chloride, nitric acid makes a nitrate, and sulphuric acid makes a sulphate. “salts”

Preparation of hydrogen

Combustion of hydrogen 2H 2 + O 2 2H 2 O

Test for water Cobalt chloride paper turns from blue to pink

Pure water? Boils at 100°C

Hydrogen and chlorine H 2(g) + Cl 2(g) 2HCl (g) Hydrogen chloride gas (covalent) dissolves in water to from hydrochloric acid (H + + Cl - )

Today’s lesson h) The transition metals - iron and copper

A treasure hunt!

1. Iron + steam iron(III) oxide + hydrogen. 2Fe (s) + 3H 2 O (g) Fe 2 O 3(s) + 3H 2(g)

2. Iron wool heated to glowing red reacts vigorously with chlorine gas in a flask. The product is red-brown solid iron(III) chloride 2Fe + 3Cl 2 2FeCl 3

3. Iron ions in solution will react with hydroxide ions to form iron hydroxides which are insoluble and very coloured Fe 2+ (aq) + 2OH - (aq) Fe(OH) 2(s) (“dirty green”) Fe 3+ (aq) + 3OH - (aq) Fe(OH) 3(s) (“rusty brown”)

4. Copper will dissolve in concentrated nitric acid to form copper nitrate and brown nitrogen dioxide gas Cu(s) + 4HNO 3 (aq) Cu(NO 3 ) 2 (aq) + 2NO 2 (g) + 2H 2 O(l)

5. copper(II) oxide is a base (does not dissolve in water) copper hydroxide is pale blue and is formed when sodium hydroxide is added to a copper salt. It us used as a test for copper.

6. Anhydrous copper sulphate is white and hydrated copper sulphate is blue (reversible) Copper carbonate decomposes at high temperatures to form copper oxide and carbon dioxide. CuCO 3 (s) → CuO (s) + CO 2 (g)

7. Copper chloride is light green There are copper(I) compounds such as copper(I) oxide

8. copper(II) ions react with ammonia to form the following complex ion (copy carefully!) [Cu(H 2 O) 2 (NH 3 ) 4 ] 2+

9. Copper and iron are typical transition metals Variable valency (ions with different charges) Coloured compounds Metals and their compounds make good catalysts Properties of variable valency Typical metals (high m.p., dense, conduct, ductile, malleable etc.)