Chemistry Themed MATERIALS Part 2 Reactivity of Metals and Redox

Size: px
Start display at page:

Download "Chemistry Themed MATERIALS Part 2 Reactivity of Metals and Redox"

Transcription

1 Chemistry Themed MATERIALS Part 2 Reactivity of Metals and Redox

2 2

3 Chemistry in the Community Materials: Reactivity of Metals and Redox W 10/5 Balancing Quiz Demo AgNO 3 + Cu and Cu(NO 3 ) 2 + Ag, pkt p 7 Animation: s/projectfolder/flashfiles/redox/aqueous.swf Close toed shoes for Tuesday! R 10/6 Lab: Relative Reactivity of Metals pkt p 8 Complete Lab Questions as a class on pkt p 9-11 Read and Take notes on Section B.13 p from textbook pkt p 13 Read C.1 textbook p. 83 and C.2 textbook p Take notes on pkt p F 10/7 Finish pkt p 9-11 Activity Series Worksheet pkt p 12 Where do we get our metals? DEMO ores, pkt p 15 Brief Cu Unlimited Discussion M 10/10 Columbus Day: No School T 10/11 Discuss C.1 and C.2 Sources of Metals (factors that influence feasibility) pkt p C.10 Mining and Refining Note Sheet, pkt p W 10/12 Mining and Refining Note Sheet, pkt p Oxidation/Reduction Extra Practice! Pkt p 18 Complete Oxidation/Reduction Extra Practice Pkt p 18 Read/Notes C.13 textbook p pkt p 20 R 10/13 Review Redox and pkt p 18 Electroplating Demo pkt p 21 Complete Summary Questions Sect B p. 79 #26-28 Summary Questions Sect C p #3-11, 23-29, 32, 35, 39 F 10/14 End of 1 st Quarter M 10/17 Discuss Summary Questions Real Life Practice Problems pkt p TEST on Reactivity of Metals and Redox! Study for test! 3

4 4

5 Chemistry Name: Period: Materials Unit: Reactivity of Metals and Redox Objectives Checklist My action plan to help me improve my learning includes: Review labs, notes, packet and activities. Use the calendar to make sure everything is reviewed. Have a family member or friend quiz me orally. Meet with my teacher in the morning/afterschool for extra help. Use the magic calculator online to check your calculation answers to appropriate labs. Complete and review homework problems by reworking them and NOT just looking at them. Use Objective Checklist throughout unit to assess understanding Ask and answer questions during class. Start studying early! (Not just the night before the test.) Re-read or review all assigned sections from the book. Do online practice quizzes available through class website or through internet. Find a study buddy from Chemistry who understands the material and I can work well with. Use Objective Checklist as a study guide Use this checklist as your personal guide to assess your level of readiness for quizzes and the unit test. Circle the descriptor that best describes how you feel about your mastery of each objective. NOTE: IF IT IS NOT A, YOU PROBABLY ARE NOT READY FOR THE QUIZ/TEST!!!!! = I get it? = I need more practice/review! = I need to get help During Unit Before Test (An asterisk indicates an overarching theme from a past unit!) I feel confident that I?!?! 1. understand what an ore is and what conditions make it profitable to mine for it.?!?! 2. understand what an activity series is and how to use it.?!?! 3. can define and recognize oxidation and reduction reactions.?!?! 4. can identify oxidized and reduced substances in a REDOX reaction.?!?! 5. can identify oxidizing agent and reducing agent in a REDOX reaction.?!?! 6. understand electrolysis.?!?! 7. understand the difference between hydro and electrometallurgy. Check off the study skills you USED to move from? or! to while studying for the test. I have carefully self-assessed my work during this unit and have taken steps to get my questions answered before the quiz/test. Student Signature: Parent Signature: Date: 5

6 6

7 Chemical Reactions and Balanced Equations: Balance the following equations, then watch your teacher perform the chemical reactions and record your observations. 1. Cu (s) + AgNO3 (aq) Ag(s) + Cu(NO3)2(aq) Observations: 2. Ag(s) + Cu(NO3)2(aq) AgNO3 + Cu(s) Observations: CONCLUSION: 7

8 RELATIVE REACTIVITY OF METALS PURPOSE: To generate an activity series (which is a ranking of the relative reactivities of different metals) based on data gathered in the lab. To explain the significance of an activity series for a chemist BACKGROUND INFORMATION: (as a class) What is an Activity Series? PROCEDURE: You will be given three different metal samples: Mg, Cu and Zn. You will test whether or not each metal will react with four different solutions: Mg(NO3)2, Cu(NO3)2, Zn(NO3)2 and AgNO3. AgNO3 - stains hands and clothes. Place a small sample of each metal in a well plate as indicated below. Add ~ 5 drops of each solution as indicated. RECORD if a reaction occurs (record what you see) or if a reaction does not occur (record as NR or No Reaction). Mg Mg(NO3)2 Cu(NO3)2 Zn(NO3)2 AgNO3 Cu Zn NOTE: You should see a total of 6 reactions, so be patient!!! No two metals should react with the same number of solutions. WASTE: dump the contents of your wellplate into the garbage can. (NO SOLIDS DOWN THE DRAIN!) Wipe out any excess with another paper towel and throw in the trash. 8

9 QUESTIONS: 1. Which metal reacted with the most solutions? 2. Which metal reacted with the least solutions? 3. Create an Activity Series from the three metals tested. CLASS DISCUSSION 4. Hypothesize the reactivity of silver metal with EACH of the solutions used in this lab. USE ONLY YOUR DATA to explain your answer. Mg Mg(NO3)2 Cu(NO3)2 Zn(NO3)2 AgNO3 Cu Zn Ag 9

10 5. List the metals (INCLUDING SILVER) in order, placing the MOST reactive metal first and the least reactive metal last. This is your Activity Series. 6. Using the activity series, why do you think the outside of a penny is made of Cu and not Zn? 7. Which of the four metals mentioned in this lab might be an even better choice than copper for the outside of a penny? Why? Why do you think this metal is not used for that purpose? 8. Given your new knowledge about the relative chemical activities of these four metals, which metal is most likely to found in an uncombined or "free" state in nature? 9. Which metal is least likely to found in an uncombined or "free" state in nature? 10. Using the activity series on the page 15 and your data, state a general rule which would allow you to predict when a metal and an ionic solution would react. 10

11 Practice Problems: 1. Will a sample of calcium metal react with a solution of silver nitrate? 2. Will a sample of lead metal react with a solution of magnesium nitrate? 3. Write out a complete balanced equation for either of the two questions above. 11

12 Activity Series Worksheet For each set of reactants below: Write out the proper formulas Use the Activity Series on the previous page to determine if a reaction will occur. o If NO reaction, write out NR o If there is a reaction, write out the reaction as a complete balanced equation. 1. Lithium and aluminum hydroxide 2. Magnesium and sodium chloride 3. Mercury and zinc nitrate 4. Calcium and zinc nitrate 5. Potassium and lithium nitrate 12

13 Take notes on textbook pages below. Section B.13 Notes 13

14 Read Section C.1 (textbook p. 83) and C.2 (textbook p 86-88) Answer the following questions: Sec C.1 1. Name 5 metals that have been used in coins. Include their chemical symbol and atomic number. Sec C.2 2. Where do we find the greatest source of chemical resources? 3. What is an ore? 4. What is a mineral? 5. What is the apple analogy that describes where the majority of earth's resources are located? 6. What is the relationship between a nations' supply of national resources and its land area and population? 7. What metals does South Africa supply more than any other country? What country is the top supplier of Copper? 8. What must be considered when determining of it is worthwhile to mine a certain metallic ore? 9. What physical properties make copper the most common metal for electrical wiring? What chemical property makes copper the most common metal for electrical wiring? 10. What percentage of an ore needs to be copper to make it economically profitable to mine it for copper? 14

15 C.10 Mining and Refining Demo Ores. Brief Description of Unit Project: Copper Unlimited As a class, you will function as a mining company to determine the best way to refine a sample of a copper containing ore. 1. What does refining mean? 2. When copper miners find the ore, what form will the copper be in? 3. How does a mining company turn ionic copper into copper atoms (the solid metal)? Explain in words and in the form of a chemical equation. Is this a gain or a loss of electrons by the ionic copper? 4. Define Reduction. Where do you think the term reduction came from? 5. What is the reverse reaction of reduction?. Define this term. 6. How did this term come about? 7. What is the most common oxidation reaction that can occur with iron, copper, silver and most metals? Is this a gain or a loss of electrons by the metal atoms? 8. True or False: Oxidation can occur without reduction. 9. Oxidation-reduction reactions are commonly called reactions. 15

16 10. TRUE OR FALSE: Electrical charges must be balanced in a REDOX reaction. 11. What is a reducing agent? 12. What is an oxidizing agent? 13. Define: a. Electrometallurgy b. Pyrometallurgy c. Hydrometallurgy pneumonic devices to choose from! Pick your favorite! OIL RIG: LEO GER: 16

17 15. In the following reactions, identify what has been oxidized and what has been reduced. Be specific! To do this, you must first determine the charge on all atoms/ions in the equation. a. Cu(s) + 2 Ag + Cu +2 (aq) + 2 Ag(s) b. Cu +2 (aq) + Mg(s) Cu(s) + Mg +2 (aq) c. 3 Ca(s) + 2 AlCl3 (aq) 3 CaCl2 (aq) + 2 Al(s) d. 2 K(s) + PbI2 (aq) 2 KI(aq) + Pb(s) e. 2 Li(s) + Cl2 (g) 2 LiCl(s) 16. Identify the reducing agent and oxidizing agent in the above reactions. 17. What is the pattern? 17

18 Oxidation/Reduction Extra Practice Problems!! For each equation below: Indicate the charge on each atom/ion Indicate which atom/ion is oxidized.. Write the oxidation half reaction. Indicate which atom/ion is reduced. Write the reduction half reaction. Identify both the oxidizing agent and reducing agent. 1. Zn (s) + HgO (aq) ZnO (aq) + Hg (l) (note: (l) stands for liquid) 2. Mg (s) + ZnCl2 (aq) Zn (s) + MgCl2 (aq) 3. Ca (s) + FeO (aq) CaO (aq) + Fe (s) 4. Be (s) + MnBr2 (aq) Mn (s) + BeBr2 (aq) 18

19 19

20 Read Section C.13 (textbook p ) and define the following key terms Electroplating Half-reaction Example: Cathode Anode 20

21 Electrolysis of copper chloride solution 1. This diagram shows the electrolysis of copper chloride solution. What are labels (a) to (e)? Choose from the words from the box. anode bubbles of gas copper copper chloride solution copper ions 2. a. Why are the chloride ions attracted to the anode? b. What happens to the chloride ions when they reach the anode? Explain in as much detail as you can. c. Are the chloride ions oxidized or reduced at the anode? 3. a. What happens to the copper ions when they reach the cathode? Explain in as much detail as you can. b. Are the copper ions oxidized or reduced at the cathode? 4. Why is a solid formed at the cathode but a gas at the anode? 5. Look at this list of ions (below). For each one write down which electrode it will attracted to and if it will be oxidized or reduced? (a) Pb 2+ (b) Br - (c) Al 3+ (d) O 2- (e ) Ag + (f) I - 21

22 REAL LIFE PRACTICE PROBLEMS Imagine that you were hired by a company that wanted you to produce some solid aluminum from an aluminum containing ore. The mineral in the ore is aluminum chloride. 1. What is the formula of aluminum chloride? 2. During this unit, we used two different processes to produce solid metals. What were they? When recovering a metal using hydrometallurgy, the mineral in the ore must be dissolved in a water based solution. The following process can be used: a. Crush the ore b. Add the crushed ore to a solution that will dissolve the mineral. (often times, the mineral will dissolve in pure water). c. Filter the rock away from the dissolved mineral. d. Now, the mineral is in an aqueous solution and ready for hydrometallurgy, which is simply adding a more reactive metal. 3. Determine two different metals that could be used to recover the aluminum. Choose one of your two metals and do the following: Write a complete, balanced equation for the reaction (include all states of matter): What was oxidized? What was reduced? Oxidation ½ reaction: Reduction ½ reaction: Reducing agent Oxidizing agent: 22

23 4. Another way to recover the aluminum is through electrometallurgy. Label the following on the diagram below: Anode Cathode Aluminum (solid) Aluminum ions, Chlorine (gas) Chloride ions Write the correct ½ reaction that is occurring at the anode. Write the correct ½ reaction that is occurring at the cathode. 23

24 Flame Test Lab PURPOSE: To show how different elements burn different colors for use in fireworks. BACKGROUND INFORMATION: A flame test is a method for identifying certain elements. The solid is heated in a flame and emits a characteristic color. The flame excites atoms and the increased energy is absorbed by electrons which are forced into higher energy levels. The atom is now unstable since the lower levels do not have complete configurations so the electron falls back down to its original energy level emitting the released energy as light. Safety: Close Toed shoes and goggles. Tie long hair back. PROCEDURE: 1. For each solid sample, take a water soaked wooden split and dip it into the container with the sample. Do not scoop up a sample! 2. Hold the sample in the blue cone of the Bunsen burner flame. Observe and RECORD the color of the flame. Be as specific as you can. 3. Rinse wooden splint under running water from faucet and throw away. 4. Wipe off counter!!! DATA: SUBSTANCE COLOR OF FLAME Sodium Chloride Copper (II) Chloride Sodium Bicarbonate Potassium Iodide Strontium Chloride 24

25 25

26 26

27 27

Oxidation and Reduction

Oxidation and Reduction Oxidation and Reduction An oxidation reaction is one in which oxygen is added to a substance. Example: Methane is oxidised when it burns in air. Oxygen is added to the carbon in methane, forming carbon

More information

[ Cl ] - [[Mg 2+ ] ] Experiment 7: Oxidation-Reduction Reactions. transfer e -

[ Cl ] - [[Mg 2+ ] ] Experiment 7: Oxidation-Reduction Reactions. transfer e - Experiment 7: OxidationReduction Reactions PURPOSE Become familiar with the concepts of oxidation and reduction and how these reactions occur. Carry out several such reactions and learn to recognize when

More information

TYPES OF CHEMICAL REACTIONS PART I INTRODUCTION

TYPES OF CHEMICAL REACTIONS PART I INTRODUCTION EXPERIMENT 10 (2 Weeks) Chemistry 100 Laboratory TYPES OF CHEMICAL REACTIONS PART I INTRODUCTION It is useful to classify reactions into different types, because products of reactions can be predicted.

More information

(a) To find out which is the more reactive metal, zinc or tin, the following experiment could be carried out. piece of zinc shiny surface

(a) To find out which is the more reactive metal, zinc or tin, the following experiment could be carried out. piece of zinc shiny surface 1 The reactivity series lists metals in order of reactivity. (a) To find out which is the more reactive metal, zinc or tin, the following experiment could be carried out. piece of zinc shiny surface tin(ii)

More information

TWEED RIVER HIGH SCHOOL 2006 PRELIMINARY CHEMISTRY. Unit 2 Metals

TWEED RIVER HIGH SCHOOL 2006 PRELIMINARY CHEMISTRY. Unit 2 Metals TWEED RIVER HIGH SCHOOL 2006 PRELIMINARY CHEMISTRY Unit 2 Metals Part 2 Metals differ in their reactivity with other chemicals and this influences their uses. Describe observable changes when metals react

More information

6 METALS & NON METALS

6 METALS & NON METALS Grade-8 Chemistry Chapter- 6 METALS & NON METALS 1. What happens in each of the following cases? a) Magnesium is burnt in oxygen. Ans: When magnesium burns in oxygen it produces magnesium oxide with dazzling

More information

Boiling point in C. Colour in aqueous solution. Fluorine 188 colourless. Chlorine 35 pale green. Bromine X orange.

Boiling point in C. Colour in aqueous solution. Fluorine 188 colourless. Chlorine 35 pale green. Bromine X orange. Q1.This question is about halogens and their compounds. The table below shows the boiling points and properties of some of the elements in Group 7 of the periodic table. Element Boiling point in C Colour

More information

There s also got to be a wire, but that s kind of taken for granted.

There s also got to be a wire, but that s kind of taken for granted. RedOx Pt 2 Electrochemical Cells (AKA simple batteries) An electrochemical cell has 3 major components: 1. The Cathode (and it s corresponding solution) 2. The Anode (and it s corresponding solution) 3.

More information

Suggest one reason why spoons are electroplated. ... Why is hydrogen produced at the negative electrode and not sodium?

Suggest one reason why spoons are electroplated. ... Why is hydrogen produced at the negative electrode and not sodium? Q1.This question is about electrolysis. (a) Metal spoons can be coated with silver. This is called electroplating. Suggest one reason why spoons are electroplated. (b) When sodium chloride solution is

More information

ADVANCED AP PLACEMENT CHEMISTRY. Activity Series. Introduction. Objective. Chemicals and Equipment

ADVANCED AP PLACEMENT CHEMISTRY. Activity Series. Introduction. Objective. Chemicals and Equipment ADVANCED AP PLACEMENT CHEMISTRY Introduction Activity Series An activity series of metals is a table of metals arranged in the order of their decreasing chemical activity or the ease at which the metal

More information

Which of these is the formula for disulfur heptoxide? A. S 2 O 7 B. S 7 O 2 C. SO 2 D. N 2 O

Which of these is the formula for disulfur heptoxide? A. S 2 O 7 B. S 7 O 2 C. SO 2 D. N 2 O Which of these is the formula for disulfur heptoxide? A. S 2 O 7 B. S 7 O 2 C. SO 2 D. N 2 O Which of these is the correct chemical formula for a molecule of oxygen? A. O B. O -2 C. O +2 D. O 2 Which of

More information

Electricity and Chemistry

Electricity and Chemistry Electricity and Chemistry Electrochemistry: It is a branch of chemistry that deals with the reactions involving the conversion of chemical energy into electrical energy and vice-versa. Electrochemical

More information

EXTRA CREDIT - EXPERIMENT G ELECTROCHEMISTRY ACTIVITY OF METALS

EXTRA CREDIT - EXPERIMENT G ELECTROCHEMISTRY ACTIVITY OF METALS EXTRA CREDIT - EXPERIMENT G ELECTROCHEMISTRY ACTIVITY OF METALS INTRODUCTION The objective of this experiment is to develop an abbreviated activity series of metals using: 1. Displacement reactions 2.

More information

Equation Writing and Predicting Products Chemistry I Acc

Equation Writing and Predicting Products Chemistry I Acc Introduction: Equation Writing and Predicting Products Chemistry I Acc If you examine your bicycle after it has been left out in the rain a number of times you will find that it has begun to rust. Rust

More information

5-4 Chemical changes Trilogy

5-4 Chemical changes Trilogy 5-4 Chemical changes Trilogy.0 A student investigated the reaction of sodium carbonate with dilute hydrochloric acid. The student used the apparatus shown in Figure. Figure Sodium carbonate This is the

More information

Edexcel GCSE Chemistry. Topic 4: Extracting metals and equilibria. Obtaining and using metals. Notes.

Edexcel GCSE Chemistry. Topic 4: Extracting metals and equilibria. Obtaining and using metals. Notes. Edexcel GCSE Chemistry Topic 4: Extracting metals and equilibria Obtaining and using metals Notes 4.1 Deduce the relative reactivity of some metals, by their reactions with water, acids and salt solutions

More information

Periodic Trends and the Properties of Elements The Alkaline Earth Metals

Periodic Trends and the Properties of Elements The Alkaline Earth Metals Introduction Periodic Trends and the Properties of Elements The Alkaline Earth Metals The periodic table is the most recognized symbol of chemistry across the world. It is a valuable tool that allows scientists

More information

METALS AND THEIR COMPOUNDS

METALS AND THEIR COMPOUNDS METALS AND THEIR COMPOUNDS Metals are elements whose atoms ionize by electron loss, while non-metals are elements whose atoms ionize by electron gain. Metals are in groups 1, 2 and 3 of the periodic table.

More information

INTRODUCTION TO ELECTROCHEMISTRY: CURRENT, VOLTAGE, & BATTERIES. Introduction. Electrochemistry Revised 4/28/14

INTRODUCTION TO ELECTROCHEMISTRY: CURRENT, VOLTAGE, & BATTERIES. Introduction. Electrochemistry Revised 4/28/14 INTRODUCTION TO ELECTROCHEMISTRY: CURRENT, VOLTAGE, & BATTERIES Introduction Electrochemical Cells In this part of the experiment, four half cells are created by immersing metal strips of zinc, copper,

More information

One of the main ores of zinc is zinc blende, ZnS. There are two stages in the extraction of zinc from this ore.

One of the main ores of zinc is zinc blende, ZnS. There are two stages in the extraction of zinc from this ore. 1 Two of the main uses of zinc are for galvanising and for making alloys. One of the main ores of zinc is zinc blende, ZnS. There are two stages in the extraction of zinc from this ore. (a) Stage 1 Zinc

More information

Compounds & Reactions Week 1. Writing Formulas & Balancing Equations. Write the chemical formula for each molecular (covalent) compound.

Compounds & Reactions Week 1. Writing Formulas & Balancing Equations. Write the chemical formula for each molecular (covalent) compound. Compounds & Reactions Week 1 Name Writing Formulas & Balancing Equations Write the chemical formula for each ionic compound. 1. Lithium fluoride 2. Copper (II) chloride 3. Manganese (II) oxide 4. Potassium

More information

85 Q.51 Which of the following carbonates would give the metal when heated with carbon? (1) MgCO 3 (2) PbCO 3 (3) K 2 CO 3 (4) CuCO 3

85 Q.51 Which of the following carbonates would give the metal when heated with carbon? (1) MgCO 3 (2) PbCO 3 (3) K 2 CO 3 (4) CuCO 3 Metal and metal reactivity / Section 2 / Sect2pp.doc / S. W. Tse / P.1 85 Q.51 Which of the following carbonates would give the metal when heated with carbon? (1) MgCO 3 (2) PbCO 3 (3) K 2 CO 3 (4) CuCO

More information

Properties A Metal B Non- metal Electronic configuration?? Nature of oxides?? Oxidizing or reducing action?? Conduction of heat and electricity??

Properties A Metal B Non- metal Electronic configuration?? Nature of oxides?? Oxidizing or reducing action?? Conduction of heat and electricity?? CLASS: X NCERT (CBSE) SCIENCE: Chemistry Page: 1 Question 1: Compare the properties of a typical metal and a non-metal on the basis of the following. Fill in Column A, B. Properties A Metal B Non- metal

More information

Combination Reactions 2H 2 + O 2 2H 2 O. 2Na + I 2 2NaI. Ca + Cl 2 CaCl 2. C + O 2 CO 2 or 2C + O 2 2CO 3H 2 + N 2 2NH 3

Combination Reactions 2H 2 + O 2 2H 2 O. 2Na + I 2 2NaI. Ca + Cl 2 CaCl 2. C + O 2 CO 2 or 2C + O 2 2CO 3H 2 + N 2 2NH 3 Combination Reactions Predict the product and write balanced reactions for each of the following. 1. Hydrogen burned in oxygen. 2H 2 + O 2 2H 2 O 2. Sodium plus iodine. 2Na + I 2 2NaI 3. Calcium burned

More information

Partner: Cathy 22 March Separation and Qualitative Determination of Cations and Anions

Partner: Cathy 22 March Separation and Qualitative Determination of Cations and Anions Partner: Cathy 22 March 2012 Separation and Qualitative Determination of Cations and Anions Purpose: The purpose of this lab is to identify the cations and anions components in the unknown solution. This

More information

Periodic Trends and the Properties of Elements

Periodic Trends and the Properties of Elements Page 1 - The Alkaline Earth Metals Introduction The periodic table is the most recognized symbol of chemistry across the world. It is a valuable tool that allows scientists not only to classify the elements

More information

Covered with a thin layer of oxide at ordinary temperatures.

Covered with a thin layer of oxide at ordinary temperatures. 1 More about Metals Physical properties of metals In general metals have luster, are malleable and ductile, good conductors of heat and electricity and have high boiling and melting points and nonmetals

More information

Iron filings (Fe) 56g IRON + SULPHUR IRON SULPHIDE

Iron filings (Fe) 56g IRON + SULPHUR IRON SULPHIDE W.S.51. Chemical reactions. All of the different materials around us have been formed by chemical reactions from about one hundred simple elements. The diagram below shows a chemical reaction between the

More information

APPLICATIONS OF ELECTROCHEMISTRY

APPLICATIONS OF ELECTROCHEMISTRY APPLICATIONS OF ELECTROCHEMISTRY SPONTANEOUS REDOX REACTIONS APPLICATIONS OF ELECTROCHEMICAL CELLS BATTERIES A galvanic cell, or series of combined galvanic cells, that can be used as a source of direct

More information

Periodic Trends. Introduction

Periodic Trends. Introduction Periodic Trends Introduction In the modern periodic table (shown below in Figure 1), elements are arranged according to increasing atomic number in horizontal rows called periods. In Figure 1, atomic numbers,

More information

Unit 5 Review Electrolytic, Electrochemical Cells, Corrosion, & Cathodic Protection

Unit 5 Review Electrolytic, Electrochemical Cells, Corrosion, & Cathodic Protection Unit 5 Review Electrolytic, Electrochemical Cells, Corrosion, & Cathodic Protection Determine the half reactions for each cell and the cell voltage or minimum theoretical voltage. 1. Zn / Mg electrochemical

More information

Nomenclature. A systematic method of writing chemical formulas and naming compounds

Nomenclature. A systematic method of writing chemical formulas and naming compounds Nomenclature A systematic method of writing chemical formulas and naming compounds Chemical symbols Symbols are used to represent elements Either one capital letter, or a capital letter with a lower case

More information

INDIAN SCHOOL MUSCAT SENIOR SECTION DEPARTMENT OF CHEMISTRY CLASS X- PRACTICAL WORKSHEET

INDIAN SCHOOL MUSCAT SENIOR SECTION DEPARTMENT OF CHEMISTRY CLASS X- PRACTICAL WORKSHEET INDIAN SCHOOL MUSCAT SENIOR SECTION DEPARTMENT OF CHEMISTRY CLASS X- PRACTICAL WORKSHEET Different types of chemical reactions Experiment No: 1(a) Combination reaction Objectives: To study the Combination

More information

Formula & Equation Writing

Formula & Equation Writing Formula & Equation Writing Book 2 H H Al Al H Al(H) 3 H Ionic Equations Ionic Formulae Balanced Equations Formula Equations Word Equations Transition Metals Using Brackets Awkward Customers More than 2

More information

CRHS Academic Chemistry Unit 1 Matter and Change HOMEWORK. Due Date Assignment On-Time (100) Late (70)

CRHS Academic Chemistry Unit 1 Matter and Change HOMEWORK. Due Date Assignment On-Time (100) Late (70) Name KEY Period CRHS Academic Chemistry Unit 1 Matter and Change HOMEWORK Due Date Assignment On-Time (100) Late (70) 1.1 1.2 1.3 Warm Ups Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic

More information

Topic 2.7 EXTRACTION OF METALS. Extraction of Iron Extraction of Aluminium Extraction of Titanium Recycling

Topic 2.7 EXTRACTION OF METALS. Extraction of Iron Extraction of Aluminium Extraction of Titanium Recycling Topic 2.7 EXTRACTION OF METALS Extraction of Iron Extraction of Aluminium Extraction of Titanium Recycling EXTRACTING METALS FROM THEIR ORES Most metals do not occur native. They exist in compounds, usually

More information

*20GSD5201* Double Award Science: Chemistry. Unit C2 Higher Tier TUESDAY 9 JUNE 2015, AFTERNOON [GSD52] *GSD52* *G5802* TIME 1 hour 15 minutes.

*20GSD5201* Double Award Science: Chemistry. Unit C2 Higher Tier TUESDAY 9 JUNE 2015, AFTERNOON [GSD52] *GSD52* *G5802* TIME 1 hour 15 minutes. Centre Number Candidate Number General Certificate of Secondary Education 2015 Double Award Science: Chemistry Unit C2 Higher Tier [GSD52] *GSD52* *G5802* *GSD52* TUESDAY 9 JUNE 2015, AFTERNOON TIME 1

More information

Today! Demonstrations of Redox Chemistry! Electrochemistry! electrons moving about! equilibrium with a control knob! The disappearing Aluminum Rod!

Today! Demonstrations of Redox Chemistry! Electrochemistry! electrons moving about! equilibrium with a control knob! The disappearing Aluminum Rod! Today! Electrochemistry! electrons moving about! equilibrium with a control knob! Redox chemistry! oxidation and reduction! Demonstrations of Redox Chemistry! The disappearing Aluminum Rod! Alkali Metals

More information

March Chemistry Project v3. Chemistry Project

March Chemistry Project v3. Chemistry Project Chemistry Project Investigate and compare the quantitative effects of changing (a) metal types and (b) fruit/vegetable type on the emf (voltage) produced across two different metals, when the electrolytes

More information

SOLUBILITY STUDY GUIDE- Multiple Choice Section

SOLUBILITY STUDY GUIDE- Multiple Choice Section SOLUBILITY STUDY GUIDE- Multiple Choice Section Multiple Choice Section: This study guide is a compilation of questions from provincial exams since 2000. I urge you to become intimately familiar with question

More information

ELECTROCHEMISTRY: ELECTROPLATING

ELECTROCHEMISTRY: ELECTROPLATING ELECTROCHEMISTRY: ELECTROPLATING Hello, I m Hafizah, a chemistry teacher from Muar Science School in Malaysia. We are going to discuss about an interesting chemistry topic related to electroplating but

More information

Metals and Non-metals

Metals and Non-metals CHAPTER 3 Metals and Non-metals In Class IX you have learnt about various elements. You have seen that elements can be classified as metals or non-metals on the basis of their properties. Think of some

More information

NOMENCLATURE (ie naming compounds)

NOMENCLATURE (ie naming compounds) NOMENCLATURE (ie naming compounds) An ionic compounds (salt) may be any one of thousands of chemical compounds How do chemists describe which salt they are discussing? There is a system that we will follow

More information

Copper Odyssey. Chemical Reactions of Copper

Copper Odyssey. Chemical Reactions of Copper Name Lab Partner(s) Copper Odyssey Chemical Reactions of Copper Date Period Elemental copper metal will be converted into copper (II) ion and then brought through a series of compound conversions until

More information

AP Chemistry Reaction Set

AP Chemistry Reaction Set Class: Date: AP Chemistry Reaction Set 2008-2009 Other 1. Sulfur trioxide gas is bubbled into a solution of sodium hydroxide. (2005) 2. Hydrogen iodide gas is bubbled into a solution of lithium carbonate.

More information

Chapter 5. Oxidation Reduction Chemistry

Chapter 5. Oxidation Reduction Chemistry Chapter 5. Oxidation and Reduction Redox Terminology Oxidation Number Rules Determination of Oxidation Numbers from Electronegativities The Difference Between Oxidation Number and Formal Charge Periodic

More information

METALS AND NON-METALS

METALS AND NON-METALS METALS AND NON-METALS VERY SHORT ANSWER TYPE QUESTIONS [1 MARK] 1. A green layer is gradually formed on a copper plate left exposed to air for a week in a bathroom. What could this green substance be?

More information

Metals. Teacher Notes. Registered Charity Number

Metals. Teacher Notes.  Registered Charity Number Metals Teacher Notes Metals is funded as part of the Reach and Teach educational programme supported by the Wolfson Foundation THE WOLFSON FOUNDATION www.rsc.org Registered Charity Number 207890 Metals

More information

Introduction to Metallurgy

Introduction to Metallurgy Metallurgy Introduction to Metallurgy Metallurgy deals with extraction and purification of metals from their sources. Very few metals like gold, silver etc. occur in native state, while most other metals

More information

GENARAL INTRODUCTION TO METALLURGY :Std: XI-CHEMISTRY

GENARAL INTRODUCTION TO METALLURGY :Std: XI-CHEMISTRY GENARAL INTRODUCTION TO METALLURGY :Std: XI-CHEMISTRY 1. What is matrix? The ore is generally associated with rock impurities like clay, sand etc. called gangue or matrix 2. What is mineral? The natural

More information

Chapter 20 CHEMISTRY. Metallurgy and the Chemistry of Metals. Dr. Ibrahim Suleiman

Chapter 20 CHEMISTRY. Metallurgy and the Chemistry of Metals. Dr. Ibrahim Suleiman CHEMISTRY Chapter 20 Metallurgy and the Chemistry of Metals Dr. Ibrahim Suleiman GENERAL PROPERTIES AND STRUCTURE OF METALS opaque good conductors of heat and electricity high malleability and ductility

More information

CONSERVATION OF MATTER AND CHEMICAL PROPERTIES

CONSERVATION OF MATTER AND CHEMICAL PROPERTIES 1 CONSERVATION OF MATTER AND CHEMICAL PROPERTIES I. OBJECTIVES AND BACKGROUND The object of this experiment is to demonstrate the conservation of matter- or more particularly, the conservation of "atoms"

More information

AP Chemistry Reaction Set

AP Chemistry Reaction Set Class: Date: AP Chemistry Reaction Set 2009-2010 Other 1. Pure solid phosphorus (white form) is burned in air. (2002) 2. Sulfur dioxide gas is bubbled into distilled water. (2001) 3. A drop of potassium

More information

New GCSE 4462/02 SCIENCE A HIGHER TIER CHEMISTRY 1

New GCSE 4462/02 SCIENCE A HIGHER TIER CHEMISTRY 1 Surname Other Names Centre Number 0 Candidate Number New GCSE 4462/02 SCIENCE A HIGHER TIER CHEMISTRY 1 ADDITIONAL MATERIALS A.M. WEDNESDAY, 18 January 2012 1 hour In addition to this paper you may require

More information

DETERMINATION of the EMPIRICAL FORMULA

DETERMINATION of the EMPIRICAL FORMULA DETERMINATION of the EMPIRICAL FORMULA One of the fundamental statements of the atomic theory is that elements combine in simple whole number ratios. This observation gives support to the theory of atoms,

More information

F321: Atoms, Bonds and Groups Group 2

F321: Atoms, Bonds and Groups Group 2 F321: Atoms, Bonds and Groups Group 2 87 Marks 1. Magnesium and strontium are in Group 2 of the Periodic Table. When reacted with oxygen, magnesium forms a white powder called magnesium oxide. Write the

More information

2015 O LEVEL CHEMISTRY 5073/02

2015 O LEVEL CHEMISTRY 5073/02 OF SCIENCE 2015 O LEVEL CHEMISTRY 5073/02 SECTION A 1. The table shows some common oxidation states for some elements in their compounds. element common oxidation states metal / non-metal A 2 non-metal

More information

Nickel Electroplating

Nickel Electroplating Nickel Electroplating In a galvanic or voltaic electrochemical cell, the spontaneous reaction occurs and electrons flow from the anode (oxidation) to the cathode (reduction). In an electrolytic cell, a

More information

5072 CHEMISTRY (NEW PAPERS WITH SPA) TOPIC 9: METALS 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) TOPIC 9: METALS

5072 CHEMISTRY (NEW PAPERS WITH SPA) TOPIC 9: METALS 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) TOPIC 9: METALS 5072 CHEMISTRY (NEW PAPERS WITH SPA) TOPIC 9: METALS 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) TOPIC 9: METALS SUB-TOPIC 9.3 TO 5 EXTRACTION OF METALS; RECYLING OF METALS; IRON LEARNING OUTCOMES

More information

look down at cross on paper paper cross on paper

look down at cross on paper paper cross on paper 1 The equation for the reaction between sodium thiosulfate and hydrochloric acid is given below. Na 2 S 2 O 3 (aq) + 2HCl (aq) 2NaCl (aq) + S(s) + SO 2 (g) + H 2 O(l) The speed of this reaction was investigated

More information

NCEA Level 1 Chemistry (90933) 2012 page 1 of 5. Q Evidence Achievement Achievement with Merit Achievement with Excellence NØ N1 N2 A3 A4 M5 M6 E7 E8

NCEA Level 1 Chemistry (90933) 2012 page 1 of 5. Q Evidence Achievement Achievement with Merit Achievement with Excellence NØ N1 N2 A3 A4 M5 M6 E7 E8 Assessment Schedule 2012 NCEA Level 1 Chemistry (90933) 2012 page 1 of 5 Chemistry: Demonstrate understanding of aspects of selected elements (90933) Evidence Statement Q Evidence with Merit with Excellence

More information

Method (0.1 to 8.0 mg/l Cu) TNTplus 860

Method (0.1 to 8.0 mg/l Cu) TNTplus 860 Chlorine, Total, Bulk Powder, 8167 DOC316.53.01255 Bathocuproine Method 1 Method 10238 (0.1 to 8.0 mg/l Cu) TNTplus 860 Scope and Application: For water, wastewater and process water. Digestion may be

More information

AP*Chemistry Solubility Equilibria

AP*Chemistry Solubility Equilibria AP*Chemistry Solubility Equilibria SOLUBILITY EQUILIBRIA (K sp, THE SOLUBILITY PRODUCT) Saturated solutions of salts are another type of chemical equilibria. Remember those solubility rules? The fine print

More information

ATOM STRUCTURE AND BONDING OF METALS

ATOM STRUCTURE AND BONDING OF METALS ATOM STRUCTURE AND BONDING OF METALS The atom is composed of a small, central nucleus, which contains protons and neutrons. Shells, or energy levels of electrons surround this nucleus. These electrons

More information

Copper Smelting by an Ancient Method

Copper Smelting by an Ancient Method Copper Smelting by an Ancient Method EXPERIMENT ## Prepared by Paul C. Smithson, Berea College, based on Yee et al., 004 Using beads of a copper-containing mineral, students will produce beads of nearly

More information

What is Electroplating?

What is Electroplating? Electroplating 1 What is Electroplating? An electrochemical process where metal ions are transferred from a solution and are deposited as a thin layer onto surface of a cathode. The setup is composed DC

More information

Energy From Electron Transfer. Chemistry in Context

Energy From Electron Transfer. Chemistry in Context Energy From Electron Transfer Chemistry in Context Energy Types Batteries Hybrid Cars (Electrical) H 2 (and Other) Fuel Cells Solar Fuel Cell Car Demo H 2 Fuel Cell Reactions Step 1: H 2 (g) 2H + (aq)

More information

Name Honors Chemistry / /

Name Honors Chemistry / / Name Honors Chemistry / / SOL Questions Chapter 1 Each of the following questions below appeared on an SOL Chemistry Exam. For each of the following bubble in the correct answer on your scantron. 1. The

More information

A TEACHER-DIRECTED, GUIDED DISCOVERY ACTIVITY FOR ADVANCED PHYSICAL SCIENCE STUDENTS

A TEACHER-DIRECTED, GUIDED DISCOVERY ACTIVITY FOR ADVANCED PHYSICAL SCIENCE STUDENTS A TEACHER-DIRECTED, GUIDED DISCOVERY ACTIVITY FOR ADVANCED PHYSICAL SCIENCE STUDENTS 1 2 FEATURES OF THIS ACTIVITY Problem solving Cooperative learning Requires student reasoning Requires student initiative

More information

Extracting and using metals. ores. native. Only the most unreactive metals such as gold and platinum are found as native metals.

Extracting and using metals. ores. native. Only the most unreactive metals such as gold and platinum are found as native metals. Extracting and using metals Only the most unreactive metals such as gold and platinum are found as native metals. ores All the other metals we use are extracted from their ores by chemical processes. native

More information

Ionic Bonding Drill. Compound Formula. tin (II) nitride. silver oxide. lithium sulfide. magnesium sulfide. copper (I) nitride.

Ionic Bonding Drill. Compound Formula. tin (II) nitride. silver oxide. lithium sulfide. magnesium sulfide. copper (I) nitride. tin (II) nitride silver oxide lithium sulfide magnesium sulfide copper (I) nitride boron iodide potassium fluoride potassium bromide sodium phosphide iron (II) chloride copper (I) bromide lead (II) sulfide

More information

Applications of electrochemistry

Applications of electrochemistry Applications of electrochemistry Electrochemistry has a number of different uses, particularly in industry. The principles of cells are used to makeelectrical batteries. In science and technology, a battery

More information

OC30 Conduct a qualitative experiment to detect the presence of dissolved solids in water samples, and test water for hardness (soap test)

OC30 Conduct a qualitative experiment to detect the presence of dissolved solids in water samples, and test water for hardness (soap test) Chemistry: 6. Water Please remember to photocopy 4 pages onto one sheet by going A3 A4 and using back to back on the photocopier Syllabus OC14 Use cobalt chloride paper or anhydrous copper sulfate to test

More information

Slide 1. Slide 2. Slide 3. Hardness. Concentration is. What s the concentration of red triangles? What s in your pipes? 500 ml

Slide 1. Slide 2. Slide 3. Hardness. Concentration is. What s the concentration of red triangles? What s in your pipes? 500 ml Slide 1 Hardness What s in your pipes? Slide 2 What s the concentration of red triangles? 500 ml 1 g 1 g 1 g A. 10 B. 10 C. D. 1 g 1 g It s all of the above! Slide 3 Concentration is any statement of the

More information

06. Electroplating Industry

06. Electroplating Industry PRTR Estimation Manual 06. Electroplating Industry January 2001 Revised: March 2002 Federation of Electro Plating Industry Association, Japan Contents 1. Class I Designated Chemical Substances (Referred

More information

Science Class 8 Topic: Elements And Compounds Reinforcement Worksheet

Science Class 8 Topic: Elements And Compounds Reinforcement Worksheet Science Class 8 Topic: Elements And Compounds Reinforcement Worksheet Name: Sec: Date: Q1.Choose the best answer. 1. Which of the following is an element? a) steam b) sugar c)dry ice d) sulphur 2. Which

More information

Warm Up (Sept 12) How will an atom change if you change the number of: a) Protons?

Warm Up (Sept 12) How will an atom change if you change the number of: a) Protons? Warm Up (Sept 12) How will an atom change if you change the number of: a) Protons? b) Electrons? c) Neutrons? 1 CH3OS Warm Up (Sept 13) 1. What is an isotope? 2. Neon has two major isotopes, Neon 20 and

More information

Chapter: The d and f Block Elements

Chapter: The d and f Block Elements Chapter: The d and f Block Elements Introduction to d block elements Question 1 In Tc ( Z = 43) and Tb( Z = 65) which one is inner transition metal and which one is transition metal and why? The outer

More information

Worksheet 5 - Naming Ionic Compounds Part 1 (Binary compounds with Group 1, 2 or 13 metals) Naming

Worksheet 5 - Naming Ionic Compounds Part 1 (Binary compounds with Group 1, 2 or 13 metals) Naming Worksheet 5 - Naming Ionic Compounds Part 1 (Binary compounds with Group 1, 2 or 13 metals) Binary compounds: have only two kinds of elements, if there are three or more it is not a binary compound. Naming

More information

INORGANIC CHEMISTRY LANTHANIDES

INORGANIC CHEMISTRY LANTHANIDES INORGANIC CHEMISTRY Topic: 5 LANTHANIDES LONG ANSWER QUESTIONS 1. What are the general characteristics of Lanthanides.. Ans: F BLOCK ELEMENTS The elements in which the differentiating electron enters the

More information

2.3 Chemical Changes corrosion Kinds of Corrosion

2.3 Chemical Changes corrosion Kinds of Corrosion 2.3 Chemical Changes Have you ever wondered why metal car bodies rust but plastic bumpers do not? As you know, different substances have different physical properties, such as colour and hardness, and

More information

Test sticks and test papers for semi-quantitative determinations

Test sticks and test papers for semi-quantitative determinations QUANTOFIX test sticks for semi-quantitative determinations QUANTOFIX test sticks meet the most important requirements for a modern quick-test: rapid dip and read convenient the analysis can be carried

More information

Chemistry 145 Exam number 4 name 11/19/98 # Faraday s constant is 96,500 c/mole of electrons.

Chemistry 145 Exam number 4 name 11/19/98 # Faraday s constant is 96,500 c/mole of electrons. Chemistry 145 Exam number 4 name 11/19/98 # Faraday s constant is 96,500 c/mole of electrons. A.(16) An electrochemical cell is prepared with a strip of manganese metal dipping in to a 1.0 M MnSO 4 solution

More information

Solutions Unit Exam Name Date Period

Solutions Unit Exam Name Date Period Name Date Period Ms. Roman Page 1 Regents Chemistry 1. Which mixture can be separated by using the equipment shown below? 6. Which ion, when combined with chloride ions, Cl, forms an insoluble substance

More information

Determination of the Empirical Formula of Magnesium Oxide

Determination of the Empirical Formula of Magnesium Oxide Determination of the Empirical Formula of Magnesium Oxide The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal. Magnesium

More information

Analysis of Calcium Carbonate Tablets

Analysis of Calcium Carbonate Tablets Experiment 9 Analysis of Calcium Carbonate Tablets Prepared by Ross S. Nord, Eastern Michigan University PURPOSE To perform a gravimetric exercise to determine weight percent of active ingredient in a

More information

1 Elements. TAKE A LOOK 2. Identify Look at the illustration and identify one source of iron that comes to Earth from somewhere else.

1 Elements. TAKE A LOOK 2. Identify Look at the illustration and identify one source of iron that comes to Earth from somewhere else. CHAPTER 4 1 Elements SECTION Elements, Compounds, and Mixtures BEFORE YOU READ After you read this section, you should be able to answer these questions: What is an element? How do elements differ from

More information

CHEM 1215 LAB NOTES EXPT #2: PHYSICAL AND CHEMICAL CHANGES 1

CHEM 1215 LAB NOTES EXPT #2: PHYSICAL AND CHEMICAL CHANGES 1 CHEM 1215 LAB NOTES EXPT #2: PHYSICAL AND CHEMICAL CHANGES 1 TECHNIQUES: chemical and physical changes, reactions, observations READING: PHYSICAL AND CHEMICAL CHANGES e.g. Tro chapter 1 SAFETY: Safety

More information

PO 4 NH 4 H + + SO 3

PO 4 NH 4 H + + SO 3 KEY TO AP CHEMISTRY EQUATIONS BY TYPE 196882, 198588, 199093, 1995 Double Replacement 1. Hydrogen sulfide is bubbled through a solution of silver nitrate. H 2 S + Ag 1+ Ag 2 S + H + 2. An excess of sodium

More information

As you saw in the last activity, a computer is made of many parts,

As you saw in the last activity, a computer is made of many parts, 23 Producing Circuit Boards R EA D I N G As you saw in the last activity, a computer is made of many parts, each manufactured from one or more materials. One essential part of a computer, and of many other

More information

AP* CHEMISTRY EQUATIONS BY TYPE

AP* CHEMISTRY EQUATIONS BY TYPE AP* CHEMISTRY EQUATIONS BY TYPE Double Replacement 1. Hydrogen sulfide is bubbled through a solution of silver nitrate. 2. An excess of sodium hydroxide solution is added to a solution of magnesium nitrate.

More information

THE EDDY WATER MANAGEMENT SYSTEM PRODUCT MANUAL

THE EDDY WATER MANAGEMENT SYSTEM PRODUCT MANUAL THE EDDY WATER MANAGEMENT SYSTEM PRODUCT MANUAL THE EDDY WATER MANAGEMENT SYSTEM (WMS) 3 CONTENTS CERTIFICATION PRODUCT INFORMATION PARTS INSTALLATION CARING FOR YOUR SYSTEM DOs AND DON Ts FEATURES SERVICE

More information

Chemical Testing of Drinking Water

Chemical Testing of Drinking Water Chemical Testing of Drinking Water Adapted from: An original Creek Connections activity. Water Chemistry Grade Level: all Duration: 50 minutes Setting: lab or classroom Summary: Students will conduct chemistry

More information

calcium oxide removes acidic oxides basic oxides acidic oxides basic oxides Iron obtained from the blast furnace is contaminated with

calcium oxide removes acidic oxides basic oxides acidic oxides basic oxides Iron obtained from the blast furnace is contaminated with 1 Iron from a blast furnace is treated with and with calcium oxide to make steel. Which substances in the are removed? removes calcium oxide removes acidic oxides basic oxides acidic oxides basic oxides

More information

Wet Cells, Dry Cells, Fuel Cells

Wet Cells, Dry Cells, Fuel Cells page 2 page 3 Teacher's Notes Wet Cells, Dry Cells, Fuel Cells How the various electrochemical cells work Grades: 7-12 Duration: 33 mins Program Summary This video is an introductory program outlining

More information

Unit F FR (part B) Solubility Equilibrium, Ksp (pg 1 of 16)

Unit F FR (part B) Solubility Equilibrium, Ksp (pg 1 of 16) Unit F FR (part B) Solubility Equilibrium, Ksp (pg 1 of 16) 1. Answer the following questions about the solubility of some fluoride salts of alkaline earth metals. (a) A student prepares 100. ml of a saturated

More information

How to Collect Your Water Sample and Interpret the Results for the Poultry Analytical Package

How to Collect Your Water Sample and Interpret the Results for the Poultry Analytical Package How to Collect Your Water Sample and Interpret the Results for the Poultry Analytical Package Bradley J. Austin, Josh B. Payne, Susan E. Watkins, Mike Daniels, and Brian E. Haggard Arkansas Water Resources

More information

Lab 2: Determination of the empirical formula of the product of magnesium heating

Lab 2: Determination of the empirical formula of the product of magnesium heating Chemistry 140 Please have parts 1, 2, 3 and 4 (tables only) ready before class on Wednesday, October 11. Write an abstract and paper-clip it to the front of your individual writeup. The abstract and the

More information

METALS

METALS METALS 3 Gallium is a metallic element in Group III. It has similar properties to aluminium. (a) (i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your

More information