IDEAL MODEL OF TEACHER MENTORING REPORT FOR JANUARY 2018

COVENANT UNIVERSITY SECONDARY SCHOOL CANAANLAND, OTA

REPORT ON CHEMISTRY MENTORING ACTIVITY

DATE: 19TH JANUARY, 2018

Brief Report on the Programme

The programme started with an opening prayer and a brief word of exhortation. The mentoring topic was on Electrolysis with the following contents: • Electrolysis and other terms used in electrolysis; • The ionic theory;

• Strong electrolytes, weak electrolytes and non-electrolytes with examples;

• Mechanism of electrolysis and;

• The factors that determine the preferential discharge of ions during electrolysis.

The mentees asked questions and gave contributions.

The mentor answered all the questions and summarized the lesson.

The programme was a huge success with high expectations in teacher’s delivery of the lesson topic in the classroom. It came to an end with a closing prayer.

ATTENDANCE

1. Mr. Oputah - Mentor

2. Mr. Adeleye Sunday- Mentee

3. Mr. Atitebi Femi - Mentee

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S /N

SCHOOL

L E S S O N OBJECTIVES

INTRODUCTION

METHODOLOGY/ INTERACTION

LESSON CONTENT RESOLUTIONS

DELIVERABLES

A C T I ON

1. Covenant University Secondar y S c h o o l (CUSS). Ota

As the lesson progresses the the Mentees should be able to; - define electrolysis and other terms used in electrolysis; - explain the ionic theory; - distinguish between strong electrolytes, weak electrolytes and non-electrolytes with examples; - explain the mechanism of electrolysis and - explain the factors that determine the preferential discharge of ions during electrolysis.

- EFFECTS OF ELECTRICITY ON MATTER: Chemical decomposition of a substance can be brought about by heating. Similarly, electrical effect can also be used to bring about chemical decomposition of substances. Effect of electricity on matter is studied under electrolysis. DEFINITION: Electrolysis is defined as the chemical decomposition of a compound (electrolyte) brought about by the passage of direct current through either a solution or the molten form of the compound.

- The Mentor explains the effects of electricity on matter and defines electrolysis. - Mentees pay attention, note vital points and ask questions.

Electrolysis can be defined as the chemical decomposition of a compound which takes place when electric current is passed through either solution or molten form of compound. It may also be defined as the chemical decomposition of a compound as a result of passage of electric current through either a solution or molten state of that compound.

Electrolysis is used to convert electrical energy to chemical energy.

The Mentor should ensure all the Mentees can define electrolysis.

Define the term electrolysis.

Electrolysis It is defined as the chemical decomposition of a compound as a result of passage of electric current through either a solution or molten state of that compound.

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2. - The Mentor defines other terms used in electrolysis.

- Mentees pay attention, note points.

(i) ELECTROLYTE: An electrolyte is a compound which conducts electricity and is decomposed in the process. To behave as an electrolyte, the compound must be in a liquid form e i t h e r a s m o l t e n compound or an aqueous solution of the compound. A non-electrolyte does not conduct electricity in this manner. ( i i ) E L E C T R O D E S : Electrodes are conductors in the form of wires, rod or plates through which an electric current leaves or enters the electrolyte. (iii) ANODE: Anode is the positive electrode by which the electrons leave an electrolyte (or by w h i c h c o n v e n t i o n a l c u r r e n t e n t e r s t h e electrolyte). It is the electrode which is joined to the positive terminal of the direct current supply. (iv) CATHODE: This is the negative electrode by which electrons enters the electrolyte. It is the electrode which is joined to the negative terminal of the electric supply. (v) ELECTROLYTIC CELL: Electrolytic cell is an assembly of two e l e c t r o d e s i n a n electrolyte used to bring a b o u t c h e m i c a l decomposition of the electrolyte by direct current. In an electrolytic cell, oxidation occurs at the anode (positive electrode) and reduction at the c a t h o d e ( n e g a t i v e electrode).

- The Mentor should e n s u r e Mentees can define all the terms used in electrolysis.

- Define the term electrodes.

- What is an electrolytic cell?

- Distinguish between the anode and cathode of an electrolytic cell.

- Mentees practise diagram of the electrolytic cell.

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3. - The Mentees explain the ionic theory.

- Mentees pay attention, note points and ask questions.

-  The ionic theory was f i r s t p r e s e n t e d b y Arrhenius to explain electrolysis. Ionic theory proposed that when an electrolyte is melted or dissolved in water, some if not all, the molecules of the substance dissociate i n t o f r e e l y m o v i n g charged particles called ions. The process of dissociation into ions is known as ionization. T h e m e t a l l i c i o n s , ammonium ions,NH4+, and hydrogen ions ,H+, are positively charged while the non metallic ions and hydroxide ions are negatively charged. When electric current is p a s s e d t h r o u g h a n electrolyte, the free ions l o s e t h e i r r a n d o m movement. The positive ions become attracted to the cathode (negative electrode) and are known as cations (i.e. cathode ions). The negative ions move towards the anode (positive electrode) and are called anions. (i.e. anode ions). Therefore, t he cu r r en t t h rough electrolyte is carried by the movement of ions to the electrodes, and not by flow of electrons in the electrolyte. Arrhenius version of the ionic theory has been modified and replaced by the modern ionic theory. The modern ionic theory p r o p o s e t h a t a n electrolytes consists of oppositely charged ions even in the solid state and such ions are pulled away from one another either as a result of the heat applied when the solid melts or with the help of the solvent molecules when the solid dissolves. ARRHENIUS THEORY:  NaCl(s) Na+(aq) + Cl-

(aq)

MODERN THEORY: Na+Cl-(s) Na+(aq) + Cl-(aq)

- The Mentor should explain the ionic theory with different ionic equations.

- Mentees write the ionic equations.

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4.- The Mentor distinguishes between electrolytes, weak electrolytes and non-electrolytes with examples.

- Menteess pay attention, note points and ask questions.

- Strong electrolytes allow the passage of electric current readily and ionize completely in the process. Examples are HCl, H2SO4, NaCl, HNO3, CuSO4 etc.

- Weak electrolytes do not allow the passage of electric current readily and ionizes partially in the process. Examples are Ethanoic acid, CH3COOH, H2CO3 etc.

- Non- electrolytes do not allow the passage of electric current and do not ionizes in the process. Examples are Ether, Kerosene, petrol, Sugar cane solution, Ethanol, Benzene, Urea etc.

- The Mentor should Ensure the Mentees can distinguish between strong electrolytes, weak electrolytes and non-electrolytes with examples.

- Distinguish between strong electrolytes and non-electrolytes, stating one example of each.

- Give one example of a weak electrolyte.

- Give two differences between a conductor and an electrolyte.

Menteess give examples of strong electrolytes, weak electrolytes and non- electrolytes.

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5.- The Mentor explains the mechanism of electrolysis.

- The Mentees pay attention, note points and ask questions.

- The electrolysis of a given electrolytes can be carried out in electrolytic cell in two forms. (i) Using the molten form of the electrolytes. (ii) Using the solution form of the electrolyte.

(i) Using the molten (fused) form of the electrolyte, only two opposite ions from the electrolyte are present.. e.g. molten NaCl contains Na+ and Cl- ions only. Na+ ions migrate to the cathode to accept electrons and become discharged to produce neutral Na atoms. Na+(aq) + e- Na(s) While chloride ions migrate to the anode to give up electrons and become discharged to produce Cl atoms which pair up to form chlorine gas, Cl2. Cl- Cl + e-

Cl + Cl Cl2(g) There is no competition for discharge of ions at the electrodes. (ii) Using the solution form of the electrolyte, ions are produced from the electrolytes and from the solvent usually water, H2O. Two opposite ions from the electrolytes e.g. Na+ and Cl- from NaCl and two from water, H+ and OH-. In such cases, the cations and anions of both the electrolyte and the solvent will migrate to the cathode and the anode respectively where they will compete with one another to be discharged. The products formed at the electrodes depend on which ions are preferentially discharged, the ions from the electrolytes or from the solvent.

- The Mentor should explain and distinguish between the electrolysis of fused and solution forms of the electrolytes.

- State the ion that migrates to the (i) cathode and (ii) anode, in the electrolysis of fused CaCl2.

-Menteess distinguish between the electrolysis of fused and solution forms of the electrolytes.

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6. - The Mentor explains the factors that determine the preferential discharge of ions during electrolysis.

- The Mentees pay attention, note points and ask questions.

The discharge of ions at the electrodes is governed by three conditions, namely: (i) Relative position of ions in electrochemical series. (ii) The concentration of ions in the electrolyte. (iii) The nature of the electrode. (i) RELATIVE POSITIONS OF THE IONS IN THE ELECTROCHEMICAL SERIES: When all other factors are constant a cathode ion which is lowest in the series (less electropositive) will be discharged in preference to the one higher up (more electropositive).This because the less electropositive element gains electron(s) more readily from the cathode and so become reduced and discharged as a neutral atom while the more electropositive element remains in the solution as positive ions. NOTE: K+, Na+ and Ca+ are never discharged at all from aqueous solution. This is because of their high electropositive values and the large gap between them and H+. However, K+, Na+ and Ca+ are discharged during the electrolysis of their molten salt. An anion which is higher up in the series (less electronegative) is preferentially discharged to the one lower down the series (more electronegative). This is because the less electronegative ions lose electrons more readily than the more electronegative ions. NOTE: F-, SO42- and NO3- are never discharged from aqueous solution because of their high electronegative values and the large gap between them and OH- (ii) CONCENTRATION OF IONS: Concentration of ions when the concentration of an ion in the electrolyte is increased, the ion tends to increase its chances of being discharged. The

The Mentor should state and explain the factors that determine the preferential discharge of ions during electrolysis.

- State three factors that affect the preferential discharge of ions in electrolysis.

- Give two examples of inert electrodes.

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LESSON PLAN FOR MENTORING ACTIVITY

Date: 19th January, 2018.

Subject: Chemistry

Topic: Electrolysis

Duration: 80 Minutes

Class: SS2

Behavioural Objectives: As the lesson continues, the Mentees should be able to;

(i) define electrolysis and other terms used in electrolysis;

(ii) explain the ionic theory;

(iii) distinguish between strong electrolytes, weak electrolytes and non-electrolytes with examples;

(iv) explain the mechanism of electrolysis and;

(v) explain the factors that determine the preferential discharge of ions during electrolysis.

Instructional Materials: Diagram of an electrolytic cell, Chart of the electrochemical series

showing the reactivity of metals and non metals, H2SO4, Ethanoic acid, Kerosene, Ethanol etc.

Reference Texts: (a) New School Chemistry for Senior Secondary Schools by Osei Yaw Ababio

(b) Essential Chemistry for Senior Secondary Schools by I.A Odesina

Previous Knowledge: The Mentees have been taught reduction and oxidation reactions.

Introduction: Electrolysis is defined as the chemical decomposition of a compound (electrolyte) brought about by the passage of direct current through either a solution or the molten form of the compound.

CONTENT

ELECTROLYSIS

EFFECTS OF ELECTRICITY ON MATTER: Chemical decomposition of a substance can be brought about by heating. Similarly, electrical effect can also be used to bring about chemical decomposition of substances. Effect of electricity on matter is studied under electrolysis.

DEFINITION OF TERMS:

(i) ELECTROLYTE: An electrolyte is a compound which conducts electricity and is decomposed in the process. To behave as an electrolyte, the compound must be in a liquid form either as molten compound or an aqueous solution of the compound. A non-electrolyte does not conduct electricity in this manner.

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(ii) ELECTRODES: Electrodes are conductors in the form of wires, rod or plates through which an electric current leaves or enters the electrolyte.

(iii) ANODE: Anode is the positive electrode by which the electrons leave an electrolyte (or by which conventional current enters the electrolyte). It is the electrode which is joined to the positive terminal of the direct current supply.

(iv) CATHODE: This is the negative electrode by which electrons enters the electrolyte. It is the electrode which is joined to the negative terminal of the electric supply.

(v) ELECTROLYTIC CELL: Electrolytic cell is an assembly of two electrodes in an electrolyte used to bring about chemical decomposition of the electrolyte by direct current.

In an electrolytic cell, oxidation occurs at the anode (positive electrode) and reduction at the cathode (negative electrode).

DIAGRAM OF AN ELECTROLYTIC CELL

IONIC THEORY

The ionic theory was first presented by Arrhenius to explain electrolysis. Ionic theory proposed that when an electrolyte is melted or dissolved in water, some if not all, the

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molecules of the substance dissociate into freely moving charged particles called ions. The process of dissociation into ions is known as ionization.

The metallic ions, ammonium ions,NH4+, and hydrogen ions,H+, are positively charged while the non metallic ions and hydroxide ions are negatively charged. When electric current is passed through an electrolyte, the free ions lose their random movement. The positive ions become attracted to the cathode (negative electrode) and are known as cations (i.e. cathode ions). The negative ions move towards the anode (positive electrode) and are called anions. (i.e. anode ions). Therefore, the current through electrolyte is carried by the movement of ions to the electrodes, and not by flow of electrons in the electrolyte.

Arrhenius version of the ionic theory has been modified and replaced by the modern ionic theory. The modern ionic theory propose that an electrolytes consists of oppositely charged ions even in the solid state and such ions are pulled away from one another either as a result of the heat applied when the solid melts or with the help of the solvent molecules when the solid dissolves.

ARRHENIUS THEORY: NaCl(s) Na+(aq) + Cl-(aq)

MODERN THEORY: Na+Cl-(s) Na+(aq) + Cl-(aq)

ELECTROLYTES AND NON ELECTROLYTES

Both metallic conductors and electrolytes can conduct electric current. A metallic conductor however conducts electricity both in solid or liquid states by the movement of electrons from atom to atom. An electrolyte conducts electricity only when molten or in solution as result of the movement of its ions to the electrode and their subsequent discharge at the electrode. Strong electrolyte is one which ionizes completely in solution and conduct electric current readily. A weak electrolyte is one which ionizes partially in solution and does not conduct electric current readily. Non electrolytes are one which does not ionize in solution and does not conduct electric current.

DIFFERENCES BETWEEN A CONDUCTOR AND AN ELECTROLYTE

STRONG ELECTROLYTES WEAK ELECTROLYTES NON ELECTROLYTES

H2SO4,NaCl, CuSO4, AgNO3, NaOH

Ethanoic acid (CH3COOH) Urea, Ethanol, Benzene, ether, cane sugar.

ELECTROLYTE CONDUCTOR

It is a compound It is an element

It uses ions as carriers of electricity It uses electrons as carriers of electricity

It undergoes decomposition It does not undergo decomposition

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MECHANISM OF ELECTROLYSIS

The electrolysis of a given electrolytes can be carried out in electrolytic cell in two forms.

(i) Using the molten form of the electrolytes

(ii) Using the solution form of the electrolyte

(i) Using the molten (fused) form of the electrolyte, only two opposite ions from the electrolyte are present.. e.g. molten NaCl contains Na+ and Cl- ions only. Na+ ions migrate to the cathode to accept electrons and become discharged to produce neutral Na atoms.

Na+(aq)+ e- Na(s)

While chloride ions migrate to the anode to give up electrons and become discharged to produce Cl atoms which pair up to form chlorine gas, Cl2 .

Cl- Cl + e-

Cl + Cl Cl2(g) There is no competition for discharge of ions at the electrodes .

(ii) Using the solution form of the electrolysis, ions are produced from the electrolytes and from the solvent usually water, H2O. Two opposite ions from the electrolytes e.g. Na+ and Cl- from NaCl and two from water, H+ and OH-. In such cases, the cations and anions of both the electrolyte and the solvent will migrate to the cathode and the anode respectively where they will compete with one another to be discharged. The products formed at the electrodes depend on which ions are preferentially discharged, the ions from the electrolytes or from the solvent.

PREFERENTIAL (SELECTIVE) DISCHARGE OF IONS

The discharge of ions at the electrodes is governed by three conditions, namely

1. Relative position of ions in electrochemical series.

2. The concentration of ions in the electrolyte.

3. The nature of the electrode.

RELATIVE POSITIONS OF THE IONS IN THE ELECTROCHEMICAL SERIES

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K+ Na+ Ca2+ Mg2+

Al3+ Zn2+ Fe2+ Sn2+ OH-Pb2+ I-H+

Br- Cu2+ Cl-Hg2+

NO3- Ag2+ SO42-Au2+ F-

When all other factors are constant a cation (cathode ion) which is lowest in the series (less electropositive) will be discharged in preference to the one higher up (more electropositive).This because the less electropositive element gains electron(s) more readily from the cathode and so become reduced and discharged as a neutral atom while the more electropositive element remains in the solution as positive ions.

NOTE: K+, Na+ and Ca+ are never discharged at all from aqueous solution. This is because of their high electropositive values and the large gap between them and H+. However, K+, Na+ and Ca+ are discharged during the electrolysis of their molten salt.

An anion which is higher up in the series (less electronegative) is preferentially discharged to the one lower down the series (more electronegative). This is because the less electronegative ions lose electrons more readily than the more electronegative ions.

NOTE: F-, SO42- and NO3- are never discharged from aqueous solution because of their high electronegative values and the large gap between them and OH-

CONCENTRATION OF IONS

Concentration of ions when the concentration of an ion in the electrolyte is increased, the ion tends to increase its chances of being discharged. The influence of concentration, however, is effective only when the two competing ions are closely positioned in the electrochemical series. The effect of concentration becomes less important as the positions of the competing ions become further apart in the series.

NATURE OF ELECTRODES

Inert electrodes (e.g. Platinum and graphite) take no part in the electrolytic reactions. However, platinum is attacked by liberated chlorine and graphite is attacked by liberated

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oxygen. Some electrodes which have strong affinity (love) for certain ions influences the ionic discharge. For example, in the electrolysis of aqueous NaCl using mercury cathode. Na+ will be discharged at the cathode to form sodium amalgam, Na/Hg

Na+(aq) + Hg(s)+ e- Na/Hg(l)

Also, in the electrolysis of CuSO4 solution using copper anode. Neither the SO42- nor the OH-

will be discharged. Rather, the Cu atoms will lose electrons more readily and go into solution

as Cu2+.

METHODOLOGY

The Mentor employs the tasking/questioning and group discussion method.

INTERACTION

Step I

Mentor’s activity: Mentor introduces the lesson topic, writes on the board.

Mentees’ activity: Mentees pay attention to the introduction of the lesson.

Step II

Mentor’s activity: Mentor defines electrolysis and other terms used in electrolysis.

Mentees’ activity: Mentees pay attention, write points.

Step III

Mentor’s activity: Mentor explains the ionic theory, strong, weak and non-electrolytes, non-

electrolytes with examples.

Mentees’ activity: Mentees pay attention and write examples of strong, weak and non-

electrolytes, non-electrolytes with examples.

Step IV

Mentor’s activity: Mentor explains the mechanism of electrolysis.

Mentees’ activity: Mentees note points and ask questions.

Step V

Mentor’s activity: Mentor explains the factor that affects the preferential discharge of ions in

electrolysis.

Mentees’ activity: Mentees pay attention and note points.

Step VI

Mentor’s activity: Mentor groups Mentees to discuss and make presentations on the lesson topic.

Mentees’ activity: Mentees move into groups to discuss and make presentations on the lesson topic.

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Step VII

Mentor’s activity: The Mentor writes evaluation questions on the board.

Mentees’ activity: The Mentees answer evaluation questions in their notes.

Step VIII

Mentor’s activity: The Mentor corrects the Mentees.

Mentees’ activity: The Mentees note the corrections made.

Step IX

Mentor’s activity: The Mentor summarizes and concludes the lesson.

Mentees’ activity: The Mentees pay attention and take notes.

SUMMARY OF LESSON

(i) Electrolysis is defined as the chemical decomposition of a compound (electrolyte) brought

about by the passage of direct current through either a solution or the molten form of the

compound.

(ii) An electrolyte is a compound which conducts electricity and is decomposed in the process. To behave as an electrolyte, the compound must be in a liquid form either as molten compound or an aqueous solution of the compound. A non-electrolyte does not conduct electricity in this manner.

(iii) Electrodes are conductors in the form of wires, rod or plates through which an electric current leaves or enters the electrolyte.

(iv) Anode is the positive electrode by which the electrons leave an electrolyte (or by which conventional current enters the electrolyte). It is the electrode which is joined to the positive terminal of the direct current supply. Cathode is the negative electrode by which electrons enters the electrolyte. It is the electrode which is joined to the negative terminal of the electric supply.

(v) Electrolytic cell is an assembly of two electrodes in an electrolyte used to bring about chemical decomposition of the electrolyte by direct current.

(vi) Strong electrolyte is one which ionizes completely in solution and conduct electric current readily. A weak electrolyte is one which ionizes partially in solution and does not conduct electric current readily. Non electrolytes are one which does not ionize in solution and does not conduct electric current.

(vii) The electrolysis of a given electrolytes can be carried out in an electrolytic cell in two forms: Using the molten form of the electrolytes and using the solution form of the electrolyte.

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(viii) The discharge of ions at the electrodes is governed by three conditions, namely: Relative position of ions in electrochemical series, concentration of ions in the electrolyte and the nature of the electrode.

APPRAISAL

(i) Define the following terms: I. Electrolysis II. Electrode III. Electrolytic cell.

(ii) Distinguish between the following. I. Cathode and anode II. Strong and weak electrolyte.

(iii) Give two differences between a conductor and an electrolyte.

EXPECTED ANSWERS

(i) I. Electrolysis is defined as the chemical decomposition of a compound (electrolyte) brought about by the passage of direct current through either a solution or the molten form of the compound. II. Electrodes are conductors in the form of wires, rod or plates through which an electric current leaves or enters the electrolyte. III. Electrolytic cell is an assembly of two electrodes in an electrolyte used to bring about chemical decomposition of the electrolyte by direct current.

(ii) I. Cathode is the negative electrode by which electrons enters the electrolyte. It is the electrode which is joined to the negative terminal of the electric supply while the anode is the positive electrode by which the electrons leave an electrolyte (or by which conventional current enters the electrolyte). It is the electrode which is joined to the positive terminal of the direct current supply. II. Strong electrolyte is one which ionizes completely in solution and conduct electric current readily. while a weak electrolyte is one which ionizes partially in solution and does not conduct electric current readily.

(iii)

ASSIGNMENT

(i) State the factors that influence the preferential discharge of ions in electrolysis.

(ii) Give two examples of inert electrodes.

EXPECTED ANSWERS • Relative position of ions in electrochemical series

• The concentration of ions in the electrolyte

• The nature of the electrode

(ii) Platinum and Graphite

ELECTROLYTE CONDUCTOR

It is a compound It is an element

It uses ions as carriers of electricity It uses electrons as carriers of electricity

It undergoes decomposition It does not undergo decomposition

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EDUCATION COMMISSION PERFORMANCE CHART ON JANUARY 2018 TEACHER

MENTORING REPORTS (FA NETWORK)

0.0%

25.0%

50.0%

75.0%

100.0%

CUSS FA BONNY LUSS FA KUBWA FA ASABA FA EKET FA EKPOMA

%

16

%

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Indicators for Measuring Good Performance in Mentoring Programme

1. Good use of approved report template

2. Well planned Lesson Note showing all required components or elements (Topic, Class, Duration, Introduction and Conclusion of Lesson, Behavioural Objectives, Teaching Aids, Procedural steps, Reference Materials etc.)

3. Clear indication of teaching/learning steps

4. Clear and Measurable objectives

5. Employment of various teaching strategies

6. Alignment with content standards

7. Full participation and involvement of mentees

8. Team based learning

9. Appropriate illustration (good use of illustrative diagrams -charts/flash cards)

10. Evaluation based on Behavioural Objectives

11. Class Evaluation on work done with expected answers

12. Homework/Assignment with expected answers

13. Evidence of research

14. Practical activities

15. Mentoring report devoid of grammatical expression errors

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16. A short brief on the exercise with number of staff present

PRINCIPAL COVENANT UNIVERSITY SECONDARY SCHOOL CANAANLAND, OTA (DCNS BODE LARTEY O.)

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