Lesson Plan: C1.7.05

LESSON PLAN

Teacher	Subject	Period	Date	Year	Ability	LSA/Other Support
	Science

Context and Landmark Assessment	C1.7.05 Landmark Assessment: Progress Observation Opportunity

Remember to have high expectations

Lesson Title: Today we are learning about
How does electrolysis split compounds?

Remember to check for PROGRESS
Focus on Knowledge, Skills and Understanding

Success Criteria:	You will show your learning by...
When an ionic compound is melted or dissolved in water, the ions are free to move about within the liquid or solution. These liquids and solutions are able to conduct electricity and are called electrolytes. (HT only) Write balanced half equations and ionic equations where appropriate. Passing an electric current through electrolytes causes the ions to move to the electrodes. Positively charged ions move to the negative electrode (the cathode), and negatively charged ions move to the positive electrode (the anode). Ions are discharged at the electrodes producing elements. This process is called electrolysis. (HT only) Throughout Section 4.4.3 Higher Tier students should be able to write half equations for the reactions occurring at the electrodes during electrolysis, and may be required to complete and balance supplied half equations. (MS) When a simple ionic compound (eg lead bromide) is electrolysed in the molten state using inert electrodes, the metal (lead) is produced at the cathode and the non-metal (bromine) is produced at the anode. Students should be able to predict the products of the electrolysis of binary ionic compounds in the molten state. (HT only) students should be able to write half equations for the reactions occurring at the electrodes during electrolysis, and may be required to complete and balance supplied half equations for this process . (MS) During electrolysis, at the cathode (negative electrode), positively charged ions gain electrons and so the reactions are reductions. At the anode (positive electrode), negatively charged ions lose electrons and so the reactions are oxidation reactions. Reactions at electrodes can be represented by half equations, for example: 2H 2e- ? H2 and 4OH- ? O2 2H2O 4e- or 4OH- 4e- ? O 2H2O

Success Criteria:

You will show your learning by...

When an ionic compound is melted or dissolved in water, the ions are free to move about within the liquid or solution. These liquids and solutions are able to conduct electricity and are called electrolytes.
(HT only) Write balanced half equations and ionic equations where appropriate.
Passing an electric current through electrolytes causes the ions to move to the electrodes. Positively charged ions move to the negative electrode (the cathode), and negatively charged ions move to the positive electrode (the anode). Ions are discharged at the electrodes producing elements. This process is called electrolysis.
(HT only) Throughout Section 4.4.3 Higher Tier students should be able to write half equations for the reactions occurring at the electrodes during electrolysis, and may be required to complete and balance supplied half equations. (MS)
When a simple ionic compound (eg lead bromide) is electrolysed in the molten state using inert electrodes, the metal (lead) is produced at the cathode and the non-metal (bromine) is produced at the anode.
Students should be able to predict the products of the electrolysis of binary ionic compounds in the molten state.
(HT only) students should be able to write half equations for the reactions occurring at the electrodes during electrolysis, and may be required to complete and balance supplied half equations for this process . (MS)
During electrolysis, at the cathode (negative electrode), positively charged ions gain electrons and so the reactions are reductions.
At the anode (positive electrode), negatively charged ions lose electrons and so the reactions are oxidation reactions.
Reactions at electrodes can be represented by half equations, for example: 2H 2e- ? H2 and 4OH- ? O2 2H2O 4e- or 4OH- 4e- ? O 2H2O

Think about how you can match the needs of ALL students

Keywords:

Links: Literacy, Numeracy, SMSC, British values

Memory Anchor:

AFL/Key Questions:

When is an ionic compound able to conduct electricity?
When an ionic compound is melted or dissolved in water, the ions are free to move about within the liquid or solution. These liquids and solutions are able to conduct electricity and are called electrolytes.
(HT) What is the balanced half equation for H ? e??? H2
T(HT)he balanced half equation is: 2H ? 2e??? H2
What happens at each of the electrodes in electrolysis when an electric current is passed through the electroytes?
Passing an electric current through electrolytes causes the ions to move to the electrodes. Positively charged ions move to the negative electrode (the cathode), and negatively charged ions move to the positive electrode (the anode). Ions are discharged at the electrodes producing elements. This process is called electrolysis.
(HT) What happens at the anode and cathode electrodes in the electrolysis of aqueous sodium chloride? (use half equations to help explain)
(HT) At the cathode sodium is formed: 2Na 2e- --> 2Na At the anode chlorine gas is formed: 2Cl- -->Cl2 2e-
Which electrode as the metals and non metals products found during electrolysis?
During electrolysis the metal product is found at the cathode as this cathode is negatively charged. The non metal product is found at the anode, this this electrode is positively charged.
What would the products be for the electrolysis of the following ionic compounds: 1. NaCl 2. PbBr2 3. NaOH 4. Al2O3
The products of electrolysis would be: 1. H2 (g) Cl2 (g) NaOH (aq) 2. Pb (s) Br2 (g) 3. H2 (g) O2 (g) Na (aq) 4. Al (s) O2 (g)
(HT) What would the half equations be for the electrolysis of NaCl?
(HT) anode: 2Cl– → Cl2 2e- (oxidation) cathode: 2H 2e– → H2 (reduction). NaOH solution is also produced.
What happens at the cathode during electrolysis? Is this an oxidation or reduction reaction?
During electrolysis, at the cathode (negative electrode), positively charged ions gain electrons and so the reactions are reductions.
What happens at the anode during electrolysis? Is this an oxidation or reduction reaction?
At the anode (positive electrode), negatively charged ions lose electrons and so the reactions are oxidation reactions.
What would the half equations be during the electrolysis of PbBr2?
anode: 2Br– → Br2 2e- (oxidation) cathode: Pb2 2e– → Pb (reduction).

Identify questions for high, middle, low and identify questioning techniques- Challenge questions

Learning Phases/Episodes

Think about how you can match the needs of ALL students
Differentiation: AGT, SEND, LLL, Disadvantaged
Remember to check for PROGRESS

Starter Activity	Differentiation and Challenge question/task
Students to copy and complete the keywords. Teacher reveals missing letters; Students correct mistakes; Discuss the scientific meanings of the words. Students to write down the definitions of the most important / new keywords. Discuss the 'Memory Anchor'. What does it show? How does it relate to the what we are learning about today (title)?

Think about PACE – Develop, consolidate and deepen knowledge, skills and understanding

Teacher or Student lead?	Differentiation and Challenge question/task

Progress Check	Extension

Remember to give time to apply knowledge, skills and understanding

Teacher or Student lead?	Differentiation and Challenge question/task

Progress Check	Extension

Teacher or Student lead?	Differentiation and Challenge question/task

Progress Check	Extension

Teacher or Student lead?	Differentiation and Challenge question/task

Progress Check	Extension

Plenary	Differentiation and Challenge question/task
Students to answer the 'Key Questions' with learning partners.
Progress Check Teacher to reveal and discuss the answers to the questions.	Extension What have learnt about the 'Big Ideas' today?

Homework	Differentiation and Challenge question/task