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at 11:30 pm 24 September 2022

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Tutorial Week 8 (26-30 Sep 2022) 1st hour

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Tutorial Week 8 (26-30 Sep 2022) 1st hour

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Learning objectives:
1. Analyse the variation in the ionic radii across period 2 and period 3

2. Analyse the variations in the first ionisation energy across a period and down a group

slide 42-62

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Tutorial Week 8 (26-30 Sep 2022) 2nd hour

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Tutorial Week 8 (26-30 Sep 2022) 2nd hour

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Learning objectives
1. Describe the anomalous cases of ionisation energy.

2. Deduce the electronic configuration of an element and its position in the periodic table based on successive ionisation energy data.

3. Explain the increase in the successive ionisation energies of an element.

Slide 64-75
Tutorial 5-7

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Tutorial Week 8 (26-30 Sep 2022) 3rd hour

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Tutorial Week 8 (26-30 Sep 2022) 3rd hour

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19 Sep2022
Pre read:
1. determine position of element based on electron configuration and vice versa

In class:
1. Quiz (google form)
2. Discuss tutorial question 1-3
3. Self-test topic 3.1

22 Sep 2022
1. Factor affecting atomic radius and explain.
2. Explain variation of ionic radius, isoelectronic species, atom & its ion
3. Explain the trend of ionisation energy and determine its group.

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F5P01(27 Sep 2022) & H2P02 (30 Sep 2022)
- Prepare standard solution via dilution method
https://www.aplustopper.com/prepare-standard-solution

- Form a group of 3-4 students and get ready to carry out following skills in the lab. Please get ready and each group will be asked to handle two of these:
1. Transferring a solution in the beaker into the volumetric flask.
2. Standard solution in a volumetric flask which reaches the calibrated mark.
3. Record reading of burette.
4. Discard air bubbles from the tip of the burette.
5. Pipette solution into a conical flask.
6. Control stopcock during gross titration.
7. Control the stopcock near the end point.
8. Pipette solution up to the calibrated mark.
9. Initial and final reading of burette.
10. Eye position when you’re doing gross reading.
11. Eye position when near the end point.
12. Rinse the half drop of solution at the tip of the burette with distilled water.
13. Transfer last drop solution in the pipette to the conical flask.

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Preparation of a standard solution by weighing method

A solution whose concentration is accurately known is called a standard solution.

A standard solution can be prepared by weighing method in the following way.
(a) The mass of solute needed is calculated and weighed.
(b) The solute is dissolved in some distilled water in a beaker.
(c) The solution is transferred into a volumetric flask.
(d) More distilled water is added to obtain the required volume. The flask is stoppered and shaken.

For example, to prepare 1.0 dm³ of 0.50 mol dm⁻³ aqueous sodium hydroxide.

A very accurate standard alkaline solution cannot be prepared using sodium hydroxide as the primary standard. This is because
(a) sodium hydroxide is deliquescent. It absorbs moisture and dissolves to form a solution.
(b) sodium hydroxide may not be pure. It reacts with carbon dioxide from the air:
2NaOH(s) + CO₂(g) → Na₂CO₃(s) + H₂O(l)
Hence, the concentration of this alkaline solution is not accurate.

Pure anhydrous sodium carbonate, Na₂CO₃, is used to prepare a primary standard alkaline solution.

Solid organic acids such as oxalic acid, H₂C₂O₄.2H₂O, is used to prepare primary standard acidic solution.

A standard solution can also be prepared by dilution method.

People also ask
Preparation of a standard solution by dilution method

A standard solution can also be made by dilution. Bench acids such as hydrochloric acid, sulphuric acid and nitric acid are all prepared by diluting the commercial concentrated acids (stock solutions) with varying amounts of distilled water.

Adding water to a concentrated solution:
(a) changes the concentration of the solution
(b) does not change the number of moles of solute present

This means that the total number of moles of solute particles before dilution is equal to the total number of moles of solute particles after the dilution is carried out.
Moles of solute before dilution = moles of solute after dilution

A dilution equation can be derived as shown below.

Since adding water does not change the number of moles of solute particles,
M₁V₁ = M₂V₂

Figure shows how Example is carried out in the laboratory.

The volume of stock solution required must be measured out accurately. Use a pipette to measure out exactly 25.0 cm³ of stock solution. Use a burette to measure out any other volumes that less than 50.0 cm³.

For example, to prepare 500 cm³ of 0.15 mol dm⁻³ sulphuric acid from a stock solution of 2.0 mol dm⁻³ sulphuric acid.
(a) Calculate the volume of stock solution required.

(b) Fill a burette with the stock solution.
Run out 37.5 cm³ of stock solution into a 500 cm³ volumetric flask containing some distilled water.

(c) Add more distilled water into the flask, with constant swirling. Then, use a dropper to add distilled water to bring the meniscus to the calibration mark. Stopper the flask and shake well to ensure thorough mixing.

1. Calculate the volume of concentrated nitric acid, 18 mol dm⁻³ which is required to prepare 5.0 dm ³ of 2.0 mol dm⁻³ nitric acid.
Solution:

2. What volume of 2.0 mol dm⁻³ sulphuric acid is needed to prepare 100 cm ³ of 0.5 mol dm⁻³ sulphuric acid?
Solution:

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How do you prepare a standard solution? Preparation of a standard solution by weighing method A solution whose concentration is accurately known is called a standard solution. A standard solution can be prepared by weighing method in the following way. (a) The mass of solute needed is calculated and weighed.

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19 Sep2022
Pre read:
1. determine position of element based on electron configuration and vice versa

In class:
1. Quiz (google form)
2. Discuss tutorial question 1-3
3. Self-test topic 3.1
-----------------------------
4. Factor affecting atomic radius and explain.
5. Explain variation of ionic radius, isoelectronic species, atom & its ion

22 Sep 2022
1. Explain the trend of ionisation energy and determine its group.
2. Acid-base oxide character
3. Assignment Part A

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Chapter 4: Draw Lewis structure & identify types of exceptional octet rule

Pre-read: https://youtu.be/G5f9NaJYAvI (watch the first 8 minutes & 16:57-21:17)

Remember the number of valence electron of the following element,
1. H - 1,
2. B - 3,
3. C - 4,
4. N - 5,
5. O, S -6,
6. F, I - 7

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20 Lewis structure (single bond with lone pair electrons) +  Exceptional to Octet Rule (Tutorial Q6)

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19 Sep2022
Pre read:
1. determine position of element based on electron configuration and vice versa

In class:
1. Quiz (google form)
2. Discuss tutorial question 1-3
3. Self-test topic 3.1
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4. Factor affecting atomic radius and explain.
5. Explain variation of ionic radius, isoelectronic species, atom & its ion

22 Sep 2022
1. Explain the trend of ionisation energy and determine its group.
2. Acid-base oxide character
3. Assignment Part A

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19 Sep 2022
1. Tutorial 3.1
2. Group discussion
3. self-test for 3.1
_______________________
4. Factor affecting atomic radius and explain.
5. Explain variation of ionic radius, isoelectronic species, atom & its ion
6. Explain the trend of ionisation energy and determine its group.

23 Sep 2022
1. Acid-base character of oxides & tutorial question 8
2. Discuss assignment part A

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F5P01
- Test from program Kecemerlangan Akademik (PKA) which still waiting further information from JK PKA
H2P02
Fri (9-11am) - carry out experiment 3
Fri (245pm) test from program PKA

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Chapter 3
1. Trend periodicity of atomic radius, ionic radius, ionisation energy, electronegativity, acid-base character of oxide
2.Meaning of isoelectronic species

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12 Sep2022
Pre read:
1. How many set of quantum number does an electron has?

2. Each set quantum number consist of how many quantum
number?

3. What are symbol for those quantum number?

In class:
1. Explain quantum number and discuss tutorial questions at the same time.

15 Sep 2022
1. Quantum number
2. Principle writing electron configuration

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Carry out Experiment 3
1. Make sure jotter for experiment is ready. Part A one diagram while Part B also one diagram.
2. Pre-lab Experiment 3: https://youtu.be/hQhpguHackU
3. Post lab Experiment 3: https://youtu.be/pmMos3WKQq0

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19 Sep2022
Pre read:
1. determine position of element based on electron configuration and vice versa

In class:
1. Quiz (google form)
2. Discuss tutorial question 1-3
3. Self-test topic 3.1

22 Sep 2022
1. Factor affecting atomic radius and explain.
2. Explain variation of ionic radius, isoelectronic species, atom & its ion
3. Explain the trend of ionisation energy and determine its group.

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12 Sep 2022
1. List down the 5 formulae in Chapter 2.1
2. Discuss tutorial questions
3.Group discussion 2.1
4. Group discussion 2.3

16 Sep 2022
1. Quiz 4
2. Assignment Part B
3. Folder

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22 Aug 2022
1. Tutorial questions
2. Determine amount of product formed

26 Aug 2022
1. Determine amount of excess reactant left
2. Determine percentage yield
3. Quiz (chapter 1)

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1. Balancing redox equation in acidic & basic medium respectively
2. Determine the limiting reactant when both amount of reactants are given.

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Chapter 3
1. Pre-read slide notes 1-32 except 19-26.
2.There is a quiz before lecture is started.
3. Determine position of element in Periodic Table based on electronic configuration and vice versa.

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Carry out Experiment 2
1. Make sure you know the amount and also chemicals that need to place in the apparatus.
2. Experiment 2: https://youtu.be/CN6baDZea7s
3. Post lab Experiment 2: https://youtu.be/DQyH_r2HZgs

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12 Sep 2022
1. Tutorial question (2.1)
2. Group discussion (True/False) related with quantum number
Pre Read
-What do you understand about electron configuration?

-How many types of electron configuration that you learnt from the lecture?

-How many rules/principles that you need to follow when writing electron configuration?

3. Discuss the 3 principles in writing electron configuration.
4. Explain the extra stability for half-filled and full-filled orbital. Discuss tutorial question 2.3

15 Sep 2022
1. Group discussion (2.3)
2. Quiz 4 (Chapter 2)

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Chapter 2
1. Different between orbit & orbital
2. Four quantum number of electron
3. Shape of orbital
4. Types of electronic configuration (spdf notation & orbital diagram)
5. Principles applied when writing electronic configuration

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22 Aug 2022
1. Determine amount of product formed
2. Determine amount of excess reactant left
3. Determine percentage yield

25 Aug 2022
1. Quiz 2 (Chapter 1)
2. Tutorial questions

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1. Definition concentration measurements
2. Problem solving in concentration measurements (without + with concentration)

Link video
https://youtu.be/Q6X0J40jzB4

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15 Aug 2022
1. Discuss tutorial 1.1 & 1.2
2. Group quiz concentration measurements
3. Balance half equation (step 1-5)
https://youtu.be/9jQeVOfaVYg
4.Balancing redox equation in both acidic and basic medium (step 6-10)
5. Determine limiting reactant

18 Aug 2022
1. Determine amount of product formed
2. Determine amount of excess reactant left
3. Determine percentage yield

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15 Aug 2022
1. Discuss tutorial 1.1 & 1.2
2. Group quiz concentration measurements
3. Balancing redox equation in both acidic and basic medium (step 6-10)
4. Determine limiting reactant
5. Determine amount of product formed

18 Aug 2022
1. Determine amount of excess reactant left
2. Determine percentage yield

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15 Aug 2022
1. Discuss tutorial 1.1 & 1.2
2. Group quiz for concentration measurements
3. Balance half equation (step 1-5)
https://youtu.be/9jQeVOfaVYg

18 Aug 2022
1. Balance redox equation
- acidic medium (step 6-7)
- basic medium (step 8-10)
2. Determine limiting reactant
3. Determine amount of product formed
4. Determine amount of excess reactant left
5. Determine percentage yield

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Pre-Lab Experiment 2
1. Handling volumetric flask
https://youtu.be/Z9BxP4p03yw
2. Handling burette
https://youtu.be/M-glDSAGAwM
3. Handling pipette
https://youtu.be/Z1rhrqd3sAs
4. Handling pipette filler
https://youtu.be/-kmHWIZ3nzs
5. How to carry out titration
https://youtu.be/CN6baDZea7s

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Chapter 2
1. Describe Bohr's atomic model (4 assumptions)
2. Formulae (5) used in the topic 2.1
3. Limitation Bohr's atomic model
4. Dual nature of electron

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1. Isotope notation
2. Average atomic mass
(abundance can be given in percentage/ratio/fraction)
3. Determine the percentage abundance based on average atomic mass
4. Empirical formula & molecular formula (mass given in grams, percentage, combustion)

Link video (Tutorial)
https://youtu.be/_B9g5lj4BNA
https://youtu.be/bPtWOpb0w4U
https://youtu.be/T76trqT8BF8

Link video (Summary)
https://youtu.be/yobbCEPTpQ4
https://youtu.be/vDCl84RVLlI

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Carry out Experiment 1
Procedure synthesize zinc chloride
https://www.youtube.com/watch?v=MufSNwg3CmA
How to use analytical balance?
https://www.youtube.com/watch?v=RdZTzCGm_HA
How to use hot plate with stirrer?
https://youtu.be/E1bFq5YLzGs

Comments based on video submitted:
1. No need to measure mass lid of crucible is ok. But then, make sure no lid is placed when measure mass of crucible and zinc chloride.
2. Make sure record mass of empty crucible.
3. Make sure mix zinc powder with hydrochloric acid in fume chamber.
4. Why need to place crucible on the white tile?
5. Why cannot place hot object on the analytical balance?

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08 Aug 2022
1.  Recall what learnt last week
2. Differentiate solute, solvent & solution
3. Definition concentration measurements
4. Quiz related with Week 1 topic

11 Aug 2022
1. calculation concentration measurement without and with assumption
2. group discussion

Link video (Tutorial)
https://youtu.be/Q6X0J40jzB4

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1. Differentiate solute, solvent & solution
2. Definition concentration measurements
3. Balance half equation
4. Definition limiting reactant

Link video
https://youtu.be/9jQeVOfaVYg

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08 Aug 2022
1.  Recall what learnt last week
2. Differentiate solute, solvent & solution
3. Definition concentration measurements
4. calculation concentration measurements without assumption

11 Aug 2022
1. calculation concnetration measurements with assumption
2. group discussion
3. Quiz related with Week 1 topic

Link video (Tutorial)
https://youtu.be/Q6X0J40jzB4