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O Level Chemistry – 2 hrs Each Lesson

1. Atomic Structure/Ionic, Covalent and Metallic Bonding – 2 lessons
2. Formulae & Equation Writing – 1 lesson
3. Mole & Chemical Calculations – 2 lessons
4. Acids and Bases – 1 lesson
5. Salts – 1 lesson
6. Chemical Analysis – 1 lesson
7. Metals – 2 lessons
8. Periodic Table – 2 lessons

If you need help in the above topics, please contact Angie @96790479 or Mr Ong 98639633

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O Level Chemistry Tuition Singapore/Chemistry O Level Tuition/Tutor

2014 Secondary 4 Preparatory Course

11-Nov Mon 10.30am to 12pm 1.5 hrs Chemical Bonding 1

12-Nov Tue 10.30am to 12pm 1.5 hrs Chemical Bonding 2

13-Nov Wed 10.30am to 12pm 1.5 hrs The Mole 1

14-Nov Thu 10.30am to 12pm 1.5 hrs The Mole 2

15-Nov Fri 10.30am to 12pm 1.5 hrs Chemical Calculation 1

18-Nov Mon 10.30am to 12pm 1.5 hrs Chemical Calculation 2

19-Nov Tue 10.30am to 12pm 1.5 hrs Acids and Bases 1

20-Nov Wed 10.30am to 12pm 1.5 hrs Acids and Bases 2

21-Nov Thu 10.30am to 12pm 1.5 hrs Salts 1

22-Nov Fri 10.30am to 12pm 1.5 hrs Salts 2

If you need help in the above topics, please contact Angie @96790479 or Mr Ong 98639633

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A-Level Chemistry Tuition Singapore/H2 Chemistry Tuition/JC Chemistry Tutor

Power Revision

A Level Chemistry – 2 hrs Each Lesson

1. Atoms Molecules and Stoichiometry – 2 lessons
2. Chemical Bonding – 2 lessons
3. Chemical Energetics- 2 lessons
4. Reaction Kinetics – 2 lessons
5. Chemical Equilibrium – 2 lessons
6. Ionic Equilibrium – 2 lessons
7. Introduction Organic/Alkanes/Alkenes – 2 lesssons
8. Arenes – 1 lessons
9. Halogen Derivatives – 2 lesons
10. Hydroxy Compounds – 2 lessons
11. Carbonyl Compounds – 2 lessons
12. Carboxylic Acids and Derivatives – 2 lessons

For enquirers please contact HP 98639633 or Hp 96790479

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Glossary of Terms

1. State
A concise answer with little or no supporting argument, e.g. a numerical answer that can be obtained ‘by inspection’ is required.

2. List
A number of points, generally each of one word, with no elaboration is required. Where a given number of points is specified, this should not be exceeded

3. Explain
Reasoning or some reference to theory is required (depending on the context)

4. Describe
State in words (using diagrams where appropriate) the main points of the topic. It is often used with reference either to particular phenomena (where answers should include reference to observations associated) or to particular experiments.

5. Discuss
A critical account of the points involved in the topic should be provided.

6. Outline
Be concise i.e. restrict the answer to giving the essentials only.

7. Predict
Make a logical connection between other pieces of information. Such information may be wholly given in the
question or may depend on answers extracted in an early part of the question.

8. Deduce
Used in a similar way as predict except that some supporting statement is required, e.g. reference to a law/principle, or the necessary reasoning is to be included in the answer

9. Comment
It is an open-ended instruction, inviting one to recall or infer points of interest relevant to the context of the question, taking account of the number of marks available.

10. Suggest
It is used in two contexts, i.e either to imply that there is no unique answer (e.g. in chemistry, two or more substances may satisfy the given conditions describing an ‘unknown’), or to imply that candidates are
expected to apply their general knowledge to a ‘novel’ situation, one that may be formally ‘not in syllabus’.

11. Find
Can be interpreted as calculate, measure, determine etc

12. Calculate
A numerical answer is required. In general working should be shown.
Note:The misuse of units and/or significant figures is liable to penalty.

13. Determine
It implies that the quantity cannot be measured directly but is obtained by calculation, substituting measured and known values of other quantities into a standard formula.

14. Sketch
When applied to graph work, the shapes and/or position o the curve need only be qualitatively correct but some quantitative aspects (e.g. passing through the origin, having an intercept at a particular value) may be looked for.

In diagrams, a simple and freehand drawing is acceptable but care should be taken over proportions and the clear exposition of important details.

15. Construct
Often used in relation to chemical equations where one is expected to write a balanced chemical equation,not by factual recall but by analogy or by using information in the question.

16. Compare
Both similarities and differences between things or concepts should be provided.

17. Classify
Group things based on common characteristics.

18. Recognise
Often used to identify facts, characteristics or concepts that are critical (relevant/appropriate) o the understanding of the situation, event, process or phenomenon.

For exam based questions with solutions please contact @9863 9633

[admin]

A-Level Chemistry Tuition Singapore/H2 Chemistry Tuition/JC Chemistry Tutor

Glossary of Terms

1. State
A concise answer with little or no supporting argument, e.g. a numerical answer that can be obtained ‘by inspection’ is required.

2. List
A number of points, generally each of one word, with no elaboration is required. Where a given number of points is specified, this should not be exceeded

3. Explain
Reasoning or some reference to theory is required (depending on the context)

4. Describe
State in words (using diagrams where appropriate) the main points of the topic. It is often used with reference either to particular phenomena (where answers should include reference to observations associated) or to particular experiments.

5. Discuss
A critical account of the points involved in the topic should be provided.

6. Outline
Be concise i.e. restrict the answer to giving the essentials only.

7. Predict
Make a logical connection between other pieces of information. Such information may be wholly given in the
question or may depend on answers extracted in an early part of the question.

8. Deduce
Used in a similar way as predict except that some supporting statement is required, e.g. reference to a law/principle, or the necessary reasoning is to be included in the answer

9. Comment
It is an open-ended instruction, inviting one to recall or infer points of interest relevant to the context of the question, taking account of the number of marks available.

10. Suggest
It is used in two contexts, i.e either to imply that there is no unique answer (e.g. in chemistry, two or more substances may satisfy the given conditions describing an ‘unknown’), or to imply that candidates are
expected to apply their general knowledge to a ‘novel’ situation, one that may be formally ‘not in syllabus’.

11. Find
Can be interpreted as calculate, measure, determine etc

12. Calculate
A numerical answer is required. In general working should be shown.
Note:The misuse of units and/or significant figures is liable to penalty.

13. Determine
It implies that the quantity cannot be measured directly but is obtained by calculation, substituting measured and known values of other quantities into a standard formula.

14. Sketch
When applied to graph work, the shapes and/or position o the curve need only be qualitatively correct but some quantitative aspects (e.g. passing through the origin, having an intercept at a particular value) may be looked for.

In diagrams, a simple and freehand drawing is acceptable but care should be taken over proportions and the clear exposition of important details.

15. Construct
Often used in relation to chemical equations where one is expected to write a balanced chemical equation,not by factual recall but by analogy or by using information in the question.

16. Compare
Both similarities and differences between things or concepts should be provided.

17. Classify
Group things based on common characteristics.

18. Recognise
Often used to identify facts, characteristics or concepts that are critical (relevant/appropriate) o the understanding of the situation, event, process or phenomenon.

For exam based questions with solutions please contact @9863 9633

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TO Master to PERFECTION before A’levels – Part 3

4. Electrochemistry
• Predict qualitatively how the value of an electrode potential varies with the concentration of the aqueous ion
*Could be a disguised change e.g.adding NaOH (aq) to ppt. Mn+.

Refer to our consolidated list last term

5. Chem Eqm
• Apply LCP to deduce qualitatively (from appropriate information)
the effects of changes in concentration, pressure or temperature, on a system at equilibrium.
• Deduce whether changes in concentration, pressure or temperature or the presence of a catalyst affect the value of the equilibrium constant for a reaction

E.g. Given Kc ↑ when temp ↓, predict if reaction is exo/endo.
6. Ionic Eqm
• Explain the choice of suitable indicators for acid-base titrations,given appropriate data
• Explain how buffer solutions (i)control pH (ii) describe and explain
their uses, including the role of H2CO3/HCO3– in controlling pH in
blood

3 main points.
With equations with SINGLEHEADED arrows

For exam based questions with solutions please contact @9863 9633

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Energy Changes

Important Definitions

1. An exothermic reaction is a reaction that gives out heats energy to the surroundings.

2. An endothermic reaction is a reaction that absorbs heat energy from the surroundings.

3. Activation energy is the minimum energy that reacting particles must posses in order for a chemical reaction to take place.

4. An clergy profile diagram is used to show the activation energy of a reaction.

5. A fuel is a substance that burns easily in air to give out heat energy.

6. A fuel cell is a chemical cell in which the chemical energy of a fuel is converted directly into electrical energy.

For more key points and exam based questions with full worked solutions please contact Mr Ong @98639833

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TO Master to PERFECTION before A’levels – Part 2

1. Atomic Structure • Ionisation Energy (Trend across the period + 2 anomalies, Down the gp, successive IE,*TM)

Remark
• Predicting position from successive IE
Refer to AMS, Gases and Atomic Structure Revision Notes

2. Bonding
• Boiling point/melting point
• Volatility
• Electrical conductivity
• Solubility

3. Energetics (entropy)
• Discuss the effects on the entropy of a chemical system by the
following:
(i) change in temperature
(ii) change in phase
(iii) change in the number of particles (especially for gaseous
systems)
(iv) mixing of particles

Remark
• Predict the effect of temperature change on the spontaneity of a
reaction, given standard enthalpy and entropy changes disorderliness”/”ways to arrange particles” are key words.
Refer to entropy lect notes.

Using Gibbs equation ΔG=ΔHTΔS.
Make sure you are comfortable with putting your thoughts into words.

For exam based questions with solutions please contact @9863 9633

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TO Master to PERFECTION before A’levels – Part 1

Standard Definitions (Don’t Memorize. But appreciate and understand why key terms are important)

– Relative atomic, isotopic, molecular and formula mass, based on the 12C scale (just give mathematical expression)
– Mole in terms of the Avogadro constant
– VSEPR (2 assumptions)
– Basic assumptions of the kinetic theory as applied to an ideal gas
– Standard enthalpies (11 of them)
– Hess’ Law
– Entropy
– Standard electrode potential and standard cell potential
– Dynamic Equilibrium, LCP
– Strong and weak acids and bases
– Kc, KP, Ka, Kb, Kw, KSP,pH etc. (m. expression)
– Rate of reaction; rate equation; order of reaction; rate constant; (m. expression)
– Half life of a reaction
– Rate-determining step
– Activation energy
– Catalysts
– Transition metal, ligands, complex, coordination number
– Proteins 1o,2o,3o structure, Denaturation

Standard Explanations (must be concise (save time), accurate and complete) – You must know this so well you have are absolutely confident of reproducing them under stressful exam conditions.

For exam based questions with solutions please contact @9863 9633

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Colour Summary

Flame Test Colors
Li Deep red
Na Yellow
K Violet
Mg Bright white
Ca Orange-red
Sr Red
Ba Green
Cu Blue-green
P Pale blue-green
S Blue
Fe Gold
Pb Blue-white
Zn Blue-green

Aqueous Ion Colors
Cu+ Green
Cu2+ Blue
[CuCl4]2- Yellow
Cu(NH3)4 2+ Dark Blue; produced when ammonia is added to Cu2+ solutions

Fe2+ yellow-green (depending on the anion)
Fe3+ orange-red (depending on the anion)
FeSCN]2+ Red-brown, Wine-red to dark orange

Co2+ Pink
CoCl42- Blue (Co2+ with HCl will form a CoCl4 2- complex that is blue)

Cr3+ Violet (Cr(NO3)3 to Green (CrCl3)
CrO4 2- Yellow
Cr2O7 2- Orange

Ni2+ Green

Mn2+ Pink
MnO4 – Purple (Mn w/ +7 oxidation state is purple)
MnO4 2- Green

Pb3+ blue-green (Pb2+ and Pb4+ are colorless)

V2+ violet
V3+ blue-green

Ti(H2O)6 3+ Purple

For exam based questions with solutions please contact @9863 9633

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The Periodic Tables

Important Definitions

1. A group is a vertical column of elements in the Periodic Table.

2. A period is a horizontal row of elements in the Periodic Table.

3. A metalloid is an element that has the properties of both a metal and a non-metal

4. An alkali metals are the Group I elements.

5. The halogens are the Group VII elements.

6. The noble gases are the Group 0 or Group VIII elements.

7. The transition elements are a block metallic elements between Group II and II in the Periodic table.

8. A catalyst is a substance that increases the speed of chemical reaction.

For more key points and exam based questions with full worked solutions please contact Mr Ong @98639833

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Electrolysis

Important Definitions

1. An electrolytic cell is a set of apparatus that uses electrical energy to produce chemical reactions.

2. Electrolysis is the process of decomposition of a compound by electricity.

3. The anode is the positive electrode and the cathode is the negative electrode of an electrolytic.

4. An electrolyte is a substance that conducts electricity in the molten state or in aqueous solution.

5. Cations are positive ions and anions are negative ions

6. The discharge of ions is the process of gaining or losing electrons at the electrode.

7. An Inert electrode is an electrode that does not take part in chemical reaction during electrolysis.

8. A reactive electrode is an electrode that participates in chemical reactions during electrolysis.

9. Electroplating is the process of coating an object with a thin layer of metal using electrolysis.

10. A simple cell is a devise that uses chemical reactions to produce electricity.

For more key points and exam based questions with full worked solutions please contact Mr Ong @98639833

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Metals

Important Definitions

1. An alloy is a mixture of metal with one or a few other elements.

2. The reactivity series is a series of metals arranged in the order of their chemical reactivity, from the most reactivity to the lease reactivity.

3. Displacement reaction of metals is a redox reaction in which a more reactive metal displaces a less reactive metal to form its salt solution.

4. Galvanising is the coating of iron or steel on zinc for protection against corrosion.

For more key points and exam based questions with full worked solutions please contact Mr Ong @98639833

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Oxidation and Reduction

Oxidation
– Gain of oxygen
– Gain of oxidation number
– loss of hydrogen
– loss of electron

Reduction
– loss of oxygen
– loss of oxidation number
– Gain of hydrogen
– Gain of electron

1. A redox reaction is a reaction involving oxidation and reduction.

2. An oxidising agent is a substance that causes oxidation on another substance.

3. An reducing agent is a substance that causes reduction on another substance.

For more key points and exam based questions with full worked solutions please contact Mr Ong @98639833

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FAQ – Gases

Gases

Difference between assumptions and conditions

• 2 assumptions of ideal gas
o Negligible intermolecular forces
o Negligible particle volume compared to volume of container

• 2 conditions at which a gas acts most ideally
o High temperature
o Low pressure

For exam based questions with solutions please contact @9863 9633

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