Question 1

Dedicated after-class support

Accepted Answer

Learning does not stop after class ends. At Explorer Academy, we provide a variety of support systems including our free 1-to-1 consultation, access to our student portal, study workshops and personalised exam paper review. Our science tutors and team are always ready to help students reach their potentials.

Question 2

Quality-Assured Curriculum

Accepted Answer

Our curriculum is carefully aligned with the O Level Chemistry syllabus. Lessons , study workshops and lessons materials are structured in a progressive manner that helps cultivate the right studying techniques and lay a strong foundation. Through our O Level Chemistry lessons, students will develop a comprehensive skillset in a positive learning environment.

Question 3

Learning through experiments

Accepted Answer

As a specialised science tuition in Singapore, our O Level Chemistry lessons are structured to ensure learning is done through exploration and discovery. Students will learn the wonders of chemistry through a series of hands-on experiments and demonstrations that will help students have a better visualisation of the chemistry concept learnt.

Question 4

Active Recalling for Science

Accepted Answer

At Explorer Academy, we developed a series of active recall strategies tailored specifically for science. Our approach goes beyond strengthening memory, it deepens understanding, making learning chemistry more accessible and effective to different learners.

Question 5

Learning from experts

Accepted Answer

Our team of science tutors consists of former MOE teachers and educators with 5 to 12 years of teaching experience. Many of our tutors hold advanced qualification such as Master’s degrees in Curriculum Development or Special Educational Needs (SEN). We regularly conduct teacher development workshop to ensure our tutors remain up-to date with the latest O Level Chemistry syllabus in Singapore and teaching methodologies.

Question 6

A place for all learners

Accepted Answer

We understand that every learner is unique and there is no one-size-fit-all approach. At Explorer Academy we provide a holistic approach in teaching. Our chemistry curriculum, lesson materials and science workshops are designed to support student with varying styles to succeed in their own way.

Question 7

Qualitative Analysis

Accepted Answer

Deduce the cation (aluminium, ammonium, calcium, copper(II), iron(II), iron(III) and zinc) present in an aqueous solution through the formations of precipitates (if any) and their solubility in aqueous sodium hydroxide and/or aqueous ammonia.
Describe tests to identify the following anions:
- Carbonate (by adding dilute acid and subsequent use of limewater)
- Chloride (by adding nitric acid and aqueous silver nitrate)
- Iodide (by adding nitric acid and aqueous silver nitrate)
- Sulfate (by adding nitric acid and aqueous barium nitrate)
- Nitrate (by reduction with aluminium in aqueous sodium hydroxide
to ammonia and subsequent use of damp red litmus paper)
Describe tests to identify the following gases:
- Ammonia (using damp red litmus paper)
- Carbon dioxide (using limewater)
- Chlorine (using damp litmus paper)
- Hydrogen (using a burning splint)
- Oxygen (using a glowing splint)
- Sulfur dioxide (using acidified potassium manganate (VII))

Question 8

Electrochemistry

Accepted Answer

Describe electrolysis as the conduction of electricity through an electrolyte (molten or aqueous solution) to form a chemical change at the electrode.
Apply the idea of selective discharge based on:
(i) Cations (through the metal reactivity series)
(ii) Anions (halides, hydroxides, sulfates)
(iii) Concentration effects (diluted and concentrated electrolyte)
Predict the likely products and construct ionic equations occurring on the electrodes for electrolysis reaction with:
(i) a molten binary ionic compound using inert electrodes
(ii) an aqueous electrolyte
Describe the electrolysis of aqueous copper(II) sulfate with copper electrodes as a means of purifying copper.
Applying the concepts of reactivity series and redox reaction, describe the production of electrical energy from simple cells.
Describe hydrogen, derived from water or hydrocarbons, as a potential fuel, reacting with oxygen to generate electricity directly in a hydrogen fuel cell.

Question 9

Organic Chemistry

Accepted Answer

Describe Biofuel as a renewable alternative to natural gas and crude oil and state how biofuel is more environmentally sustainable in terms of carbon dioxide emission.
Describe the separation technique by fractional distillation to produce fractions of hydrocarbon and state the uses of each fraction.
Describe homologous series and explain the relationship between the increase in the size and mass of organic molecules and its physical properties (viscosity and melting and boiling point).
Show an understanding of chemical and physical properties of alkane, alkene, alcohol and carboxylic acid.
Apply the concept of isomerism and draw structures of branched and unbranched alkane, alkene and alcohol.
Describe the manufacture of margarine by the addition of hydrogen to unsaturated vegetable oils to form a solid product.
Describe polymers as large molecules built up from small units (monomers), different polymers having different units and/or different linkages.
Show an understanding of the formation of polymers from monomers through reactions such as addition polymerisation and condensation polymerisation.
State the uses of poly(ethene), nylon from polyamide and terylene from polyester.
Describe the use of physical methods and chemical methods (depolymerisation and cracking) to recycle plastics and discuss the social, economic and environmental issues of recycling plastic.
Using hydrolysis of polyesters in the presence of an acid catalyst, explain the process of depolymerization of polymers to form monomers.

Question 10

Maintaining Air Quality

Accepted Answer

Describe the volume composition of gases in dry air to be approximately 78% nitrogen, 21% oxygen, 0.04% carbon dioxide and the remainder being noble gases (mainly argon).
State the sources and harmful effects of atmospheric pollutants such as carbon monoxide; methane; nitrogen oxides (NO and NO2); ozone; sulfur dioxide; unburned hydrocarbons.
Describe the use of catalytic converter to remove carbon monoxides, nitrogen oxides and unburnt hydrocarbon through redox reaction.
Describe the use of calcium carbonate to remove acid rain and in flue gas desulfurisation.
Discuss the importance of the ozone layer and the problems involved with the depletion of ozone by reaction with chlorinecontaining compounds, chlorofluorocarbons (CFCs)
Describe the carbon cycle through processes such as combustion, aerobic respiration and photosynthesis and discuss the importance of carbon cycle in regulating the amount of carbon dioxide in the atmosphere.
Describe the source for excessive greenhouse gases (carbon dioxide and methane) emission and environmental impacts of global warming.

Question 11

Chemical Bonding

Accepted Answer

Describe and illustrate using ‘dot-and-cross’ diagrams, the formation of ionic bonds by electron loss/gain to achieve noble gas electronic configuration.
Relate the ionic bond physical properties (melting point, electricity conductivity, solubility) of ionic compounds to their lattice structure and electrostatic attraction.
Describe and illustrate using ‘dot-and-cross’ diagrams, the formation of covalent bonds by the sharing of electrons to achieve noble gas electronic configuration.
Relate the covalent bond physical properties (melting point, electricity conductivity, solubility) of covalent compounds to their simple molecular structure and van deer waals force.
Describe metallic bonding through the formation of a lattice of positive ions in a ‘sea of electrons’.
Deduce the physical properties of metals as solid with high melting and boiling point, malleable, good conductors of heat and electricity from their structure and metallic bond.
Compare the bonding and structures of macromolecules (diamond and graphite) and deduce their properties such as electrical conductivity, lubricating or cutting action.

Question 12

Chemical formula and equation

Accepted Answer

State the symbols of the elements and formulae of the compounds mentioned in the periodic table.
Deduce formulae of ionic compounds with polyatomic ions such as nitrate, sulfates, phosphate, hydroxide and ammonium ions.
Deduce the formulae of simple compounds from the relative numbers of atoms present
Construct chemical equations and ionic equations with state symbols.

Question 13

The Mole Concept and Stoichiometry

Accepted Answer

Define terminology such as relative atomic mass, Ar, relative molecular mass, Mr and mole.
Calculate the percentage mass of an element in a compound.
Calculate empirical and molecular formulae from relevant data
Apply concepts from stoichiometric reacting masses and volumes of gases (one mole of gas occupies 24 dm3 at room temperature and pressure) to solve problems with and without limiting reactants.
Apply the concept of solution concentration (in mol/dm3 or g/dm3)
to process and solve problem from the volumetric experiments (e.g. titration) data.
Calculate % yield and % purity

Question 14

Acid-Base Chemistry

Accepted Answer

Describe the meanings of the terms acid and alkali in terms of the ions they produce in aqueous solution.
Describe neutrality and relative acidity and alkalinity in terms of relative H+ and OHion concentrations, colour in Universal Indicator and the pH scale.
Describe the chemical reactions of acids with metals, carbonates and bases (neutralisation) to form salts.
Describe the chemical and physical tests to test the presence of acids and alkaline.
Describe the chemical reactions of bases with acids and ammonium salts.
Apply the concepts of chemical properties of acids and bases to describe the importance of controlling the pH in soils and how excess acidity can be treated using calcium hydroxide (liming).
Classify oxides as acidic, basic, amphoteric or neutral based on metallic/non-metallic character

Term 1	Term 2	Term 3	Term 4
Experimental Chemistry	Chemical Formulae & Equations	The Periodic Table	End-Of-Year Preparation
Kinetic Particle Theory	Mole Concept & Stoichiometry	Reactivity Series
Atomic Structure	Acids and Bases	Redox Reaction
Chemical Bonding	Salts	Ammonia
	Qualitative Analysis

Term 1	Term 2	Term 3	Term 4
Rate of Reaction	Organic Chemistry: Fuel and Crude Oil	Thematic Chemistry Revision	O Level Chemistry Preparation
Chemical Energetics	Organic Chemistry: Hydrocarbon	Prelim Preparation	Chemistry Application-based questions revision
Electrochemistry	Organic Chemistry: Alcohols, Carboxylic Acids and Esters
	Polymers
	Maintaining Air Quality

Class	Day	Time
Chemistry	Tuesday	5:30 PM - 7:00 PM
Chemistry	Wednesday	5:30 PM - 7:00 PM
Chemistry	Saturday	11:15 AM - 12:45 PM
Chemistry	Sunday	1:45 PM - 3:15 PM

Class	Day	Time
Chemistry	Wednesday	5:30PM - 7:00PM
Chemistry	Saturday	1:45PM - 3:15PM
Chemistry	Sunday	11:00AM - 12:30PM

O' Level Chemistry Tuition

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