Parents looking for a Secondary 2 Chemistry tutor in Hougang often describe the problem this way: “My child can recognise the words atom, element and molecule but cannot explain the particle diagrams.” The best starting point is to rebuild those distinctions and connect them to the chemical symbols and formulae that students encounter as they move towards upper-secondary Science.
At eduKateSG, our premium three-student small-group tutorials help learners from Hougang, Kovan and Buangkok make sense of atoms, molecules, ions, particle models, elements and compounds. For most Secondary 2 students these are Chemistry-related ideas within lower-secondary Science, not a separate Pure Chemistry examination. Our reference teaching centre is 8 Fourth Avenue, Singapore 268674, near Sixth Avenue MRT, not physically in Hougang. The established reference lesson is 1.5 hours weekly for three pupils; confirm the actual available class and timetable during consultation.
The immediate goal is practical: a student should be able to explain why oxygen is written O₂, why water is H₂O, why Na⁺ is still sodium, and why a formula such as NaCl does not represent an isolated molecule in an ordinary solid crystal. The depth should follow the child’s actual school G1, G2 or G3 Science programme. We do not push every learner into advanced ionic Chemistry before the foundation is secure.
Arrange a parent–student Science consultation or enquire about small-group teaching.
Why symbols suddenly make Science feel more difficult
Lower-secondary students often begin with visible objects and familiar changes: ice melting, salt dissolving, gas filling a balloon or iron rusting.
Chemical notation asks them to describe an invisible model with compressed symbols. The letters H and O no longer mean everyday labels; they represent particular elements. A subscript indicates an atom count in a chemical formula. A charge sign refers to an ion.
A student can memorise the formula of water yet still think it means two kinds of gas floating together. Another can draw three identical circles but cannot say whether the picture shows three atoms, one molecule or the basic repeating unit of a giant structure.
A good Chemistry-related Science tutor finds the confusion at that level. We teach what the symbols represent before asking students to perform complicated calculations with them.
Matter is made of particles—but which particles?
The word particle is useful because it can refer generally to tiny constituents of matter in a simplified scientific model. However, it does not automatically mean the same specific object in every context.
Depending on the substance and the syllabus, the particles might be atoms, molecules, ions or formula units used to describe ionic arrangements.
A glass of water contains an enormous number of water molecules, each consisting of bonded hydrogen and oxygen atoms. Sodium chloride in water is best described at the relevant level using dissolved sodium and chloride ions.
The tutor asks a child what each circle or label in a diagram is intended to represent. A scientific model becomes confusing when the student treats every drawn circle as the same kind of particle in every situation.
What is an atom?
An atom is a basic chemical unit of an element, with a nucleus containing protons and, in most atoms, neutrons, surrounded by electrons.
An element’s identity is determined by its number of protons, or atomic number. A neutral atom has equal numbers of protons and electrons, because their positive and negative charges balance.
The scale is important: real atoms are extremely small, and an ordinary classroom particle diagram is a simplification rather than a photograph.
Students do not need to memorise an elaborate quantum-mechanical model to recognise an atom. They do need to distinguish an atom of oxygen from the common oxygen molecule and to understand why electron gain or loss can produce an ion without changing the element.
What is a chemical element?
An element is a substance consisting of atoms that all have the same proton number. Carbon, hydrogen, helium, copper and oxygen are familiar elements.
A common mistake is to say that an element must contain only one atom. That is false. A sample of pure oxygen gas contains enormous numbers of oxygen molecules, each typically O₂, but oxygen remains an element because each atom in those molecules is oxygen.
Likewise, a piece of copper contains large numbers of copper atoms, arranged in a metallic structure. It is still an element because the atoms share the same elemental identity.
The tutor helps learners distinguish the number of atoms in a sample, the number of types of atoms and the number of atoms in one molecule. These are three different questions.
Why some elements are written with a subscript
In common school examples, hydrogen gas is H₂, oxygen gas O₂ and nitrogen gas N₂. Their molecules contain two atoms of the same element bonded together.
Other elements may occur in different elemental structures. Helium is a noble gas commonly represented as individual He atoms. A piece of copper is represented as Cu rather than a fixed molecule Cu₂.
A child may ask, “Why can’t I write all elements as single letters?” Because a chemical symbol identifies an element, while a chemical formula represents the composition of the relevant substance or particle.
The symbol O identifies oxygen as an element; O₂ describes the familiar diatomic oxygen molecule. The number matters.
See the related explanation: Why oxygen is O₂ but helium is He.
What is a molecule?
A molecule consists of two or more atoms chemically bonded together as a discrete unit. The atoms may belong to the same element or to different elements.
O₂ is a molecule of an element. H₂O is a molecule of a compound. CO₂ is another familiar molecular compound.
A student sometimes assumes that every molecule must contain atoms of different elements. That is incorrect. An oxygen molecule has two atoms of the same element.
Another mistake is to claim that every compound is made of separate molecules. Many familiar ionic compounds form extended lattices, so a formula can express their ionic ratio rather than the identity of an independent molecule.
We teach the simplest correct distinction before extending to more complex bonding and structure.
Molecule versus compound: a helpful comparison
A compound is a substance in which different elements are chemically combined in fixed proportions. Many compounds are molecular, but not every compound consists of discrete molecules.
Water, H₂O, is a molecular compound. It contains hydrogen and oxygen chemically bonded in each water molecule.
Sodium chloride, NaCl, is an ionic compound. In an ordinary sodium chloride crystal, the ions form an extended three-dimensional arrangement. The formula NaCl describes the simplest sodium-to-chloride ion ratio.
Therefore, the statements “every compound is a molecule” and “every molecule is a compound” are both false.
A good tutor asks for one counterexample to each statement. This is more powerful than repeating two definitions from a worksheet.
Worked comparison: oxygen, water and salt
Consider three pure substances:
Oxygen gas, O₂: contains molecules with two oxygen atoms. It is an element because the atoms are all oxygen.
Pure water, H₂O: contains molecules with hydrogen and oxygen atoms in a fixed 2:1 ratio. It is a compound.
Solid sodium chloride, NaCl: contains an extended ionic arrangement with sodium and chloride ions in a 1:1 ratio. It is a compound, but not a collection of isolated NaCl molecules.
Now change the problem. Suppose sodium chloride is dissolved in water. The sample is a mixture of water and dissolved ions, rather than a single compound newly formed by dissolving.
The student has to move between classification, particle identity and physical state. That combination is exactly what makes the question valuable.
Chemical symbols: capital letters matter
An element symbol begins with a capital letter, and any second letter is lowercase. Co represents cobalt, while CO represents carbon monoxide, a compound consisting of carbon and oxygen.
A learner who writes “NA” instead of Na or “cl” instead of Cl may accidentally create incorrect notation.
This is not about decorative handwriting. Chemical symbols are a precise communication system, and changing their capitals can change their meaning.
We encourage students to practise writing names and symbols in both directions: element name to symbol, then symbol back to name.
A short unfamiliar matching task reveals whether the child understands the notation or has only memorised the look of a textbook chart.
Formula subscripts: what the little number means
In H₂O, the subscript 2 belongs to hydrogen. One water molecule contains two hydrogen atoms and one oxygen atom.
In CO₂, one carbon dioxide molecule contains one carbon atom and two oxygen atoms.
If no subscript is printed after an element symbol, the implied number is one within that formula unit or molecule.
A student should be able to count atoms in simple molecular formulae without confusing the number of letters with the number of atoms.
For example, one molecule of C₂H₆ contains 2 carbon atoms and 6 hydrogen atoms, giving 8 atoms in total.
Counting letters alone would produce the wrong answer.
Coefficients versus subscripts: two very different numbers
Consider 3H₂O. The coefficient 3 means three water molecules in the particle-counting context. Each contains two hydrogen atoms and one oxygen atom.
Therefore, three water molecules contain 6 hydrogen atoms and 3 oxygen atoms.
The formula H₂O remains unchanged. We have changed how many molecules are represented, not the chemical identity of a water molecule.
By contrast, H₂O₂ is hydrogen peroxide, a different compound.
This distinction prepares students for balanced chemical equations later. We may introduce it gently as a model-reading skill even before the school’s formal equation-balancing unit.
A simple counting question: 2CO₂ versus CO₂
A pupil is shown the formula 2CO₂ and asked how many carbon and oxygen atoms are represented.
There are two carbon dioxide molecules. Each has one carbon atom and two oxygen atoms.
Total carbon atoms = 2 × 1 = 2. Total oxygen atoms = 2 × 2 = 4.
Now show 3CO₂. The new counts are three carbon and six oxygen atoms. The atom ratio stays 1:2 in each molecule.
A useful follow-up is: “Does doubling the number of carbon dioxide molecules turn them into another substance?” No. The amount changes but the chemical identity does not.
We use changed numbers to establish understanding rather than simply repeat the first worked calculation.
Protons, neutrons and electrons: which one defines the element?
The number of protons defines the element. Neutrons contribute to the mass of a nucleus; electrons carry negative charge and participate in chemical interactions.
A neutral sodium atom has 11 protons and 11 electrons. A sodium ion Na⁺ has lost one electron under the familiar ionic model, so it has 11 protons and 10 electrons.
It remains sodium because its proton number has not changed.
A student who says that Na⁺ became neon merely because it now has 10 electrons has confused electron configuration with elemental identity. It can have the same electron count as neon without having the same number of protons.
This is an important distinction for learners preparing for later atomic structure.
What is an ion?
An ion is an atom or group of bonded atoms with a net electrical charge. It forms when the numbers of positively charged protons and negatively charged electrons are unequal.
A cation has a net positive charge. An anion has a net negative charge.
A sodium atom losing one electron forms Na⁺. A chlorine atom gaining one electron forms Cl⁻. The nuclei remain those of sodium and chlorine respectively.
The ion model is introduced at the depth appropriate to the child’s school programme. Not every G1, G2 or G3 Secondary 2 question requires complex polyatomic ions, and we do not make advanced ion-formula drills the first lesson for a confused beginner.
The priority is that charge arises from an electron imbalance, not a mysterious extra atom or change in proton identity.
Worked example: sodium, magnesium and chloride ions
Consider three familiar ions.
Na⁺: one fewer electron than a neutral sodium atom; charge +1.
Mg²⁺: two fewer electrons than a neutral magnesium atom; charge +2.
Cl⁻: one more electron than a neutral chlorine atom; charge −1.
A common error is to read the 2+ on Mg²⁺ as meaning that the ion contains two magnesium atoms. It does not. It is a charge magnitude, not a subscript.
The tutor places Mg²⁺ beside Mg₂ to illustrate that superscripts and subscripts have entirely different jobs. The second form would not mean a magnesium ion with charge +2.
This precise notation is essential to avoid accumulating errors when students reach ionic bonding and formula writing.
How an ionic formula balances charge
A neutral ionic compound has a total positive charge balanced by its total negative charge.
For sodium chloride, Na⁺ and Cl⁻ combine in a 1:1 ratio, giving formula NaCl.
For magnesium chloride, Mg²⁺ requires two chloride ions, each Cl⁻, to balance its +2 charge. The simplest formula is MgCl₂.
The charge check is:
(+2) + 2(−1) = 0.
The subscript 2 does not turn the magnesium ion into a molecule. It tells us the simplest ratio of ions in the neutral formula.
This can be introduced as an extension for an able Secondary 2 learner preparing for upper-secondary Chemistry, but it should not replace the lower-secondary atom and molecule foundation.
The distinction between mixing and reacting
Imagine mixing oxygen gas and hydrogen gas in a suitable conceptual example without initiating a reaction. The mixture contains the original hydrogen and oxygen molecules.
That mixture is not already water simply because both elements are present. Producing water involves a chemical reaction under appropriate conditions that creates a different compound.
We do not encourage any physical experiment combining combustible gases. The example is a conceptual particle-model comparison, not a laboratory instruction.
A tutor can draw separate H₂ and O₂ molecules on one side and H₂O molecules on the other, then explain that a reaction rearranges atoms into new chemical combinations.
The same elements may appear before and after, but the substances and bonding can differ.
Physical state changes do not change the molecular formula
Ice, liquid water and water vapour are different physical states of the same chemical substance, H₂O.
In a simple particle model, the arrangement and motion of molecules differ across these states. The water molecules do not turn into H₂ and O₂ merely because the water boils.
This is a surprisingly persistent misconception. Some pupils see a diagram of widely spaced gas particles and write that the particles have “broken apart into hydrogen and oxygen”.
We clarify that breaking intermolecular attractions during vaporisation is not the same as breaking the covalent bonds within a water molecule.
That distinction should be taught in age-appropriate language. Students need not master advanced bond energies before they can explain a physical change accurately.
Worked particle diagram: a pure element and a mixture
Imagine Diagram A shows five identical two-circle groups. Each group contains two bonded circles of the same colour, representing identical diatomic molecules of one element.
Diagram B shows three groups of one kind and four groups of a different kind, all unreacted and physically present together.
Diagram A represents a pure elemental molecular substance under the diagram’s key. Diagram B represents a mixture of two molecular substances, assuming each group represents a different chemical particle.
The student should not decide that Diagram B must be a compound merely because two colours appear. A compound would require the different elements to be chemically combined in its constituents.
The diagram’s key matters. Without knowing what the colours or shapes represent, we should not invent specific element identities.
How to read a particle diagram with four colours
A student may be given a box containing pairs of different-coloured circles. If every pair has exactly the same combination, the model may represent a pure compound made from molecules containing two types of atom.
If the box also contains unpaired circles of one colour, the drawing may instead represent a mixture of that compound with an elemental species, depending on the key.
We ask the child to answer two separate questions:
What particles are present? Identify the distinct chemical species represented.
Are different substances physically mixed, or are different elements bonded within each particle? Use bonding and identity rather than colour count alone.
This is the difference between reading a diagram and memorising the appearance of a familiar answer.
An extension: isotopes are not different elements
For a learner ready for an additional distinction, isotopes are atoms of the same element with equal proton number but different neutron number.
A chlorine-35 atom and a chlorine-37 atom each have 17 protons, so both are chlorine. Their neutron counts differ.
They belong to the same element because the proton number determines chemical identity. This explains why a Periodic Table can show a non-integer relative atomic mass: it reflects a weighted average across isotopes in the relevant sample.
A student should not conclude that every chlorine atom has “half a neutron” because the printed relative atomic mass is near 35.5.
This can be introduced gently as an enrichment connection, not as a mandatory advanced lesson for every Secondary 2 pupil.
What happens when salt dissolves?
Solid sodium chloride forms an ionic lattice. When it dissolves in water under ordinary conditions, it produces hydrated sodium and chloride ions distributed through the liquid.
It is not accurate to draw a dissolved salt solution as sodium chloride atoms that vanish when the solid disappears.
Nor is it correct to claim that the sodium and chloride ions cease to exist. Their distribution and interactions with water change.
At a basic level, the student should know that dissolving does not necessarily mean a chemical reaction creates a new substance, and that the resulting solution contains dissolved material.
For an advanced learner, distinguishing dissolved ions from intact molecular solutes such as sugar can strengthen the explanation.
Read Solubility, Dissolving and Separation Techniques.
Formulae and conservation of atoms
A balanced chemical equation expresses how reactant and product quantities relate while conserving atoms in ordinary chemical reactions.
An introductory example is:
2H₂ + O₂ → 2H₂O.
Count before reaction: four hydrogen atoms and two oxygen atoms. Count after reaction: four hydrogen atoms and two oxygen atoms.
The formulae identify substances, while the coefficients indicate how many molecules are involved in the simplified particle counting.
The student should not change H₂O into H₂O₂ to fix the oxygen count. That changes the product substance.
Equation balancing may be taught formally later, but this example can help a capable Secondary 2 learner see why the earlier distinction between coefficient and subscript matters.
The idea of a model’s limits
A particle drawing is a helpful way to reason about matter, but it cannot show every microscopic detail.
Circles may be enlarged so they can be seen. Interparticle distances are rarely drawn to scale. A fixed number of circles represents a much larger sample.
The colours are usually conventions chosen by the author of the diagram, not the actual visible colours of individual atoms.
A student who interprets one green circle as a tiny green atom has treated the model as a photograph.
We ask learners to explain what the drawing is intended to show and which features are merely representational choices. This is an important part of scientific literacy that carries forward into atomic structure and bonding.
A practical method for checking unfamiliar symbols
We encourage students to work in a clear sequence whenever a notation question appears:
1. Identify the element symbols using correct capitalisation. 2. Identify any subscripts, which belong to the chemical formula. 3. Identify any superscript charge signs, which describe ions. 4. Identify any coefficients, which multiply the stated quantity of the formula. 5. If a diagram is supplied, read its key before naming the particles. 6. Decide whether the question concerns composition, charge, amount or classification.
Each of these questions has a different purpose. They help a student avoid combining four ideas into one uncertain guess.
The tutor may remove the labels and give a changed example to see whether the learner can repeat the sequence independently.
A compound that looks like an element
Some formulas are deceptively compact. CO, for example, contains one carbon atom and one oxygen atom per molecule of carbon monoxide.
It is a compound, even though its formula contains only two letters. Co, with a lowercase o, is the symbol for cobalt, an element.
This is an excellent miniature diagnostic of symbol reading. A child who assumes capital letters have no chemical meaning may make an error even when their wider Science concept is correct.
A second example is NO₂, nitrogen dioxide, which is a compound with one nitrogen atom and two oxygen atoms. It should not be confused with N₂O merely because the same elements and total atom count appear.
Formula order and subscripts are part of substance identity.
Why the number of atom types matters
A pure sample of oxygen gas contains only oxygen atoms, despite the individual oxygen molecules containing two atoms.
A pure sample of water contains atoms of two types—hydrogen and oxygen—chemically combined in the same molecular ratio.
A mixture of water and ethanol contains two substances, each of which has its own chemical composition.
A question may ask for the number of substances, elements, molecules or atoms. The correct numerical answer depends on which quantity is being counted.
We teach learners to underline the noun. “How many elements?” is not the same as “How many different molecules?” or “How many atoms are present in one molecule?”
This single reading habit prevents many easily avoidable errors.
Common Secondary 2 misconceptions and their repair
Misconception 1: all particles are atoms. We compare atoms, molecules and ions, showing that “particle” is a broader modelling term.
Misconception 2: every element is made of isolated single atoms. We contrast He with familiar O₂ molecules.
Misconception 3: all molecules are compounds. We use O₂ as a counterexample.
Misconception 4: all compounds consist of separate molecules. We introduce ionic lattices and the role of formula units at an appropriate level.
Misconception 5: a chemical symbol’s capitalisation is optional. We contrast Co and CO.
Misconception 6: a subscript is the same as an ion charge. We compare MgCl₂ with Mg²⁺ and explain the position of the notation.
Misconception 7: a positive ion has gained protons. We show that ordinary ion formation involves electron transfer, not a change in proton number.
Misconception 8: boiling breaks water into hydrogen and oxygen. We distinguish intermolecular attractions from the covalent bonds within a water molecule.
Misconception 9: a mixture is always visibly nonuniform. We discuss clear homogeneous solutions.
Misconception 10: a particle diagram must reveal the exact real size or colour of atoms. We identify the limits and conventions of models.
Misconception 11: a coefficient changes the substance. We compare H₂O with 2H₂O and H₂O₂.
Misconception 12: two elements present together automatically form a compound. We distinguish physical mixing from chemical reaction.
The correct teaching response depends on which misconception the student actually holds.
How a three-student tutorial helps
Imagine three learners looking at a particle diagram of water.
One thinks the two hydrogen atoms are separate hydrogen gas molecules. Another recognises H₂O but believes the oxygen atom disappears when the water evaporates. The third understands both ideas but calls water a mixture because it contains two elements.
All three students need feedback, but not identical explanations.
In a group of three, the tutor can ask every child to describe what each circle represents before allowing peer discussion. Each learner then redraws the model and explains the corrected idea.
The final step is an unfamiliar diagram, not simply the original picture copied correctly. Independent transfer is what shows that the explanation has become usable.
The Fencing Method: one pair at a time
A student who confuses element with compound does not benefit from hearing every definition in Chemistry at once.
We begin with oxygen gas, O₂, and water, H₂O. Both contain molecules, but only water combines different elements in its molecules.
Next compare water with an ionic compound such as sodium chloride. Both are compounds, but their structures are described differently.
Finally, show a mixture of water and dissolved sodium chloride. The child must explain why a mixture can contain a compound and still be a mixture overall.
This sequence keeps one contrast clear long enough for understanding to stabilise.
An illustrative 90-minute small-group Science lesson
The reference eduKateSG teaching arrangement is three pupils for 1.5 hours weekly. A lesson might include:
- 10 minutes: retrieve what an element, compound, atom and molecule mean without notes.
- 15 minutes: interpret two particle diagrams and correct typical modelling mistakes.
- 20 minutes: compare molecular and elemental examples using H₂O, O₂, CO₂ and NaCl.
- 20 minutes: read chemical symbols, subscripts, coefficients and selected ion charges.
- 15 minutes: independently classify unfamiliar particle diagrams and formulae.
- 10 minutes: review each learner’s earliest incorrect distinction and set one short retrieval task.
This is an example teaching sequence rather than a promise of identical activities every week. The tutor adapts depth and pace to the child’s current school programme.
How this connects to Secondary 3 Chemistry
Upper-secondary Chemistry uses the same basic language with greater precision: electron arrangements, common ion charges, bonding types, formulae, chemical equations and mole calculations.
A student who cannot distinguish Na⁺ from Na, or O₂ from 2O₂, may struggle with equation balancing for reasons that have little to do with mathematical ability.
That is why a good Secondary 2 transition programme repairs the notation and model before accelerating into a stack of advanced equations.
The most effective preparation is conceptual accuracy, not the appearance of being two chapters ahead.
Where appropriate, a capable student can preview ionic charges and simple formula writing, while a learner needing repair should become fluent in the core Science distinctions first.
G1, G2 and G3 lower-secondary Science
Under Full Subject-Based Banding, students may study Science at different subject levels. The expected depth, terminology and school assessment sequence vary.
The MOE G2/G3 lower-secondary Science framework includes the model of matter and atoms and molecules. We align teaching with the child’s actual Science level and current school topics rather than treating all Secondary 2 pupils as future separate Pure Chemistry candidates.
Not every child needs detailed polyatomic-ion formula writing at this stage. Extension is useful when the understanding is secure and the learner is ready.
Our goal is a stable transition into whichever upper-secondary Science combination the student eventually takes.
How Hougang parents can check understanding at home
Ask your child: “Why is oxygen an element even when oxygen gas contains molecules?”
Then: “What does the 2 mean in H₂O, and what changes if I write 3H₂O?”
Then: “If sodium loses one electron, has it become another element?”
Finally: “How is a compound different from a mixture?”
The important thing is to invite explanations, not just single-word labels. If the student is unsure, let them check school notes and try again.
These questions require no chemical reagents or laboratory equipment. An accurate, independent five-minute explanation can reveal more than a long worksheet copied from a model answer.
How we judge progress
Look for a learner who reads chemical symbols accurately, classifies diagrams using the right criterion, distinguishes molecules from atoms and ions, and uses particle models without inventing new substances during physical changes.
Students should explain why a solid ionic compound and a molecular compound cannot be treated as structurally identical, at a depth suited to their course.
They should also know the limits of a simplified drawing. A scientific model is useful because of what it explains, not because it reproduces every physical detail.
We assess unfamiliar independent questions across lessons rather than promising a guaranteed score improvement in a fixed number of weeks.
Frequently asked questions
Is Secondary 2 Chemistry a separate subject in Singapore?
For most students, Chemistry-related ideas are taught within lower-secondary Science. The tutor should follow the child’s actual G1, G2 or G3 school programme.
Is every molecule a compound?
No. O₂ is a molecule of an element, while H₂O is a molecule of a compound.
Is every compound made of molecules?
No. Ionic compounds such as solid sodium chloride form extended ionic structures rather than discrete NaCl molecules.
What is the difference between an atom and an ion?
An ion has a net electrical charge because its electron count differs from the proton count. The proton number still determines the element.
Does the subscript in H₂O mean two water molecules?
No. The subscript means two hydrogen atoms in each water molecule. A coefficient, as in 2H₂O, changes the number of water molecules represented.
Why does capitalisation matter in chemical symbols?
Element symbols use prescribed letters and case. Co represents cobalt; CO represents carbon monoxide.
Should a Secondary 2 student memorise all ionic charges?
The appropriate scope depends on the school and learner. Correct understanding of atoms, elements and molecules comes first; common ionic charges may be introduced as meaningful preparation.
Are three-student tutorials suitable for a struggling learner?
A small group can allow close diagnosis and feedback, provided its level and pace suit the student. We confirm fit before recommending placement.
Is the tuition centre located in Hougang?
No. Our reference centre is 8 Fourth Avenue, Singapore 268674, near Sixth Avenue MRT. Hougang families should confirm travel and the actual available class.
Continue the Secondary Chemistry pathway
- Secondary 2 Chemistry Tutor Hougang | Small Groups Tutorials
- Preparing for Secondary 3 Chemistry and Science Choices
- Diffusion, Gas Pressure and Particle Movement
- Secondary 1: Matter, Particles and Mixtures
- Secondary 3: Chemical Formulae, Equations and Mole Calculations
- Secondary 3: Ionic, Covalent and Metallic Bonding Explained
- MOE Lower Secondary Science
Arrange a Secondary 2 Chemistry-related Science consultation
Bring the student’s subject level, a marked Science paper and one particle-model or chemical-symbol question they cannot explain alone. We can discuss whether a premium three-student tutorial would be appropriate, and confirm the current venue and lesson availability.
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