Find qualified chemistry tutors

Subject qualifications, teacher training and experience with a particular course answer different questions. A chemistry degree shows a subject background; a teaching credential concerns preparation for teaching. Neither description tells you, by itself, how someone will explain a difficult idea to this learner.

In England, qualified teacher status (QTS) and a postgraduate certificate in education (PGCE) are different. Some teacher-training courses award both, while a PGCE alone does not establish that someone holds QTS. Check the actual award and the education system it relates to, especially when comparing qualifications gained in different countries. If the credential matters to your choice, ask to see evidence of the named qualification or status.

Consider this unbalanced equation: Mg + O₂ → MgO. There are two oxygen atoms on the left, but only one on the right. A learner might try to fix this by writing MgO₂. That changes the formula of the product; it is no longer the magnesium oxide named in the question.

Instead, place a 2 in front of MgO: Mg + O₂ → 2MgO. There are now two magnesium atoms on the right, so put a 2 in front of Mg too. The balanced equation is 2Mg + O₂ → 2MgO: two magnesium atoms and two oxygen atoms on each side. The small numbers within a formula stay unchanged; the numbers in front multiply the whole formula when you count atoms.

A useful explanation makes the atom count visible before asking the learner to practise. As a follow-up, try H₂ + O₂ → H₂O. The balanced answer is 2H₂ + O₂ → 2H₂O, with four hydrogen atoms and two oxygen atoms on each side. Being able to explain that count is a better check of understanding than copying the first answer. These are illustrative teaching examples, not exam-board model answers.

A common confusion is to read “equilibrium” as “the same amount of reactants and products”. At dynamic equilibrium in a closed system, the forward and reverse reactions continue at equal rates. The concentrations remain constant, but they do not have to be equal.

For an illustrative calculation, suppose the gaseous reaction H₂(g) + I₂(g) ⇌ 2HI(g) has these equilibrium concentrations at a fixed temperature: [H₂] = 0.20 mol dm⁻³, [I₂] = 0.30 mol dm⁻³ and [HI] = 0.60 mol dm⁻³. Square brackets mean concentration. The expression is Kc = [HI]² ÷ ([H₂][I₂]), so Kc = 0.60² ÷ (0.20 × 0.30) = 6.0. The power of 2 comes from the coefficient of HI in the balanced equation.

A stronger explanation connects the calculation back to the idea: these concentrations are unequal, yet they can stay constant because the forward and reverse reaction rates are equal. To check the distinction, ask the learner to correct “At equilibrium the reactions stop”. A better response is “Both reactions continue, but at equal rates, so the concentrations no longer change.”

Latimer offers online one-to-one tuition. Microsoft Teams is the default lesson platform, although a tutor and learner can agree another platform. For chemistry, check that the learner can share their written working clearly and read equations on the screen; a readable photograph of a question can help prepare a discussion.

You can request a tutor match free of charge. The free introductory meeting is for discussing goals, teaching approach and arrangements, so use it to explain the course, any particular teaching qualification you want and the learner’s main difficulty. Confirm the proposed lesson length, timetable and expectations for practice before booking.

Each tutor sets their own hourly rate, shown on their profile. Latimer invoices for lessons after they take place on a pay-as-you-go basis. Compare the rate alongside the tutor’s relevant experience and the proposed focus of the lessons. Agree what feedback or preparation is included so the arrangement fits your budget.