Periodic Table Reaction Predictor
Choose two reactants by typing formulas or clicking elements in a compact periodic table. The predictor applies six textbook rules — metal + nonmetal synthesis, combustion, acid–base neutralisation, metal + acid, single displacement and reactive metal + water — using common ion charges and the metal activity series. It balances the predicted equation, explains the reasoning, and tells you when no reaction is expected and why. It is an educational guide, not a substitute for chemical knowledge or lab safety advice.
How to use the Periodic Table Reaction Predictor
- Type Reactant A and Reactant B, or click an element in the table to fill the highlighted slot.
- Press Predict reaction, or try one of the examples.
- Read the reaction type, balanced equation and explanation.
- Check the notes for real-world caveats such as peroxide formation or protective oxide layers.
Features
- Metal + nonmetal → ionic compound using common oxidation states (e.g. Al + O2 → Al2O3)
- Complete combustion of hydrocarbons and C/H/O compounds
- Strong-acid neutralisation with metal hydroxides
- Metal + acid and metal + salt displacement using the activity series
- Group 1 and 2 metals with water
- Every predicted equation balanced with the exact equation balancer
Benefits
- Practise predicting products and check your reasoning
- Understand why some combinations, like copper and hydrochloric acid, do not react
- Honest about what the rules cannot predict
Frequently asked questions
How accurate are the predictions?
They follow standard school-level rules and are correct for the textbook cases those rules cover. Real reactions also depend on concentration, temperature, solubility and kinetics, which this tool does not model.
Why does it say "no reaction" for copper and hydrochloric acid?
Copper is below hydrogen in the activity series, so it cannot displace hydrogen from a non-oxidising acid. That is the expected textbook result.
Why is nitric acid with metals not predicted?
Nitric acid is an oxidising acid. With most metals it produces nitrogen oxides rather than hydrogen gas, and the products depend on concentration, so a simple rule would give misleading answers.
Can I use it to plan an experiment?
No. It is a learning aid. Many of these reactions are hazardous; only carry out experiments under qualified supervision with proper safety equipment.
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