Formula Sheet: Metals and Non-metals
This chapter focuses on the classification, properties, and reactivity of metals and non-metals.
Mathematical Derivations, Constant Metrics, and Variable Demystification Indices
All engineering, algebraic, and chemical glyph variables are rendered with complete structural precision for Class 10 Science.
Metals and Non-metals – Formula & Equation Sheet
Essential formulas and equations from Science, tailored for Class X in Science.
This one-pager compiles key formulas and equations from the Metals and Non-metals chapter of Science. Ideal for exam prep, quick reference, and solving time-bound numerical problems accurately.
Formula sheet
Key concepts & formulas
Essential formulas, key terms, and important concepts for quick reference and revision.
Formulas
Metal + Oxygen → Metal oxide
Metals react with oxygen to form metal oxides. Example: 4Al + 3O₂ → 2Al₂O₃. This is fundamental in understanding corrosion and combustion of metals.
Metal + Water → Metal hydroxide + Hydrogen
Reactive metals react with water to form metal hydroxides and hydrogen gas. Example: 2Na + 2H₂O → 2NaOH + H₂. Important for understanding reactivity series.
Metal + Acid → Salt + Hydrogen
Metals react with acids to produce salts and hydrogen gas. Example: Zn + 2HCl → ZnCl₂ + H₂. Key for understanding metal-acid reactions.
Metal A + Salt solution of B → Salt solution of A + Metal B
More reactive metals displace less reactive metals from their salt solutions. Example: Fe + CuSO₄ → FeSO₄ + Cu. Essential for displacement reactions.
Roasting: 2ZnS + 3O₂ → 2ZnO + 2SO₂
Sulphide ores are converted to oxides by heating in air. Crucial for metallurgy processes.
Calcination: ZnCO₃ → ZnO + CO₂
Carbonate ores are heated in limited air to form oxides. Important step in extraction of metals.
Reduction: ZnO + C → Zn + CO
Metal oxides are reduced to metals using carbon. Example of extracting metals from their ores.
Thermit reaction: Fe₂O₃ + 2Al → 2Fe + Al₂O₃
Highly exothermic reaction used to join railway tracks. Demonstrates displacement and reactivity.
Electrolytic refining: At cathode: Cu²⁺ + 2e⁻ → Cu
Pure metal is deposited at cathode during refining. Key for understanding purification of metals.
Anodising: 2Al + 3O₂ → 2Al₂O₃
Process to increase thickness of natural oxide layer on aluminium. Prevents corrosion.
Equations
2Cu + O₂ → 2CuO
Copper reacts with oxygen to form copper(II) oxide, a black oxide. Example of metal oxide formation.
4Al + 3O₂ → 2Al₂O₃
Aluminium forms aluminium oxide, an amphoteric oxide. Shows dual nature of some metal oxides.
2K + 2H₂O → 2KOH + H₂
Potassium reacts violently with water. Demonstrates high reactivity of alkali metals.
Ca + 2H₂O → Ca(OH)₂ + H₂
Calcium reacts with water less violently than potassium. Shows reactivity trend in metals.
3Fe + 4H₂O → Fe₃O₄ + 4H₂
Iron reacts with steam to form iron(II,III) oxide and hydrogen. Important for understanding metal-water reactions.
Zn + 2HCl → ZnCl₂ + H₂
Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas. Example of metal-acid reaction.
Fe + CuSO₄ → FeSO₄ + Cu
Iron displaces copper from copper sulphate solution. Demonstrates displacement reaction.
2HgS + 3O₂ → 2HgO + 2SO₂
Cinnabar is roasted to form mercuric oxide. Step in extraction of mercury.
2HgO → 2Hg + O₂
Mercuric oxide decomposes to mercury and oxygen. Final step in mercury extraction.
Na₂O + H₂O → 2NaOH
Sodium oxide reacts with water to form sodium hydroxide. Shows basic nature of metal oxides.
