Formula Sheet
Explore the properties, reactions, and uses of metals and non-metals, understanding their role in daily life and industrial applications.
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.
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.
Explore the fundamentals of chemical reactions, types, and balancing equations in this chapter, essential for understanding chemistry basics.
Explore the properties, reactions, and uses of acids, bases, and salts in everyday life and their importance in chemistry.
Explore the versatile world of carbon, its allotropes, and the vast array of compounds it forms, including hydrocarbons and their derivatives, in this comprehensive chapter.
Life Processes explores the essential functions that sustain living organisms, including nutrition, respiration, transportation, and excretion.
