Some Basic Concepts of Chemistry
Class 11 Chemistry · Chemistry Part I · Chapter 1
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Summary
Chemistry is the science that studies the preparation, properties, structure and reactions of material substances. Matter — anything that has mass and occupies space — exists in three interconvertible physical states (solid, liquid, gas) and is classified into pure substances (elements and compounds) and mixtures (homogeneous or heterogeneous). Properties may be physical or chemical, and are measured using the SI scheme of seven base units. Because every measurement carries uncertainty, results are expressed using scientific notation \(N\times10^{n}\), significant figures, and the factor-label method of dimensional analysis. Five laws of chemical combination — the law of conservation of mass (Lavoisier), the law of definite proportions (Proust), the law of multiple proportions (Dalton), Gay-Lussac's law of gaseous volumes, and Avogadro's law — led John Dalton to his atomic theory. Atomic masses are referred to the carbon-12 standard, and average atomic mass accounts for isotopic abundance. The mole, containing \(6.022\times10^{23}\) entities, links mass to number of particles; molar mass in grams equals the atomic, molecular or formula mass in unified mass units. Percentage composition yields empirical and molecular formulae, and stoichiometry uses balanced equations, the limiting-reagent idea and concentration terms such as mass per cent, mole fraction, molarity and molality.
Nature and classification of matterProperties of matter and SI unitsUncertainty in measurement and significant figuresLaws of chemical combinationDalton's atomic theoryAtomic and molecular massesMole concept and molar massPercentage composition and formulaeStoichiometry and limiting reagent
Key terms
Matter
Anything that has mass and occupies space; it exists in three physical states — solid, liquid and gas.
Significant figures
The meaningful digits of a measurement that are known with certainty plus one estimated (uncertain) digit.
Mole
The SI unit of amount of substance; one mole contains exactly \(6.022\times10^{23}\) elementary entities (Avogadro number).
Empirical formula
A formula giving the simplest whole-number ratio of the atoms present in a compound.
Limiting reagent
The reactant present in the least relative amount, which is consumed first and limits the quantity of product formed.
Molarity
The number of moles of solute dissolved per litre of solution, \(M=n_{solute}/V_{solution}\).
Extra questions & answers
Try one from this chapter
The law of conservation of mass was proposed by: