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Some Basic Concepts of Chemistry

🎓 Class 11📖 Chemistry Part-I📖 11 notes🧠 15 Q&A⏱️ ~17 min
Chapter 1 of 6Structure of Atom

Some Basic Concepts of ChemistryStudy Notes

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Development of Chemistry

Explanation

Development of Chemistry

Chemistry, as a scientific discipline, is relatively young compared to other fields of knowledge. It emerged historically from human curiosity and the quest for two mythical substances: the Philosopher's Stone (Paras) which was believed to convert base metals like iron and copper into gold, and the Elixir of Life which was thought to grant immortality. Ancient India had a rich tradition of chemical knowledge long before modern science. This knowledge was applied in various fields such as metallurgy, medicine, cosmetics, glass, and dye manufacture. Archaeological excavations at sites like Mohenjodaro and Harappa reveal early chemical processes such as mass production of pottery, use of baked bricks, glazing techniques, and metallurgy involving metals like lead, silver, gold, and copper. The Harappans improved copper hardness by alloying with tin and arsenic. Glass objects colored by metal oxides were found in ancient Indian sites, indicating advanced chemical technology. Copper metallurgy dates back to chalcolithic cultures, and technologies for extraction of copper and iron were developed indigenously. Ancient texts like Rigveda mention tanning and dyeing practices. The golden gloss of black polished ware from northern India remains a chemical mystery. Kautilya's Arthashastra describes salt production from the sea. Vedic literature and ancient Ayurvedic texts such as Charaka Samhita and Sushruta Samhita describe preparation of acids, oxides, sulphates, and carbonates of various metals. Rasopanishada details gunpowder preparation, and Tamil texts describe fireworks using sulphur, charcoal, saltpetre, mercury, and camphor. Nagarjuna, a renowned Indian scientist, contributed to alchemy and metallurgy, discussing mercury compounds and metal extraction methods. Chakrapani discovered mercury sulphide and invented soap using mustard oil and alkalies. Ancient Indian paintings at Ajanta and Ellora demonstrate advanced knowledge of glutinous materials for wall and roof coatings derived from plant extracts and resins. Varāhmihir's Brihat Samhita and Atharvaveda mention dyes, perfumes, cosmetics, and hair dyes derived from natural sources. The concept of matter being composed of indivisible particles (Paramānu) was formulated by Acharya Kanda (600 BCE) in the Vaiseshika Sutras, predating Dalton's atomic theory by about 2500 years. Charaka Samhita discusses reduction of particle size (nanotechnology) and use of metal bhasmas in medicine. After the decline of alchemy and iatrochemistry, modern chemistry developed in India during the 19th century, influenced by European scientists. Chemistry today is the science of atoms and molecules, studying composition, structure, properties, and transformations of matter.

  • Chemistry originated from the search for Philosopher's Stone and Elixir of Life.
  • Ancient India had advanced chemical knowledge applied in metallurgy, medicine, and crafts.
  • Archaeological evidence shows early chemical processes like pottery, glazing, and metal extraction.
  • Acharya Kanda proposed atomic theory (Paramānu) centuries before Dalton.
  • Ancient texts describe preparation of acids, gunpowder, dyes, and medicinal compounds.
  • Modern chemistry in India developed in the 19th century under European influence.
  • 📌 Philosopher's Stone: mythical substance to convert base metals into gold.
  • 📌 Elixir of Life: mythical substance granting immortality.
  • 📌 Paramānu: ancient Indian term for indivisible atoms.

1.1 Importance of Chemistry

Explanation

1.1 Importance of Chemistry

Chemistry plays a central role in science and is deeply interconnected with other disciplines such as physics, biology, and geology. Its principles are fundamental to understanding natural phenomena and technological advancements. Chemistry is involved in diverse areas including weather patterns, brain function, computer operation, and industrial production. Industries manufacturing fertilizers, alkalis, acids, salts, dyes, polymers, drugs, soaps, detergents, metals, and alloys rely heavily on chemistry. It contributes significantly to the national economy and human welfare by improving food production, healthcare, and quality of life. For example, large-scale production of fertilizers and pesticides enhances agricultural yield. Chemistry also enables the isolation and synthesis of life-saving drugs such as cisplatin and taxol for cancer therapy, and AZT for AIDS treatment. Advances in chemistry have led to the design and synthesis of new materials with specific magnetic, electric, and optical properties, including superconducting ceramics, conducting polymers, and optical fibers. These materials have transformed industries and everyday life. Environmental challenges like ozone depletion caused by chlorofluorocarbons (CFCs) have been addressed by developing safer alternatives. However, issues like greenhouse gas management remain critical. Understanding biochemical processes and using enzymes for large-scale chemical production are ongoing challenges. India, as a developing country, requires talented chemists to meet these challenges. A strong foundation in basic chemical concepts is essential for aspiring chemists to contribute effectively.

  • Chemistry is fundamental to various scientific disciplines and natural phenomena.
  • It supports industries producing fertilizers, dyes, drugs, polymers, and metals.
  • Chemistry contributes to national economy and improves quality of life.
  • Development of new materials with tailored properties is a key achievement.
  • Environmental issues like ozone depletion are addressed through chemistry.
  • Future challenges include biochemical process understanding and sustainable chemistry.
  • 📌 Chlorofluorocarbons (CFCs): chemicals causing ozone depletion.
  • 📌 Superconducting ceramics: materials with zero electrical resistance.
  • 📌 Enzymes: biological catalysts used in chemical production.

1.2 Nature of Matter

Explanation

1.2 Nature of Matter

Matter is defined as anything that has mass and occupies space. Everything around us, including solids, liquids, gases, living beings, and non-living objects, is composed of matter. Matter exists in three physical states: solid, liquid, and gas. In

Practice QuestionsSome Basic Concepts of Chemistry

Includes NCERT exercise questions with answers

Q1.Calculate the molar mass of the following: (i) H2O (ii) CO2 (iii) CH4

Answer:

Solution: (i) Molar mass of H2O = (2 × 1.008) + 16.00 = 2.016 + 16.00 = 18.016 g/mol (ii) Molar mass of CO2 = 12.01 + (2 × 16.00) = 12.01 + 32.00 = 44.01 g/mol (iii) Molar mass of CH4 = 12.01 + (4 × 1.008) = 12.01 + 4.032 = 16.042 g/mol

Explanation:

Molar mass is calculated by adding the atomic masses of all atoms present in the molecule. For H2O: 2 hydrogen atoms and 1 oxygen atom. For CO2: 1 carbon atom and 2 oxygen atoms. For CH4: 1 carbon atom and 4 hydrogen atoms.

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Q2.Calculate the mass per cent of different elements present in sodium sulphate (Na2SO4).

Answer:

Solution: Molar mass of Na2SO4 = (2 × 22.99) + 32.07 + (4 × 16.00) = 45.98 + 32.07 + 64.00 = 142.05 g/mol Mass % of Na = (45.98 / 142.05) × 100 = 32.37% Mass % of S = (32.07 / 142.05) × 100 = 22.57% Mass % of O = (64.00 / 142.05) × 100 = 45.06%

Explanation:

Mass percent of an element = (mass of element in 1 mole of compound / molar mass of compound) × 100. Calculate molar mass first, then find mass percent for each element.

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Q3.Determine the empirical formula of an oxide of iron, which has 69.9% iron and 30.1% dioxygen by mass.

Answer:

Solution: Assume 100 g of compound: Fe = 69.9 g, O = 30.1 g Moles of Fe = 69.9 / 55.85 = 1.251 mol Moles of O = 30.1 / 16.00 = 1.881 mol Divide by smallest: Fe = 1.251 / 1.251 = 1, O = 1.881 / 1.251 = 1.5 Multiply by 2 to get whole numbers: Fe2O3 Empirical formula is Fe2O3.

Explanation:

Empirical formula is found by converting mass percentages to moles, dividing by smallest mole value, and adjusting to whole numbers.

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Q4.Calculate the amount of carbon dioxide that could be produced when (i) 1 mole of carbon is burnt in air. (ii) 1 mole of carbon is burnt in 16 g of dioxygen. (iii) 2 moles of carbon are burnt in 16 g of dioxygen.

Answer:

Solution: Reaction: C + O2 → CO2 (i) 1 mole C reacts with 1 mole O2 to produce 1 mole CO2. Amount of CO2 produced = 1 mole. (ii) 16 g O2 = 16/32 = 0.5 mole O2. Carbon available = 1 mole. O2 is limiting reagent (0.5 mole). Amount of CO2 produced = 0.5 mole. (iii) Carbon = 2 moles, O2 = 0.5 mole (16 g). O2 is limiting reagent. Amount of CO2 produced = 0.5 mole.

Explanation:

Use stoichiometry of reaction: 1 mole C reacts with 1 mole O2 to form 1 mole CO2. Limiting reagent determines amount of product formed.

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Q5.Calculate the mass of sodium acetate (CH3COONa) required to make 500 mL of 0.375 molar aqueous solution. Molar mass of sodium acetate is 82.0245 g mol⁻¹.

Answer:

Solution: Molarity (M) = moles/volume(L) Moles required = M × volume = 0.375 × 0.5 = 0.1875 mol Mass = moles × molar mass = 0.1875 × 82.0245 = 15.38 g Mass of sodium acetate required = 15.38 g.

Explanation:

Calculate moles from molarity and volume, then convert moles to mass using molar mass.

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Q6.Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g mL⁻¹ and the mass per cent of nitric acid in it being 69%.

Answer:

Solution: Density = 1.41 g/mL = 1410 g/L Mass of HNO3 in 1 L = 69% of 1410 g = 0.69 × 1410 = 972.9 g Molar mass of HNO3 = 1 + 14 + (3 × 16) = 63 g/mol Moles of HNO3 = 972.9 / 63 = 15.44 mol Concentration = 15.44 mol/L.

Explanation:

Calculate mass of solution per litre using density, then find mass of solute using mass percent, convert to moles and divide by volume.

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Q7.How much copper can be obtained from 100 g of copper sulphate (CuSO4)?

Answer:

Solution: Molar mass of CuSO4 = 63.55 + 32.07 + (4 × 16) = 63.55 + 32.07 + 64 = 159.62 g/mol Mass of Cu in 1 mole CuSO4 = 63.55 g Mass of Cu in 100 g CuSO4 = (63.55 / 159.62) × 100 = 39.8 g Copper obtained = 39.8 g.

Explanation:

Calculate mass percent of copper in copper sulphate and apply to 100 g sample.

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Q8.Determine the molecular formula of an oxide of iron, in which the mass per cent of iron and oxygen are 69.9 and 30.1, respectively.

Answer:

Solution: From Q1.3, empirical formula is Fe2O3. Calculate empirical formula mass = (2 × 55.85) + (3 × 16) = 111.7 + 48 = 159.7 g/mol Given molecular mass is not provided, so assume molecular formula = empirical formula. Hence molecular formula is Fe2O3.

Explanation:

Molecular formula is a whole number multiple of empirical formula. Without molecular mass, molecular formula equals empirical formula.

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