1st Year Chemistry Notes

• Here are the detailed 1st year chemistry notes pdf to help you prepare for your exams.
• History of Atom
• Evidence of Atoms
• Define atom.
• Define ion. How cation and anion are formed?
• How molecular ions are formed?
• Define relative atomic mass. 
• Define isotopes. Give two examples.
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• Why isotopes have same chemical properties but different physical properties?
• How does no individual neon atom in the sample of the element has mass 20.18 amu? 
• Define mass spectrometer.
• Mention principle or working of mass spectrometer. 
• How percentage of an element is determined? 
• Define empirical formula and molecular formula.
• What are the steps to determine empirical formula? 
• Our comprehensive 1st year chemistry notes pdf download will ensure you're fully prepared for your exams.
• Define mole and Avogadro’s number. OR What is the relation between mole and Avogadro’s number? 
• Why sizes and masses do not affect volume?
• One mole of H2O has 2 moles of bonds, 3 moles of atoms, 10 moles of electrons, and 28 moles of total fundamental particles present in it. 
• Calculate the percentage of nitrogen in urea. 
• Define analytical chemistry.
• Difference between qualitative analysis and quantitative analysis. 
• Define filtration.
• Tell about Gooch crucible and sintered glass crucible. 
• How fluted filter paper increases rate of filtration?
• What are the characteristics of a good solvent?
• How decolourization of undesirable colours is done?
• What is the disadvantage of using filter paper for drying the crystals? 
• Mention types of chromatography/ Difference between adsorption and partition chromatography. 
• Define one atmospheric pressure. Give units.
• What are gas laws? 
• What is absolute zero? What happens to real gases while approaching it?
• Why Celsius scale does not justify Charles’ law? AND Which scale justifies Charles’ law?
• Calculate the units of ideal gas constant (R) in SI units.
• State Dalton’s law of partial pressures.
• How Dalton’s law of partial pressures is applicable to the collection of gases under water?
• Give four fundamental postulates of KMT.
• State Graham’s law of diffusion.
• State Joule-Thomson effect. 
• Water vapors do not behave ideally at 273K. Give reason. 
• Pressure of ammonia gas at given conditions is less as calculated by Vander Waal equation than that calculated by general gas equation. Why?
• What is the difference between natural and artificial plasma.
• What are dipole-dipole forces of attraction? Explain with examples. 
• What are dipole-induced dipole forces or Debye forces? Give examples. 
• What are instantaneous dipole-induced dipole forces or London dispersion forces?
• Why evaporation causes cooling?
• Cleavage of crystals is anisotropic behaviour. Why?
• Define crystal lattice.
• Define lattice energy.
• Why electrical conduction decreases with increasing temperature?
• Why metals have metallic luster? 
• In the closest packing of atoms of metals, only 74% space is occupied. Justify. 
• Why the pressure of the gas is kept very low in gas discharge tube experiment? 
• How negative charge of cathode rays was proved? 
• How cathode rays produce fluorescence?
• How it is proved that cathode rays travel in straight lines? 
• How it is proved that cathode rays possess momentum?
• Why e/m of cathode rays is independent of the nature of the gas used in discharge tube?
• The e/m value of positive rays depends upon the nature of the gas used in the discharge tube. Justify. 
• How were neutrons discovered? 
• Mention the defects of Rutherford’s model of atom.
• How do you justify that the distances between adjacent orbits of Hydrogen atom go on increasing from lower to the higher orbits? 
• How do you come to know that the velocities of electrons in higher orbitsare less than those in lower orbits of hydrogen atom?
• Energy of an electron is inversely proportional to ‘n2 ’ but energy of higher orbits is always greater than those of the lower orbits. Why? 
• What is the difference between continuous spectrum and line spectrum?
• What is the difference between atomic emission spectrum and atomic absorption spectrum? 
• State Moseley’s law. 
• State Heisenberg’s uncertainty principle and give its equation.
• Briefly tell about principal quantum number/azimuthal quantum number/magnetic quantum number and spin quantum number. 
• What is octet rule? Give one example of compound which obeys it and two examples of compounds which do not obey it. 
• Bond distance is the compromise distance between the two atoms making molecule. OR 75.4 pm is the bond distance between two hydrogen atoms. Justify.
• Why the radius of an atom can’t be determined precisely?
• Why is the size of cation smaller than parent atom?
• What is the trend of ionization energy in the periodic table? 
• What is the trend of electron affinity in the periodic table? 
• What is the trend of electronegativity in the periodic table?
• What is the basic assumption of VSEPR Theory?
• Write two points of Valence Bond Theory.
• Why pi bond is more diffused than sigma bond?
• What is the difference between VBT and MOT? 
• Why the energy of anti-bonding molecular orbital is higher than corresponding bonding molecular orbital? 
• Why the melting points, boiling points, heats of sublimation and heats of vaporization of electrovalent compounds are higher as compared with those of covalent compounds? 
• What is thermochemical equation? What information do they convey? Give two examples.
• What is the difference between a spontaneous and a non-spontaneous reaction?
• Burning of candle is a spontaneous process. Justify.
• Define enthalpy of a reaction, enthalpy of formation, enthalpy of atomization, enthalpy of neutralization, enthalpy of combustion and enthalpy of solution. 
• State Hess’s Law of Constant Heat Summation.
• What is meant by state of chemical equilibrium.
• Define reversible and irreversible reaction. Give examples.
• Discuss the change of concentration of a product on reversible reaction.
• What is ionic product of water and how it varies with temperature?
• What is Henderson’s equation and for what purpose it is used?
• What is Lowry-Bronsted acid base concept? 
• What is common ion effect. Give two applications.
• Define molarity and molality. Give examples.
• Why molality is independent of temperature but molarity depends upon temperature? 
• State Raoult’s law. OR Give two statements of Raoult’s law.
• Define solubility. Give an example.
• Define colligative properties.
• Define ebullioscopic constant and cryoscopic constant. 
• Why ethylene glycol is used as an anti-freeze in car radiators?
• Differentiate between hydration and hydrolysis. 
• Define electrochemistry.
• Explain extraction of sodium by Down’s cell. 
• How the process of electrolysis is applied in the production of caustic soda? 
• How impure copper is purified by the process of electrolysis? 
• What is the function of salt bridge? 
• How electrochemical series predict feasibility of a reaction?
• How relative tendency of elements for redox reactions can be compared by using electrochemical series? 
• Define reaction kinetics. 
• What happens to rate of reaction with the passage of time?
• Define instantaneous and average rate.
• Define order of reaction. Give an example.
• Define half life period. Give an example. 
• The radioactive decay is always a first order reaction. Give reason. 
• Give the relation between half-life and initial concentration of reactant. 
• What is the effect of temperature on rate of reaction? 
• What are the types of catalysis? OR What is the difference between homogeneous catalysis and heterogeneous catalysis?
• Define promotor or activator. 
• Define negative catalysis 
• Characteristics of Enzyme Catalysis