Guess Chemistry 1st year ● What are monoisotopic elements? Give the name and symbol of such an element. ● Calculate gram atoms. In 0.1 gm of sodium (at mass of sodium =23)? ● Differentiate between actual yield and theoretical yield. ● Why theoretical yield of a chemical reaction is greater than the actual yield. ● How is the efficiency of a reaction expressed? ● 23 g of sodium and 238 g of uranium have an equal number of atoms in them. ● No individual Neon atom in the sample of the element has a mass of 20.18 amu why? LONG QUESTIONS. ● Write a detailed note on. i) Avogadro’s number ii) Molar volume. ● Define stoichiometry. Give its assumptions. Mention two important laws which help to perform the stoichiometric calculation. ● What is a limiting reactant? How does it control the quantity of the product formed? ● Define yield. How do we calculate the percentage yield of chemical reactions? Also mention the factors which are responsible for low yield of products. CHAPTER NO. 2 EXPERIMENTAL TECHNIQUES IN CHEMISTRY. SHORT QUESTIONS. ● State distribution law. ● What do you mean by solvent extraction? Which law controls it? ● Differentiate between stationary and mobile phase used in chromatography. ● Write down the uses of chromatography. ● What is chromatography and R1 value? LONG QUESTIONS. ● Write down the main characteristics of a solvent selected for crystallization of. Of a compound. ● Why is there a need to crystallize the crude product? CHAPTER NO. 3 GASES. SHORT QUESTIONS. ● Explain the plot of PV versus P is a straight line at constant temperature and with a fixed number of moles of an ideal gas. ● Write an expression for the kinetic equation and root mean square velocity of gases. ● Why do pilots feel uncomfortable berating in an unpressurised cabin? ● Derive Boyle’s law from KMT. ● Write two uses of plasma. LONG QUESTIONS. ● What is Kinetic molecular theory of gases? Give its postulates. ● State and explain Boyle’s law and verify this law by an experiment. CHAPTER NO. 4 LIQUIDS AND SOLIDS. SHORT QUESTIONS. ● What are dipole-dipole forces of attraction? Explain with an example. ● What are Debye forces? Explain. ● What are dipole-induced dipole forces? ● Define polarizability. How does it affect London dispersion forces? ● How do soaps and detergents do their cleansing action? ● Why water is liquid at room temperature but H2S and H2Se are gases, comments. ● Give reason for the lowest boiling point of hydride of group IV-A elements. LONG QUESTIONS. ● What are ionic solids? Give their properties. ● What are molecular crystals? Give their properties. CHAPTER NO. 6 CHEMICAL BONDING. SHORT QUESTIONS. ● Define ionic and covalent radii. ● Define covalent radius with an example. ● Why is the cationic radius smaller than the parent atom? ● Ionization energy is indexed to the metallic character. Why? ● How does electron affinity vary in the periodic table? ● Why are polar bonds stronger than nonpolar bonds? ● Why do lone pair electrons repel more strongly than the bond pair of electrons? LONG QUESTIONS. ● What is a chemical bond? Discuss the formation of ionic and covalent bonds. ● Define bond energy. Explain the various parameters which determine its strength. CHAPTER NO. 7 THERMOCHEMISTRY SHORT QUESTIONS. ● Define ‘system” and “surroundings”. ● Define heat of solution. Give an example. ● Define standard enthalpy of combustion. Give one example. ● What is the standard enthalpy of solution? LONG QUESTIONS. ● Define and explain Hess’s law of constant heat summation with examples. ● Describe bomb-calorimeter method for determination of enthalpy of reaction. CHAPTER NO. 8 CHEMICAL EQUILIBRIUM. SHORT QUESTIONS. ● What are irreversible reactions? Give one example. ● How does a catalyst affect a reversible reaction? ● What conditions are required for the best possible yield of SO2? ● What is the effect of common ion on solubility? ● What is an acidic buffer? Give one example. ● Write down Henderson’s equation and for which purpose it was used. ● Explain the term Buffer capacity. LONG QUESTIONS. ● What is the percentage ionization of acetic acid in a solution in which 0.1 moles of it has been dissolved per dm2 of solution Ka for CH3COOH = 1.85 x 105 CHAPTER NO. 9 SOLUTIONS SHORT QUESTIONS. ● Difference between ideal and non- ideal. ● Boiling points of liquids are increased when a solute is added to them. Justify it. ● What are the names of major parts of apparatus used in Landsbergis’s method for elevation of Boiling point? ● What are colligative properties? And why are they called so? ● State different from of Roault’s Law. How this law can help us to understand the ideality of a solution. LONG QUESTIONS. ● Define solubility curve. Explain different types of solubility curves with the help of graphs. ● Describe one method to determine the boiling point of elevation of solutes. ● Describe Landeberger’s method for the measurement of boiling point elevation. CHAPTER NO. 10 ELECTROCHEMISTRY SHORT QUESTIONS. ● Calculate oxidation number of chromium in the following compounds. CrCl2 (ii) K2CrO4 ● Define oxidation number and calculate the oxidation state of the underlined element. H2PO4 ii) Ca(ClO3)2 ● What is ionization and electrolysis? ● What is Anodized Aluminium? ● What is ionization and electrolysis? ● Difference between primary and secondary cells giving one example each. ● What is electrode potential? LONG QUESTIONS. ● State rules for assigning oxidation number of elements with example. ● What is electrolysis? Discuss the electrolysis of fused salt PbBr. ● Write construction and working of voltaic cells. CHAPTER NO. 11. REACTION KINETICS SHORT QUESTIONS. ● Guess Chemistry 1st yearWhat is the rate of reaction, also give name of four physical methods used to determine the rate of reaction? ● What is meant by order of reaction? Give an example. ● What is meant by the half-life period? Give one example. ● The radioactive decay is always a first order reaction. ● What do you mean by Activation complex of a reaction? LONG QUESTIONS. ● What are enzymes? Mention the characteristics of enzyme catalysis. ● How does the Arrhenius equation help us to calculate the energy of activation of a reaction?