1st Year Chemistry Guess Paper

• Here are the detailed first year chemistry guess paper to help you prepare for your exams.
• Important Short questions of all chapters.
• What is molecular ion? How it is formed?
• Why isotopes have same chemical properties but different physical properties?
• No individual Ne (neon) atom in the sample has a mass of 20.18 a.m.u justify. 
• 23g of sodium and 238g of uranium have equal number of atoms in them. Justify.
• Mg atom is twice heavier than that of carbon atom.
• 180g of glucose and 342 g of sucrose have the same number of molecules but different number of atoms present in them. Justify.
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• Write down the steps involved in the determination of a limiting reactant.
• Concept of limiting reactant is not applicable on reversible reactions. Justify. 
• Law of conservation of mass has to be obeyed during stoichiometric calculations.
• CO and N2 have same number of electrons protons and neutrons.
• Many chemical reactions taking place in our surrounding involve limiting reactant.
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• Differentiate between stationary phase and mobile phase.
• Differentiate between adsorption chromatography and partition chromatography. 
• Why do we get a straight line when pressures exerted on a gas are plotted against inverse of volume?
• Differentiate between mean square velocity and root mean square velocity. 
• Define hydrogen bonding and show H-bonding in HF, NH3, CHCl3-acetone.
• Why HF is weaker acid as compared to HCl, HBr, HI?
• H2O is liquid while H2S and H2Se are gases at room temperature. Give reason.
• Boiling point of H2O is greater than that of HF. Justify.
• Water and ethanol can mix easily and in all proportions. Justify. 
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• In a very cold winter the fish in garden ponds owe their lives to hydrogen bonding.
• Why boiling point of water is different at Murree hills and at Mount Everest?
• Define Polarizibility. How it effect London dispersion forces?
• How liquid crystals are used to find the potential failure in electrical circuits?
• How liquid crystals are used to locate infections and tumors in body? 
• Draw the shape, axes and angles of hexagonal, cubic and orthorhombic system.
• Why ionic crystals do not conduct electricity in the solid state?
• Why ionic crystals are brittle?
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• Diamond is hard and an electrical insulator. Give reason.
• The electrical conductivity of metals decreases with the increase in temperature. Why?
• Define H-bonding and explain H-bonding in biological molecules ( proteins, DNA ).
• Explain the terms ( isomorphism-polymorphism, Transition temperature, types of solids).
• Why is it necessary to decrease the pressure in discharge tube?
• Whichever gas is used in the discharge tube, the nature of the cathode rays remains the same.
• Why the nature of cathode rays is independent of the nature of gas used in discharge tube?
• Why e\m value of the cathode rays is just equal to that of electron?
• Why positive rays are also called canal rays?
• The e\m value for positive rays obtained from hydrogen gas is 1836 times less than that of cathode rays. Justify it. 
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• Differentiate between atomic emission and atomic absorption spectrum.
• State Moseley’s law. Give its mathematical expression.
• Define Heisenberg’s uncertainty principle with mathematical relation.
• State Hund’s rule, Aufbau principle and Pauli’s exclusion principle.
• Define quantum numbers and explain ( Azimuthal, principal , magnetic ) quantum numbers.
• How the nature of a chemical bond is predicted with the help of electronegativity values?
• Define ionization energy and electronegativity. Write its periodic trend.
• Differentiate between polar and non-polar covalent bond with examples.
• Why the lone pair of electrons occupies more space than bond pairs?
• Bond angles of CH4, NH3 and H2O are different while all these show sp3 - hybridization.
• Differentiate between bonding and antibonding molecular orbitals.
• The dipole moment of CO2 and CS2 is zero while CO and SO2 is not zero. Justify.
• How the percentage ionic character of a covalent bond is determined by dipole moment?
• Why it is necessary to mention the physical states of reactants and products in thermochemical reactions?
• Define system, surrounding and state function with examples.
• State 1st law of thermodynamic with mathematical formula. 
• How some reactions are effected by volume at equilibrium stage?
• What is the effect of temperature on solubility?
• How ammonia is synthesized by Haber’s process? Also write its conditions.
• Define common ion effect with one example.