1st Year Chemistry Notes Chapter 1

• Here are the detailed 1st year chemistry chapter 1 notes to help you prepare for your exams.
• Important Fill in the blanks with answers of Chapter Number 1: Basic Concepts of First-year Chemistry Punjab Textbook Boards.
• Write "T" for a true statement and "F" for a false statement.
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• Differentiate between homo-atomic and hetero-atomic molecule with examples?
• Calculate mass in grams of 10-3 moles of H20. Molecular mass of H20 = 18?
• Calculate the percentage of Nitrogen in NH3.
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• Why Atomic Masses mentioned in literature are in fraction? OR Why elements have fractional atomic masses?
• Define atomic mass unit. Give its value in grams?
• Why atoms cannot be observed by an ordinary optical microscope?
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• Differentiate between atom and molecule?
• Define ion and give its two examples?
• N2 and CO have the same number of electrons, protons and neutrons. Explain with reason?
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• Define atomicity? Give two examples.
• Differentiate between ion and molecular ion? with examples.
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• Define cation and anion? For example
• What are isotopes? Why they have same chemical but different physical properties?
• Explain relative abundance of isotopes with suitable example
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• How do no individual Ne atom in the sample of the element has mass of 20.18 a.m.u?
• Write only names of any four methods employed for the separation of Isotopes.
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• Explain mathematical relationship for m/e of an ion in mass 'spectrometry?
• What is the Function of ionization Chamber in Mass Spectrometer?
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• Vapours are allowed to enter the ionization chamber where fast moving electrons are thrown upon them. The atoms of isotopic elements present in the form of vapours are ionized. These positively charged ions of isotopes of an element have different masses depending upon the nature of the isotopes present in them. 
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• Write down the names of water absorber and CO2 absorber in combustion analysis experiment?
• Molecular formula is a nth multiple of empirical formula. Explain with examples.
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• 180g of glucose and 342g of sucrose have the same number of molecules but different number of atoms present in them. Why?
• What do you know about gram atom? How we can calculate gram atom of an element? Give its relationship.
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• One mole of H2SO4 should completely react with two moles of NaOH. How does Avogadro's number help to explain it?
• Why do 2g of H2 16g of CH4 , 44g of CO2 occupy separately the volume of 22.414 dm3 although the sizes and masses of molecules of three gases are very different from each other?
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• Law of conservation of mass has to be obeyed during stoichiometric calculations. Justify it.
• How do many chemical reactions take place in our surroundings involve the limiting reactant?
• Many chemical reactions taking place in our surroundings involve the limiting reactants.
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• Why we use the term relative atomic mass? OR Define Relative atomic mass. Give two examples.
• How many moles of C02 can be produced from burning one mole of octane, Mass of octane is 114?
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• Write down role of magnetic separator in mass spectrometer. What is function of magnetic field in mass spectrometer?
• What is Justification of two strong peaks of almost equal heights in mass spectrum of Bromine?
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• Define stoichiometry. Give two assumptions for stoichiometric calculations. Justify it.
• What is combustion analysis? How can you calculate the percentage of the carbon, hydrogen and oxygen in an organic compound by this method?
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• Define the following and give one example of each. (i). Avogadro's number. (ii). Molecular ion. (iii). Mole. (iv). Isotopes.
• Write a note on limiting reactant and explain by giving two examples. OR Define Limiting reactant and how it is identified by different steps.
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