Question

3. Define: 1) Mole, id) Molar mass.
4. Calculate the number of oxygen atoms in the following compound:
#. 20g of CaCO3
b. 10 moles of CaCO,
5. What is empirical and molecular formula? How are they related to each other?
6. Calculate mass percentage of calcium, carbon, and oxygen in CaCO). (Ca -40C12,
O=16)
7. An inorganic salt on analysis gave the following percentage composition:
Pb = 62.6. N = 8.4.0=29.0. What is empirical formula of the compound?
8. Define Limiting Reagent.
9. Ig of magnesium is burnt with 0.56g of Oz in a closed vessel. Which reactant is left in excess and
how much?
STRUCTURE OF ATOM
10. Describe Bohr's Model of Atom and explain its usefulness.
11. Explain qualitatively the line spectrum of hydrogen using Bohr's model.
12. Derive de-Broglie equation for microscopic particles.
13. State Heisenberg's uncertainty principle. Give its mathematical expression
14. What are the differences between orbit and orbital?
15. Discuss the types of quantum numbers and their significance.
16. Define (1) Aufbau principle, (11) Hund's rule of maximum multiplicity, (ii) Pauli's exclusion
principle.
17. Write the electronic configuration of jyCu, zaCu", aFe 2. Cr.​

Answer 1

Answer:

3

The molar mass is defined as the mass in grams of 1 mol of that substance. One mole of isotopically pure carbon-12 has a mass of 12 g. That is, the molar mass of a substance is the mass (in grams per mole) of 6.022 × 10 23 atoms, molecules, or formula units of that substance. ...

4 is remaining

5

Empirical formulas show the simplest whole-number ratio of atoms in a compound, molecular formulas show the number of each type of atom in a molecule, and structural formulas show how the atoms in a molecule are bonded to each other