An element’s atomic structure refers to the structure of its nucleus and the arrangement of electrons around it. The atomic structure of matter is primarily composed of protons, electrons, and neutrons.
The nucleus of the atom is made up of protons and neutrons, which are surrounded by the atom’s electrons. An element’s atomic number describes the total number of protons in its nucleus.
Neutral atoms contain the same number of protons and electrons. On the other hand, atoms can gain or lose electrons to increase their stability, and the resulting charged entity is known as an ion.
Because different elements have different numbers of protons and electrons, their atomic structures differ. This is the cause of the unique characteristics of different elements.
Download PDF of Class 11 Chemistry Chapter 2 Structure of Atom – Set 1
CBSE Class 11 Chemistry Worksheet Chapter 2 Structure of Atom – Set 1
Q1. Which of the following orbitals do not make sense?
a.) 6s
b.) 3p
c.) 2d
d.) 4f
Q2. Orbital angular momentum depends on:
a.) l
b.) n and l
c.) n and m
d.) m and s
Q3. In the manganese atom, Mn (Z = 25), the total number of orbitals populated by one or more electrons (in the ground state) is:
a.) 15
b.) 14
c.) 12
d.) 10
Q4. The following quantum numbers are possible for how many orbitals?
n = 3, l = 2, ml = +2
a.) 1
b.) 2
c.) 3
d.) 4
Q5. In Bohr’s orbit, the ratio of total kinetic energy and the total energy of the electron is:
a.) –2
b.) –1
c.) +2
d.) 0
Q6. Define Hund’s rule of maximum multiplicity.
Q7. Define electromagnetic spectrum.
Q8. How many protons, electrons, and neutrons are there in the following nuclei?
i.) 178O
ii.) 2512Mg
iii.) 8035Br
Q9. State the drawbacks of the Rutherford Model of an atom.
Q10. Calculate and compare the energies of two radiations, one with a wavelength of 800 nm and the other with a wavelength of 400 nm.
Q11. State Heisenberg’s Uncertainty principle.
Q12. i.) An atomic orbital has n = 3. What are the possible values of l and ml?
ii.) List the quantum numbers (ml and l) of electrons for the 3-d orbital.
iii.) Which of the following orbitals are possible 1p, 2s, 2p and 3f?
Q13. The radius of the fourth orbit in a hydrogen atom is 0.85 nm. Calculate the velocity of the electron in this orbit (mass of electron = 9.1 × 10–31 kg).
Q14. State and explain Pauli’s exclusion principle. Write the electronic configuration of the element with atomic number 24.
Q15. a.) What is the Aufbau principle? Write electronic configurations of the elements with atomic numbers 16, 20 and 35.
b.) Explain why half-filled and completely filled orbitals have extra stability?
Q16. How many unpaired electrons are present in the ground state of
i.) P (Z = 15)
ii.) Fe2+ (Z = 26)
iii.) Cl– (Z = 17)
Q17. On the basis of Heisenberg’s uncertainty principle, show that an electron cannot exist within the atomic nucleus of a radius of 10–15 m.
Q18. An electron is moving with a kinetic energy of 2.275 × 10–25 J. Calculate its de-Broglie wavelength.
(Mass of electron = 9.1 × 10–31 kg, h = 6.6 × 10–34 J s)
Q19. In the Rydberg equation, a spectral line corresponds to n1 = 3 and n2 = 5.
i.) Calculate the wavelength and frequency of this spectral line.
ii) To which spectral series does this line belong?
iii.) In which region of the electromagnetic spectrum will this line fall?
Q20. What is the photoelectric effect? State the results of the photoelectric effect experiment that could not be explained based on the laws of classical physics. Explain this effect based on the quantum theory of electromagnetic radiations.
Download PDF to access answers of the Chemistry Worksheet for Class 11 Chemistry Chapter 2 Structure of Atom Set – 1.
Read Also:
- Class 11 Chemistry Chapter 2 Structure of Atom MCQs
- Important Questions for Class 11 Chemistry Chapter 2 Structure of Atom
- Chemistry Concept Questions and Answers
- CBSE Class 11 Chemistry Practical
- Aufbau Principle
- Subatomic Particles
- Rutherford Atomic Model
- Planck’s Quantum Theory: Quantisation of Energy
- Bohr’s Model of An Atom
