Balbharati solutions for Chemistry [English] 11 Standard chapter 4 - Structure of Atom [Latest edition]

Choose the correct option.

The energy difference between the shells goes on ________ when moved away from the nucleus.

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The value of Plank’s constant is -

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p-orbitals are _________ in shape.

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“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -

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Principal Quantum number describes -

Make the pairs:

Complete the following information about the isotopes in the chart given below:

Match the following:

Answer in one sentence:

If an element ‘X’ has mass number 11 and it has 6 neutrons, then write its representation.

Answer in one sentence:

Name the element that shows the simplest emission spectrum.

State Heisenberg uncertainty principle.

Give the names of quantum numbers.

Identify from the following the isoelectronic species:

Ne, O^2-, Na⁺ OR Ar, Cl^2-, K^⊕

Differentiate between Isotopes and Isobars.

Define the term Isotones.

Define the term Isoelectronic species

Define the term Electronic configuration

State and explain Pauli’s exclusion principle.

State Hund’s rule of maximum multiplicity with a suitable example.

Write the drawbacks of Rutherford’s model of an atom.

Write postulates of Bohr’s Theory of hydrogen atom.

Mention demerits of Bohr’s Atomic model.

State the order of filling atomic orbitals following Aufbau principle.

Explain the anomalous behaviour of copper.

Explain the anomalous behaviour of chromium.

Write orbital notations for the electron in orbitals with the following quantum numbers.

n = 2, l = 1

Write orbital notations for the electron in orbitals with the following quantum numbers.

n = 4, l = 2

Write orbital notations for the electron in orbitals with the following quantum numbers.

n = 3, l = 2

Write electronic configurations of \[\ce{Fe, Fe2+, Fe3+}\].

Write condensed orbital notation of electronic configuration of the following element:

Lithium (Z = 3)

Write condensed orbital notation of electronic configuration of the following element:

Carbon (Z = 6)

Write condensed orbital notation of electronic configuration of the following element:

Oxygen (Z = 8)

Write condensed orbital notation of electronic configuration of the following element:

Silicon (Z = 14)

Write condensed orbital notation of electronic configuration of the following element:

Chlorine (Z = 17)

Write condensed orbital notation of electronic configuration of the following element:

Calcium (Z = 20)

Draw shapes of 2s orbitals.

Draw shapes of 2p orbitals.

Explain in brief, the significance of the azimuthal quantum number.

If n = 3, what are the quantum number l and m?

The electronic configuration of oxygen is written as 1s² 2s² \[\ce{2p^2_{{x}}}\] \[\ce{2p^1_{{y}}}\] \[\ce{2p^1_{{z}}}\] and not as 1s² 2s² \[\ce{2p^2_{{x}}}\], \[\ce{2p^2_{{y}}}\] \[\ce{2p^0_{{z}}}\], Explain.

Write a note on ‘Principal Quantum number.

Using the concept of quantum numbers, calculate the maximum numbers of electrons present in the ‘M’ shell. Give their distribution in shells, subshells, and orbitals.

Indicate the number of unpaired electrons in \[\ce{Si}\] (Z = 14).

Indicate the number of unpaired electron in:

Cr (Z = 24)

An atom of an element contains 29 electrons and 35 neutrons. Deduce the number of protons.

An atom of an element contains 29 electrons and 35 neutrons. Deduce the electronic configuration of that element.