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Structure of Atom

Short Answer Type

221.

What subshells are possible in n = 3 energy level?

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222. What is the lowest value of n that allows g orbitals to exist ?

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223.

Using s, p, d notations describe the orbital with the following quantum numbers :
(a) n = 1, l = 0,
(b) n = 3, l = 1,
(c) n = 4, l = 2,
(d) n = 4, l = 3.

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Long Answer Type

224.

State and explain Pauli's Exclusion Principle.

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Short Answer Type

225. Why Pauli’s exclusion principle is called exclusion principle?

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226. Why in the building of the atom, the filling of 4s orbital takes place before 3d orbital?

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Long Answer Type

227. Describe Aufbau Principle.

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228.
Discuss the shapes of s-orbitals.

For s-orbital, l = 0 and hence m = 0. Thus s-orbital has only one orientation. This means that probability of finding an electron in s-orbital is same in all directions at a given distance from the nucleus. In other words. Is orbital is non-directional and spherically symmetrical.

The s-orbitals of higher energy levels (2s, 3s, etc.) are also non-directional and spherically symmetrical. However, the effective volume or size is larger than Is orbital. Thus 2s-orbital is larger than 1s-orbital. Also in 2s-orbital, there is a spherical shell within the orbital where the probability of finding the electron is practically zero. This is called a node or nodal plane or nodal surface.
In general, the number of nodes in s-orbital of any energy level is equal to (n - 1), where n represents the principal quantum number.

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Short Answer Type

229. Give three points of difference between 1s and 2s orbitals.

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230.

The bromine atom possesses 35 electrons. It contains 6 electrons in 2p orbital, 6 electrons in 3p orbital and 5 electrons in 4p orbital. Which of these electron experiences the lowest effective nuclear charge?

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