Maximum number of electrons that can be filled in a d-subshell is:

10

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Solution

The correct option is A $10$
In $d - s u b s h e l l$ there are 5 magnetic quantum number values. hence, it contains 5 orbitals, where each orbital can acommodate 2 electrons with opposite spin. Therefore, total number of electrons in d-subshell is 10.

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Maximum number of electrons that can be accommodated in the subshell with azimuthal quantum number l = 4, is

Q. Maximum number of electrons that can be accommodated in the subshell with the azimuthal quantum number

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[A r] 4 s^{1} 3 d^{10}

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100

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Which of the following statements related to the modern periodic table is incorrect?
(a) The p-block has 6 columns, because a maximum of 6 electrons can occupy all the orbitals in a p-shell.
(b) The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.
(c) Each block contains a number of columns equal to the number of electrons that can occupy that subshell.
(d) The block indicates value of azimuthal quantum number (l ) for the last subshell that received electrons in building up the electronic configuration.

Maximum number of electrons that can be accommodated in the subshell with azimuthal quantum number l = 4, is

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Maximum number of electrons that can be filled in a d-subshell is:

The correct option is A 10In d−subshell there are 5 magnetic quantum number values. hence, it contains 5 orbitals, where each orbital can acommodate 2 electrons with opposite spin. Therefore, total number of electrons in d-subshell is 10.

The correct option is A $10$
In $d - s u b s h e l l$ there are 5 magnetic quantum number values. hence, it contains 5 orbitals, where each orbital can acommodate 2 electrons with opposite spin. Therefore, total number of electrons in d-subshell is 10.