Question:
Which of the following statements(s) is (are) correct?
Which of the following statements(s) is (are) correct?
Updated On: Jun 18, 2022
- The electronic configuration of Cr (at. no: 24) is $\left[Ar\right]3d^{5} 4S^{1}$
- The magnetic quantum number may have a negative value
- In Ag (at. no: 47), 23 electrons have spins of one type and 24 electrons have spins of opposite type
- The oxidation state of nitrogen in $HN_{3}$ is - 3
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The Correct Option is C
Solution and Explanation
Electronic configuration of $Cr\to\left[Ar\right]3d^{5} 4S^{1}$
$\to$ Let l = 1, $m_{1}$ = -1, 0, +1
$\to Ag\to1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10} 4s^{2}4p^{6}4d^{10}5s^{1}$
No. of electrons having $m_{s} =+1/2 \, or-1/2 =$ 24 and rest 23
$\to$ oxidation number of N in $\,HN_{3} in -\frac{1}{3}$
$\to$ Let l = 1, $m_{1}$ = -1, 0, +1
$\to Ag\to1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10} 4s^{2}4p^{6}4d^{10}5s^{1}$
No. of electrons having $m_{s} =+1/2 \, or-1/2 =$ 24 and rest 23
$\to$ oxidation number of N in $\,HN_{3} in -\frac{1}{3}$
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Concepts Used:
d block elements
The elements, in the columns of the periodic table in which d subshells are being occupied are known as d block elements.
These are the elements that have the capability of forming stable cations with incompletely filled d orbitals. Elements like mercury and Zinc are not considered transition metals because they have electronic configurations: (n-1)d10 ns2. These elements have filled d-orbitals in their ground state and, therefore, even in some of their oxidation states.
General Properties Of d-Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behaviour and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high. This is because of the presence of unpaired electrons and partially filled d orbitals. Because of these two things, they form strong bonds and therefore have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements