Question:
The number of elements present in the $d$-block of the periodic table is
The number of elements present in the $d$-block of the periodic table is
Updated On: Jan 30, 2025
- 40
- 41
- 45
- 46
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The Correct Option is A
Approach Solution - 1
The number of elements present in the d-block of the periodic table is $40$. Four series of transition elements (each series having $10$ elements) constitute $d$-block.
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The right answer to our question is 40, because the number of elements in the periodic table's d-block is 40. D-block elements are also referred to as transition metals because they exhibit transient conductivity between s-square and p-block components. D block components are those that can be found from the third to the twelfth gatherings of the most recent intermittent table. These components' valence electrons are in the d orbital. D block components are also known as change components or progress metals. The first three columns of the d block components correspond to the 3d, 4d, and 5d orbitals, respectively.
The following table displays material components made of nuclear numbers, beginning with the component with the lowest nuclear number, hydrogen, and progressing to the component with the highest nuclear number. The intermittent table's components are organized by nuclear number. This list includes all 118 components of science. Because of how the components are organized, it is known as the intermittent table. Even lines (from left to right) are termed "periods," while vertical portions (from up to down) are called “gatherings”.
The following table displays material components made of nuclear numbers, beginning with the component with the lowest nuclear number, hydrogen, and progressing to the component with the highest nuclear number. The intermittent table's components are organized by nuclear number. This list includes all 118 components of science. Because of how the components are organized, it is known as the intermittent table. Even lines (from left to right) are termed "periods," while vertical portions (from up to down) are called “gatherings”.
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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