The basic character of the transition metal monoxides follows the order: (Atomic no. - Ti = 22, V = 23, Cr = 24, Fe = 26)
The basic character of the transition metal monoxides follows the order: (Atomic no. - Ti = 22, V = 23, Cr = 24, Fe = 26)
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Transition metals belong to the d-block of the periodic table. In these elements, the last electron goes to the d orbital.
VO > CrO > TiO > FeO
CrO >VO > FeO > TiO
TiO > FeO > VO > CrO
TiO > VO > CrO > FeO
The Correct Option is D
Approach Solution - 1
As the metal ion size decreases from Ti to Fe, the basic nature of their monoxide decreases. So. the basic character of oxides decreases with an increase in atomic number.
Hence, the basic character of the transition metal monoxides follows the order TiO > VO > CrO > FeO.
Approach Solution -2
Hint: Transition metals belong to the d-block of the periodic table. In these elements, the last electron goes to the d orbital. The basic character of a compound is calculated by the ability to donate lone pairs of electrons to other substances. This type of base is called lewis base.
Complete Answer:
- As we move from the left to the right side of the transition series, the atomic number of elements and no. of electrons increases.
- The size of elements decreases from left to right as the effective nuclear charge of the nucleus on the outermost shell electron increases.
- As the electronegativity of atoms increases from left to right, the power of donation of electrons decreases and hence the basicity of the element decreases.
So, option D is the correct answer - TiO > VO > CrO > FeO.
Note: In periods, with increasing atomic number, the size decreases and in the groups with an increase in atomic number, the size also increases.
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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