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Question:
Identify the set of acidic oxides.
Identify the set of acidic oxides.
Updated On: Apr 4, 2024
- $Na_2O, CaO, BaO$
- $ZnO,PbO,BeO$
- $CO, NO,N_2O$
- $Mn_2 O_7, CrO_3, V_2O_5$
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The Correct Option is D
Solution and Explanation
Acidic oxides $\rightarrow Mn _{2} O _{7}, \,CrO _{3},\, V _{2} O _{5}$
(due to higher oxidation state of central metal) Basic oxide $\rightarrow Na _{2} O , CaO , BaO$
(due to lower oxidation state of central metal) Alkaline and alkali metal oxide are always basic. Neutral oxides $\rightarrow CO , NO , N _{2} O$
Amphoteric oxides $\rightarrow ZnO , PbO , BeO$ (acidic as well as basic)
(due to higher oxidation state of central metal) Basic oxide $\rightarrow Na _{2} O , CaO , BaO$
(due to lower oxidation state of central metal) Alkaline and alkali metal oxide are always basic. Neutral oxides $\rightarrow CO , NO , N _{2} O$
Amphoteric oxides $\rightarrow ZnO , PbO , BeO$ (acidic as well as basic)
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Concepts Used:
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 behavior 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 because of the presence of unpaired electrons and partially filled d orbitals. They form strong bonds and 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
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