A) \[A{{l}_{2}}{{O}_{3}}<MgO<N{{a}_{2}}O<{{K}_{2}}O\]
B) \[Mg\,O\]\[<{{K}_{2}}O\]\[<\]\[A{{I}_{2}}{{O}_{3}}\]\[<N{{a}_{2}}O\]
C) \[N{{a}_{2}}O\]\[<{{K}_{2}}O\]\[<MgO\]\[<\]\[A{{I}_{2}}{{O}_{3}}\]
D) \[{{K}_{2}}O\]\[<N{{a}_{2}}O\]\[<\]\[A{{I}_{2}}{{O}_{3}}\]\[<MgO\]
Correct Answer: A
Solution :
[a] In a period, the nature of oxides varies from basic to acidic while in a group, basic nature of oxides increases. \[Oxides\underleftarrow{Decreaes}\]In a period, basic nature Changes to acidic nature| \[\downarrow \]Basic nature | |||
| Increases in a group | |||
| Group | 1 | 2 | 13 |
| Period 3\[\to \] | \[N{{a}_{2}}O\] | \[MgO\] | \[A{{l}_{2}}{{O}_{3}}\] |
| (Amphotiric oxide) | |||
| Period 4\[\to \] | \[{{K}_{2}}O\] | (Strongly basic) | |
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