Class 11ChemistryClassification of Elements and Periodicity in PropertiesMix Examples - Classification of Elements and Periodicity in Properties
EasyIn what properties do the first elements of a group differ from the subsequent elements of the same group?
(N/A) The first elements of a group (e.g.,$Li, Be, B, C, N, O, F$) exhibit anomalous properties compared to the rest of the elements in their respective groups due to their small size,high electronegativity,and absence of $d$-orbitals.
| $1$. First element of the group | $2$. Subsequent elements of the group |
| They can form a maximum of $4$ bonds (e.g.,$[BF_4]^-$). | They can form more than $4$ covalent bonds (e.g.,$[Al(H_2O)_6]^{3+}$). |
| They form multiple bonds with themselves and other elements (e.g.,$C=C, N=N, C\equiv C, N\equiv N, C=O, C\equiv N, N=O$). | They do not typically form multiple bonds. |
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Similar Questions
Which of the following statements is incorrect?
Difficult
View SolutionWhich of the following is not a periodic property?
Two statements are given below.
Statement $I$: Nitrogen has more ionization enthalpy and electronegativity than beryllium.
Statement $II$: $CrO_3$ and $B_2O_3$ are acidic oxides.
Correct answer is
Statement $I$: Nitrogen has more ionization enthalpy and electronegativity than beryllium.
Statement $II$: $CrO_3$ and $B_2O_3$ are acidic oxides.
Correct answer is
Which of the following pairs shows a diagonal relationship?
Which of the following order$(s)$ is/are correct?
$(1) Li < Be < B < C$ $(IE_1)$
$(2) Li < Na < K < Rb < Cs$ (Reducing power in gaseous state)
$(3) Li^{+} < Na^{+} < K^{+} < Rb^{+} < Cs^{+}$ (Ionic mobility in aqueous solution)
$(4) S > Se > Te > O$ $(EA)$
$(1) Li < Be < B < C$ $(IE_1)$
$(2) Li < Na < K < Rb < Cs$ (Reducing power in gaseous state)
$(3) Li^{+} < Na^{+} < K^{+} < Rb^{+} < Cs^{+}$ (Ionic mobility in aqueous solution)
$(4) S > Se > Te > O$ $(EA)$
Difficult
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