Class 11ChemistryClassification of Elements and Periodicity in PropertiesMix Examples - Classification of Elements and Periodicity in Properties
MediumWhat are the differences between the first element of a group and the subsequent elements in the same group?
(N/A) The first element of a group differs from the subsequent elements due to its small size,high electronegativity,and the absence of $d$-orbitals in its valence shell. The differences are summarized below:
| First element of the group | Other elements of the group |
|---|---|
| Forms covalent compounds. | Forms ionic compounds. |
| Small atomic/ionic size. | Larger atomic/ionic size. |
| High charge/radius ratio. | Low charge/radius ratio. |
| High electronegativity. | Low electronegativity. |
| Only $4$ orbitals available in the valence shell ($s$ and $p$). | $9$ orbitals available in the valence shell ($s, p,$ and $d$). |
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Similar Questions
Which of the following does not depend on stable electronic configuration?
Medium
View SolutionWhich of the following statements is not correct?
Medium
View SolutionMatch the following and select the correct option:
List-$I$ List-$II$ $(A)$ Ionization enthalpy $(i)$ $P < Si < Mg < Na$ $(B)$ Metallic character $(ii)$ $I < N < O < F$ $(C)$ Electron gain enthalpy $(iii)$ $B < Be < C < O < N$ $(D)$ Electronegativity $(iv)$ $I < Br < F < Cl$
| List-$I$ | List-$II$ |
|---|---|
| $(A)$ Ionization enthalpy | $(i)$ $P < Si < Mg < Na$ |
| $(B)$ Metallic character | $(ii)$ $I < N < O < F$ |
| $(C)$ Electron gain enthalpy | $(iii)$ $B < Be < C < O < N$ |
| $(D)$ Electronegativity | $(iv)$ $I < Br < F < Cl$ |
Identify the incorrect statement.
Medium
View SolutionConsider the following values of $IE$ $(eV)$ for elements $W$ and $X$:
Element $IE_1$ $IE_2$ $IE_3$ $IE_4$ $W$ $10.5$ $15.5$ $24.9$ $79.8$ $X$ $8$ $14.8$ $78.9$ $105.8$
Other two elements $Y$ and $Z$ have outer electronic configuration $ns^2 np^4$ and $ns^2 np^5$ respectively. According to the given information,which of the following compound$(s)$ is/are not possible?
$(a) W_2Y_3, (b) X_2Y_3, (c) WZ_2, (d) XZ_2$
| Element | $IE_1$ | $IE_2$ | $IE_3$ | $IE_4$ |
| $W$ | $10.5$ | $15.5$ | $24.9$ | $79.8$ |
| $X$ | $8$ | $14.8$ | $78.9$ | $105.8$ |
Other two elements $Y$ and $Z$ have outer electronic configuration $ns^2 np^4$ and $ns^2 np^5$ respectively. According to the given information,which of the following compound$(s)$ is/are not possible?
$(a) W_2Y_3, (b) X_2Y_3, (c) WZ_2, (d) XZ_2$
Difficult
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