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Nitrogen (atomic number $7$) and phosphorus (atomic number $15$) belong to group $15$ of the Periodic Table. Write the electronic configuration of these two elements. Which of these will be more electronegative? Why?
Solution
| Element | $K$ | $L$ | $M$ |
| Nitrogen | $2$ | $5$ | – |
| Phosphorus | $2$ | $8$ | $5$ |
Nitrogen is more electronegative than phosphorus. On moving down a group, the number of shell increases. Therefore, the valence electrons move away from the nucleus and the effective nuclear charge decreases. This causes the decrease in the tendency to attract electron and hence electronegativity decreases.
Similar Questions
The position of three elements $A$, $B$ and $C$ in the Periodic Table are shown below
| Group $16$ | Group $17$ |
| – | – |
| – | $A$ |
| – | – |
| $B$ | $C$ |
$(a)$ Will $C$ be larger or smaller in size than $B$ ?
$(b) $ Which type of ion, cation or anion, will be formed by element $A$ ?
The position of three elements $A$, $B$ and $C$ in the Periodic Table are shown below
| Group $16$ | Group $17$ |
| – | – |
| – | $A$ |
| – | – |
| $B$ | $C$ |
$ (a)$ State whether $A$ is a metal or non-metal.
$(b)$ State whether $C$ is more reactive or less reactive than $A$.
