Medium
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 $A$?
| 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 $A$?
(N/A) will be smaller in size than $B$. As we move from left to right across a period,the nuclear charge increases,which pulls the electrons closer to the nucleus,resulting in a decrease in atomic size.
$(b)$ $A$ will form an anion. Since $A$ belongs to Group $17$,it has $7$ valence electrons and needs one more electron to complete its octet,thus it gains an electron to form a negatively charged ion (anion).
$(b)$ $A$ will form an anion. Since $A$ belongs to Group $17$,it has $7$ valence electrons and needs one more electron to complete its octet,thus it gains an electron to form a negatively charged ion (anion).
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Similar Questions
Which element has
$(a)$ a total of three shells,with four electrons in its valence shell?
$(b)$ a total of two shells,with three electrons in its valence shell?
$(c)$ twice as many electrons in its second shell as in its first shell?
$(a)$ a total of three shells,with four electrons in its valence shell?
$(b)$ a total of two shells,with three electrons in its valence shell?
$(c)$ twice as many electrons in its second shell as in its first shell?
Medium
View SolutionThe 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 $A$.
| 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 $A$.
Medium
View SolutionNitrogen (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?
Medium
View SolutionAn atom has an electronic configuration of $2, 8, 7$.
$(a)$ What is the atomic number of this element?
$(b)$ To which of the following elements would it be chemically similar? (Atomic numbers are given in parentheses.)
$N(7), F(9), P(15), Ar(18)$
$(a)$ What is the atomic number of this element?
$(b)$ To which of the following elements would it be chemically similar? (Atomic numbers are given in parentheses.)
$N(7), F(9), P(15), Ar(18)$
Medium
View SolutionHow does the electronic configuration of an atom relate to its position in the Modern Periodic Table?
Easy
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