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(D) Electronegativity generally increases as we move up a group in the periodic table due to a decrease in atomic size and an increase in effective nu

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$Be$

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(D) Electronegativity generally increases as we move up a group in the periodic table due to a decrease in atomic size and an increase in effective nuclear charge. All the given elements ($Be$,$Mg$,$Ca$,$Sr$) belong to Group $2$ (Alkaline Earth Metals). The order of elements from top to bottom in Group $2$ is $Be$,$Mg$,$Ca$,$Sr$. Since $Be$ is at the top of this group,it has the smallest atomic size and the highest electronegativity among the given options.

Which of the following elements has the highest electronegativity?

Similar Questions

Arrange the following elements in the decreasing order of their electronegativity values.

Given below are two statements:
Statement $I$: The correct order of electronegativity of fluorine, oxygen and nitrogen is $F > O > N$.
Statement $II$: The oxidation state of oxygen in $OF_2$ is $+2$ and in $Na_2O$ is $-2$.

Arrange $F$,$Cl$,$O$,and $N$ in the decreasing order of electronegativity.

The element with the highest electronegativity value after fluorine $(F)$ is:

Pauling's electronegativity values for elements are useful in predicting:

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