Element ‘A’ and 'B' both have atomic numbers 18 and 16 which of respectively. Which of these two would be more reactive and why?

Open in App

Solution

Electronic configuration of ‘A’ (Z =18) = 2,8,8
Electronic configuration of ‘B’ (Z =16) = 2,8,6
Element 'A' has completely filled outermost shell (M-shell). It would be, therefore, least reactive.
Element 'B' has an incomplete outermost shell (M-shell has 6 electrons) only.
Conclusion: Therefore, element 'B' would be more reactive than element 'A'.

Suggest Corrections

Similar questions

Q. Nitrogen (atomic number

7

) and phosphorus (atomic number

15

) belong to the group

15

of the Periodic Table. Write the electronic configuration of these two elements. Which of these will be more electronegative and Why?

Q. (a) What were the two major shortcomings of Mendeleev's periodic table? How have these been removed in the modern periodic table?
(b) Two elements X and Y have atomic numbers 12 and 16 respectively. Write the electronic configuration for these elements. To which period of the modern periodic table do these two elements belong? What type of bond will be formed between them and why?
(c) To which groups of the modern periodic table do the elements X and Y belong? Give reason for your answer.
(d) What could the elements X and Y be? Write their names and symbols.

Nitrogen (atomic number 7) and phosphorus (atomic number 15) belong to group 15 of the periodic table. Write the electronic configurations of these two elements. Which of these will be more electronegative? Why?

Elements A and B have mass numbers 18 and 16 respectively. Which of these is more reactive and why?

Q. Which of the two will be chemically more reactive; element A with atomic number 16 or element B with atomic number 17? Why?

Join BYJU'S Learning Program