Consider the location of barium, chlorine, iodine, and strontium on the periodic table. Electronegativities Which type of atom has the strongest attraction for electrons in bond formation? barium (Ba) chlorine (Cl) iodine (I) strontium (Sr)

The more right you are and the more up you are, the stronger the connection.

Start by going left to right. The two furthest are Iodine and Chlorine (so barium and strontium are eliminated). Then look at that column vertically. Chlorine is further up, so that is your answer.

Answer: The correct answer is Chlorine (Cl).

Explanation: Electronegativity is the property of an element to attract the shared pair of electron towards itself. In a periodic table, the electronegativity increases as we move from left to right and it decreases as we move from top to bottom.

The location of the given elements are:

Barium (Ba) : It belongs to Group 2 and Period 6 of the periodic table.

Chlorine (Cl) : It belongs to Group 17 and Period 3 of the periodic table.

Iodine (I) : It belongs to Group 17 and Period 5 of the periodic table.

Strontium (Sr) : It belongs to Group 2 and Period 5 of the periodic table.

From the above information, Chlorine belongs to the lowest period and greatest group number. Hence, it has the highest electronegativity and will attract the shared pair of electron towards itself strongly.

Therefore, the correct answer is Chlorine (Cl).