To determine which type of atom has the strongest attraction for electrons in bond formation, we need to consider the concept of electronegativity. Electronegativity is a measure of an atom's ability to attract and bond with electrons. Atoms with higher electronegativity have a stronger attraction for electrons in bond formation.
Let's analyze the options given:
1. Barium (Ba): Barium is an alkaline earth metal found in Group 2 of the periodic table. Alkaline earth metals generally have low electronegativity because they tend to lose electrons and form positive ions.
2. Chlorine (Cl): Chlorine is a halogen found in Group 17 of the periodic table. Halogens are known for their high electronegativity because they tend to gain electrons and form negative ions. Chlorine, specifically, has one of the highest electronegativities among the elements.
3. Iodine (I): Iodine is also a halogen and is found in Group 17. While iodine is quite electronegative, it is less electronegative than chlorine due to its larger atomic radius, which makes it less effective at attracting electrons compared to chlorine.
4. Strontium (Sr): Strontium is another alkaline earth metal in Group 2, similar to barium. Like other members of its group, strontium has a relatively low electronegativity.
Given that electronegativity increases across a period from left to right and decreases down a group in the periodic table, we can conclude that among the options provided, chlorine (Cl) has the highest electronegativity and consequently, the strongest attraction for electrons in bond formation.
Therefore, the atom with the strongest attraction for electrons in bond formation is:
Chlorine (Cl).
