Hydrogen, Oxygen, Chlorine, Fluorine, Iodine, Bromine, Tellurium, Selenium, Sulphur, Nitrogen, etc.
Elements from Group 1 (such as sodium) and Group 2 (such as magnesium) would bond ionically with chlorine. Sodium would form NaCl (sodium chloride) and magnesium would form MgCl2 (magnesium chloride) through ionic bonds with chlorine.
Elements lower in electronegativity such as lithium, sodium, or potassium would form an ionic bond with fluorine. This is because they are more likely to lose an electron to achieve a stable electron configuration and form a bond with the highly electronegative fluorine, which tends to gain electrons.
The pair of elements that is most likely to form an ionic bond are potassium (K) and fluorine (F). This is because potassium is a metal (it can lose electrons) and fluorine is a nonmetal (it can gain electrons), making them likely to transfer electrons and form an ionic bond.
Elements that are close to each other on the periodic table and have similar electronegativities are more likely to bond together conveniently. This is because they are more likely to share electrons in a more stable manner, forming covalent bonds. Examples include hydrogen and fluorine, or sodium and chlorine.
Sodium and chlorine will form an ionic bond, where sodium will donate an electron to chlorine, resulting in the formation of sodium chloride (table salt).
Elements from Group 1 (such as sodium) and Group 2 (such as magnesium) would bond ionically with chlorine. Sodium would form NaCl (sodium chloride) and magnesium would form MgCl2 (magnesium chloride) through ionic bonds with chlorine.
Elements lower in electronegativity such as lithium, sodium, or potassium would form an ionic bond with fluorine. This is because they are more likely to lose an electron to achieve a stable electron configuration and form a bond with the highly electronegative fluorine, which tends to gain electrons.
An element such as sodium, which readily gives up an electron to achieve a stable electron configuration, would likely form an ionic compound with fluorine. Sodium would form a sodium cation (Na+) and fluorine would form a fluoride anion (F-), creating an ionic bond between the two elements.
The pair of elements that is most likely to form an ionic bond are potassium (K) and fluorine (F). This is because potassium is a metal (it can lose electrons) and fluorine is a nonmetal (it can gain electrons), making them likely to transfer electrons and form an ionic bond.
Elements that are close to each other on the periodic table and have similar electronegativities are more likely to bond together conveniently. This is because they are more likely to share electrons in a more stable manner, forming covalent bonds. Examples include hydrogen and fluorine, or sodium and chlorine.
Sodium chloride has ionic bonds.
Sodium and chlorine will form an ionic bond, where sodium will donate an electron to chlorine, resulting in the formation of sodium chloride (table salt).
It will bond with sodium to create NaCl, salt. This is because it has more attractive force. Take a look at an activity series that will tell you which elements will form a compound over another element in a chemical reaction. See the link below.
Sodium would most likely combine with an element like chlorine to form sodium chloride, which is a common type of salt. This type of combination typically involves sodium donating an electron to chlorine to form a stable ionic bond.
Sodium would most likely form an ionic bond with chlorine to form sodium chloride (table salt). Sodium easily loses an electron to achieve a stable electron configuration, while chlorine easily gains an electron to achieve a stable electron configuration.
Metals - especailly alkali and alkaline earths, and halogens.
If you meant to say "elements ARE most likely to bond with," which is probably what you meant, then the answer would be 7A(or 17), also called the Halogens. "Halogen" actually means "salt-forming." When you take a chlorine (7A) and sodium (1A), you end up with table salt! ---- In a nutshell, the answer is Group 7A, or 17.