If Na, K, Mg, and Ca formed an ion, what would the charge of the ion be? and what is the electron configuration? AND... Which of those elements is the largest and has the highest electronegativity?
2006-11-15 08:49:07 · 2 answers · asked by Tater Tott 1 in Science & Mathematics ➔ Chemistry
Na+ and K+ (both group 1)
Ca2+ and Mg2+ (both group 2).
Na+ and Mg2+ have the electron arrangement of neon, and the other two that of argon.
Ionic radius decreases from left to right, and increases top to bottom, so K+ is the largest of all these.
Electronegativity increases upwards and to the right of the Periodic Table, so Mg has the highest value of these four.
2006-11-15 08:54:48 · answer #1 · answered by Gervald F 7 · 1⤊ 0⤋
The charges of these elements end up equalling +4. I believe that calcium would be the biggest particle, seeing as it has the biggest atomic mass, and also because 20 protons and neutrons, and 20 electrons, configured 2, 8, 8, and 2. The big ion would have 8 full electron rings, with the last ring containing 4. This configuration would be 2,8,8,8,8,8,8,8,4. The potassium particle I think would have the highest electronegativity, because it has only one electron in its outer ring, and it is bigger than the sodium particle with only one electron in its outer ring.
2006-11-15 17:02:24 · answer #2 · answered by lordblair2002 1 · 0⤊ 0⤋