Element A loses one electron to form a unipositive cation A+. Element B gains two electrons to form a dipositive anion B2-. They combine through an ionic bond to form the compound A2B.
A particular element A has one electron in its third shell. There is another element B with six electrons in its second shell. (i) How many electrons does A tend to give or take to become stable? (ii) What kind of ion would it form? (iii) How many electrons does B tend to give or take to become stable? (iv) What kind of ion would it form? (v) If A and B were to combine, what kind of bond would be formed? (vi) What would be the formula for the compound thus formed?
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Element A has one valence electron, so it loses one electron to achieve an octet, forming a positive cation A+. Element B has six valence electrons and requires two electrons to complete its outer octet, forming a negative anion B2-. The transfer of electrons creates an ionic bond between them. Balancing their positive and negative charges gives the chemical formula A2B.
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