Question

question: how are ionic compounds formed? 1. observe: look at the purple lithium atom and the red oxygen atom. recall that most atoms are stable when their outermost ring has eight electrons. some atoms, such as lithium and beryllium, are stable when their outermost ring has two electrons. a. how many electrons will the lithium atom give up to become stable? b. how many electrons does the oxygen atom need to become stable? c. can a stable compound be made from these two atoms? explain why or why not. 2. form bonds: click add metal to add another lithium atom, and then transfer electrons from the lithium to the oxygen. click check. a. did you make a stable compound? b. turn on show formula. what is the formula of this compound? c. turn on show charge. what is the charge of each ion? li li o

Explanation:

Step1: Determine lithium's electron - giving number

Lithium has 3 electrons with 1 in outer shell. It gives 1 electron to be stable.

Step2: Determine oxygen's needed electrons

Oxygen has 6 outer - shell electrons and needs 2 more to have 8 in outer shell for stability.

Step3: Analyze compound formation possibility

One lithium gives 1 electron but oxygen needs 2. So one lithium can't form a stable compound. Two lithiums are needed.

Step4: Check compound stability after adding two lithiums

Two lithiums each giving 1 electron to oxygen makes oxygen have 8 outer - shell electrons and lithiums have full outer shells (2 for lithium). A stable compound is formed.

Step5: Determine compound formula

Two lithium (Li) and one oxygen (O) form $Li_2O$.

Step6: Determine ion charges

Lithium loses 1 electron, so $Li^+$; oxygen gains 2 electrons, so $O^{2 - }$.

Answer:

1. A. 1

B. 2
C. No, because oxygen needs 2 electrons and one lithium can only give 1.

1. A. Yes

B. $Li_2O$
C. $Li^+$, $Li^+$, $O^{2 - }$