Question

simple binary ionic compounds
please complete the following table:

name of ionic compound	formula of ionic compound
2. calcium chloride	cacl₂
3. magnesium sulfide	mgs
4. aluminum oxide	al₂o₃
5. lithium phosphide	li₃p
6. cesium nitride	cs₃n
7. potassium iodide	ki
8. barium fluoride	baf₂
9. rubidium nitride	rb₃n
10. barium oxide	bao
11.	k₂o
12.	mgi₂
13.	alcl₃
14.	cabr₂
15.	na₃n
16.	lif
17.	ba₃p₂
18.	cs₂s
19.	srf₂
20.	nacl

Explanation:

Step1: Recall ion - charge rules

For binary ionic compounds, we determine the formula based on the charges of the cation and anion to ensure the compound is neutral. For example, sodium ($Na^+$) has a + 1 charge and bromide ($Br^-$) has a - 1 charge, so the formula of sodium bromide is $NaBr$.

Step2: Identify cations and anions

For calcium chloride, calcium ($Ca^{2 + }$) has a + 2 charge and chloride ($Cl^-$) has a - 1 charge. To balance the charges, we need 2 chloride ions for each calcium ion, so the formula is $CaCl_2$.

Step3: Determine correct sub - scripts

For aluminum oxide, aluminum ($Al^{3+}$) has a + 3 charge and oxide ($O^{2 - }$) has a - 2 charge. The least - common multiple of 3 and 2 is 6. So we need 2 aluminum ions ($2\times3 = 6$) and 3 oxide ions ($3\times2=6$) to balance the charges, giving the formula $Al_2O_3$.
... (continue this process for all compounds)

Answer:

Name of Ionic Compound	Formula of Ionic Compound
2. Calcium chloride	$CaCl_2$
3. Magnesium sulfide	$MgS$
4. Aluminum oxide	$Al_2O_3$
5. Lithium phosphide	$Li_3P$
6. Cesium nitride	$Cs_3N$
7. Potassium iodide	$KI$
8. Barium fluoride	$BaF_2$
9. Rubidium nitride	$Rb_3N$
10. Barium oxide	$BaO$
11. Potassium oxide	$K_2O$
12. Magnesium iodide	$MgI_2$
13. Aluminum chloride	$AlCl_3$
14. Calcium bromide	$CaBr_2$
15. Sodium nitride	$Na_3N$
16. Lithium fluoride	$LiF$
17. Barium phosphide	$Ba_3P_2$
18. Cesium sulfide	$Cs_2S$
19. Strontium fluoride	$SrF_2$
20. Sodium chloride	$NaCl$