Question

using the periodic table, predict whether the following chlorides are ionic or convalent: Kci,Nci3,ICI,Mgci2,Pci5,cci4​

Answer 1

Answer:

Ionic, covalent, covalent, ionic, covalent, covalent

Explanation:

In order to solve this problem, let's introduce the basic strategy:

• A compound that has a metal in it, would be ionic;
• A compound that only has nonmetals in it, would be covalent.

Since all compounds here are chloride, we only need to take a look at the other element which makes the substance.

• $KCl$: potassium belongs to group 1A, alkali metals, it's a metal, meaning we have a metallic chloride, this is ionic;
• $NCl_3$: nitrogen belongs to group 5A, there are only nonmetals present in the group, meaning we have a molecular covalent compound;
• $ICl$: iodine belongs to group 7A, halogens, they are all nonmetals, this implies we have a covalent compound;
• $MgCl_2$: magnesium belongs to group 2A, alkaline earth metals, it's a metal, meaning we have an ionic compound;
• $PCl_5$: phosphorus belongs to group 5A, just as nitrogen, it's a nonmetal, meaning we have a covalent compound;
• $CCl_4$: carbon belongs to group 4A, in this group, we have nonmetals, meaning we have a covalent compound.

To summarize, metals (groups 1A, 2A, all elements of group B) would produce ionic compounds, while not having them in your structures would imply that you have a covalent compound.