Ionic compund question

Top two are ionic (made up of a metal and non-metal), last one is molecular (two non-metals).

Hope that's a good start to your question!

Okay, lets start with some definitions:

An IONIC COMPOUND: Consist of a NONMETAL (right side and in the middle of the periodic table) and a METAL(left side of the periodic table). More specifically an ionic compounds consist of 2 ions (cation =+ charge and an anion=- charge) with a net charge of 0.

Examples: NaCl, AgCl, MgO...

A molecular compound: consist of two nonmetals (on the right side of the periodic table) and does not necessarily have a net charge of 0

Examples: CH(4), C2H6 (the numbers are underscript)

Alright here we go.

a) Ca is on the left(metal) Br is on the right(nonmetal) so from my definition above it is an Ionic Compound

B) Na is a metal and N is a nonmetal therefore it is an Ionic Compound

C) C is a nonmetal and H is also a nonmetal therefore it is a Molecular Compound

Ionic Character

Key:

White= No data

0-.66

.66-1

1-1.33

1.33-1.66

1.66-2

2-2.33

2.33-2.66

2.66-

Generally, ionic characters increase as you go right and upwards on a periodic table.

Ionic compounds form when there is an electronegativity difference between atoms greater than 2.5. Also, the simpler explanation is that generally (not exactly always), bonds between metals and non-metals are ionic. What happens is that the electron sharing is so unequal, that one atom (the less electronegative) somewhat just gives up its electrons completely to the other atom.

A) Ca2+ is a metal, and Br2 is a halogen (non-metal). Thus, ionic.
B) Na+ is metal, and N is a non-metal. Thus, ionic.
C) CH4; both atoms are non-metals. The EN of C is 2.5, and the EN of H is 2.2. There is not a significant electronegativity difference, thus it is not ionic.