Sodium Acetate and Ionic Bonds

This video tutorial explains how to write the Lewis structure for sodium acetate (CH3COONa). It begins by discussing the ionic nature of sodium acetate, highlighting the positive charge of the sodium ion and the negative charge of the acetate ion. The tutorial explains how these charges lead to the formation of an ionic bond. It also covers the structure of the acetate ion, a polyatomic ion, and provides guidance on drawing the Lewis structure for sodium acetate, emphasizing the importance of charge attraction in forming ionic bonds.

What is unusual about the chemical formula of sodium acetate?

• It contains no metal.

• The nonmetals are listed first.

• The metal is placed at the end.

• It has more than one metal.

What charge does sodium typically have in ionic compounds?

• Negative two

• Positive one

• Positive two

• Negative one

Where can you find information about the acetate ion?

• On the periodic table

• In a table of common polyatomic ions

• In a list of metals

• In a list of noble gases

What is the chemical formula for the acetate ion?

• CH3COOH

• C2H4O2

• C2H3O2-

• CH3COO-

What is the overall charge of the acetate ion?

• Negative

• Neutral

• Positive

• Variable

What type of bond is formed between sodium and the acetate ion?

• Ionic bond

• Covalent bond

• Hydrogen bond

• Metallic bond

What is the main type of bond within the acetate ion?

• Metallic bond

• Covalent bond

• Ionic bond

• Hydrogen bond

Why do we put brackets around the acetate ion in the Lewis structure?

• To denote it is a single atom

• To highlight its positive charge

• To show it is a metal

• To indicate it is a polyatomic ion

What happens to sodium when it forms an ionic bond with acetate?

• It remains neutral

• It shares an electron

• It loses an electron

• It gains an electron

What is the significance of the positive and negative charges in sodium acetate?

• They repel each other

• They form a covalent bond

• They attract each other to form an ionic bond

• They have no effect