Lesson 4: Chemical Bonding and Diversity of Matter

7. Self-Check Assessment

Title

Draw a Lewis symbol for sulfur. Identify lone pairs and bonding e-

Draw Lewis symbols for all of the group 1 elements. How are these elements similar?

The group number provides information about the number of valence electrons. Elements in group 1(1A) all have one valence electron. 2 lone pairs and 2 bonding e-.

Now, draw Lewis symbols for 16A elements. What did you notice?

They all have 6 valence electrons.

Draw Lewis symbols and structural diagrams of the molecular chlorine and bromine.

SC 2. VSEPR and Polarity

Using the electronegativity, describe the bonds between Cl-Cl, P-Cl, and Na-Cl.

Classify and compare the strength of intramolecular and intermolecular bonds.

What can you tell about the bonding in SiO2(s) and Ni2O4?

SiO2: Elements that are non-metals favour covalent over ionic bond formation. The difference between their electronegativity high enough to create bonds dipole so the molecule is polar. Ni2O4: ionic compounds contain ions when difference between electronegativity relatively big. In nickel(1V) oxide, the electrons lost by the nickel in forming N4+ have been gained by the oxygen to form O2-.

Predict the polarity of the BF3, OF2 and CS2. Show a stereochemical formula and bond dipoles.