Chemical Bonding

Find the electronegativity difference between Br and Br.

0

Find the electronegativity difference between Mg and Br.

1.6

Find the electronegativity difference between Si and O.

1.7

Determine the bond angle for CBr4.

109.5∘

Determine the bond angle for BH3.

120∘

Determine the bond angle for H2CO.

120∘

Determine the bond angle for CS2.

180∘

Find the electronegativity difference between Al and F.

2.5

Determine the molecular geometry of each of the following molecules. CBr4 H2CO CS2 BH3

CBr4 = tetrahedral H2CO = trigonal planar CS2 = linear BH3 = trigonal planar

Classify each of the following molecules as polar or nonpolar. CH3Cl CH4 SO2 CS2

CH3Cl = polar CH4 = nonpolar SO2 = polar CS2 = nonpolar

Determine the molecular geometry of each of the following polyatomic ions. CO2−3 ClO−2 NO−3 NH+4

CO2−3 = trigonal planar ClO−2 = bent NO−3 = trigonal planar NH+4 = tetrahedral

Which Lewis structure below correctly represents the compound formed between magnesium and sulfur?

Mg+2 [: S..⋅⋅ :]−2

Draw the electron-dot formula for the element sulfur.

Sulfur belongs to group 16 of the periodic table, so it has six valence electrons.

Select the correct electron-dot formulas. You can refer to the periodic table if necessary. Check all that apply. B, Ca, Na, C, F, Ne

To draw the electron-dot formula, place the symbol of the atom at the center. The electrons are drawn in a clockwise manner starting on the right. The next electron is drawn underneath the symbol, and then on the left side. Finally, an electron is drawn above the symbol. Although this is generally the order in which electrons are drawn, it is not the absolute method.

Having eight valence electrons is very stable and is called an octet.

True

Classify the bond that occurs between Al and F.

ionic

Determine the number of lone pairs around the central atom for CH4.

n=0

Determine the number of lone pairs around the central atom for CS2.

n=0

Determine the number of lone pairs around the central atom for NF3.

n=1

Determine the number of bonding groups for CS2.

n=2

Determine the number of bonding groups for OF2.

n=2

Determine the number of lone pairs around the central atom for OF2.

n=2

Determine the number of bonding groups for NF3.

n=3

Determine the number of bonding groups for CH4.

n=4

For each polar molecule, choose the molecule and indicate the positive and negative ends of the dipole moment. F2

nonpolar

For each polar molecule, choose the molecule and indicate the positive and negative ends of the dipole moment. O2

nonpolar

Classify the bond that occurs between Mg and Br.

polar covalent

Classify the bond that occurs between Si and O.

polar covalent

Classify the bond that occurs between Br and Br.

pure covalent

For each polar molecule, choose the molecule and indicate the positive and negative ends of the dipole moment. HBr

δ+ δ− H−Br ⟶

For each polar molecule, choose the molecule and indicate the positive and negative ends of the dipole moment. CO

δ+ δ− C≡O ⟶