Final exam review

After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?

• Place dots until everything has eight
• Place dots only around the terminal atoms
• Add a multiple bond
• Have eight only around the central atom

In a Lewis structure, what do you do  with the total number of valence if your ion is 2- charged?

• Add 2 to the valence number
• Subtract 2 from the valence number
• Multiply the valence number by 2
• Divide the valence number by 2

Which of the following describes covalent bonds?

• Bonds form because of opposite charges
• Bonds form to fill outer electron shells
• Electrons are transferred between atoms
• Covalent bonds are magical

How many covalent bonds does carbon need to form in order to have a full octet?

• 2
• 3
• 4
• 5

According to the octet rule most elements need _______ valence electrons.

• 2
• 8
• 6
• 18

If electrons are shared unequally then the bond is....

• Non-polar covalent
• Ionic
• Non-polar ionic
• Polar covalent

Choose the correct shape for this molecule:

• Trigonal planar
• Trigonal pyramidal
• Bent
• Tetrahedral

According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?

• Pairs of valence electrons
• Inner shell electrons
• Mobile Electrons
• Electrons closest to the nucleus

What is the VSEPR theory used to predict?

• Bond Strength
• Polarity
• Molecular Shape
• Electronegativity

Who could this molecule be?

• CH₄
• CO₂
• PCl₅
• BF₃