Bronsted-Lowry and Lewis Acids

The lecture explores the interaction between atomic orbitals of Lewis acids and bases, defining Lewis acids as molecules with empty orbitals and Lewis bases as those with electron pairs. It illustrates the interaction using a methyl cation and hydride, explaining how their orbitals overlap to form bonds. The energy diagram of this interaction is discussed, highlighting the formation of bonding and anti-bonding molecular orbitals. The lecture also covers Bronsted-Lowry acids and bases, explaining how acid strength increases with s character due to electron proximity to the nucleus.

What is a characteristic feature of a Lewis acid?

• Contains a pair of nonbonding electrons

• Contains an empty atomic orbital

• Donates an H ion

• Accepts an H ion

Which of the following is an example of a Lewis base?

• Hydride ion

• Methyl cation

• Chloride ion

• Proton

What happens when a Lewis acid reacts with a Lewis base?

• Their atomic orbitals overlap to form a bond

• They form a gas

• They release energy

• They form a new element

In the energy diagram of Lewis acid-base interaction, why is the 1s orbital lower in energy than the 2p orbital?

• Because it is further from the nucleus

• Because it is closer to the nucleus

• Because it has more electrons

• Because it is larger in size

Which orbital interaction results in the formation of a bonding molecular orbital?

• 1s and 3p

• 2p and 2p

• 1s and 2p

• 1s and 1s

What defines a Bronsted-Lowry acid?

• A molecule with a filled orbital

• A molecule that accepts an H ion

• A molecule that donates an H ion

• A molecule with an empty orbital

How does the s-character affect the strength of a Bronsted-Lowry acid?

• Increases the acid's ability to donate electrons

• Decreases the acid's ability to donate electrons

• Increases the acid's ability to donate an H ion

• Decreases the acid's ability to donate an H ion

What is formed when a Bronsted-Lowry acid reacts?

• A new element

• A solid

• A conjugate base

• A gas

Why does increased s-character lead to a stronger acid?

• It decreases the size of the molecule

• It increases the size of the molecule

• It makes the conjugate base more stable

• It makes the conjugate base less stable

What happens to the energy level of an atom as an electron gets closer to the nucleus?

• The energy level fluctuates

• The energy level remains the same

• The energy level decreases

• The energy level increases