Understanding Lewis Theory and Bond Polarity

What is one of the main limitations of Lewis Theory when representing electrons in molecules like HCl?

• It ignores the presence of lone pairs.

• It cannot represent ionic bonds.

• It only applies to diatomic molecules.

• It assumes electrons are always shared equally.

What happens to HCl molecules when exposed to an electric field?

• Chlorine atoms are attracted to the positive plate.

• Hydrogen atoms are attracted to the positive plate.

• Chlorine atoms are attracted to the negative plate.

• They align randomly.

How can bond polarity be represented visually?

• By drawing a circle around the molecule.

• Using a double-headed arrow.

• With a lowercase delta and an arrow.

• Using a zigzag line.

What does electronegativity measure?

• The number of protons in an atom.

• The ability of an atom to attract electrons.

• The size of an atom.

• The mass of an atom.

Which element is the most electronegative among the halogens?

• Fluorine

• Iodine

• Bromine

• Chlorine

How does electronegativity change across a period in the periodic table?

• It fluctuates randomly.

• It increases.

• It remains constant.

• It decreases.

What type of bond is formed when two identical atoms share electrons?

• Pure covalent bond

• Polar covalent bond

• Ionic bond

• Metallic bond

What characterizes an ionic bond?

• A large electronegativity difference.

• A small electronegativity difference.

• Electrons are shared equally.

• It occurs between two non-metals.

Which type of bond is typically formed between metals and non-metals?

• Hydrogen bond

• Polar covalent bond

• Ionic bond

• Pure covalent bond

What determines the degree of polarity in a bond?

• The temperature of the environment.

• The difference in electronegativity between the atoms.

• The size of the atoms involved.

• The number of bonds formed.