7C Lewis Diagrams and Bonding Concepts

These flashcards cover key concepts from Lewis Diagrams and bonding, including bonding types, the octet rule, and exceptions to common bonding rules.

Why do atoms form bonds?

Atoms form bonds to lower their potential energy by storing energy in the bond.

How do atoms lower their energy in ionic bonds?

Atoms lower their energy in ionic bonds by transferring electrons between metal and nonmetal.

What is the purpose of Lewis electron dot structures?

They visually represent how many valence electrons an atom has and how they can be shared in a bond.

What is the octet rule?

The octet rule states that atoms tend to gain, lose, or share electrons to have a full set of 8 valence electrons.

How do ionic bonds satisfy the octet rule? What about Covalent bonds?

Ionic bonds satisfy the octet rule by transferring electrons, while covalent bonds satisfy it by sharing electrons.

What are lone pairs?

Lone pairs are pairs of electrons that are not involved in bonding.

What are bonding pairs?

Bonding pairs are pairs of electrons that are shared between atoms to form a bond.

What is meant by bond order?

Bond order indicates how many pairs of electrons are being shared between two atoms.

Why can some elements be exceptions to the octet rule?

Some elements can be exceptions to the octet rule because they may have fewer than 8 electrons or can use d-orbitals to have expanded octets.

What is resonance?

Resonance is when multiple Lewis structures can represent the same molecule, showing how electrons are distributed.

What is the difference between a molecule and a formula unit?

A molecule is an individual particle while a formula unit is a ratio of ions in a larger crystal structure

Single, Double, and Triple Bonds each represent ___ electrical domain

1

NM + NM = ?

Covalent

M + NM = ?

Ionic