Bonding & Lewis Structures Lecture

These flashcards cover key concepts from the Bonding & Lewis Structures lecture, focusing on the Octet Rule, types of bonds, Electronegativity, Lattice Energy, Lewis Structures, and Resonance.

What is the Octet Rule?

When atoms form a compound, they will gain, lose, or share electrons to obtain a noble gas electron configuration.

How many valence electrons do most noble gases have?

Most noble gases have 8 valence electrons, except Helium, which has 2.

What do Electron Dot Symbols represent?

Electron Dot Symbols represent the valence electrons of an atom.

What is Electronegativity?

Electronegativity is an atom's ability to attract electrons in a bond.

What determines the bond type between two atoms?

The difference in Electronegativity (∆EN) between the two bonded atoms determines the bond type.

What is the Lattice Energy?

Lattice energy is the energy released when gas ions combine to form a solid lattice.

What happens to lattice energy as the charge increases?

As charge increases, lattice energy increases.

What are the properties of Ionic Solids?

Ionic solids are hard, brittle, and do not dent or bend easily.

What is the difference between Nonpolar and Polar Covalent Bonds?

Nonpolar covalent bonds involve equal sharing of electrons, while polar covalent bonds involve unequal sharing.

What is Resonance in chemistry?

Resonance is the ability to draw multiple valid Lewis structures for a molecule, where electrons can be redistributed.

What is the purpose of calculating Formal Charge in Lewis structures?

Formal charge helps to determine the most stable Lewis structure by showing the distribution of charge among atoms.

What are the steps to drawing Lewis Structures?

1. Calculate total valence electrons. 2. Identify the central atom. 3. Connect outer atoms using single bonds. 4. Fill octets for outer atoms, then central atom. 5. Calculate formal charges.

How do you identify the best resonance structure?

The best resonance structure has the smallest formal charges and places negative charges on the most electronegative atoms.

In which direction do dipoles point?

Dipoles point towards the more electronegative atom in a polar bond.

What is a common misconception about resonance structures?

Resonance structures do not mean that the molecule switches between forms; instead, the true structure is a hybrid of all possible resonance forms.

What happens to bond strength as the number of shared electrons increases?

More electrons in a bond result in stronger bonds.

What is the overall goal of drawing a Lewis Structure?

To represent the bonding between atoms, showing lone pairs and shared electrons, resulting in the most stable configuration.

An atom has 6 valence electrons. To achieve a stable octet, it will most likely…

…gain 2 electrons.

If the electronegativity difference (∆EN) between two atoms is between 0.4 and 1.7, what type of bond is generally formed?

A Polar Covalent Bond.

In the Lewis structure for CO_2, which atom is generally considered the central atom?

Carbon (C), because it is less electronegative than Oxygen and can form more bonds.

Why is it important to consider resonance when describing the bonding