Chemistry: Chemical Bonding

What type of bond involves the electrostatic attraction between oppositely charged ions formed by the complete transfer of electrons?

This describes an ionic bond, typically formed between a metal and a nonmetal, where one atom donates electrons and another accepts them.

What type of bond forms when two atoms share one or more pairs of electrons?

This is a covalent bond, which occurs predominantly between nonmetal atoms to achieve stable electron configurations.

Define electronegativity and state its general trend across a period in the periodic table.

Electronegativity is an atom's ability to attract electrons in a chemical bond. It generally increases from left to right across a period.

How does the difference in electronegativity between two bonded atoms determine if a bond is nonpolar covalent, polar covalent, or ionic?

A small difference (0-0.4) indicates nonpolar covalent, a moderate difference (0.4-1.7) indicates polar covalent, and a large difference (>1.7) indicates an ionic bond.

What is the Octet Rule and why is it important in chemical bonding?

The Octet Rule states that atoms tend to gain, lose, or share electrons to achieve eight valence electrons. This stability is the driving force behind most chemical bonding.

What is the main purpose of drawing a Lewis structure?

A Lewis structure is a diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule, helping to visualize valence electron distribution.

According to VSEPR theory, what determines the molecular geometry of a molecule?

VSEPR theory states that electron domains (bonding and non-bonding pairs) around a central atom will orient themselves as far apart as possible to minimize repulsion, thus determining the molecular geometry.

What is the molecular geometry and approximate bond angle for a molecule with three bonding domains and zero lone pairs around its central atom?

This describes a trigonal planar geometry with bond angles of approximately 120 degrees, as seen in molecules like BF3.

What is atomic orbital hybridization?

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds, often leading to stronger bonds and specific geometries.

Differentiate between a sigma (σ) bond and a pi (π) bond.

A sigma bond is formed by the direct, head-on overlap of atomic orbitals along the internuclear axis, while a pi bond is formed by the sideways overlap of p orbitals above and below the internuclear axis.

What are intermolecular forces (IMFs) and how do they differ from intramolecular bonds?

IMFs are attractive forces between molecules, while intramolecular bonds are the forces holding atoms together within a molecule. IMFs are generally much weaker than intramolecular bonds.

Describe hydrogen bonding and provide an example of a molecule that exhibits it.

Hydrogen bonding is a strong type of dipole-dipole interaction occurring when hydrogen is covalently bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine. Water (H2O) is a classic example.

List two general physical properties characteristic of ionic compounds.

Ionic compounds typically have high melting points and boiling points, are brittle, and conduct electricity when molten or dissolved in water.

List two general physical properties characteristic of simple molecular covalent compounds.

Simple molecular covalent compounds generally have low melting points and boiling points, and are poor conductors of electricity.

What is a metallic bond?

A metallic bond is the electrostatic attraction between a lattice of positive metal ions and a 'sea' of delocalized valence electrons, which accounts for properties like high conductivity and malleability.