Chapter 3: Chemical Bonding - Chemistry 11

Flashcards about chemical bonding, covering definitions, Lewis diagrams, types of bonds, electronegativity, types of formulas, VSEPR model, bond dipole, intermolecular forces, and types of crystals.

Bonding Capacity

The maximum amount of bonds an atom can make with another atom.

Lewis Diagram

A model that represents the valence electrons of an atom.

Valence Electrons

Electrons on the final layer of an atom.

Covalent Bonds

Chemical bonds between a nonmetal and a nonmetal where electrons are shared.

Ionic Bonds

Chemical bonds between a metal and a nonmetal where electrons are transferred.

Characteristics of Covalent Bonds

Having definite and predictable shapes, being very strong, and having low melting and boiling points.

Characteristics of Metallic Bonds

Being good conductors of heat and electricity, being a strong solid, ductile, and having luster.

Characteristics of Ionic Bonds

Being a crystalline solid, having high melting and boiling points, conducting electricity in molten or solution state, and having extreme polar bonds.

Electronegativity

The measure of attraction an atom has to share with another electron.

Covalent Bond (based on Electronegativity)

Electronegativity difference is less than 0.5.

Polar Covalent (based on Electronegativity)

Electronegativity difference is from 0.5 to 1.9.

Ionic Bond (based on Electronegativity)

Electronegativity difference is above 1.9

Empirical Formula

Shows the whole number ratio of the atoms in the compound.

Molecular Formula

Shows the true amount of atoms in the compound.

Lewis Formula

Uses element symbols and valence electrons to show covalent bonds.

Structural Formula

Uses element symbols and lines to show the number of covalent bonds.

Stereochemical Formula

Similar to structural but presents it in 3D, adding wedges and dotted lines.

VSEPR Model

A model used to predict the shape of a molecule based on the repulsion of paired valence electrons.

Bond Dipole (Bond Polarity)

Occurs when the electronegativity difference of two bonded electrons move the electrons, creating a partially positive and partially negative side.

Intermolecular Forces

Forces between other molecules.

Intramolecular Forces

Forces within the molecule.

Van der Waals Forces (London Forces)

A force where electron movements temporarily shift the electron density, causing a weak attraction (the only force nonpolar molecules feel).

Dipole-Dipole Interactions

A force that affects polar molecules where the opposite charged ends of each other attract.

Hydrogen Bonding

The force that hydrogen with a very electronegative atom (O, F, N) will feel as an attraction.

Cohesion

The intermolecular attraction between like molecules.

Adhesion

The attraction between unlike molecules.

Surface Tension

The amount of energy needed to spread out and create a larger surface area.

Viscosity

Measure of fluid resistance when flowing; increases with intermolecular force.

Ionic Crystals

Lattice points occupied by cations and anions, held together by electrostatic forces, hard and brittle with high melting points, poor conductors of heat and electricity.

Molecular Crystals

Lattice points occupied by molecules, held together by intermolecular forces, soft and low melting points, poor conductors of heat and electricity.

Covalent Crystals

Lattice points occupied by atoms, held together by covalent bonds, hard and high melting points, poor conductors of electricity and heat.

Metallic Crystals

Lattice points occupied by metal atoms, held together by metallic bonds, can be soft to hard and have low to high melting points, good conductors of heat and electricity.