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Fundamentals of Chemistry I
University of Victoria
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Neil Burford

Neil Burford

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CHEM 101 Lecture 1: CHEM 101-Lecture 1-Course Information

Cornelia bohne: monday 4:30 to 5:30 pm, and tuesday 1:30 to 2:30 pm. Neil burford: wednesday 4:30 to 5:30 pm, and thursday 12:00 to 1:00 pm. In-lecture

CHEM 101 Lecture Notes - Lecture 2: Electromagnetic Radiation, Sunburn, Transverse Wave

Alpha particles were directed at an extremely thin piece of gold foil surrounded by a fluorescent screen. Most particles passed straight through the go

CHEM 101 Lecture Notes - Lecture 3: Rydberg Formula, Rydberg Constant, Emission Spectrum

CHEM 101 Lecture Notes - Lecture 4: Heinrich Hertz, Photon

CHEM 101 Lecture Notes - Lecture 5: George Paget Thomson, Louis De Broglie, Uncertainty Principle

* louis de broglie proposed that, just as light can have particle-like properties, matter can have wave-like properties. * any particle that has a velo

CHEM 101 Lecture Notes - Lecture 6: Max Born

In the early 20th century, many new scientific discoveries were made that advanced quantum mechanics and changed people"s understanding of the atom. Th

CHEM 101 Lecture Notes - Lecture 7: Magnetic Quantum Number

An orbital is a volume in space in which an electron can be located. Orbitals are based on probability; an orbital is the region where is is most likel

CHEM 101 Lecture Notes - Lecture 8: Magnetic Quantum Number, Photographic Plate

Orbitals represent the region with the greatest probability of finding an electron. The center of the orbital has a higher electron density than the ed

CHEM 101 Lecture Notes - Lecture 9: Electron Configuration, Aufbau Principle, Pauli Exclusion Principle

The way in which electrons are arranged within an atom"s orbitals. The most stable, or lowest energy, configuration is called the ground state. To dete

CHEM 101 Lecture Notes - Lecture 10: Alkali Metal, Electron Configuration, Periodic Table

Columns are called groups , while rows are called periods. The order that the orbitals are filled in any atom, according to the aufbau principle, is: 1

CHEM 101 Lecture Notes - Lecture 11: Electron Configuration, Isoelectronicity, Transition Metal

Ions are atoms which have lost or gained electrons. Atoms which have lost electrons are called cations , and are positively charged. Atoms which have g

CHEM 101 Lecture Notes - Lecture 12: Diamagnetism, Valence Electron, Paramagnetism

Paramagnetic atoms/ions have unpaired electrons, and interact with a magnetic field. Diamagnetic atoms/ions have only paired electrons, and do not inte

CHEM 101 Lecture Notes - Lecture 13: Atomic Radius, Fluorine, Electron Configuration

Size increases moving down a group due to the increasing number of energy levels. Size decreases across a period because the nuclear charge increases a

CHEM 101 Lecture Notes - Lecture 14: Bond Length, Electronegativity, Chemical Polarity

Stated that main group elements (any element which is not a transition metal) tend to form compounds which give them eight valence electrons. Main grou

CHEM 101 Lecture Notes - Lecture 15: Effective Nuclear Charge, Valence Electron, Electron Affinity

Electron affinity is the energy released by an isolated, gaseous atom or ion when it gains one electron. Measured as a negative energy value (joules) E

CHEM 101 Lecture Notes - Lecture 16: Sulfur Hexafluoride, Lewis Structure, Formal Charge

Elements which are in the third row or higher of the periodic table can expand their octet and form bonds with more than four other atoms. This is due

CHEM 101 Lecture Notes - Lecture 17: Molecular Orbital Theory, Vsepr Theory, Lewis Structure

Valence shell electron pair repulsion (vsepr) theory. Uses the lewis structure of the molecule to determine the 3 dimensional shape. Explains molecular

CHEM 101 Lecture Notes - Lecture 18: Trigonal Planar Molecular Geometry, Steric Number, Vsepr Theory

According to vsepr theory, there are fundamental shapes. Of two to six (two to six for molecules with a steric number electron domains around the centr

CHEM 101 Lecture Notes - Lecture 19: Lone Pair, Steric Number, Lewis Structure

See-saw molecules (one lone pair, four bonds) Lone pair is always found at an equatorial position (not an axial position), in order to reduce electron

CHEM 101 Lecture Notes - Lecture 20: Lewis Structure, Lone Pair, Trigonal Bipyramidal Molecular Geometry

Chem 101-lecture 20-review of molecular geometries and lewis structures. Includes lone pairs, single bonds, and multiple bonds. Can include unpaired lo

CHEM 101 Lecture Notes - Lecture 21: Dipole, Bond Dipole Moment, Chemical Polarity

Electronegativity is the ability of an atom to attract electrons to itself. Electronegativity increases moving right across a period. There are more pr

CHEM 101 Lecture Notes - Lecture 22: Pauli Exclusion Principle, Valence Electron, Vsepr Theory

Aufbau principle: fill orbitals in order of increasing energy. Exact order can be determined from the periodic table: 1s, 2s, 2p, 3s, 3p, 4s, 3d, Pauli

CHEM 101 Lecture Notes - Lecture 23: Trigonal Planar Molecular Geometry, Orbital Hybridisation, Sigma Bond

Formed on the internuclear axis between the two bonding atoms. Can form between s-orbitals, hybrid orbitals, or p-orbitals which overlap only on one si

CHEM 101 Lecture Notes - Lecture 24: Bond-Dissociation Energy, Trigonal Bipyramidal Molecular Geometry, Endothermic Process

The energy lost or gained in any chemical reaction. If h reaction is negative, energy was released (exothermic reaction) If h reaction is positive, ene

CHEM 101 Lecture Notes - Lecture 25: Molecular Orbital Theory, Orbital Hybridisation, Atomic Orbital

Molecular orbital theory can be used to explain aspects of bonding that are not explained by lewis structures, vsepr theory, or hybrid orbital theory,

CHEM 101 Lecture Notes - Lecture 26: Molecular Orbital Theory, Principal Quantum Number, Atomic Orbital

CHEM 101 Lecture Notes - Lecture 27: Lewis Structure, Nylon, Butane

Organic chemistry is the study of carbon-containing compounds. Hydrocarbons: only contain carbon and hydrogen atoms. Alcohols and ethers: contain a car

CHEM 101 Lecture 28: CHEM 101-Lecture 28-Types of Hydrocarbons

Base name is the prefix for the number of carbons in the carbon chain, with the suffix. The first and last carbon atoms of the carbon chain join to for

CHEM 101 Lecture Notes - Lecture 29: Carbon Group, Substituent, Propionaldehyde

: contain an oxygen atom with two single bonds. Oxygen atom is single-bonded to one carbon atom and one hydrogen atom, creating a hydroxyl group. The c

CHEM 101 Lecture Notes - Lecture 32: Alkyne, Alkene, Covalent Bond

Since c-h bonds are nonpolar, hydrocarbons are nonpolar molecules. Name is the base name for the number of carbon atoms, with the suffix -ane. Called s

CHEM 101 Lecture Notes - Lecture 33: Structural Formula, Stereoisomerism, Substituent

A chiral molecule other and cannot be superimposed. Is any molecule which has two forms that are mirror images of each. Molecule with carbon centres at

CHEM 101 Lecture Notes - Lecture 34: Cannabinoid Receptor, Tetrahydrocannabinol, Medicinal Chemistry

CHEM 101 Lecture Notes - Lecture 35: London Dispersion Force, Intermolecular Force, Chemical Polarity

The state of a substance is dependant on two factors: the kinetic energy of the molecules, which separates molecules, the intermolecular forces, which

CHEM 101 Lecture Notes - Lecture 36: Intermolecular Force, Ionic Bonding, Hydrogen Bond

Between a metal cation (positive) and a nonmetal anion (negative) The atoms must have an electronegativity difference greater than 2. Ex: bond between

CHEM 101 Lecture Notes - Lecture 37: Intermolecular Force, Boiling Point, Surface Tension

In a liquid, molecules are close together, but are able to move past each other. The kinetic energy separating the particles is approximately equal to

CHEM 101 Lecture Notes - Lecture 38: Metal, Intermolecular Force, Network Covalent Bonding

Matter is in a solid state when its particles are in a fixed position and cannot move past one another. Solids can be amorphous (particles arranged ran

CHEM 101 Lecture Notes - Lecture 39: Antibonding Molecular Orbital

CHEM 101 Lecture Notes - Lecture 40: Polyvinyl Chloride, Chain-Growth Polymerization, Polystyrene

Are molecules that are formed from repeating subunits ( monomers . Generally, they are long chains with a high molecular mass. Some examples of polymer