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Lecture

Chemical Bonding: Lewis Structures and Molecular Shapes

In course

CH-160(en): Advanced general chemistry (english)

This course aims to teach essential notions of the structure of matter, chemical equilibria and reactivity. Classes and exercises provide the means to analyze and solve, by reasoning and calculation, novel problems of geeneral chemistry. ...

Description

This lecture covers the fundamentals of chemical bonding, including energy, bond types, Lewis structures, and exceptions to the octet rule. It also explores molecular shapes using the VSEPR theory, the effect of lone pairs on bond angles, and the polarity of molecules.

Instructors (2)

Thomas Rizzo

EDUCATION Ph.D., Chemistry, University of Wisconsin, Madison, 1983 B.S., Chemistry, cum laude, Rensselaer Polytechnic Institute, 1978 ACADEMIC AND ADMINISTRATIVE POSITIONS Dean, Faculty of Basic Sciences, EPFL, 2004-present Head, Department of Chemistry, EPFL, 1997-2004 Professor of Chemistry, EPFL, 1994-present Professor of Chemistry, University of Rochester, 1993-1994 Assistant Professor of Chemistry, University of Rochester, 1986-1992 Research Associate, The James Franck Institute, University of Chicago, 1984-1986

Samuel Terrettaz

Official source

Ontological neighbourhood

Chemistry

Inorganic chemistry: Coordination chemistry

Related concepts (32)

Chemical bond

A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures. The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds, or through the sharing of electrons as in covalent bonds. The strength of chemical bonds varies considerably; there are "strong bonds" or "primary bonds" such as covalent, ionic and metallic bonds, and "weak bonds" or "secondary bonds" such as dipole–dipole interactions, the London dispersion force, and hydrogen bonding.

VSEPR theory

Valence shell electron pair repulsion (VSEPR) theory (ˈvɛspər,_vəˈsɛpər , ), is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. It is also named the Gillespie-Nyholm theory after its two main developers, Ronald Gillespie and Ronald Nyholm. The premise of VSEPR is that the valence electron pairs surrounding an atom tend to repel each other. The greater the repulsion, the higher in energy (less stable) the molecule is.

Ionic bonding

Ionic bonding is a type of chemical bonding that involves the electrostatic attraction between oppositely charged ions, or between two atoms with sharply different electronegativities, and is the primary interaction occurring in ionic compounds. It is one of the main types of bonding, along with covalent bonding and metallic bonding. Ions are atoms (or groups of atoms) with an electrostatic charge. Atoms that gain electrons make negatively charged ions (called anions). Atoms that lose electrons make positively charged ions (called cations).

Electron counting

In chemistry, electron counting is a formalism for assigning a number of valence electrons to individual atoms in a molecule. It is used for classifying compounds and for explaining or predicting their electronic structure and bonding. Many rules in chemistry rely on electron-counting: Octet rule is used with Lewis structures for main group elements, especially the lighter ones such as carbon, nitrogen, and oxygen, 18-electron rule in inorganic chemistry and organometallic chemistry of transition metals, Hückel's rule for the π-electrons of aromatic compounds, Polyhedral skeletal electron pair theory for polyhedral cluster compounds, including transition metals and main group elements and mixtures thereof, such as boranes.

Bond energy

In chemistry, bond energy (BE), also called the mean bond enthalpy or average bond enthalpy is a measure of bond strength in a chemical bond. IUPAC defines bond energy as the average value of the gas-phase bond-dissociation energy (usually at a temperature of 298.15 K) for all bonds of the same type within the same chemical species. The bond dissociation energy (enthalpy) is also referred to as bond disruption energy, bond energy, bond strength, or binding energy (abbreviation: BDE, BE, or D).

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Chemical Bonds: Types and Properties

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Chemical Bonding: Lewis Structures

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Chemical Bonding: Lewis Structures and Molecular Geometries

Explores chemical bonding through Lewis structures, molecular geometries, and dipole moments.

Chemical Bonding Fundamentals

Introduces the fundamentals of chemical bonding, covering types of bonds, Lewis representation, VSEPR theory, and molecular geometry.

Chemical Bonding: Lewis Theory