Lecture

Chemical Bonding

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In course

CH-244: Quantum chemistry

Introduction to Quantum Mechanics with examples related to chemistry ...

Description

This lecture covers the fundamentals of chemical bonding, including concepts such as atomic orbitals, bond order, and molecular structure. The instructor discusses the interaction between atoms and the formation of different types of bonds, such as covalent and ionic bonds.

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Instructor

Marcel Drabbels

Dr. Marcel Drabbels studied experimental physics at the University of Nijmegen (the Netherlands) and in 1993 obtained his Ph.D. at that same university. He then moved to the University of California at Santa Barbara where he studied the dynamics of highly vibrationally excited molecules and developed a new detection technique to investigate the photodissociation of molecules. When he returned to the Netherlands in 1996 he joined the FOM Institute for Atomic and Molecular Physics in Amsterdam where he worked on the development of new types of infrared imaging and streak cameras. In 1997 Dr. Drabbels was awarded a fellowship of the Royal Dutch Academy of Sciences and he moved to the Free University of Amsterdam where he studied the collision dynamics of molecules and initiated photodissociation experiments using ultrafast lasers. In October 1998 he was appointed as senior scientist at the EPFL where he studies the spectroscopy and dynamics of nanoscale systems. In March 2021 he was promoted to titular professor.

Official source

Ontological neighbourhood

Chemistry

Inorganic chemistry: Coordination chemistry

Related concepts (29)

Covalent bond

A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs. The stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding. For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration. In organic chemistry, covalent bonding is much more common than ionic bonding.

−1

In mathematics, −1 (negative one or minus one) is the additive inverse of 1, that is, the number that when added to 1 gives the additive identity element, 0. It is the negative integer greater than negative two (−2) and less than 0. Multiplying a number by −1 is equivalent to changing the sign of the number – that is, for any x we have (−1) ⋅ x = −x. This can be proved using the distributive law and the axiom that 1 is the multiplicative identity: x + (−1) ⋅ x = 1 ⋅ x + (−1) ⋅ x = (1 + (−1)) ⋅ x = 0 ⋅ x = 0.

25 (number)

25 (twenty-five) is the natural number following 24 and preceding 26. It is a square number, being 52 = 5 × 5, and hence the third non-unitary square prime of the form p2. It is one of two two-digit numbers whose square and higher powers of the number also ends in the same last two digits, e.g., 252 = 625; the other is 76. Twenty five has an even aliquot sum of 6, which is itself the first even and perfect number root of an aliquot sequence; not ending in (1 and 0).

5 (five) is a number, numeral and digit. It is the natural number, and cardinal number, following 4 and preceding 6, and is a prime number. It has garnered attention throughout history in part because distal extremities in humans typically contain five digits. The evolution of the modern Western digit for the numeral 5 cannot be traced back to the Indian system, as for the digits 1 to 4. The Kushana and Gupta empires in what is now India had among themselves several forms that bear no resemblance to the modern digit.

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).

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Organic Chemistry: Atomic Orbitals and Molecular Bonds

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Chemical Bonds: Types and Properties

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