Chemical Bonding and Molecular Structure

Covalent Bonds

Created byVinay Arya

Last updated 3/2020

English

What you'll learn

Different types of Bonds

Course content

1 section • 14 lectures • 2h 36m total length

4.1. Introduction to Contents of Bonding11:49
Introduce the sequence and criteria for studying bonding and molecular structure, then explore covalent and ionic bonds, resonance, and hydrogen bonding to explain molecular stability.
4.2. Lewis Approach15:28
Explore Lewis approach to chemical bonding, using electron dot structures to show ionic transfer and covalent sharing. It covers the octet rule and the method's limitations for molecular geometry.
4.3. Covalent Bonds22:49
Explore covalent bonds formed by sharing electrons, including single, double, and triple bonds, with factors like ionization energy, nuclear attraction, electron affinity, electronic activity, and coordinate bonds.
4.4. Ionic Bonds14:03
Explore how ionic bonds form through electron transfer between metals and nonmetals, creating cations and anions that achieve octet stability in a crystal lattice, as in sodium chloride.
4.5. Resonance and rules for writing Structures9:08
Learn resonance and the rules for writing resonating structures, including rotations at 120 degrees producing different resonance structures, and understand resonance energy versus the actual molecule.
4.6. VSEPR Theory8:42
Use VSEPR theory to predict molecular geometry by considering lone pairs and bond pairs around a central atom, reducing repulsion to explain shapes like water, methane, and ammonia.
4.7. Sigma and pi bonds8:58
Explore sigma and pi bonds through head-to-head and sideways overlap, and learn how a double bond forms from one sigma and one pi bond.
4.8. Valence bond theory8:26
This lecture presents valence bond theory as a quantum model of bonding, highlighting valence electrons, orbital overlap, opposite-spin pairs, and the formation of covalent sigma bonds, exemplified by hydrogen.
4.9. Overlapping and types of overlapping6:56
Explore how orbital overlap forms covalent bonds, outlining sigma bonds from head-to-head overlap and pi bonds from sideways p-orbital overlap, with simple examples. Learn how overlap extent predicts bond strength.
4.10. Hybridization sp313:06
This lecture introduces sp3 hybridization, where one s and three p orbitals form four hybrid orbitals. It uses methane to show tetrahedral carbon geometry with about 109 degrees.
4.11. Hybridization sp2 ,sp , sp3d8:55
The lecture explains sp, sp2, sp3d hybridization and how mixing orbitals forms sigma bonds and determines molecular structure, guiding predictions of structures in various molecules.
4.12. Hybridization sp3d2, sp3d35:40
Investigate sp3d2 and sp3d3 hybridization, detailing how electrons shift from ground to excited states to form new hybrid orbitals and influence molecular structure.
4.13. Molecular Orbital Theory15:04
Learn how molecular orbital theory describes bonding and antibonding orbitals formed from atomic orbitals; energy depends on overlap, with bonding orbitals lower in energy and guiding bond formation.
4.14. Hydrogen Bonding and its types7:12
Discover hydrogen bonding as an electrostatic attraction between a hydrogen attached to a highly electronegative atom and a lone-pair atom, including intermolecular and intramolecular forms, seen in water and ammonia.
Innovation

Requirements

Basics of Bonding

Description

Chemical bond: In a molecule, different atoms are held together by a force of attraction called chemical bond.

When two atoms come closer, the electrons of one atom come under the influence of the electrons and the nucleus of the other atom. The interaction might produce an attraction between the two atoms.

Types of Chemical Bonds. Atoms combine in order to complete their respective octets mainly in two ways:

(i)By complete transfer of electrons. The chemical bond so formed is known as electrovalent bond or ionic bond.

(ii) By sharing of electrons. There are two types of such bonds:

(a)covalent bond - shared electrons are contributed equally by both the combining atoms.

(b) coordinate or dative bond - shared electrons are contributed only by one of the atoms.

Lewis symbols or electron dot symbols. According to this shorthand notation, the symbol of an element stands for the nucleus as well as the electrons in the inner energy shells. Each of the electrons in the outermost shell is represented by a dot near the symbol of the element. In case of ions, the ionic charge is also shown along with the symbol. The Lewis Structures of molecules are made by a combination of Lewis symbols of atoms or ions in accordance with the mode of formation of bonds.

Who this course is for:

Beginners, 11 grade students and research Scholars