ENLACE COVALENTE COORDINADO O ENLACE DATIVO

Welcome and Introduction to Chemical Bonding

In this section, the instructor introduces the topic of chemical bonding, specifically focusing on the octet rule, ionic bonds, and covalent bonds.

Understanding the Octet Rule

• Atoms bond to fulfill the octet rule by completing their valence shell with 8 electrons for stability.

• The number of valence electrons an atom has determines its ability to form bonds.

• Elements with one or two valence electrons tend to lose them in ionic bonding due to difficulty reaching an octet.

Exploring Ionic Bonds

• Ionic bonds occur when atoms transfer electrons to achieve a full outer shell.

• Oppositely charged ions attract each other in an ionic bond, leading to electron transfer for stability.

Covalent Bonds and Coordinate Covalent Bonding

This section delves into covalent bonding, where atoms share electrons, and introduces coordinate covalent bonding where one atom contributes both shared electrons.

Covalent Bond Formation

• Atoms share electrons in covalent bonds when neither can donate or accept electrons outright.

• Shared pairs of electrons are represented by a line between bonded atoms in a covalent bond.

Coordinate Covalent Bonding

• In coordinate covalent bonding, one atom provides both shared electrons to fulfill the octet rule of both atoms involved.

Chemical Bonding Examples

In this section, various examples of chemical bonding are discussed, including covalent bonds and coordinated covalent bonds.

Chemical Bonding Examples

• Covalent bond representation using an arrow to show that argon lent electrons to oxygen for octet rule fulfillment. This is an active or coordinated covalent bond.

• Illustration of ammonia molecule where nitrogen shares its lone pair with oxygen to satisfy the octet rule. Oxygen gains two electrons from nitrogen, completing its octet.

• Explanation of a scenario involving oxygen and sulfur atoms lacking two electrons each to fulfill the octet rule. Both atoms share two electrons each, resulting in both achieving an octet configuration through mutual electron sharing.

Coordinated Covalent Bonds: Monoxide Sulfur Molecule

The concept of coordinated covalent bonds is further explored through the example of a sulfur monoxide molecule.

Coordinated Covalent Bonds: Monoxide Sulfur Molecule

• Introduction to the molecule monoxide sulfur where all atoms have satisfied the octet rule, leading to a discussion on coordinated covalent bonds.