CHM 4411: Physical Chemistry

In this video, we demonstrate the creation of Lewis structures for methane, carbon dioxide, hydrogen selenide, and ammonia, highlighting the arrangement of atoms and bonds in each molecule. The video emphasizes the importance of Lewis structures in visualizing atomic bonding and the presence of lone electron pairs.

Discover the distinct geometries of molecules like N?O, SO?, H?S, and PF?. Unravel the difference between molecular and electron shapes. Master the basics of linear, bent, tetrahedral, and trigonal pyramidal structures.

Examine the nature of bonds in methylamine, ethane, fluoromethane, and methanol. Identify ethane's nonpolar covalent bond and understand why fluoromethane's bond leans toward the ionic spectrum. Grasp essential concepts in molecular bonding with this deep analysis.

Explore how to calculate the theoretical yield of TiCl? in moles based on different initial quantities of reactants in the chemical equation Ti + 2 Cl? ? TiCl?.

Master metric unit conversions with step-by-step examples, including cm to meters, g to kilograms, cm to millimeters, and mL to liters.

Unravel the electron configurations of diverse ions and discern their noble gas resemblances. Understand how atoms and ions strive for full outer electron shells for ultimate stability.