CHM $1020$ Lab

Week $4$ Assignment $a,b,$ and c

Atomic Structure, Chemical Bonding, Lewis Structure, and $3$D Molecular Shape

Objectives

In this lab, you will apply valence bond theory to draw appropriate Lewis structures, use electronegativity differences to classify bonds as ionic, polar covalent, or nonpolar covalent, and apply valence shell electron pair repulsion theory $($VSEPR$)$ to predict molecular geometry. We will also use molecular kits to create ball and stick models of molecules of interest to you.

Theory

Atoms of certain species tend to bond together. An atom is more stable if its valence shell $($electrons in its outermost energy level$)$ is similar to that of a Noble Gas $($typically eight electrons$),$ and this number is most often achieved when atoms combine. Notice that atoms of elements in the same group on the periodic table tend to have the same number of valence electrons; for example, halogens, Group $7$A elements $($Figure $1),$ have seven valence electrons.

$\backslash$table$[[,$Group $1$A$,$Group $2A,$Group $3A,$Group $4$A$,$Group $5A,$Group $6$A$,$Group $7A,$Group $8$A$],[$Period $1,*H,,,n,,,,$: $He$