Molecular and Ionic Bonding

Three pi bonds

One pi bond

Two pi bonds

No pi bonds

VESPR

Lewis's Law

Pauli Exclusion Principle

Hund's Law

Four electron groups (two bonding pairs, two lone pairs)

Two electron groups (two bonding pairs)

Three electron groups (two bonding pairs, one lone pair)

Five electron groups (two bonding pairs, three lone pairs)

Does an increase in covalent character lead to higher electrical conductivity in metalloid compounds compared to their non-metal counterparts?

What is the correlation between atomic radius size differences and potential energy within a set of binary compounds?

How do variations in electron domain geometries affect dipole moments across a series of heteronuclear diatomic molecules with differing electronegativities?

Can we associate changes in ionization energy with alterations in metallic character down a group on the periodic table for diatomic species?

Bent

Tetrahedral

Trigonal planar

Linear

NOCl, as it has a permanent dipole but less capacity for hydrogen bonding compared to acetic acid

Carbon monoxide, although it contains a triple-bonded oxygen atom, does not readily participate in substantial dipole-dipole interactions with water due to overall nonpolarity

NH4Cl, despite being highly soluble due primarily to strong coulombic attractions rather than extensive hydrogen bond networks

Acetic acid (CH3COOH), due to both hydroxyl and carbonyl groups that enable it to form multiple hydrogen bonds with water

sp^2 hybridized orbitals

sp^3d hybridized orbitals

sp hybridized orbitals

sp^3 hybridized orbitals

Trigonal planar

Bent or angular

Tetrahedral

Bent

Trigonal Pyramidal

Linear

Trigonal Planar

There is no effect on equilibrium since temperature remains constant.

The rate constants for both forward and reverse reactions decrease proportionally.

The equilibrium shifts toward products, resulting in decreased total gas volume.

The equilibrium shifts toward reactants to increase pressure according to Le Chatelier's principle.