Molecular and Ionic Bonding

It increases because there are more reactant molecules to collide with proper orientation.

It decreases due to an increase in activation energy required for the reaction.

It remains the same as rates are independent of concentrations at equilibrium.

It halves because doubling reactant concentration drives the equilibrium towards products.

Covalent network bonding

London dispersion forces

Hydrogen bonds

Dipole-dipole interactions

Hydrogen bonds

Ion-dipole forces

Dipole-dipole interactions

Dispersion forces

By decreasing overall enthalpy changes making processes less spontaneous

By increasing thermal motion which favors product formation at high temps

By reducing kinetic barrier heights irrelevant to thermodynamic spontaneity

By increasing entropy only relevant above certain temperatures thresholds

Hydrogen Bond

Ionic Bond

Covalen Bond

Metalic Bond

The ability to donate and accept protons facilitating solute-solvent interactions

The cohesiveness between water molecules reducing entropy changes upon dissolution

The dipole moment enhancing ion-dipole interactions with solutes

The molecular geometry providing maximal coverage around solutes

Linear

Tetrahedral

Bent

Trigonal planar

Greater differences in atomic radii

Greater differences in electron affinity

Greater differences in ionization energy

Greater differences in electronegativity

It reacts with water to produce hydrogen gas and chlorine gas.

It dissociates into sodium and chloride ions that conduct electricity.

It remains unchanged and the solution becomes acidic.

It forms covalent bonds between sodium and chloride atoms preventing conduction.

CO_2, a linear molecule where dipole moments cancel out resulting in no net dipole moment.

SO_2, a polar molecule with a bent shape causing a permanent dipole moment.

N_2, a nonpolar molecule with negligible dipole moments.

O_2, a nonpolar molecule with negligible dipole moments.