CHEM 106 Learning Goals

Define Solution

any homogenous mixture composed of a solute dissolved in a solvent

How do intermolecular forces determine states of matter?

The stronger the forces of attraction, the more solid the form of matter.

What are dipole-dipole forces?

Attractions between polar molecules that have a dipole. Ex: H2O

What are dispersion forces?

These forces occur in every molecule, but are the only attraction in non-polar bonds. Ex: CH4

How are boiling points affected by IMF strength?

The greater the intermolecular forces, the greater the boiling point.

How does molecular surface area affect boiling point?

As surface area increases, the boiling point also increases. Ex: Straight chain molecules (n-pentane) have a greater boiling point than more rounded molecules (2,2 dimethyl propane)

What is hydrogen bonding?

Hydrogen bonding is an attraction between polar molecules that meet the requirements. Ex: H2O and NH3

What are the requirements for hydrogen bonding?

• Must have a hydrogen covalently bonded to an oxygen, nitrogen, or fluorine atom (highly electronegative)

• The Hydrogen must interact with another fluorine, nitrogen, or oxygen atom on a neighboring molecule

How does H-bonding affect physical properties?

Relate boiling point to vapor pressure

Relate boiling point to atmospheric pressure

Define 🔺Hvap

Calculate 🔺Hvap from the Clausius Clapeyron equation

Define solution

Any homogenous mixture composed of a solute dissolved in a solvent

Predict solubility from IMFs

What are colligative properties?

Raults Law (non volatile) equation

Raults Law (2 volatile) equation

A solute dissolved in a solvent ________ freezing point

lowers

A solute dissolved in a solvent _______ boiling point

raises

1st integrated rate law

2nd integrated rate law

How and why does temp affect reaction rate?

What is activation energy?

How does activation energy’s magnitude affect reaction rate?

What is a catalyst and how does it work?