Chemistry Exam 3 (CH.12)

States of matter in terms of K.E & P.E

Name different changes of state and identify nature of enthalpty

Understand heating/cooling curves

/ = temp is increasing on a single phase

- = phase change is occurring

• adding heat increases K.E (on diagonal lines)

• adding heat increase P.E (on horizontal lines)

Define dynamic equilibrium and how it describes: vapor pressure, boiling point, melting point, and sublimation

Purpose of Clausius - Clapeyron equation

finding an unknown vapor pressure / boiling point

Label all parts of a Phase Diagram

Triple point: unique temp. where temp. & press. of a substance’s solid, liquid, & gas phases co-exist in equilibrium

Critical point: liquid & gas become indistinguishable

explain differences in IMF

• Ion - induced dipole goes after disperson

• Both dispersion and Ion - induced dipole are temporary

Surface Tension, Viscosity, & Capillarity

• S.T: stronger IMF = stronger S.T | stronger Temp. = weaker S.T |

• V: stronger IMF = strong V | strong Temp. = weaker V |

• C: stronger IMF = weaker C | stronger Temp. = stronger C |

• stronger IMF = stronger boiling/freezing point

Cohesion vs Adhesion

~ attraction of molecules from same substance

~ Attraction of molecules from different substance

Solvent, Thermal, and Surface Properties of Water

• universal solvent

• HIGH specific heat capacity

• HIGH heat of vaporization

• HIGH surface tension

• Solid Water is less dense than liquid water (due to lattice structure)

Name the different types of cubic unit cells

Equations to solve different types of lattices

Differentiate between the different types of crystalline solids

relationship between vapor pressure and temperature

proportional (increases/ decreases together)

relationship between vaporization and IMF

inversely proportional (one increases / other decreases)