Chem0960 Final Review

1

100

E = kQq/d

Lattice Energy Equation

200

Temperature-Pressure graph to plot states of matter

Phase Diagram / Triple-point graph

300

Intermolecular forces based off the movement of electrons. Higher Molecular weight = stronger forces.

London Forces

400

Meaning of no unpaired electrons in an MO diagram

diamagnetic

500

Amount of heat required to raise an object's temperature by 1 degree C or K

Heat capacity

2

100

Absolute zero in deg C

-273

200

The only intermolecular force that needs a mixture

Ion-Dipole Interactions

300

SCN^-

Thiocyanate

400

Hybridization if 5 domains around central atom

sp³d

500

Rank by Boiling Point:

H₂

BaCl₂

Ne

1. BaCl2 - Ionic bonds are strongest

2. Ne - only has london forces

3. H2 - only has london forces, but lower MW than Ne

3

100

The simplest whole number ratio of atoms present in a compound

Empirical Formula

200

C₂H₃O₂^-

Acetate

300

Equation consisting of individual compounds that are solid in water. Ex.

Pb²⁺(aq) + 2I^-(aq)  ->  PbI₂(aq)

Net ionic equation / ionic equation

400

h in E=hv

Planck's Constant

(Photoelectric effect states that light behaves in particles called photons - energy is this equation)

500

What is this equation used for:

ln(P₁/P₂) = -dH/R (1/T₂-1/T₁)

relate vapor pressure to temperature

4

100

Strongest yet shortest form of bond

triple bond

200

Increasing the strength of intermolecular forces ______ their boiling/melting point.

increases

300

Number of sigma bonds in a triple bond

1

400

The 3 atoms that are required for hydrogen bond (answer all 3)

F, N, O

500

Name 2 exceptions to the electron filling order

Cu, Cr, Mo, Ag, Au
(columns 4 and 9 in transition metal (d) block)

5

100

Positive delta H

Endothermic

200

ClO^-

Hypochlorite

300

Temperature at STP

0C or 273K

400

Determine the reducing agent:

2Ca(s) + O₂(g)  -> 2CaO(s)

Ca

500

hydrocarbon + O₂  ->  CO₂ + H₂O

general combustion reaction equation