Atomic Structure & Properties
Properties of Substances & Mixtures
Kinetics
Equilibrium
Thermodynamics & Electrochemistry
100
This is the number of neutrons in an isotope of Uranium with a mass number of 238
146
100
Name two of the three intermolecular forces present between molecules of methanol shown above.
Dipole-Dipole Interactions
Hydrogen Bonding
London Dispersion Forces
100
This image represents this order for a chemical reaction.
First Order
100
When Q < K, this shift occurs
Shift to the right (More products must be made)
100
This is the direction (and process that occurs) of electron flow through the electrodes of a galvanic cell.
Anode (oxidation) to Cathode (reduction)
200
This is the shorthand electron configuration for Tin
[Kr] 5s2 4d10 5p2
200
This is the weakest type of intermolecular force and is found in all substances
London Dispersion Forces
200
In a reaction mechanism, this is the term for a species that is formed and then consumed during the reaction
Intermediate
200
A +2B ⇌ 3C Keq = 1.042
This is the value of the equilibrium constant for the reverse reaction
0.9597
200
This is the value of the equilibrium constant (Keq) when ΔG° is negative.
K > 1
300
This rule states that electrons will fill degenerate orbitals singly before pairing up.
Hund's Rule
300
These types of solids have significantly weak IMFs, due to its structure of nonmetal atoms covalently bonded to one another.
Molecular Solids
300
This is the name given to the peak(s) on a reaction coordinate diagram.
Transition State
300
This is how equilibrium is affected in a constant volume container when a catalyst is added.
Equilibrium does not change
300
This is when a reaction will be spontaneous given the following information:
ΔG = Unknown
ΔH= Positive
ΔS = Positive
High Temperatures
400
This is the reason why atomic radii decrease as you move across a period on the periodic table
Increasing nuclear charge (nucleus attracts electrons more stongly)
400
The graph above show this sample at the highest temperature
Sample C
400
This is the reason that Reaction B has a greater activation energy than Reaction A
Reaction B is uncatalyzed
400
A saturated solution of CaF₂ is in equilibrium with its ions. When solid NaF is added to the solution to create a fluoride ion concentration of 0.25 M, what is the new solubility of CaF₂?
(Ksp for CaF₂ = 3.9 × 10⁻¹¹)
6.24 x 10-10 M
400
This is the cell potential of the following reaction
2K+ + Mg → Mg2+ + 2K
K+ + e- → K Reduction Potential = -2.93 V
Mg2+ + e- → Mg Reduction Potential = -2.37 V
+ 0.56 V
500
Below is the PES of Phosphorus. This change is necessary for the PES of Chlorine.
Peak at 1 MJ/mol increase to 5 electrons
500
The Graph above shows this sample as the lightest sample.
Sample C
500
This is the rate law for the table below
Rate = k[C3H6O]
500
This is the value of Kp for the reaction at equilibrium for methane gas (0.20 atm) and dihydrogen sulfide gas (0.25 atm) to produce carbon disulfide gas (0.52 atm) and hydrogen gas (0.10 atm).
4.2 x 10-3
500
This is the standard entropy of the following reaction:
2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l)
S∘ C2H6(g) = 229.5 J/mol K
S∘ O2(g) = 205.0 J/mol K
S∘ CO2(g) = 213.7 J/mol K
S∘ H2O (l) = 69.9 J/mol K
-619.8 J/mol K