WorksheetsGeneral Chemistry PT 2
Total questions: 108
Worksheet time: 2hrs 35mins
transfer of electrons
(a)
electrostatic
(a)
sharing of electrons
(a)
– sideway overlap
Pi bond
Sigma bond
– head on overlap of atomic orbitals
Sigma bond
Pi-Bond
unequal sharing of electrons
Polar
non Polar
Depicts the bonds between atoms and unbonded electron pairs
(a)
Predicts the geometry of molecules from electrostatic repulsion
(a)
what is the acronym VSEPR Theory
(a)
linear
trigonal planar
tetrahedral
trigonal planar
tetrahedral
trigonal bipyramid
tetrahedral
trigonal pyramid
trigonal planar
trigonal bipyramid
octahedral
tetrahedral
octahedral
tetrahedral
trigonal planar
Water molecule exhibits a bent shape, which is a special type
(a)
GAS LAWS
Isothermal
Boyle’s law
Charles Law
Gay Lussacs Law
Avogadro’s law
Isobaric
Charles Law
Ideal Gas Law
Boyle’s law
Law of combining volumes ; isochoric
Gay Lussacs Law
Avogadro’s law
Charles Law
Boyle’s law
Constant pressure and temperature
Avogadro’s law
Ideal Gas Law
Gay Lussacs Law
PV=nRT
Gas law
Avogadro’s law
Gay Lussacs Law
universal gas constant
(a)
PT = P1 + P2 + P3 + …
Dalton’s Law of Partial Pressure
Ideal Gas Law
Graham’s Law of diffusion/ effusion
Rate of diffusion is inversely proportional to the density of gas
Graham’s Law of diffusion/ effusion
Ideal Gas Law
Gay Lussacs Law
max amount of solute is dissolved in a solvent
(a)
high Solvent
(a)
high Solute; metastable; easily crystallized
(a)
Factors Affecting Solubility
(a)
Temperature
→ Generally, higher temperature = _____ ____
(a)
Temperature
→ Gases wherein higher temperature = (a)
Pressure
→ Higher pressure = (a) solubility
Surface area
→ More SA = (a) solubility
FORMULA:
M = molarity
(a)
FORMULA
m = molality
(a)
FORMULA
N = normality
(a)
FORMULA
Vapor pressure lowering
(a)
FORMULA
Boiling point elevation
(a)
FORMULA
Freezing point depression
(a)
FORMULA
Osmotic pressure
(a)
Arrhenius theory
→ Acid: yields (a) in water
Arrhenius theory
→ Base: yields (a) in water
Bronsted Lowry theory
→ Acid: ____ proton
→ Base: ____ proton
(answer/answer)
(a)
Lewis theory
→ Acid: ___ electron pair
→ Base: ___ electron pair
(a)
FORMULA
Kw
(a)
FORMULA
pH
(a)
Ka: ↑Ka = (a) acidity
(higher/lower)
Kb: ↑Kb = (a) basicity
(higher or lower)
Rate of reaction is directly proportional to effective collision
Collision theories
Transition state
Rate of reaction is directly proportional to the formation of intermediate complex
Transition state
Collision theories
minimum energy that molecules must posses for the reaction to take place
(a)
Nature of reactants:
→ More reactive = (a) reaction
(faster/slower)
Temperature
→ Higher temperature = (a) reaction
(faster/slower)
Higher kinetic energy = ____ effective collision = ____ reaction
(higher/lower) = (faster/lower)
(a)
Concentration of reactants
→ Higher concentration = (a) reaction
(faster/slower)
→ Speeds up reaction rate by lowing the activation energy needed
(a)
→ Can provide an alternative pathway
(a)
Regenerated at the end of the reaction
(a)
Surface area
Increase SA = (a) reaction
More reactive = faster reaction
(a)
→ Higher temperature = faster reaction
→ Collision theory
(a)
→ Higher concentration = faster reaction
(a)
→ Increase SA = faster reaction
(a)
Factors affecting reaction rates
Nature of reactants
Temperature
Pressure
Catalyst
Factors affecting reaction rates
Concentration of reactants
Surface area
Freezing point
– part of the universe
(a)
the rest of the universe that interacts with the system
(a)
allows the exchange of energy and matter
(a)
allows the exchange of energy
(a)
impermeable to both energy and matter
(a)
Path independent
Initial and final status
(a)
Path dependent
(a)
absorbes heat
(a)
releases heat
(a)
heat loss = heat gain
does not effect the substance
(a)
work is done ON the system
(a)
work is done BY the system
(a)
no change in volume
(a)
Expendable amount of energy in a system
(a)
State of randomness/ disorderness
(a)
Heat content at constant volume and it is the Total energy of the system
(a)
Heat content (amount needed to burn)
(a)
Energy is neither created nor destroyed, but can be converted from one form to another
3 rd law
Zeroth law
1 st law of conservation of energy
2 nd law of entropy
The entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process
1 st law of conservation of energy
2 nd law of entropy
3 rd law
zeroth law
→ The entropy of a perfect crystalline substance is 0 at the absolute 0 (0K) temperature
3 rd law
Zeroth law
1 st law of conservation of energy
2 nd law of entropy
If 2 systems are in thermal equilibrium respectively with a third system, they must be in thermal equilibrium with each other
Zeroth law
3 rd law
2 nd law of entropy
1 st law of conservation of energy
Rate of forward reaction is (a) to the rate of backward reaction
(lower/equal/higher)
forward reaction is favored
K > 1
K < 1
backward reaction is favored
K < 1
K > 1
Reactant and product = same phase
Homogenous equilibria
Heterogenous equilibria
Reactant and product = different phase
Solids and liquids are not included
Heterogenous equilibria
Homogenous equilibria
solubility product constant and describe saturated solution of ionic compounds of relatively low solubility
(a)
Insoluble salts (Ksp)
Higher Ksp = (a) soluble
(more/few)
If an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches new equilibrium position
(a)
Concentration and temperature
• Higher Pressure, lower volume = shift to where there are fewer gas moles
(a)
Endothermic + Higher temp
(a)
Endothermic + Lower temp
(a)
Exothermic + lower temp
(a)
exothermic + Higher temp
(a)
Anode
(a)
Cathode
(a)
Spontaneous
(a)
Non-spontaneous
(a)
Galvanic/ voltaic cells
Electrolytic cells
(a)
Depends on nuclear stability
(a)
Spontaneous emission of particles/ionizing radiation by unstable nuclei of heavier elements
(a)
what is the bond angle of linear
(a)
trigonal planar angle
(a)
trigonal angle
(a)
bipyramid angle
(a)
