Instructions:

• Answer 50 questions in 15 minutes.
• If you are not ready to take this test, you can study here.
• Match each statement with the correct term.
• Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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2. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
phase equilibrium
electronegativity
state (thermodynamics)


3. The heat required to change 1mole of solid completely to vapor.
irreversible and reversible processes
positive
molar heat of sublimation
negative


4. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f
bohr model
kinetic molecular theory
equivalent point
point particles


5. The change in enthalpy of an exothermic reaction is ________.
electrolytic cells
second law of thermodynamics
anode rays
negative


6. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
Charles law
...
sublimation
system (thermodynamics)


7. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l
isothermal process (thermodynamics)
combined gas law
irreversible and reversible processes
combination


8. Electronegativities _______ as you go down a group.
heats of formation
Raoults law
Van der Waals
decreases


9. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.
temperature
pressure
dynamic equilibrium
reversible


10. A hypothetical gas would follow Boyles law under all conditions and is called?
ideal gas
Le Chatelier's principle
melting point
kinetic molecular theory


11. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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12. A state function in which it is the heat content of a substance.
enthalpy
freezing point depression
end point
emits (in atomic spectra)


13. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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14. The vapor pressure increases with increasing _____.
Van der Waals
boiling point
positive
temperature


15. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
decreases
system (thermodynamics)
molar heat of sublimation
Charles law


16. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
decomposition
positive
kinetic molecular theory
Van der Waals


17. A process that occurs whent eh system is maintained at constant pressure.
base - acid
emits (in atomic spectra)
isopiestic process (thermodynamics)
specific heat


18. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
reversible reaction
hybridyzation
state (thermodynamics)
negative


19. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
moles (Le Chatelier's principle)
freezing point depression
Le Chatelier's principle
specific heat


20. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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21. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
upper right corner
entropy
kinetic molecular theory
positive


22. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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23. The molecules in a gas are in constant - continueous - random - and straight-line motion.
electromotive force (emf)/ cell
phase equilibrium
kinetic molecular theory
second law of thermodynamics


24. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
state functions (thermodynamics)
bohr model
double replacement/displacement


25. The freezing point is always lowered by addition of solute.
base - acid
catalysts
freezing point depression
moles (Le Chatelier's principle)


26. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.

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27. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
positive
electromotive force (emf)/ cell
heat capacity
kinetic molecular theory


28. Electronegativities ________ from left to right in a period.
Raoults law
heats of formation
increases
saturated solution


29. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
melting point
boiling point elevation
electronegativity
single replacement/displacement


30. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
heats of formation
reversible
second law of thermodynamics
Boyles law


31. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
...
activation energy barrier (Le Chatelier's principle)
electrolytic reactions
pressure


32. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
kinetic molecular theory
hybridyzation
increasing
Raoult's law


33. When the rate of evaporation equals the rate of condensation - the system is in __________.
vapor pressure
equilibrium
negative
kinetic molecular theory


34. The heat change during a process carried out at a constant pressure.
Nernst equation
electrolytic cells
change in enthalpy
moles (Le Chatelier's principle)


35. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.
Valence Shell Electron Pair Repulsion (VSEPR)
upper right corner
Raoult's law
heat capacity


36. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.
equivalent point
Van der Waals
equation of state
electronegativity


37. The most active metals are found in what corner of the periodic table?
sublimation
enthalpy
lower left corner
positive


38. In an exothermic process - energy is released and ^E of reaction is ________.
kinetic molecular theory
end point
molar heat of sublimation
negative


39. **Proceeding across a period from left to right - the ionization energy _______.
metallic
pressure
decreases
increases


40. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g
valence
negative
titration
left - right (Le Chatelier's principle)


41. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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42. Metals have electronegativities less than ____
Valence Shell Electron Pair Repulsion (VSEPR)
2
Le Chatelier's principle
positive


43. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
ionization energy
activation energy
titration
anode rays


44. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.
Charles law
Van der Waals
colligative property law
isopiestic process (thermodynamics)


45. Liquids with strong attractive forces have ______ boiling points.
double replacement/displacement
kinetic molecular theory
moles (Le Chatelier's principle)
high


46. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.
first law of thermodynamics
base - acid
high
Raoult's law


47. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
electrolytic reactions
kinetic molecular theory
point particles


48. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.
wave mechanical model
left (Le Chatelier's principle)
...
activation energy barrier (Le Chatelier's principle)


49. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
positive charge
titration
total pressure (Le Chatelier's principle)
pressure


50. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
Van der Waals
wave mechanical model
isopiestic process (thermodynamics)