Instructions:

• Answer 50 questions in 15 minutes.
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• 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. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.
combination
VSEPR
specific heat
kinetic molecular theory


2. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Van der Waals
kinetic molecular theory
heat capacity
activation energy


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

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4. In titration - this is the point at which a particular indicator changes color.
end point
Charles law
moles (Le Chatelier's principle)
adiabatic process (thermodynamics)


5. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
activation energy
left (Le Chatelier's principle)
single replacement/displacement
pressure


6. Liquids with strong attractive forces have ______ boiling points.
high
wave mechanical model
increases
lower left corner


7. This process occurs when the system is thermally isolated so that no heat enters or leaves.
zero
adiabatic process (thermodynamics)
metallic
Charles law


8. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
decreases
negative
Charles law
first law of thermodynamics


9. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
hydrolysis
equivalent point
third law of thermodynamics


10. *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.
decomposition
state (thermodynamics)
...
positive


11. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
Van der Waals
entropy
Boyles law
positive


12. Electronegativities ________ from left to right in a period.
increases
2
pi bonds
kinetic molecular theory


13. 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.
Daltons law
combination
total pressure (Le Chatelier's principle)
colligative property law


14. In an exothermic process - energy is released and ^E of reaction is ________.
enthalpy
negative
activation energy
double replacement/displacement


15. A solution in which solid solute is in equilibrium with dissolved solute.
second law of thermodynamics
boiling point
saturated solution
base - acid


16. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
Le Chatelier's principle
equilibrium
left (Le Chatelier's principle)


17. 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.
state functions (thermodynamics)
reversible
pi bonds
equivalent point


18. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
colligative property law
metallic
increases
VSEPR


19. Rays made up of electrons in basic electron charges.
cathode rays
crystallizes
Charles law
colligative property law


20. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
anode rays
third law of thermodynamics
Valence Shell Electron Pair Repulsion (VSEPR)
specific heat


21. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
decomposition
hybridyzation
left - right (Le Chatelier's principle)
boiling point


22. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
electronegativity
Van der Waals
point particles
temperature


23. The temperature at which a substance's solid and liquid phases are in equilibrium.
absorbs (in atomic spectra)
melting point
enthalpy
isothermal process (thermodynamics)


24. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
colligative property law
kinetic molecular theory
single replacement/displacement
ionization energy


25. When an electron moves from an excited state to the ground state - it _______ energy.
vapor pressure
emits (in atomic spectra)
left - right (Le Chatelier's principle)
pressure


26. 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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27. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
pi bonds
sublimation
...


28. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.
...
state functions (thermodynamics)
lower left corner
decomposition


29. _____ bonds are present in molecules containing double or triple bonds.
Raoults law
electrolytic cells
pi bonds
adiabatic process (thermodynamics)


30. The change in enthalpy of an endothermic reaction is ________.
positive
third law of thermodynamics
enthalpy
high


31. 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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32. Heat added to a system and work done by a system are considered _________ quantities.
hybridyzation
Le Chatelier's principle
Van der Waals
positive


33. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).
state functions (thermodynamics)
anode rays
dynamic equilibrium
state (thermodynamics)


34. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
negative
emits (in atomic spectra)
decreases


35. 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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36. The heat change during a process carried out at a constant pressure.
right (Le Chatelier's principle)
change in enthalpy
state functions (thermodynamics)
melting point


37. A chemical reaction formed from the union of its elements.
combination
total pressure (Le Chatelier's principle)
activation energy barrier (Le Chatelier's principle)
system (thermodynamics)


38. The most active nonmetals are found in what corner of the periodic table?
irreversible and reversible processes
increases
upper right corner
electromotive force (emf)/ cell


39. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
decomposition
standard atmospheric pressure
third law of thermodynamics
kinetic molecular theory


40. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
pi bonds
molar heat of sublimation
adiabatic process (thermodynamics)
heats of formation


41. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.
Van der Waals
combined gas law
catalysts
left - right (Le Chatelier's principle)


42. Metals have electronegativities less than ____
freezing point depression
2
10 degrees
combination


43. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
combination
2
decreases


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

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45. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
dynamic equilibrium
positive
bohr model
heat capacity


46. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
zero
cathode rays
Raoults law


47. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
increases
irreversible and reversible processes
valence


48. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
Avogrados law
limiting law
adiabatic process (thermodynamics)
zero


49. The change in enthalpy of an exothermic reaction is ________.
isothermal process (thermodynamics)
temperature
positive
negative


50. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
lower left corner
high
reversible