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. _____ bonds are present in molecules containing double or triple bonds.
partial
pi bonds
increases
freezing point depression


2. A chemical reaction formed from the union of its elements.
third law of thermodynamics
combination
VSEPR
...


3. *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.
enthalpy
temperature
...
state functions (thermodynamics)


4. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
reversible
non-ideal
limiting law
electromotive force (emf)/ cell


5. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
Van der Waals
emits (in atomic spectra)
titration


6. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
equation of state
wave mechanical model
dynamic equilibrium
heats of formation


7. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
standard atmospheric pressure
Charles law
decomposition
increases


8. 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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9. The temperature at which a substance's solid and liquid phases are in equilibrium.
moles (Le Chatelier's principle)
melting point
Van der Waals
decreases


10. 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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11. A hypothetical gas would follow Boyles law under all conditions and is called?
negative
ideal gas
zero
increases


12. When the electron moves from the ground state to an excited state - it ______ energy.
decomposition
ionization energy
Van der Waals
absorbs (in atomic spectra)


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

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14. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
negative
2
zero
third law of thermodynamics


15. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.

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16. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
...
vapor pressure
single replacement/displacement
increasing


17. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
electromotive force (emf)/ cell
saturated solution
combination
point particles


18. The freezing point is always lowered by addition of solute.
Raoult's law
reversible
freezing point depression
third law of thermodynamics


19. *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.
metallic
equation of state
increasing
sublimation


20. This process occurs when the system is maintained at the same temperature throughout an experiment.
Le Chatelier's principle
isothermal process (thermodynamics)
kinetic molecular theory
total pressure (Le Chatelier's principle)


21. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.
increasing
kinetic molecular theory
moles (Le Chatelier's principle)
Raoults law


22. A state function in which it is the heat content of a substance.
second law of thermodynamics
enthalpy
reversible
activation energy


23. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
left - right (Le Chatelier's principle)
2
Boyles law


24. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
crystallizes
moles (Le Chatelier's principle)
hybridyzation
Le Chatelier's principle


25. Deviations from Boyles law that occur with real gases represent _______ behavior.
electromotive force (emf)/ cell
non-ideal
equation of state
Van der Waals


26. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
positive charge
equation of state
2


27. Liquids with strong attractive forces have ______ boiling points.
Charles law
high
Van der Waals
increases


28. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _
limiting law
titration
activation energy
crystallizes


29. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.
increases
catalysts
kinetic molecular theory
Van der Waals


30. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
positive charge
2
decreases


31. The molecules in a gas are in constant - continueous - random - and straight-line motion.
activation energy
decreases
kinetic molecular theory
left (Le Chatelier's principle)


32. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
irreversible and reversible processes
vapor pressure
10 degrees
first law of thermodynamics


33. 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.
reversible
...
state functions (thermodynamics)
double replacement/displacement


34. 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.
catalysts
negative
emits (in atomic spectra)
ideal gas


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

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36. *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
high
electrolytic cells
Van der Waals
valence


37. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
single replacement/displacement
high
Le Chatelier's principle
standard atmospheric pressure


38. Metals have electronegativities less than ____
negative
state functions (thermodynamics)
Le Chatelier's principle
2


39. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
zero
boiling point
kinetic molecular theory
heat capacity


40. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
hybridyzation
increases
change in enthalpy
pressure


41. 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.
VSEPR
moles (Le Chatelier's principle)
increases
high


42. 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.
hybridyzation
state functions (thermodynamics)
electromotive force (emf)/ cell
...


43. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.
wave mechanical model
emits (in atomic spectra)
decomposition
total pressure (Le Chatelier's principle)


44. A process that occurs whent eh system is maintained at constant pressure.
ionization energy
isopiestic process (thermodynamics)
melting point
Daltons law


45. Rays made up of electrons in basic electron charges.
sublimation
electromotive force (emf)/ cell
Avogrados law
cathode rays


46. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
Van der Waals
equilibrium
kinetic molecular theory


47. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
anode rays
Nernst equation
second law of thermodynamics
specific heat


48. 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
cathode rays
boiling point
high


49. The heat required to change 1mole of solid completely to vapor.
VSEPR
molar heat of sublimation
irreversible and reversible processes
entropy


50. This process occurs when the system is thermally isolated so that no heat enters or leaves.
state (thermodynamics)
moles (Le Chatelier's principle)
heats of formation
adiabatic process (thermodynamics)