Instructions:

• Answer 50 questions in 15 minutes.
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• Match each statement with the correct term.
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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. 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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2. 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.
lower left corner
kinetic molecular theory
wave mechanical model
Charles law


3. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.
single replacement/displacement
change in enthalpy
...
melting point


4. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
base - acid
kinetic molecular theory
end point
vapor pressure


5. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
kinetic molecular theory
increasing
left (Le Chatelier's principle)
pi bonds


6. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
entropy
kinetic molecular theory
Daltons law
dynamic equilibrium


7. Electronegativities _______ as you go down a group.
single replacement/displacement
boiling point elevation
decreases
equilibrium


8. The change in enthalpy of an exothermic reaction is ________.
hybridyzation
positive
boiling point elevation
negative


9. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
10 degrees
crystallizes
base - acid


10. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
Le Chatelier's principle
Daltons law
electrolytic reactions
state (thermodynamics)


11. 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).
pi bonds
positive
state (thermodynamics)
anode rays


12. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
left (Le Chatelier's principle)
Avogrados law
...
valence


13. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
heat capacity
state functions (thermodynamics)
electronegativity


14. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
entropy
increases
saturated solution
heats of formation


15. Electronegativities ________ from left to right in a period.
equilibrium
freezing point depression
VSEPR
increases


16. A state function in which it is the heat content of a substance.
dynamic equilibrium
enthalpy
increases
cathode rays


17. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.
phase equilibrium
2
bohr model
equivalent point


18. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
increases
sublimation
emits (in atomic spectra)
specific heat


19. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
metallic
2
kinetic molecular theory
negative


20. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
decomposition
heats of formation
reversible
pi bonds


21. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
phase equilibrium
positive
reversible reaction
Le Chatelier's principle


22. The heat required to change 1mole of solid completely to vapor.
positive
activation energy
ideal gas
molar heat of sublimation


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

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24. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Boyles law
Van der Waals
pi bonds
single replacement/displacement


25. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
negative
equivalent point
third law of thermodynamics
temperature


26. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.
left (Le Chatelier's principle)
Daltons law
upper right corner
total pressure (Le Chatelier's principle)


27. The heat change during a process carried out at a constant pressure.
change in enthalpy
decreases
third law of thermodynamics
ideal gas


28. 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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29. Cells that convert electrical energy into chemical energy.
heat capacity
electronegativity
Charles law
electrolytic cells


30. 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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31. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
heat capacity
metallic
left - right (Le Chatelier's principle)
decomposition


32. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Le Chatelier's principle
positive
heat capacity
electrolytic reactions


33. The temperature at which a substance's solid and liquid phases are in equilibrium.
Le Chatelier's principle
activation energy barrier (Le Chatelier's principle)
melting point
...


34. The most active nonmetals are found in what corner of the periodic table?
left (Le Chatelier's principle)
left - right (Le Chatelier's principle)
kinetic molecular theory
upper right corner


35. *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
combined gas law
emits (in atomic spectra)
Van der Waals


36. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
activation energy barrier (Le Chatelier's principle)
zero
second law of thermodynamics


37. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
end point
positive charge
base - acid
limiting law


38. 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
wave mechanical model
heats of formation


39. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
bohr model
pi bonds
increases
point particles


40. When an electron moves from an excited state to the ground state - it _______ energy.
irreversible and reversible processes
emits (in atomic spectra)
total pressure (Le Chatelier's principle)
Le Chatelier's principle


41. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

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42. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
left (Le Chatelier's principle)
kinetic molecular theory
valence
boiling point


43. 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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44. 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.
Avogrados law
VSEPR
colligative property law
second law of thermodynamics


45. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge
positive charge
state (thermodynamics)
state functions (thermodynamics)
absorbs (in atomic spectra)


46. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
anode rays
Raoult's law
second law of thermodynamics
Charles law


47. In an exothermic process - energy is released and ^E of reaction is ________.
hydrolysis
Raoults law
heats of formation
negative


48. The molecules in a gas are in constant - continueous - random - and straight-line motion.
entropy
kinetic molecular theory
boiling point elevation
specific heat


49. A chemical reaction formed from the union of its elements.
pi bonds
combination
point particles
state functions (thermodynamics)


50. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
activation energy barrier (Le Chatelier's principle)
boiling point elevation
boiling point
Valence Shell Electron Pair Repulsion (VSEPR)