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. 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. 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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3. The change in enthalpy of an exothermic reaction is ________.
negative
dynamic equilibrium
kinetic molecular theory
Le Chatelier's principle


4. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
cathode rays
kinetic molecular theory
isopiestic process (thermodynamics)
zero


5. **Proceeding across a period from left to right - the ionization energy _______.
system (thermodynamics)
increases
Boyles law
valence


6. 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.
limiting law
activation energy
VSEPR
Charles law


7. Electronegativities _______ as you go down a group.
activation energy
left (Le Chatelier's principle)
vapor pressure
decreases


8. 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.
Charles law
sublimation
Van der Waals
limiting law


9. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
positive
saturated solution
entropy
phase equilibrium


10. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Avogrados law
Raoult's law
equation of state
negative


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

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12. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
right (Le Chatelier's principle)
increases
limiting law
pressure


13. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Raoult's law
adiabatic process (thermodynamics)
wave mechanical model
Avogrados law


14. This process occurs when the system is maintained at the same temperature throughout an experiment.
saturated solution
zero
isothermal process (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)


15. 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.
colligative property law
electrolytic cells
Le Chatelier's principle
activation energy


16. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
kinetic molecular theory
metallic
bohr model
titration


17. 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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18. *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.
heat capacity
positive
negative
equation of state


19. 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.
total pressure (Le Chatelier's principle)
reversible
kinetic molecular theory
pi bonds


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


21. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
sublimation
absorbs (in atomic spectra)
partial


22. _____ bonds are present in molecules containing double or triple bonds.
...
pi bonds
valence
increasing


23. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.
Charles law
valence
10 degrees
activation energy barrier (Le Chatelier's principle)


24. Metals have electronegativities less than ____
negative
heats of formation
2
electrolytic cells


25. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
ideal gas
emits (in atomic spectra)
positive
second law of thermodynamics


26. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).
2
increases
Van der Waals
decreases


27. 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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28. 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
freezing point depression
bohr model
high
metallic


29. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
valence
Raoult's law
base - acid


30. The energy required to remove an electron from an isolated atom in its ground state.
pressure
left - right (Le Chatelier's principle)
zero
ionization energy


31. A state function in which it is the heat content of a substance.
positive charge
irreversible and reversible processes
enthalpy
Daltons law


32. 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.
kinetic molecular theory
VSEPR
cathode rays
state functions (thermodynamics)


33. In an endothermic process - energy is absorbed and ^E is _______.
lower left corner
positive
electrolytic cells
metallic


34. The heat change during a process carried out at a constant pressure.
kinetic molecular theory
change in enthalpy
state functions (thermodynamics)
double replacement/displacement


35. Rays made up of electrons in basic electron charges.
heat capacity
isopiestic process (thermodynamics)
cathode rays
anode rays


36. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
boiling point
vapor pressure
decreases
melting point


37. 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 _____ _
kinetic molecular theory
equation of state
irreversible and reversible processes
limiting law


38. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
hydrolysis
molar heat of sublimation
total pressure (Le Chatelier's principle)


39. A solution in which solid solute is in equilibrium with dissolved solute.
sublimation
positive
end point
saturated solution


40. *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.
cathode rays
point particles
absorbs (in atomic spectra)
...


41. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
upper right corner
reversible
...


42. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
left - right (Le Chatelier's principle)
sublimation
increases
valence


43. The vapor pressure increases with increasing _____.
positive charge
temperature
single replacement/displacement
left - right (Le Chatelier's principle)


44. 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
sublimation
melting point
non-ideal
positive charge


45. Electronegativities ________ from left to right in a period.
increases
partial
decomposition
kinetic molecular theory


46. The most active metals are found in what corner of the periodic table?
pressure
kinetic molecular theory
lower left corner
Le Chatelier's principle


47. 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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48. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
crystallizes
point particles
temperature
zero


49. When the rate of evaporation equals the rate of condensation - the system is in __________.
combined gas law
negative
entropy
equilibrium


50. In titration - this is the point at which a particular indicator changes color.
negative
anode rays
double replacement/displacement
end point