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.
VSEPR
Le Chatelier's principle
negative
equation of state


2. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
hybridyzation
catalysts
electrolytic reactions
sublimation


3. 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.
combination
first law of thermodynamics
activation energy
Daltons law


4. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
hydrolysis
Van der Waals
equivalent point
reversible reaction


5. When the electron moves from the ground state to an excited state - it ______ energy.
Valence Shell Electron Pair Repulsion (VSEPR)
combined gas law
absorbs (in atomic spectra)
moles (Le Chatelier's principle)


6. 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
hydrolysis
irreversible and reversible processes
Le Chatelier's principle
left (Le Chatelier's principle)


7. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
vapor pressure
increases
positive


8. 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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9. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
cathode rays
left - right (Le Chatelier's principle)
kinetic molecular theory
ideal gas


10. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
Raoult's law
kinetic molecular theory
change in enthalpy


11. A state function in which it is the heat content of a substance.
electrolytic reactions
enthalpy
reversible reaction
base - acid


12. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
single replacement/displacement
reversible reaction
specific heat
...


13. 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.
isopiestic process (thermodynamics)
left (Le Chatelier's principle)
equivalent point
pressure


14. *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.
freezing point depression
wave mechanical model
entropy
saturated solution


15. The most active nonmetals are found in what corner of the periodic table?
Daltons law
irreversible and reversible processes
upper right corner
increases


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

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17. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
enthalpy
phase equilibrium
...
Boyles law


18. The action of salts of weak acids or bases with water to form acidic or basic solutions.
decreases
reversible reaction
colligative property law
hydrolysis


19. Rays made up of positive electrodes in basic electron charges.
anode rays
activation energy barrier (Le Chatelier's principle)
titration
boiling point


20. The freezing point is always lowered by addition of solute.
wave mechanical model
kinetic molecular theory
freezing point depression
hybridyzation


21. 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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22. 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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23. 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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24. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
molar heat of sublimation
Avogrados law
combination
point particles


25. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
...
specific heat
decomposition
Raoult's law


26. _____ bonds are present in molecules containing double or triple bonds.
kinetic molecular theory
total pressure (Le Chatelier's principle)
temperature
pi bonds


27. 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.
Van der Waals
...
colligative property law
Valence Shell Electron Pair Repulsion (VSEPR)


28. 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
electronegativity
standard atmospheric pressure
pressure


29. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
heats of formation
boiling point elevation
temperature
boiling point


30. 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.
negative
state functions (thermodynamics)
electromotive force (emf)/ cell
third law of thermodynamics


31. The change in enthalpy of an endothermic reaction is ________.
titration
2
positive
base - acid


32. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.
titration
Valence Shell Electron Pair Repulsion (VSEPR)
activation energy barrier (Le Chatelier's principle)
kinetic molecular theory


33. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
moles (Le Chatelier's principle)
Le Chatelier's principle
VSEPR


34. Electronegativities _______ as you go down a group.
melting point
Raoult's law
emits (in atomic spectra)
decreases


35. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
crystallizes
2
bohr model
titration


36. The change in enthalpy of an exothermic reaction is ________.
negative
first law of thermodynamics
end point
Le Chatelier's principle


37. Electronegativities ________ from left to right in a period.
decreases
kinetic molecular theory
Van der Waals
increases


38. 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)
enthalpy
combined gas law
second law of thermodynamics


39. The heat change during a process carried out at a constant pressure.
change in enthalpy
left (Le Chatelier's principle)
metallic
positive


40. 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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41. *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
Charles law
boiling point
10 degrees


42. In an exothermic process - energy is released and ^E of reaction is ________.
negative
titration
state functions (thermodynamics)
combined gas law


43. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
heat capacity
valence
point particles


44. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
increases
freezing point depression
combined gas law
crystallizes


45. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.
Van der Waals
moles (Le Chatelier's principle)
irreversible and reversible processes
Raoults law


46. 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 _____ _
pressure
...
Valence Shell Electron Pair Repulsion (VSEPR)
limiting law


47. Metals have electronegativities less than ____
Avogrados law
2
activation energy barrier (Le Chatelier's principle)
increases


48. 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.
combination
reversible
vapor pressure
temperature


49. 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 (thermodynamics)
first law of thermodynamics
left (Le Chatelier's principle)
activation energy barrier (Le Chatelier's principle)


50. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
point particles
standard atmospheric pressure
first law of thermodynamics
kinetic molecular theory