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Test your basic knowledge |
CLEP Chemistry 1
Start Test
Study First
Subjects
:
clep
,
science
,
chemistry
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. Rays made up of electrons in basic electron charges.
lower left corner
zero
left - right (Le Chatelier's principle)
cathode rays
2. 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).
Van der Waals
emits (in atomic spectra)
valence
bohr model
3. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
Van der Waals
negative
...
Charles law
4. *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.
negative
Boyles law
heats of formation
equation of state
5. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.
decomposition
ideal gas
electronegativity
decreases
6. Liquids with strong attractive forces have ______ boiling points.
activation energy
zero
Van der Waals
high
7. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
standard atmospheric pressure
crystallizes
activation energy barrier (Le Chatelier's principle)
Raoults law
8. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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9. In an endothermic process - energy is absorbed and ^E is _______.
cathode rays
specific heat
positive charge
positive
10. When an electron moves from an excited state to the ground state - it _______ energy.
decomposition
emits (in atomic spectra)
isothermal process (thermodynamics)
Raoult's law
11. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
end point
Van der Waals
base - acid
positive
12. *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.
Nernst equation
wave mechanical model
increases
enthalpy
13. 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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14. The vapor pressure increases with increasing _____.
Raoults law
base - acid
temperature
pi bonds
15. 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 _____ _
equation of state
Van der Waals
limiting law
end point
16. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
boiling point elevation
positive
...
Nernst equation
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.
positive
VSEPR
equivalent point
pressure
18. The freezing point is always lowered by addition of solute.
zero
melting point
pi bonds
freezing point depression
19. 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).
10 degrees
Van der Waals
metallic
state (thermodynamics)
20. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
Van der Waals
absorbs (in atomic spectra)
Van der Waals
21. 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.
left (Le Chatelier's principle)
Valence Shell Electron Pair Repulsion (VSEPR)
high
partial
22. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
system (thermodynamics)
Le Chatelier's principle
electronegativity
23. When the electron moves from the ground state to an excited state - it ______ energy.
pressure
heats of formation
positive
absorbs (in atomic spectra)
24. A solution in which solid solute is in equilibrium with dissolved solute.
irreversible and reversible processes
Le Chatelier's principle
Raoults law
saturated solution
25. The heat required to change 1mole of solid completely to vapor.
zero
VSEPR
negative
molar heat of sublimation
26. In an exothermic process - energy is released and ^E of reaction is ________.
change in enthalpy
10 degrees
reversible
negative
27. 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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28. *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
equivalent point
right (Le Chatelier's principle)
left (Le Chatelier's principle)
29. Deviations from Boyles law that occur with real gases represent _______ behavior.
equivalent point
right (Le Chatelier's principle)
pressure
non-ideal
30. Heat added to a system and work done by a system are considered _________ quantities.
positive
Van der Waals
ideal gas
adiabatic process (thermodynamics)
31. The change in enthalpy of an endothermic reaction is ________.
increasing
2
electrolytic cells
positive
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
lower left corner
base - acid
moles (Le Chatelier's principle)
33. **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.
...
left - right (Le Chatelier's principle)
electrolytic cells
system (thermodynamics)
34. 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.
activation energy
sublimation
ionization energy
kinetic molecular theory
35. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
Valence Shell Electron Pair Repulsion (VSEPR)
equilibrium
ideal gas
36. 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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37. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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38. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
electrolytic reactions
decomposition
left (Le Chatelier's principle)
Daltons law
39. This process occurs when the system is thermally isolated so that no heat enters or leaves.
heat capacity
left (Le Chatelier's principle)
kinetic molecular theory
adiabatic process (thermodynamics)
40. The energy required to remove an electron from an isolated atom in its ground state.
molar heat of sublimation
ionization energy
third law of thermodynamics
entropy
41. 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 (thermodynamics)
left (Le Chatelier's principle)
third law of thermodynamics
reversible
42. The change in enthalpy of an exothermic reaction is ________.
system (thermodynamics)
Nernst equation
negative
kinetic molecular theory
43. 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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44. 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.
Raoult's law
lower left corner
Raoults law
base - acid
45. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
change in enthalpy
positive charge
isopiestic process (thermodynamics)
46. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Boyles law
freezing point depression
sublimation
increases
47. 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.
decreases
...
colligative property law
Nernst equation
48. 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.
ideal gas
Avogrados law
non-ideal
catalysts
49. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
increases
Charles law
Van der Waals
50. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
irreversible and reversible processes
positive
electronegativity