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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. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
kinetic molecular theory
metallic
moles (Le Chatelier's principle)
hydrolysis
2. Metals have electronegativities less than ____
2
base - acid
Van der Waals
ionization energy
3. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
2
equivalent point
dynamic equilibrium
Boyles law
4. 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 _____ _
melting point
kinetic molecular theory
phase equilibrium
limiting law
5. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
kinetic molecular theory
upper right corner
third law of thermodynamics
6. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
point particles
positive charge
zero
negative
7. The heat required to change 1mole of solid completely to vapor.
enthalpy
saturated solution
cathode rays
molar heat of sublimation
8. *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.
equation of state
activation energy
positive
reversible reaction
9. 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.
moles (Le Chatelier's principle)
colligative property law
irreversible and reversible processes
negative
10. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
crystallizes
isothermal process (thermodynamics)
Avogrados law
catalysts
11. 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.
equivalent point
end point
boiling point elevation
electrolytic reactions
12. The energy required to remove an electron from an isolated atom in its ground state.
isopiestic process (thermodynamics)
Van der Waals
combined gas law
ionization energy
13. The pressure exerted by each gas in a mixture is called its _____ pressure.
Charles law
hydrolysis
increases
partial
14. The molecules in a gas are in constant - continueous - random - and straight-line motion.
crystallizes
kinetic molecular theory
heat capacity
negative
15. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
electronegativity
total pressure (Le Chatelier's principle)
activation energy barrier (Le Chatelier's principle)
sublimation
16. 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.
17. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
zero
irreversible and reversible processes
10 degrees
heat capacity
18. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
Valence Shell Electron Pair Repulsion (VSEPR)
double replacement/displacement
melting point
catalysts
19. 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.
melting point
catalysts
electronegativity
Le Chatelier's principle
20. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
equivalent point
equation of state
specific heat
Van der Waals
21. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
isothermal process (thermodynamics)
VSEPR
Avogrados law
phase equilibrium
22. The change in enthalpy of an endothermic reaction is ________.
Valence Shell Electron Pair Repulsion (VSEPR)
positive
Nernst equation
limiting law
23. When the electron moves from the ground state to an excited state - it ______ energy.
enthalpy
ideal gas
kinetic molecular theory
absorbs (in atomic spectra)
24. The most active metals are found in what corner of the periodic table?
Charles law
catalysts
combination
lower left corner
25. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
equation of state
state functions (thermodynamics)
Charles law
26. 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.
27. 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.
Daltons law
Le Chatelier's principle
vapor pressure
Valence Shell Electron Pair Repulsion (VSEPR)
28. When the rate of evaporation equals the rate of condensation - the system is in __________.
enthalpy
equilibrium
...
lower left corner
29. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
Charles law
activation energy
absorbs (in atomic spectra)
30. A process that occurs whent eh system is maintained at constant pressure.
melting point
combination
isopiestic process (thermodynamics)
anode rays
31. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
32. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
Van der Waals
boiling point elevation
absorbs (in atomic spectra)
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.
hydrolysis
...
temperature
absorbs (in atomic spectra)
34. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
pressure
combined gas law
double replacement/displacement
kinetic molecular theory
35. A hypothetical gas would follow Boyles law under all conditions and is called?
...
equilibrium
non-ideal
ideal gas
36. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
irreversible and reversible processes
positive
state functions (thermodynamics)
37. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
boiling point elevation
Charles law
increases
vapor pressure
38. 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.
hydrolysis
titration
third law of thermodynamics
melting point
39. Liquids with strong attractive forces have ______ boiling points.
high
Charles law
combined gas law
heat capacity
40. **Proceeding across a period from left to right - the ionization energy _______.
limiting law
Charles law
negative
increases
41. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
equilibrium
Nernst equation
increasing
VSEPR
42. The change in enthalpy of an exothermic reaction is ________.
titration
combination
negative
enthalpy
43. The freezing point is always lowered by addition of solute.
state (thermodynamics)
decreases
colligative property law
freezing point depression
44. 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.
45. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
electronegativity
lower left corner
Boyles law
ideal gas
46. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
second law of thermodynamics
anode rays
negative
base - acid
47. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
state (thermodynamics)
left - right (Le Chatelier's principle)
kinetic molecular theory
system (thermodynamics)
48. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
single replacement/displacement
right (Le Chatelier's principle)
boiling point
49. *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.
reversible reaction
positive charge
Valence Shell Electron Pair Repulsion (VSEPR)
wave mechanical model
50. 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.