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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 solution in which solid solute is in equilibrium with dissolved solute.
VSEPR
crystallizes
reversible reaction
saturated solution
2. The action of salts of weak acids or bases with water to form acidic or basic solutions.
VSEPR
cathode rays
hydrolysis
Le Chatelier's principle
3. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
phase equilibrium
Charles law
reversible reaction
hybridyzation
4. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
specific heat
...
Nernst equation
single replacement/displacement
5. 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.
molar heat of sublimation
...
Le Chatelier's principle
Valence Shell Electron Pair Repulsion (VSEPR)
6. The change in enthalpy of an endothermic reaction is ________.
positive
isothermal process (thermodynamics)
limiting law
total pressure (Le Chatelier's principle)
7. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
activation energy
isopiestic process (thermodynamics)
adiabatic process (thermodynamics)
decreases
8. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
positive
first law of thermodynamics
kinetic molecular theory
change in enthalpy
9. The freezing point is always lowered by addition of solute.
upper right corner
phase equilibrium
change in enthalpy
freezing point depression
10. Metals have electronegativities less than ____
left - right (Le Chatelier's principle)
temperature
2
cathode rays
11. 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.
wave mechanical model
catalysts
state (thermodynamics)
hybridyzation
12. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
increases
Valence Shell Electron Pair Repulsion (VSEPR)
kinetic molecular theory
13. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
14. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
electrolytic cells
emits (in atomic spectra)
reversible reaction
15. *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.
metallic
catalysts
...
absorbs (in atomic spectra)
16. 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.
17. When an electron moves from an excited state to the ground state - it _______ energy.
vapor pressure
emits (in atomic spectra)
reversible reaction
combination
18. *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.
combination
10 degrees
double replacement/displacement
wave mechanical model
19. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
right (Le Chatelier's principle)
equation of state
saturated solution
20. **Proceeding across a period from left to right - the ionization energy _______.
positive charge
freezing point depression
increases
2
21. 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.
isopiestic process (thermodynamics)
isothermal process (thermodynamics)
Van der Waals
positive charge
22. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
vapor pressure
kinetic molecular theory
dynamic equilibrium
cathode rays
23. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Boyles law
emits (in atomic spectra)
heats of formation
Charles law
24. **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.
...
increases
change in enthalpy
valence
25. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
Daltons law
phase equilibrium
upper right corner
activation energy
26. A hypothetical gas would follow Boyles law under all conditions and is called?
negative
ideal gas
Van der Waals
base - acid
27. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hydrolysis
hybridyzation
positive
VSEPR
28. 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.
melting point
lower left corner
positive
kinetic molecular theory
29. Electronegativities ________ from left to right in a period.
...
Raoult's law
second law of thermodynamics
increases
30. Cells that convert electrical energy into chemical energy.
decreases
electrolytic cells
positive
molar heat of sublimation
31. Rays made up of positive electrodes in basic electron charges.
single replacement/displacement
non-ideal
anode rays
enthalpy
32. 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.
standard atmospheric pressure
colligative property law
system (thermodynamics)
equilibrium
33. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
Le Chatelier's principle
...
titration
decomposition
34. 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.
35. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
increases
boiling point elevation
high
36. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
cathode rays
negative
pressure
pi bonds
37. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
molar heat of sublimation
increases
pressure
38. In titration - this is the point at which a particular indicator changes color.
vapor pressure
limiting law
end point
wave mechanical model
39. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
Le Chatelier's principle
valence
boiling point
kinetic molecular theory
40. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
limiting law
increasing
left - right (Le Chatelier's principle)
Van der Waals
41. In an exothermic process - energy is released and ^E of reaction is ________.
negative
electrolytic reactions
second law of thermodynamics
increases
42. 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
catalysts
titration
enthalpy
43. 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
limiting law
pressure
decreases
bohr model
44. 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
freezing point depression
catalysts
irreversible and reversible processes
Van der Waals
45. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
wave mechanical model
non-ideal
upper right corner
electrolytic reactions
46. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
phase equilibrium
...
single replacement/displacement
...
47. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
vapor pressure
third law of thermodynamics
left (Le Chatelier's principle)
boiling point
48. The most active metals are found in what corner of the periodic table?
Valence Shell Electron Pair Repulsion (VSEPR)
metallic
lower left corner
...
49. When the electron moves from the ground state to an excited state - it ______ energy.
...
absorbs (in atomic spectra)
Van der Waals
increases
50. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
heat capacity
crystallizes
increases
heats of formation