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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.
saturated solution
Charles law
ideal gas
positive charge
2. Electronegativities ________ from left to right in a period.
...
isopiestic process (thermodynamics)
colligative property law
increases
3. 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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4. A chemical reaction formed from the union of its elements.
hybridyzation
increases
combination
base - acid
5. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
emits (in atomic spectra)
positive
sublimation
system (thermodynamics)
6. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
positive
Van der Waals
saturated solution
7. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
valence
adiabatic process (thermodynamics)
Boyles law
heat capacity
8. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
left - right (Le Chatelier's principle)
kinetic molecular theory
negative
10 degrees
9. The energy required to remove an electron from an isolated atom in its ground state.
first law of thermodynamics
Nernst equation
ionization energy
bohr model
10. 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
isopiestic process (thermodynamics)
point particles
first law of thermodynamics
11. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
double replacement/displacement
vapor pressure
combined gas law
pressure
12. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Avogrados law
increasing
cathode rays
left (Le Chatelier's principle)
13. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
Charles law
colligative property law
decreases
heat capacity
14. 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).
standard atmospheric pressure
negative
electrolytic cells
state (thermodynamics)
15. This process occurs when the system is maintained at the same temperature throughout an experiment.
hydrolysis
isothermal process (thermodynamics)
left - right (Le Chatelier's principle)
metallic
16. The freezing point is always lowered by addition of solute.
Raoults law
vapor pressure
freezing point depression
positive charge
17. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
point particles
electrolytic reactions
second law of thermodynamics
combined gas law
18. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
third law of thermodynamics
equilibrium
equivalent point
kinetic molecular theory
19. The heat change during a process carried out at a constant pressure.
...
change in enthalpy
Valence Shell Electron Pair Repulsion (VSEPR)
irreversible and reversible processes
20. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
sublimation
saturated solution
equation of state
dynamic equilibrium
21. *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.
wave mechanical model
equation of state
third law of thermodynamics
moles (Le Chatelier's principle)
22. Liquids with strong attractive forces have ______ boiling points.
high
left (Le Chatelier's principle)
colligative property law
state functions (thermodynamics)
23. The vapor pressure increases with increasing _____.
titration
temperature
positive charge
Boyles law
24. The action of salts of weak acids or bases with water to form acidic or basic solutions.
decomposition
increasing
irreversible and reversible processes
hydrolysis
25. The most active metals are found in what corner of the periodic table?
cathode rays
hydrolysis
lower left corner
double replacement/displacement
26. 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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27. In an endothermic process - energy is absorbed and ^E is _______.
Boyles law
electromotive force (emf)/ cell
positive
bohr model
28. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
kinetic molecular theory
isopiestic process (thermodynamics)
increases
sublimation
29. When the electron moves from the ground state to an excited state - it ______ energy.
increasing
absorbs (in atomic spectra)
single replacement/displacement
phase equilibrium
30. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
right (Le Chatelier's principle)
absorbs (in atomic spectra)
reversible reaction
31. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
Charles law
Van der Waals
heats of formation
32. 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.
point particles
left (Le Chatelier's principle)
hybridyzation
Daltons law
33. Heat added to a system and work done by a system are considered _________ quantities.
positive
...
electromotive force (emf)/ cell
double replacement/displacement
34. 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.
increasing
2
decomposition
catalysts
35. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
Le Chatelier's principle
increases
electronegativity
36. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
increases
single replacement/displacement
wave mechanical model
hybridyzation
37. 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.
electrolytic reactions
second law of thermodynamics
Charles law
reversible
38. 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.
kinetic molecular theory
decomposition
Charles law
...
39. The heat required to change 1mole of solid completely to vapor.
equilibrium
boiling point
non-ideal
molar heat of sublimation
40. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.
pi bonds
combination
first law of thermodynamics
hybridyzation
41. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
negative
electrolytic cells
activation energy
42. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
metallic
molar heat of sublimation
increases
Nernst equation
43. Metals have electronegativities less than ____
partial
equilibrium
limiting law
2
44. *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.
limiting law
ionization energy
...
saturated solution
45. 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.
freezing point depression
equivalent point
system (thermodynamics)
titration
46. The most active nonmetals are found in what corner of the periodic table?
Van der Waals
upper right corner
double replacement/displacement
anode rays
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.
colligative property law
bohr model
kinetic molecular theory
boiling point
48. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
titration
Boyles law
positive
increases
49. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy barrier (Le Chatelier's principle)
Charles law
base - acid
activation energy
50. 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.
increases
high
Raoults law
reversible reaction