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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 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
wave mechanical model
bohr model
Raoults law
single replacement/displacement
2. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Van der Waals
right (Le Chatelier's principle)
Boyles law
bohr model
3. A chemical reaction formed from the union of its elements.
dynamic equilibrium
valence
equivalent point
combination
4. The action of salts of weak acids or bases with water to form acidic or basic solutions.
activation energy barrier (Le Chatelier's principle)
hydrolysis
increases
reversible reaction
5. 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.
wave mechanical model
titration
Charles law
ionization energy
6. The energy required to remove an electron from an isolated atom in its ground state.
negative
ionization energy
boiling point elevation
point particles
7. 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 _____ _
Daltons law
limiting law
boiling point elevation
positive
8. 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.
electrolytic cells
activation energy barrier (Le Chatelier's principle)
state functions (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
9. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
ideal gas
standard atmospheric pressure
reversible
10. The vapor pressure increases with increasing _____.
absorbs (in atomic spectra)
Daltons law
temperature
combined gas law
11. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
electrolytic reactions
colligative property law
kinetic molecular theory
point particles
12. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
combined gas law
point particles
bohr model
hybridyzation
13. 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).
kinetic molecular theory
reversible
state (thermodynamics)
high
14. Rays made up of electrons in basic electron charges.
...
cathode rays
valence
lower left corner
15. In titration - this is the point at which a particular indicator changes color.
end point
standard atmospheric pressure
Raoults law
electrolytic cells
16. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
heat capacity
Van der Waals
...
17. 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.
electronegativity
Nernst equation
heats of formation
increases
18. When the rate of evaporation equals the rate of condensation - the system is in __________.
double replacement/displacement
equilibrium
adiabatic process (thermodynamics)
absorbs (in atomic spectra)
19. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
upper right corner
heats of formation
2
Le Chatelier's principle
20. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
base - acid
Daltons law
boiling point elevation
Raoults law
21. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
pi bonds
increases
Raoults law
boiling point
22. The pressure exerted by each gas in a mixture is called its _____ pressure.
positive charge
third law of thermodynamics
Van der Waals
partial
23. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
...
decreases
first law of thermodynamics
point particles
24. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
electrolytic cells
valence
pressure
specific heat
25. The change in enthalpy of an exothermic reaction is ________.
equation of state
sublimation
negative
system (thermodynamics)
26. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
dynamic equilibrium
hybridyzation
electronegativity
cathode rays
27. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
VSEPR
equilibrium
reversible reaction
anode rays
28. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
...
lower left corner
moles (Le Chatelier's principle)
dynamic equilibrium
29. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
reversible reaction
...
single replacement/displacement
pressure
30. *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
Van der Waals
cathode rays
valence
31. Heat added to a system and work done by a system are considered _________ quantities.
Raoults law
hydrolysis
anode rays
positive
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.
saturated solution
Daltons law
system (thermodynamics)
titration
33. The most active metals are found in what corner of the periodic table?
Van der Waals
system (thermodynamics)
lower left corner
positive
34. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
Charles law
10 degrees
upper right corner
system (thermodynamics)
35. *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.
...
Le Chatelier's principle
decreases
hybridyzation
36. Deviations from Boyles law that occur with real gases represent _______ behavior.
bohr model
non-ideal
Nernst equation
increases
37. 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
state (thermodynamics)
Avogrados law
increasing
irreversible and reversible processes
38. 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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39. When an electron moves from an excited state to the ground state - it _______ energy.
single replacement/displacement
increasing
end point
emits (in atomic spectra)
40. The change in enthalpy of an endothermic reaction is ________.
enthalpy
positive
ideal gas
crystallizes
41. **Proceeding across a period from left to right - the ionization energy _______.
increases
ionization energy
activation energy barrier (Le Chatelier's principle)
end point
42. 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
lower left corner
cathode rays
activation energy barrier (Le Chatelier's principle)
43. 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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44. 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.
zero
colligative property law
electronegativity
Van der Waals
45. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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46. Rays made up of positive electrodes in basic electron charges.
anode rays
positive
Avogrados law
...
47. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
increases
decomposition
vapor pressure
temperature
48. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
activation energy barrier (Le Chatelier's principle)
hybridyzation
boiling point
49. In an endothermic process - energy is absorbed and ^E is _______.
increases
Le Chatelier's principle
moles (Le Chatelier's principle)
positive
50. The heat change during a process carried out at a constant pressure.
state (thermodynamics)
change in enthalpy
boiling point
state functions (thermodynamics)
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