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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. 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.
equation of state
hydrolysis
equivalent point
Van der Waals
2. 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
saturated solution
high
Valence Shell Electron Pair Repulsion (VSEPR)
3. 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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4. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
positive
Van der Waals
boiling point
5. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
electromotive force (emf)/ cell
standard atmospheric pressure
phase equilibrium
Charles law
6. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
Raoult's law
titration
Van der Waals
7. In titration - this is the point at which a particular indicator changes color.
ideal gas
end point
cathode rays
equation of state
8. 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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9. The change in enthalpy of an exothermic reaction is ________.
left (Le Chatelier's principle)
negative
absorbs (in atomic spectra)
hydrolysis
10. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
crystallizes
bohr model
sublimation
electronegativity
11. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
state (thermodynamics)
sublimation
combination
boiling point
12. A solution in which solid solute is in equilibrium with dissolved solute.
valence
point particles
saturated solution
base - acid
13. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
VSEPR
kinetic molecular theory
increasing
isopiestic process (thermodynamics)
14. Liquids with strong attractive forces have ______ boiling points.
cathode rays
high
third law of thermodynamics
point particles
15. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
increases
third law of thermodynamics
phase equilibrium
16. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
high
left - right (Le Chatelier's principle)
Raoult's law
17. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
end point
vapor pressure
cathode rays
system (thermodynamics)
18. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
first law of thermodynamics
Valence Shell Electron Pair Repulsion (VSEPR)
bohr model
19. The energy required to remove an electron from an isolated atom in its ground state.
VSEPR
Daltons law
ionization energy
activation energy barrier (Le Chatelier's principle)
20. *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.
change in enthalpy
...
standard atmospheric pressure
metallic
21. Deviations from Boyles law that occur with real gases represent _______ behavior.
adiabatic process (thermodynamics)
ideal gas
absorbs (in atomic spectra)
non-ideal
22. This process occurs when the system is thermally isolated so that no heat enters or leaves.
ionization energy
equation of state
adiabatic process (thermodynamics)
increases
23. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
ideal gas
molar heat of sublimation
Avogrados law
point particles
24. 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
left - right (Le Chatelier's principle)
emits (in atomic spectra)
25. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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26. 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 _____ _
double replacement/displacement
limiting law
isothermal process (thermodynamics)
boiling point
27. *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.
Raoult's law
equation of state
positive
colligative property law
28. Rays made up of positive electrodes in basic electron charges.
anode rays
positive
kinetic molecular theory
Valence Shell Electron Pair Repulsion (VSEPR)
29. **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.
partial
combined gas law
reversible
...
30. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
bohr model
increases
state (thermodynamics)
kinetic molecular theory
31. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
equilibrium
Avogrados law
Van der Waals
10 degrees
32. In an endothermic process - energy is absorbed and ^E is _______.
Boyles law
combination
positive
Van der Waals
33. 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.
reversible
double replacement/displacement
lower left corner
combined gas law
34. In an exothermic process - energy is released and ^E of reaction is ________.
freezing point depression
sublimation
negative
catalysts
35. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
valence
negative
equilibrium
Charles law
36. The most active metals are found in what corner of the periodic table?
negative
lower left corner
pi bonds
kinetic molecular theory
37. Heat added to a system and work done by a system are considered _________ quantities.
anode rays
positive
10 degrees
titration
38. The temperature at which a substance's solid and liquid phases are in equilibrium.
irreversible and reversible processes
decomposition
...
melting point
39. *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
specific heat
valence
Daltons law
hydrolysis
40. 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.
first law of thermodynamics
absorbs (in atomic spectra)
catalysts
vapor pressure
41. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
melting point
negative
double replacement/displacement
equilibrium
42. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
bohr model
heat capacity
positive
Le Chatelier's principle
43. A state function in which it is the heat content of a substance.
irreversible and reversible processes
titration
melting point
enthalpy
44. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
increases
electrolytic reactions
second law of thermodynamics
pressure
45. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
activation energy
titration
upper right corner
zero
46. Electronegativities ________ from left to right in a period.
adiabatic process (thermodynamics)
phase equilibrium
hydrolysis
increases
47. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
Avogrados law
dynamic equilibrium
activation energy barrier (Le Chatelier's principle)
second law of thermodynamics
48. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
crystallizes
ideal gas
single replacement/displacement
49. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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50. 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
heats of formation
irreversible and reversible processes
kinetic molecular theory
heat capacity