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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. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge
freezing point depression
Avogrados law
combination
positive charge
2. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
...
Raoult's law
right (Le Chatelier's principle)
electromotive force (emf)/ cell
3. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
system (thermodynamics)
saturated solution
boiling point elevation
4. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
Charles law
reversible reaction
sublimation
activation energy
5. *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
bohr model
Van der Waals
change in enthalpy
valence
6. When the rate of evaporation equals the rate of condensation - the system is in __________.
zero
ionization energy
equilibrium
first law of thermodynamics
7. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
standard atmospheric pressure
system (thermodynamics)
kinetic molecular theory
8. 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.
Raoult's law
double replacement/displacement
increases
Raoults law
9. 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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10. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
saturated solution
crystallizes
Boyles law
single replacement/displacement
11. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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12. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
standard atmospheric pressure
electrolytic cells
phase equilibrium
13. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
non-ideal
irreversible and reversible processes
third law of thermodynamics
14. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
Nernst equation
metallic
reversible reaction
increases
15. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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16. 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).
left (Le Chatelier's principle)
state (thermodynamics)
equation of state
Van der Waals
17. 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.
first law of thermodynamics
kinetic molecular theory
molar heat of sublimation
Le Chatelier's principle
18. Cells that convert electrical energy into chemical energy.
electrolytic reactions
negative
melting point
electrolytic cells
19. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
high
specific heat
valence
positive
20. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
dynamic equilibrium
molar heat of sublimation
Charles law
21. Liquids with strong attractive forces have ______ boiling points.
hybridyzation
absorbs (in atomic spectra)
high
decreases
22. 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.
reversible
anode rays
kinetic molecular theory
Daltons law
23. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.
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24. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
double replacement/displacement
VSEPR
2
25. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
positive
Nernst equation
titration
26. 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
ideal gas
specific heat
double replacement/displacement
bohr model
27. A chemical reaction formed from the union of its elements.
combination
positive
dynamic equilibrium
electrolytic reactions
28. *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.
kinetic molecular theory
pi bonds
...
temperature
29. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
activation energy
heat capacity
phase equilibrium
electronegativity
30. Heat added to a system and work done by a system are considered _________ quantities.
Charles law
metallic
enthalpy
positive
31. 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.
decreases
kinetic molecular theory
sublimation
base - acid
32. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
heat capacity
reversible reaction
electrolytic reactions
...
33. 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.
colligative property law
equivalent point
equilibrium
pi bonds
34. When the electron moves from the ground state to an excited state - it ______ energy.
electrolytic reactions
absorbs (in atomic spectra)
specific heat
metallic
35. The most active metals are found in what corner of the periodic table?
boiling point
catalysts
lower left corner
cathode rays
36. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
pi bonds
isothermal process (thermodynamics)
equivalent point
37. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
Daltons law
negative
hybridyzation
combined gas law
38. 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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39. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
Raoult's law
specific heat
system (thermodynamics)
Le Chatelier's principle
40. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
base - acid
Boyles law
temperature
zero
41. 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.
ideal gas
Daltons law
positive
state functions (thermodynamics)
42. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
state (thermodynamics)
single replacement/displacement
kinetic molecular theory
partial
43. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
combined gas law
Daltons law
kinetic molecular theory
44. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
catalysts
isothermal process (thermodynamics)
...
saturated solution
45. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
valence
negative
second law of thermodynamics
46. 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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47. The pressure exerted by each gas in a mixture is called its _____ pressure.
10 degrees
crystallizes
Charles law
partial
48. The heat change during a process carried out at a constant pressure.
change in enthalpy
catalysts
Van der Waals
heat capacity
49. The energy required to remove an electron from an isolated atom in its ground state.
boiling point elevation
positive
ionization energy
isopiestic process (thermodynamics)
50. 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.
Van der Waals
10 degrees
emits (in atomic spectra)
base - acid