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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. 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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2. When the electron moves from the ground state to an excited state - it ______ energy.
end point
absorbs (in atomic spectra)
cathode rays
decreases
3. *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.
lower left corner
decomposition
wave mechanical model
pi bonds
4. A hypothetical gas would follow Boyles law under all conditions and is called?
crystallizes
lower left corner
increases
ideal gas
5. 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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6. The action of salts of weak acids or bases with water to form acidic or basic solutions.
entropy
hydrolysis
Van der Waals
dynamic equilibrium
7. 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.
entropy
Raoults law
reversible reaction
first law of thermodynamics
8. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
freezing point depression
electrolytic reactions
Avogrados law
...
9. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
melting point
decreases
vapor pressure
...
10. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
combination
second law of thermodynamics
Avogrados law
dynamic equilibrium
11. This process occurs when the system is maintained at the same temperature throughout an experiment.
emits (in atomic spectra)
isothermal process (thermodynamics)
non-ideal
hydrolysis
12. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
high
system (thermodynamics)
crystallizes
13. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
electromotive force (emf)/ cell
increases
specific heat
second law of thermodynamics
14. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
melting point
point particles
...
moles (Le Chatelier's principle)
15. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
freezing point depression
positive
end point
16. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).
left - right (Le Chatelier's principle)
equilibrium
...
Van der Waals
17. 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
partial
isopiestic process (thermodynamics)
positive
18. This process occurs when the system is thermally isolated so that no heat enters or leaves.
double replacement/displacement
vapor pressure
kinetic molecular theory
adiabatic process (thermodynamics)
19. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
Van der Waals
Raoults law
...
20. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
double replacement/displacement
Raoults law
increasing
21. In titration - this is the point at which a particular indicator changes color.
Van der Waals
specific heat
end point
boiling point
22. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
wave mechanical model
combination
standard atmospheric pressure
Van der Waals
23. 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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24. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
right (Le Chatelier's principle)
crystallizes
Charles law
25. Heat added to a system and work done by a system are considered _________ quantities.
isopiestic process (thermodynamics)
increases
increasing
positive
26. *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.
negative
increases
10 degrees
equation of state
27. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
emits (in atomic spectra)
system (thermodynamics)
increasing
ideal gas
28. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
combined gas law
negative
kinetic molecular theory
activation energy
29. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
10 degrees
double replacement/displacement
entropy
30. In an exothermic process - energy is released and ^E of reaction is ________.
state functions (thermodynamics)
first law of thermodynamics
colligative property law
negative
31. A solution in which solid solute is in equilibrium with dissolved solute.
increases
kinetic molecular theory
crystallizes
saturated solution
32. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
titration
kinetic molecular theory
molar heat of sublimation
change in enthalpy
33. The heat change during a process carried out at a constant pressure.
combination
negative
change in enthalpy
metallic
34. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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35. Electronegativities ________ from left to right in a period.
increases
Raoults law
right (Le Chatelier's principle)
positive
36. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
equation of state
limiting law
standard atmospheric pressure
kinetic molecular theory
37. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
activation energy
crystallizes
electrolytic reactions
kinetic molecular theory
38. 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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39. Liquids with strong attractive forces have ______ boiling points.
vapor pressure
high
equivalent point
bohr model
40. 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.
isopiestic process (thermodynamics)
Nernst equation
electronegativity
single replacement/displacement
41. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
left (Le Chatelier's principle)
positive charge
kinetic molecular theory
Nernst equation
42. 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.
state functions (thermodynamics)
electronegativity
reversible
...
43. 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)
positive
boiling point
44. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
positive charge
Charles law
standard atmospheric pressure
boiling point
45. 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.
electronegativity
Charles law
Daltons law
high
46. 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
single replacement/displacement
colligative property law
bohr model
electromotive force (emf)/ cell
47. The energy required to remove an electron from an isolated atom in its ground state.
ionization energy
sublimation
...
specific heat
48. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
Daltons law
molar heat of sublimation
Boyles law
49. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
freezing point depression
point particles
pressure
Charles law
50. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
reversible
electrolytic reactions
Nernst equation