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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 a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
catalysts
decreases
dynamic equilibrium
left (Le Chatelier's principle)
2. 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).
Avogrados law
emits (in atomic spectra)
electronegativity
Van der Waals
3. This process occurs when the system is thermally isolated so that no heat enters or leaves.
specific heat
adiabatic process (thermodynamics)
wave mechanical model
activation energy
4. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.
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5. 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.
partial
increases
Charles law
Valence Shell Electron Pair Repulsion (VSEPR)
6. When the electron moves from the ground state to an excited state - it ______ energy.
decreases
emits (in atomic spectra)
pi bonds
absorbs (in atomic spectra)
7. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
isopiestic process (thermodynamics)
...
...
8. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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9. 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
point particles
heats of formation
isopiestic process (thermodynamics)
10. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
combination
reversible reaction
catalysts
absorbs (in atomic spectra)
11. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
increases
absorbs (in atomic spectra)
heat capacity
12. 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).
10 degrees
Raoults law
state (thermodynamics)
reversible reaction
13. 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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14. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
end point
sublimation
Le Chatelier's principle
boiling point
15. The most active nonmetals are found in what corner of the periodic table?
upper right corner
hybridyzation
...
increasing
16. Metals have electronegativities less than ____
vapor pressure
...
limiting law
2
17. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
combination
Nernst equation
absorbs (in atomic spectra)
boiling point elevation
18. 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.
increasing
melting point
base - acid
Daltons law
19. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
electronegativity
negative
double replacement/displacement
base - acid
20. In an exothermic process - energy is released and ^E of reaction is ________.
negative
emits (in atomic spectra)
upper right corner
specific heat
21. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
positive
...
emits (in atomic spectra)
kinetic molecular theory
22. Electronegativities _______ as you go down a group.
decreases
phase equilibrium
total pressure (Le Chatelier's principle)
vapor pressure
23. The temperature at which a substance's solid and liquid phases are in equilibrium.
specific heat
combination
upper right corner
melting point
24. *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
state (thermodynamics)
valence
saturated solution
electrolytic reactions
25. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
ionization energy
kinetic molecular theory
increasing
Avogrados law
26. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
Van der Waals
left - right (Le Chatelier's principle)
system (thermodynamics)
kinetic molecular theory
27. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
system (thermodynamics)
reversible reaction
decomposition
28. 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
boiling point
double replacement/displacement
irreversible and reversible processes
pressure
29. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
sublimation
Charles law
crystallizes
30. When the rate of evaporation equals the rate of condensation - the system is in __________.
high
equilibrium
right (Le Chatelier's principle)
electronegativity
31. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
melting point
Avogrados law
standard atmospheric pressure
negative
32. 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
wave mechanical model
Daltons law
crystallizes
33. 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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34. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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35. 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.
titration
point particles
partial
isothermal process (thermodynamics)
36. 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.
electromotive force (emf)/ cell
electronegativity
reversible
kinetic molecular theory
37. A solution in which solid solute is in equilibrium with dissolved solute.
colligative property law
activation energy barrier (Le Chatelier's principle)
saturated solution
entropy
38. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
wave mechanical model
boiling point
10 degrees
Daltons law
39. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
third law of thermodynamics
zero
decreases
negative
40. 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
state functions (thermodynamics)
left - right (Le Chatelier's principle)
Raoults law
41. 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.
left - right (Le Chatelier's principle)
equilibrium
sublimation
colligative property law
42. 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.
kinetic molecular theory
increases
saturated solution
titration
43. The change in enthalpy of an endothermic reaction is ________.
third law of thermodynamics
saturated solution
positive
...
44. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
...
system (thermodynamics)
...
single replacement/displacement
45. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
entropy
high
freezing point depression
46. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
first law of thermodynamics
heat capacity
Charles law
equilibrium
47. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
electrolytic cells
boiling point elevation
crystallizes
temperature
48. 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
titration
VSEPR
bohr model
49. The most active metals are found in what corner of the periodic table?
kinetic molecular theory
valence
lower left corner
2
50. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
Le Chatelier's principle
decreases
VSEPR
reversible reaction