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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 the electron moves from the ground state to an excited state - it ______ energy.
partial
catalysts
kinetic molecular theory
absorbs (in atomic spectra)
2. 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
equation of state
irreversible and reversible processes
decreases
3. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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4. 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).
state (thermodynamics)
increasing
activation energy
enthalpy
5. 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)
second law of thermodynamics
third law of thermodynamics
pi bonds
6. This process occurs when the system is thermally isolated so that no heat enters or leaves.
reversible reaction
base - acid
second law of thermodynamics
adiabatic process (thermodynamics)
7. A hypothetical gas would follow Boyles law under all conditions and is called?
ideal gas
negative
temperature
2
8. The heat change during a process carried out at a constant pressure.
Avogrados law
change in enthalpy
titration
Charles law
9. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
colligative property law
negative
vapor pressure
increasing
10. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Van der Waals
boiling point
equation of state
Charles law
11. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
equivalent point
crystallizes
Avogrados law
phase equilibrium
12. *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.
equation of state
state functions (thermodynamics)
wave mechanical model
boiling point
13. **Proceeding across a period from left to right - the ionization energy _______.
specific heat
Daltons law
increases
single replacement/displacement
14. 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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15. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
vapor pressure
kinetic molecular theory
heat capacity
total pressure (Le Chatelier's principle)
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).
positive
Van der Waals
combined gas law
temperature
17. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
lower left corner
...
second law of thermodynamics
bohr model
18. In an exothermic process - energy is released and ^E of reaction is ________.
negative
freezing point depression
Van der Waals
titration
19. A state function in which it is the heat content of a substance.
...
enthalpy
kinetic molecular theory
change in enthalpy
20. *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.
positive
equation of state
base - acid
left (Le Chatelier's principle)
21. This process occurs when the system is maintained at the same temperature throughout an experiment.
second law of thermodynamics
increases
positive charge
isothermal process (thermodynamics)
22. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
metallic
Van der Waals
boiling point
valence
23. **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.
Avogrados law
...
increases
positive
24. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
hybridyzation
crystallizes
kinetic molecular theory
entropy
25. When the rate of evaporation equals the rate of condensation - the system is in __________.
anode rays
vapor pressure
equilibrium
kinetic molecular theory
26. The most active metals are found in what corner of the periodic table?
decreases
lower left corner
kinetic molecular theory
enthalpy
27. The change in enthalpy of an exothermic reaction is ________.
positive
decreases
kinetic molecular theory
negative
28. The temperature at which a substance's solid and liquid phases are in equilibrium.
Valence Shell Electron Pair Repulsion (VSEPR)
melting point
reversible reaction
catalysts
29. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
isopiestic process (thermodynamics)
positive charge
combination
30. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
increases
combined gas law
electrolytic reactions
isopiestic process (thermodynamics)
31. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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32. 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
second law of thermodynamics
titration
moles (Le Chatelier's principle)
positive charge
33. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
point particles
equivalent point
system (thermodynamics)
boiling point
34. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
positive
dynamic equilibrium
end point
decreases
35. The vapor pressure increases with increasing _____.
metallic
Charles law
combined gas law
temperature
36. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
enthalpy
ionization energy
activation energy barrier (Le Chatelier's principle)
zero
37. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
electromotive force (emf)/ cell
pressure
decreases
absorbs (in atomic spectra)
38. Rays made up of electrons in basic electron charges.
ideal gas
cathode rays
third law of thermodynamics
equilibrium
39. The pressure exerted by each gas in a mixture is called its _____ pressure.
reversible
partial
pi bonds
titration
40. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
right (Le Chatelier's principle)
cathode rays
ionization energy
41. 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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42. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
electrolytic cells
single replacement/displacement
metallic
first law of thermodynamics
43. Electronegativities _______ as you go down a group.
decreases
Van der Waals
reversible reaction
pi bonds
44. The heat required to change 1mole of solid completely to vapor.
...
molar heat of sublimation
Le Chatelier's principle
single replacement/displacement
45. 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.
right (Le Chatelier's principle)
Valence Shell Electron Pair Repulsion (VSEPR)
electromotive force (emf)/ cell
negative
46. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
Charles law
Van der Waals
boiling point elevation
47. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
Le Chatelier's principle
Charles law
Nernst equation
48. Deviations from Boyles law that occur with real gases represent _______ behavior.
electronegativity
non-ideal
Boyles law
hybridyzation
49. Electronegativities ________ from left to right in a period.
negative
Charles law
specific heat
increases
50. 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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