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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. *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
...
2
valence
electromotive force (emf)/ cell
2. 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.
kinetic molecular theory
melting point
Van der Waals
phase equilibrium
3. 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).
reversible reaction
electrolytic reactions
wave mechanical model
Van der Waals
4. 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.
Daltons law
VSEPR
first law of thermodynamics
Charles law
5. The change in enthalpy of an endothermic reaction is ________.
kinetic molecular theory
total pressure (Le Chatelier's principle)
positive
ionization energy
6. 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.
Daltons law
positive
pi bonds
isopiestic process (thermodynamics)
7. The temperature at which a substance's solid and liquid phases are in equilibrium.
metallic
base - acid
melting point
increases
8. The change in enthalpy of an exothermic reaction is ________.
molar heat of sublimation
negative
isopiestic process (thermodynamics)
equation of state
9. *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.
negative
wave mechanical model
electronegativity
Boyles law
10. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
temperature
activation energy barrier (Le Chatelier's principle)
moles (Le Chatelier's principle)
11. 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.
positive charge
kinetic molecular theory
Van der Waals
Daltons law
12. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
third law of thermodynamics
increases
ideal gas
13. This process occurs when the system is maintained at the same temperature throughout an experiment.
positive charge
decreases
isothermal process (thermodynamics)
boiling point
14. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
zero
dynamic equilibrium
point particles
equivalent point
15. When the rate of evaporation equals the rate of condensation - the system is in __________.
system (thermodynamics)
third law of thermodynamics
equilibrium
Van der Waals
16. **Proceeding across a period from left to right - the ionization energy _______.
partial
increases
catalysts
double replacement/displacement
17. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
metallic
saturated solution
negative
18. Deviations from Boyles law that occur with real gases represent _______ behavior.
Valence Shell Electron Pair Repulsion (VSEPR)
non-ideal
metallic
kinetic molecular theory
19. 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
negative
Raoults law
electronegativity
irreversible and reversible processes
20. 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.
...
bohr model
equivalent point
temperature
21. The action of salts of weak acids or bases with water to form acidic or basic solutions.
cathode rays
increases
hydrolysis
equilibrium
22. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
catalysts
Charles law
heats of formation
equivalent point
23. Rays made up of electrons in basic electron charges.
...
...
Raoult's law
cathode rays
24. 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.
...
single replacement/displacement
Le Chatelier's principle
catalysts
25. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.
freezing point depression
Le Chatelier's principle
pi bonds
Charles law
26. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
kinetic molecular theory
10 degrees
bohr model
kinetic molecular theory
27. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
melting point
end point
decreases
Boyles law
28. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
metallic
2
decreases
Avogrados law
29. Electronegativities _______ as you go down a group.
valence
base - acid
...
decreases
30. _____ bonds are present in molecules containing double or triple bonds.
heats of formation
pi bonds
entropy
Charles law
31. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
electrolytic cells
Le Chatelier's principle
double replacement/displacement
decreases
32. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
metallic
double replacement/displacement
temperature
33. 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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34. 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 _____ _
increasing
Avogrados law
limiting law
decreases
35. The heat required to change 1mole of solid completely to vapor.
Valence Shell Electron Pair Repulsion (VSEPR)
molar heat of sublimation
freezing point depression
Van der Waals
36. 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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37. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
negative
Nernst equation
end point
decreases
38. The most active metals are found in what corner of the periodic table?
positive
lower left corner
VSEPR
boiling point elevation
39. The most active nonmetals are found in what corner of the periodic table?
equilibrium
state (thermodynamics)
upper right corner
absorbs (in atomic spectra)
40. Rays made up of positive electrodes in basic electron charges.
anode rays
titration
Nernst equation
specific heat
41. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
VSEPR
left - right (Le Chatelier's principle)
crystallizes
vapor pressure
42. The vapor pressure increases with increasing _____.
temperature
pressure
second law of thermodynamics
Charles law
43. Heat added to a system and work done by a system are considered _________ quantities.
entropy
Raoults law
heat capacity
positive
44. *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.
moles (Le Chatelier's principle)
equation of state
sublimation
ideal gas
45. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
10 degrees
Nernst equation
Boyles law
change in enthalpy
46. A chemical reaction formed from the union of its elements.
standard atmospheric pressure
combination
decomposition
VSEPR
47. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
metallic
kinetic molecular theory
boiling point
decreases
48. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
end point
Van der Waals
third law of thermodynamics
positive
49. In an endothermic process - energy is absorbed and ^E is _______.
positive
heat capacity
activation energy barrier (Le Chatelier's principle)
decreases
50. In an exothermic process - energy is released and ^E of reaction is ________.
kinetic molecular theory
upper right corner
negative
positive