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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. 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)
state (thermodynamics)
hydrolysis
valence
2. 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.
entropy
Le Chatelier's principle
colligative property law
wave mechanical model
3. Cells that convert electrical energy into chemical energy.
electrolytic cells
Van der Waals
positive
electrolytic reactions
4. In an endothermic process - energy is absorbed and ^E is _______.
titration
state (thermodynamics)
temperature
positive
5. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
entropy
partial
specific heat
freezing point depression
6. Liquids with strong attractive forces have ______ boiling points.
high
change in enthalpy
molar heat of sublimation
Charles law
7. 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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8. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
cathode rays
increases
Daltons law
Nernst equation
9. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
heats of formation
Van der Waals
boiling point
10. The heat change during a process carried out at a constant pressure.
bohr model
third law of thermodynamics
metallic
change in enthalpy
11. 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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12. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
Valence Shell Electron Pair Repulsion (VSEPR)
positive charge
entropy
hybridyzation
13. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
activation energy barrier (Le Chatelier's principle)
kinetic molecular theory
ionization energy
10 degrees
14. Electronegativities _______ as you go down a group.
single replacement/displacement
decreases
electromotive force (emf)/ cell
Van der Waals
15. 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.
Raoults law
anode rays
Van der Waals
dynamic equilibrium
16. The action of salts of weak acids or bases with water to form acidic or basic solutions.
decreases
hydrolysis
decomposition
standard atmospheric pressure
17. 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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18. *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.
...
boiling point
adiabatic process (thermodynamics)
standard atmospheric pressure
19. 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).
Van der Waals
state (thermodynamics)
electrolytic cells
electrolytic reactions
20. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
base - acid
kinetic molecular theory
heats of formation
double replacement/displacement
21. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
limiting law
increases
kinetic molecular theory
22. The change in enthalpy of an exothermic reaction is ________.
negative
metallic
standard atmospheric pressure
colligative property law
23. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
boiling point elevation
colligative property law
combination
decreases
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.
decreases
partial
system (thermodynamics)
catalysts
25. The freezing point is always lowered by addition of solute.
equilibrium
negative
freezing point depression
activation energy barrier (Le Chatelier's principle)
26. 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.
kinetic molecular theory
electronegativity
decreases
Daltons law
27. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
pressure
kinetic molecular theory
metallic
negative
28. 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
base - acid
titration
absorbs (in atomic spectra)
29. The most active nonmetals are found in what corner of the periodic table?
state functions (thermodynamics)
activation energy barrier (Le Chatelier's principle)
upper right corner
wave mechanical model
30. Electronegativities ________ from left to right in a period.
negative
increases
decreases
Daltons law
31. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
...
2
enthalpy
decreases
32. The change in enthalpy of an endothermic reaction is ________.
increasing
single replacement/displacement
absorbs (in atomic spectra)
positive
33. Heat added to a system and work done by a system are considered _________ quantities.
increases
standard atmospheric pressure
Van der Waals
positive
34. A process that occurs whent eh system is maintained at constant pressure.
activation energy barrier (Le Chatelier's principle)
Daltons law
specific heat
isopiestic process (thermodynamics)
35. A chemical reaction formed from the union of its elements.
standard atmospheric pressure
heats of formation
positive
combination
36. 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
increasing
colligative property law
first law of thermodynamics
irreversible and reversible processes
37. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
heat capacity
positive
double replacement/displacement
boiling point
38. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
base - acid
vapor pressure
dynamic equilibrium
bohr model
39. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
electrolytic cells
zero
combination
activation energy barrier (Le Chatelier's principle)
40. 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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41. In titration - this is the point at which a particular indicator changes color.
upper right corner
crystallizes
end point
...
42. The molecules in a gas are in constant - continueous - random - and straight-line motion.
lower left corner
boiling point
Van der Waals
kinetic molecular theory
43. A solution in which solid solute is in equilibrium with dissolved solute.
total pressure (Le Chatelier's principle)
third law of thermodynamics
zero
saturated solution
44. 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
enthalpy
hybridyzation
increases
45. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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46. A hypothetical gas would follow Boyles law under all conditions and is called?
ideal gas
boiling point
positive
phase equilibrium
47. Deviations from Boyles law that occur with real gases represent _______ behavior.
pi bonds
increases
non-ideal
Raoults law
48. 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
...
positive charge
sublimation
Van der Waals
49. Metals have electronegativities less than ____
2
negative
partial
high
50. When the rate of evaporation equals the rate of condensation - the system is in __________.
decreases
Valence Shell Electron Pair Repulsion (VSEPR)
positive charge
equilibrium