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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 _____ 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.
increases
catalysts
zero
base - acid
2. *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.
kinetic molecular theory
increasing
anode rays
equation of state
3. The molecules in a gas are in constant - continueous - random - and straight-line motion.
Charles law
equilibrium
increases
kinetic molecular theory
4. The heat required to change 1mole of solid completely to vapor.
Boyles law
negative
adiabatic process (thermodynamics)
molar heat of sublimation
5. In an endothermic process - energy is absorbed and ^E is _______.
positive
increases
kinetic molecular theory
negative
6. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
state (thermodynamics)
boiling point
electromotive force (emf)/ cell
total pressure (Le Chatelier's principle)
7. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.
bohr model
colligative property law
VSEPR
end point
8. _____ bonds are present in molecules containing double or triple bonds.
limiting law
second law of thermodynamics
pi bonds
melting point
9. The change in enthalpy of an endothermic reaction is ________.
VSEPR
Charles law
positive
first law of thermodynamics
10. 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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11. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
kinetic molecular theory
colligative property law
melting point
equilibrium
12. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
kinetic molecular theory
positive
increasing
bohr model
13. *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
end point
bohr model
valence
Daltons law
14. 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.
Le Chatelier's principle
right (Le Chatelier's principle)
saturated solution
Valence Shell Electron Pair Repulsion (VSEPR)
15. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
lower left corner
isopiestic process (thermodynamics)
equivalent point
third law of thermodynamics
16. 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
combination
positive charge
...
17. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
electrolytic cells
emits (in atomic spectra)
adiabatic process (thermodynamics)
18. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
Le Chatelier's principle
decreases
crystallizes
pressure
19. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
...
combined gas law
double replacement/displacement
negative
20. 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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21. 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
irreversible and reversible processes
left - right (Le Chatelier's principle)
electronegativity
boiling point
22. A hypothetical gas would follow Boyles law under all conditions and is called?
double replacement/displacement
hybridyzation
ideal gas
dynamic equilibrium
23. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
kinetic molecular theory
kinetic molecular theory
colligative property law
24. In an exothermic process - energy is released and ^E of reaction is ________.
negative
vapor pressure
phase equilibrium
activation energy barrier (Le Chatelier's principle)
25. Liquids with strong attractive forces have ______ boiling points.
zero
high
non-ideal
standard atmospheric pressure
26. **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.
emits (in atomic spectra)
...
double replacement/displacement
Boyles law
27. 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.
increases
colligative property law
pressure
Valence Shell Electron Pair Repulsion (VSEPR)
28. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
Charles law
heats of formation
positive
electronegativity
29. A chemical reaction formed from the union of its elements.
activation energy barrier (Le Chatelier's principle)
combination
kinetic molecular theory
equivalent point
30. 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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31. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
isothermal process (thermodynamics)
sublimation
second law of thermodynamics
left - right (Le Chatelier's principle)
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
heat capacity
partial
positive charge
decreases
33. 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.
decreases
VSEPR
Van der Waals
catalysts
34. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
...
non-ideal
sublimation
10 degrees
35. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
kinetic molecular theory
colligative property law
10 degrees
vapor pressure
36. When an electron moves from an excited state to the ground state - it _______ energy.
right (Le Chatelier's principle)
state (thermodynamics)
emits (in atomic spectra)
entropy
37. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
kinetic molecular theory
negative
positive
38. 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)
total pressure (Le Chatelier's principle)
positive charge
Van der Waals
39. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
Charles law
combination
temperature
sublimation
40. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
specific heat
hydrolysis
Van der Waals
41. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
10 degrees
melting point
combined gas law
wave mechanical model
42. The freezing point is always lowered by addition of solute.
freezing point depression
dynamic equilibrium
change in enthalpy
left (Le Chatelier's principle)
43. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
positive
...
high
44. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
reversible reaction
VSEPR
crystallizes
45. Rays made up of positive electrodes in basic electron charges.
kinetic molecular theory
combination
colligative property law
anode rays
46. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
ideal gas
VSEPR
specific heat
dynamic equilibrium
47. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
limiting law
reversible reaction
system (thermodynamics)
48. 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.
bohr model
upper right corner
positive
Raoults law
49. The action of salts of weak acids or bases with water to form acidic or basic solutions.
equilibrium
high
right (Le Chatelier's principle)
hydrolysis
50. 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.
molar heat of sublimation
reversible reaction
first law of thermodynamics
hydrolysis