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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 normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
valence
electrolytic cells
partial
standard atmospheric pressure
2. The energy required to remove an electron from an isolated atom in its ground state.
dynamic equilibrium
ionization energy
2
positive
3. The change in enthalpy of an endothermic reaction is ________.
total pressure (Le Chatelier's principle)
freezing point depression
dynamic equilibrium
positive
4. 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.
5. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
positive
lower left corner
electrolytic reactions
left - right (Le Chatelier's principle)
6. 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.
boiling point elevation
VSEPR
cathode rays
activation energy barrier (Le Chatelier's principle)
7. 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 _____ _
Le Chatelier's principle
colligative property law
limiting law
equivalent point
8. 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).
increases
crystallizes
Van der Waals
point particles
9. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
lower left corner
right (Le Chatelier's principle)
freezing point depression
single replacement/displacement
10. 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.
electrolytic reactions
catalysts
Van der Waals
Valence Shell Electron Pair Repulsion (VSEPR)
11. The molecules in a gas are in constant - continueous - random - and straight-line motion.
base - acid
kinetic molecular theory
metallic
increases
12. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
titration
10 degrees
end point
Daltons law
13. Electronegativities ________ from left to right in a period.
end point
...
negative
increases
14. 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.
Raoult's law
wave mechanical model
decreases
state functions (thermodynamics)
15. In an exothermic process - energy is released and ^E of reaction is ________.
kinetic molecular theory
10 degrees
negative
positive
16. Heat added to a system and work done by a system are considered _________ quantities.
...
positive
moles (Le Chatelier's principle)
kinetic molecular theory
17. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
non-ideal
Boyles law
kinetic molecular theory
18. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
limiting law
equation of state
...
19. 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.
equivalent point
second law of thermodynamics
titration
left - right (Le Chatelier's principle)
20. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
state (thermodynamics)
saturated solution
negative
double replacement/displacement
21. Cells that convert electrical energy into chemical energy.
electrolytic cells
boiling point
decomposition
third law of thermodynamics
22. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
upper right corner
system (thermodynamics)
sublimation
left - right (Le Chatelier's principle)
23. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
limiting law
partial
positive
crystallizes
24. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
adiabatic process (thermodynamics)
partial
increases
25. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
upper right corner
state functions (thermodynamics)
electrolytic cells
Charles law
26. 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.
27. 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
Valence Shell Electron Pair Repulsion (VSEPR)
melting point
irreversible and reversible processes
28. The freezing point is always lowered by addition of solute.
wave mechanical model
...
total pressure (Le Chatelier's principle)
freezing point depression
29. Metals have electronegativities less than ____
positive
2
point particles
crystallizes
30. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
Le Chatelier's principle
state functions (thermodynamics)
increases
31. The heat required to change 1mole of solid completely to vapor.
crystallizes
absorbs (in atomic spectra)
change in enthalpy
molar heat of sublimation
32. A state function in which it is the heat content of a substance.
equilibrium
enthalpy
Boyles law
Charles law
33. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
upper right corner
Van der Waals
electrolytic cells
zero
34. 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.
Charles law
boiling point
heats of formation
positive
35. 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.
heat capacity
boiling point elevation
Valence Shell Electron Pair Repulsion (VSEPR)
standard atmospheric pressure
36. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
2
temperature
ideal gas
dynamic equilibrium
37. _____ bonds are present in molecules containing double or triple bonds.
emits (in atomic spectra)
third law of thermodynamics
pi bonds
Le Chatelier's principle
38. The vapor pressure increases with increasing _____.
positive
electronegativity
temperature
second law of thermodynamics
39. The change in enthalpy of an exothermic reaction is ________.
Raoult's law
Le Chatelier's principle
negative
titration
40. 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
standard atmospheric pressure
Charles law
upper right corner
41. In an endothermic process - energy is absorbed and ^E is _______.
second law of thermodynamics
activation energy barrier (Le Chatelier's principle)
Raoults law
positive
42. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
third law of thermodynamics
emits (in atomic spectra)
2
Avogrados law
43. The most active nonmetals are found in what corner of the periodic table?
upper right corner
high
Avogrados law
negative
44. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
combined gas law
ionization energy
phase equilibrium
melting point
45. This process occurs when the system is thermally isolated so that no heat enters or leaves.
titration
single replacement/displacement
adiabatic process (thermodynamics)
kinetic molecular theory
46. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
Charles law
sublimation
increases
47. **Proceeding across a period from left to right - the ionization energy _______.
adiabatic process (thermodynamics)
increases
Le Chatelier's principle
zero
48. 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
dynamic equilibrium
positive charge
activation energy
49. Rays made up of electrons in basic electron charges.
valence
kinetic molecular theory
lower left corner
cathode rays
50. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
upper right corner
boiling point elevation
wave mechanical model
decreases