SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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 vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
increases
specific heat
boiling point elevation
Van der Waals
2. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
metallic
irreversible and reversible processes
boiling point elevation
third law of thermodynamics
3. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
emits (in atomic spectra)
sublimation
adiabatic process (thermodynamics)
4. 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
Van der Waals
combined gas law
Avogrados law
5. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Le Chatelier's principle
...
heat capacity
right (Le Chatelier's principle)
6. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
Valence Shell Electron Pair Repulsion (VSEPR)
Van der Waals
single replacement/displacement
increases
7. *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.
wave mechanical model
system (thermodynamics)
VSEPR
point particles
8. 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 _______.
9. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
kinetic molecular theory
entropy
increases
electrolytic reactions
10. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
valence
metallic
Nernst equation
11. 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
freezing point depression
kinetic molecular theory
adiabatic process (thermodynamics)
12. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
irreversible and reversible processes
Le Chatelier's principle
Boyles law
ionization energy
13. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
Le Chatelier's principle
temperature
vapor pressure
14. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
hydrolysis
first law of thermodynamics
specific heat
15. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
zero
limiting law
non-ideal
pressure
16. Electronegativities _______ as you go down a group.
limiting law
state (thermodynamics)
decreases
Valence Shell Electron Pair Repulsion (VSEPR)
17. In an endothermic process - energy is absorbed and ^E is _______.
change in enthalpy
increases
valence
positive
18. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
positive
...
increasing
double replacement/displacement
19. The temperature at which a substance's solid and liquid phases are in equilibrium.
total pressure (Le Chatelier's principle)
combination
melting point
double replacement/displacement
20. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
Nernst equation
left (Le Chatelier's principle)
partial
21. 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.
upper right corner
VSEPR
state functions (thermodynamics)
Le Chatelier's principle
22. A solution in which solid solute is in equilibrium with dissolved solute.
catalysts
saturated solution
standard atmospheric pressure
state functions (thermodynamics)
23. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
entropy
zero
activation energy
double replacement/displacement
24. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
Valence Shell Electron Pair Repulsion (VSEPR)
first law of thermodynamics
isothermal process (thermodynamics)
25. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
non-ideal
irreversible and reversible processes
vapor pressure
26. The most active metals are found in what corner of the periodic table?
lower left corner
end point
equation of state
electronegativity
27. Cells that convert electrical energy into chemical energy.
sublimation
Daltons law
2
electrolytic cells
28. 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.
29. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
ionization energy
Van der Waals
Charles law
equation of state
30. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
change in enthalpy
state (thermodynamics)
decreases
10 degrees
31. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
hybridyzation
limiting law
temperature
metallic
32. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
wave mechanical model
point particles
end point
double replacement/displacement
33. 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
Valence Shell Electron Pair Repulsion (VSEPR)
Daltons law
pi bonds
34. 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.
kinetic molecular theory
Le Chatelier's principle
electrolytic cells
bohr model
35. Electronegativities ________ from left to right in a period.
total pressure (Le Chatelier's principle)
adiabatic process (thermodynamics)
temperature
increases
36. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
Van der Waals
kinetic molecular theory
decomposition
standard atmospheric pressure
37. In an exothermic process - energy is released and ^E of reaction is ________.
electrolytic cells
negative
reversible
kinetic molecular theory
38. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
absorbs (in atomic spectra)
boiling point elevation
base - acid
limiting law
39. In titration - this is the point at which a particular indicator changes color.
irreversible and reversible processes
end point
partial
negative
40. 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
vapor pressure
equation of state
positive charge
zero
41. Rays made up of electrons in basic electron charges.
pi bonds
crystallizes
increasing
cathode rays
42. The vapor pressure increases with increasing _____.
temperature
first law of thermodynamics
base - acid
...
43. A process that occurs whent eh system is maintained at constant pressure.
decomposition
positive
isopiestic process (thermodynamics)
Boyles law
44. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
Le Chatelier's principle
vapor pressure
lower left corner
45. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
change in enthalpy
standard atmospheric pressure
boiling point
valence
46. _____ bonds are present in molecules containing double or triple bonds.
decomposition
...
kinetic molecular theory
pi bonds
47. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
kinetic molecular theory
phase equilibrium
negative
bohr model
48. 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.
49. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f
heat capacity
electromotive force (emf)/ cell
isopiestic process (thermodynamics)
bohr model
50. *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.
increasing
upper right corner
...
reversible