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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 molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
third law of thermodynamics
freezing point depression
kinetic molecular theory
negative
2. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
pressure
wave mechanical model
boiling point elevation
entropy
3. A chemical reaction formed from the union of its elements.
Raoults law
hydrolysis
combination
catalysts
4. Metals have electronegativities less than ____
reversible
Van der Waals
2
single replacement/displacement
5. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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6. The most active metals are found in what corner of the periodic table?
heats of formation
Le Chatelier's principle
lower left corner
first law of thermodynamics
7. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
increases
hydrolysis
decreases
adiabatic process (thermodynamics)
8. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
hydrolysis
Van der Waals
kinetic molecular theory
9. 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)
...
Raoults law
crystallizes
10. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
partial
base - acid
positive
increasing
11. The heat change during a process carried out at a constant pressure.
change in enthalpy
equilibrium
activation energy barrier (Le Chatelier's principle)
Avogrados law
12. 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.
end point
valence
kinetic molecular theory
limiting law
13. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
Boyles law
phase equilibrium
...
equivalent point
14. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.
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15. *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.
Raoults law
...
double replacement/displacement
catalysts
16. A state function in which it is the heat content of a substance.
Nernst equation
melting point
enthalpy
...
17. When the rate of evaporation equals the rate of condensation - the system is in __________.
state functions (thermodynamics)
high
equilibrium
temperature
18. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
increases
...
Van der Waals
crystallizes
19. Deviations from Boyles law that occur with real gases represent _______ behavior.
Le Chatelier's principle
isopiestic process (thermodynamics)
non-ideal
increases
20. 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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21. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
hybridyzation
kinetic molecular theory
double replacement/displacement
Nernst equation
22. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
Van der Waals
base - acid
third law of thermodynamics
23. 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).
bohr model
lower left corner
Van der Waals
Le Chatelier's principle
24. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
combination
boiling point
kinetic molecular theory
reversible reaction
25. 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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26. Rays made up of positive electrodes in basic electron charges.
equation of state
anode rays
increases
decreases
27. The freezing point is always lowered by addition of solute.
freezing point depression
left - right (Le Chatelier's principle)
kinetic molecular theory
colligative property law
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.
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29. The pressure exerted by each gas in a mixture is called its _____ pressure.
third law of thermodynamics
decreases
decomposition
partial
30. *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
valence
10 degrees
negative
double replacement/displacement
31. **Proceeding across a period from left to right - the ionization energy _______.
metallic
standard atmospheric pressure
specific heat
increases
32. The change in enthalpy of an exothermic reaction is ________.
2
negative
third law of thermodynamics
Daltons law
33. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
combination
Charles law
hybridyzation
reversible
34. 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
VSEPR
increases
bohr model
specific heat
35. When an electron moves from an excited state to the ground state - it _______ energy.
specific heat
emits (in atomic spectra)
negative
Boyles law
36. Electronegativities _______ as you go down a group.
decreases
irreversible and reversible processes
...
heats of formation
37. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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38. 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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39. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
ideal gas
kinetic molecular theory
equation of state
40. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Raoults law
increasing
electrolytic reactions
increases
41. 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.
hybridyzation
hydrolysis
VSEPR
system (thermodynamics)
42. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
electrolytic reactions
positive charge
emits (in atomic spectra)
metallic
43. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
electrolytic cells
kinetic molecular theory
moles (Le Chatelier's principle)
absorbs (in atomic spectra)
44. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
single replacement/displacement
...
kinetic molecular theory
Van der Waals
45. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
freezing point depression
activation energy
Van der Waals
Le Chatelier's principle
46. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
moles (Le Chatelier's principle)
Boyles law
melting point
state (thermodynamics)
47. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
right (Le Chatelier's principle)
Charles law
positive charge
entropy
48. 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.
10 degrees
titration
non-ideal
activation energy
49. **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.
Van der Waals
Boyles law
...
equation of state
50. Liquids with strong attractive forces have ______ boiling points.
high
ideal gas
phase equilibrium
absorbs (in atomic spectra)