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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 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
Charles law
Raoult's law
Valence Shell Electron Pair Repulsion (VSEPR)
2. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
pi bonds
specific heat
system (thermodynamics)
3. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
...
moles (Le Chatelier's principle)
kinetic molecular theory
Van der Waals
4. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
decomposition
heats of formation
freezing point depression
Charles law
5. 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.
isothermal process (thermodynamics)
adiabatic process (thermodynamics)
molar heat of sublimation
reversible
6. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
enthalpy
specific heat
entropy
decomposition
7. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
decomposition
system (thermodynamics)
temperature
decreases
8. The change in enthalpy of an exothermic reaction is ________.
negative
kinetic molecular theory
moles (Le Chatelier's principle)
pi bonds
9. *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.
end point
increases
base - acid
wave mechanical model
10. 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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11. 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.
equilibrium
Le Chatelier's principle
left - right (Le Chatelier's principle)
Charles law
12. Rays made up of positive electrodes in basic electron charges.
anode rays
increases
irreversible and reversible processes
Charles law
13. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
pressure
crystallizes
electromotive force (emf)/ cell
positive charge
14. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
hydrolysis
Van der Waals
metallic
positive
15. A hypothetical gas would follow Boyles law under all conditions and is called?
2
positive
ideal gas
vapor pressure
16. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
combination
activation energy
isothermal process (thermodynamics)
specific heat
17. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
Raoults law
boiling point elevation
increases
crystallizes
18. The vapor pressure increases with increasing _____.
pressure
temperature
state functions (thermodynamics)
partial
19. Cells that convert electrical energy into chemical energy.
second law of thermodynamics
Boyles law
equivalent point
electrolytic cells
20. 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
partial
melting point
isopiestic process (thermodynamics)
21. 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.
enthalpy
...
titration
ionization energy
22. The molecules in a gas are in constant - continueous - random - and straight-line motion.
reversible reaction
catalysts
dynamic equilibrium
kinetic molecular theory
23. A state function in which it is the heat content of a substance.
isopiestic process (thermodynamics)
left - right (Le Chatelier's principle)
emits (in atomic spectra)
enthalpy
24. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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25. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
...
combined gas law
equilibrium
26. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
combined gas law
kinetic molecular theory
phase equilibrium
boiling point
27. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
equilibrium
heats of formation
negative
Raoults law
28. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
right (Le Chatelier's principle)
reversible reaction
Daltons law
Boyles law
29. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
high
boiling point elevation
limiting law
increasing
30. 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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31. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
electrolytic reactions
double replacement/displacement
high
cathode rays
32. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
change in enthalpy
decomposition
melting point
crystallizes
33. 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
partial
second law of thermodynamics
phase equilibrium
34. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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35. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
partial
standard atmospheric pressure
saturated solution
combination
36. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
Daltons law
...
positive
37. 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).
double replacement/displacement
isothermal process (thermodynamics)
pi bonds
state (thermodynamics)
38. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
first law of thermodynamics
second law of thermodynamics
emits (in atomic spectra)
electrolytic reactions
39. The most active metals are found in what corner of the periodic table?
increasing
lower left corner
equation of state
kinetic molecular theory
40. The change in enthalpy of an endothermic reaction is ________.
activation energy barrier (Le Chatelier's principle)
electrolytic cells
kinetic molecular theory
positive
41. 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.
reversible reaction
positive
electronegativity
saturated solution
42. The pressure exerted by each gas in a mixture is called its _____ pressure.
electrolytic cells
Daltons law
partial
kinetic molecular theory
43. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
high
cathode rays
positive charge
Nernst equation
44. *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.
...
left - right (Le Chatelier's principle)
non-ideal
kinetic molecular theory
45. Metals have electronegativities less than ____
second law of thermodynamics
point particles
2
Daltons law
46. The heat required to change 1mole of solid completely to vapor.
kinetic molecular theory
high
molar heat of sublimation
first law of thermodynamics
47. When an electron moves from an excited state to the ground state - it _______ energy.
Boyles law
Nernst equation
emits (in atomic spectra)
kinetic molecular theory
48. 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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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.
ionization energy
...
Daltons law
kinetic molecular theory
50. 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
hybridyzation
third law of thermodynamics
boiling point