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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. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
irreversible and reversible processes
double replacement/displacement
hybridyzation
electronegativity
2. **Proceeding across a period from left to right - the ionization energy _______.
irreversible and reversible processes
combined gas law
saturated solution
increases
3. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
Boyles law
combination
emits (in atomic spectra)
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.
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5. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
increasing
heat capacity
valence
Boyles law
6. 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.
end point
single replacement/displacement
Van der Waals
saturated solution
7. 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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8. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Valence Shell Electron Pair Repulsion (VSEPR)
wave mechanical model
heat capacity
equation of state
9. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
kinetic molecular theory
increasing
heats of formation
heat capacity
10. 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
saturated solution
electrolytic reactions
irreversible and reversible processes
isothermal process (thermodynamics)
11. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
standard atmospheric pressure
irreversible and reversible processes
kinetic molecular theory
12. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
increases
Daltons law
combined gas law
10 degrees
13. 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.
right (Le Chatelier's principle)
catalysts
...
kinetic molecular theory
14. In titration - this is the point at which a particular indicator changes color.
end point
left - right (Le Chatelier's principle)
cathode rays
isopiestic process (thermodynamics)
15. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
colligative property law
activation energy
electromotive force (emf)/ cell
Charles law
16. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
Valence Shell Electron Pair Repulsion (VSEPR)
left - right (Le Chatelier's principle)
reversible
specific heat
17. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
absorbs (in atomic spectra)
positive
melting point
crystallizes
18. The heat change during a process carried out at a constant pressure.
...
change in enthalpy
point particles
vapor pressure
19. The energy required to remove an electron from an isolated atom in its ground state.
positive
ionization energy
electromotive force (emf)/ cell
moles (Le Chatelier's principle)
20. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
vapor pressure
activation energy
increasing
21. 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).
phase equilibrium
state (thermodynamics)
positive
negative
22. This process occurs when the system is maintained at the same temperature throughout an experiment.
dynamic equilibrium
temperature
isothermal process (thermodynamics)
double replacement/displacement
23. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
partial
increasing
first law of thermodynamics
24. 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.
state functions (thermodynamics)
emits (in atomic spectra)
increases
VSEPR
25. In an exothermic process - energy is released and ^E of reaction is ________.
negative
third law of thermodynamics
double replacement/displacement
base - acid
26. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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27. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
specific heat
metallic
reversible
28. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
change in enthalpy
electrolytic reactions
decreases
zero
29. Electronegativities ________ from left to right in a period.
combination
base - acid
electrolytic cells
increases
30. When the rate of evaporation equals the rate of condensation - the system is in __________.
Boyles law
sublimation
equilibrium
hybridyzation
31. 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
change in enthalpy
...
kinetic molecular theory
32. Cells that convert electrical energy into chemical energy.
kinetic molecular theory
left - right (Le Chatelier's principle)
electrolytic cells
hydrolysis
33. **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.
catalysts
saturated solution
...
valence
34. The freezing point is always lowered by addition of solute.
heats of formation
phase equilibrium
equilibrium
freezing point depression
35. 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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36. The molecules in a gas are in constant - continueous - random - and straight-line motion.
reversible reaction
kinetic molecular theory
melting point
molar heat of sublimation
37. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
Avogrados law
cathode rays
vapor pressure
38. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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39. The most active metals are found in what corner of the periodic table?
third law of thermodynamics
lower left corner
equivalent point
Boyles law
40. *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.
...
double replacement/displacement
increases
non-ideal
41. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
standard atmospheric pressure
kinetic molecular theory
Van der Waals
partial
42. 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 _____ _
equation of state
melting point
kinetic molecular theory
limiting law
43. Rays made up of electrons in basic electron charges.
non-ideal
third law of thermodynamics
upper right corner
cathode rays
44. 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.
...
Daltons law
crystallizes
Charles law
45. Rays made up of positive electrodes in basic electron charges.
anode rays
kinetic molecular theory
catalysts
adiabatic process (thermodynamics)
46. Metals have electronegativities less than ____
single replacement/displacement
kinetic molecular theory
2
right (Le Chatelier's principle)
47. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
state functions (thermodynamics)
positive
combination
48. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
decreases
kinetic molecular theory
left - right (Le Chatelier's principle)
49. 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.
sublimation
pi bonds
heats of formation
first law of thermodynamics
50. Liquids with strong attractive forces have ______ boiling points.
upper right corner
high
negative
second law of thermodynamics