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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 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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2. The heat change during a process carried out at a constant pressure.
double replacement/displacement
standard atmospheric pressure
change in enthalpy
right (Le Chatelier's principle)
3. 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.
partial
freezing point depression
Valence Shell Electron Pair Repulsion (VSEPR)
phase equilibrium
4. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
point particles
partial
...
boiling point elevation
5. Heat added to a system and work done by a system are considered _________ quantities.
ideal gas
equation of state
Charles law
positive
6. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
Avogrados law
partial
kinetic molecular theory
7. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
saturated solution
boiling point elevation
boiling point
sublimation
8. Electronegativities _______ as you go down a group.
enthalpy
non-ideal
decreases
electrolytic cells
9. 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.
electronegativity
freezing point depression
absorbs (in atomic spectra)
dynamic equilibrium
10. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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11. 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
positive
Van der Waals
left - right (Le Chatelier's principle)
12. 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.
absorbs (in atomic spectra)
upper right corner
Van der Waals
sublimation
13. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Valence Shell Electron Pair Repulsion (VSEPR)
adiabatic process (thermodynamics)
Van der Waals
titration
14. *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
VSEPR
valence
bohr model
vapor pressure
15. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
heats of formation
Avogrados law
...
colligative property law
16. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
decomposition
ionization energy
equilibrium
17. 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.
phase equilibrium
state functions (thermodynamics)
first law of thermodynamics
Avogrados law
18. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
equivalent point
emits (in atomic spectra)
limiting law
19. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
kinetic molecular theory
electrolytic reactions
kinetic molecular theory
lower left corner
20. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
positive
absorbs (in atomic spectra)
base - acid
high
21. Liquids with strong attractive forces have ______ boiling points.
absorbs (in atomic spectra)
high
anode rays
Charles law
22. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
state (thermodynamics)
kinetic molecular theory
Boyles law
moles (Le Chatelier's principle)
23. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
enthalpy
reversible reaction
ideal gas
heats of formation
24. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
freezing point depression
Avogrados law
increases
25. 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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26. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
moles (Le Chatelier's principle)
pi bonds
increases
27. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
valence
heats of formation
metallic
28. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
base - acid
kinetic molecular theory
state (thermodynamics)
Van der Waals
29. The most active metals are found in what corner of the periodic table?
hybridyzation
lower left corner
...
kinetic molecular theory
30. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
kinetic molecular theory
crystallizes
...
31. 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 _______.
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32. 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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33. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
equation of state
decreases
wave mechanical model
crystallizes
34. The vapor pressure increases with increasing _____.
temperature
phase equilibrium
base - acid
equivalent point
35. Deviations from Boyles law that occur with real gases represent _______ behavior.
electrolytic reactions
Le Chatelier's principle
non-ideal
equilibrium
36. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
10 degrees
Boyles law
point particles
heat capacity
37. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
boiling point elevation
Nernst equation
dynamic equilibrium
ideal gas
38. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
2
increases
hydrolysis
...
39. The action of salts of weak acids or bases with water to form acidic or basic solutions.
adiabatic process (thermodynamics)
heats of formation
hydrolysis
equivalent point
40. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
combination
right (Le Chatelier's principle)
specific heat
electronegativity
41. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
base - acid
melting point
point particles
42. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
non-ideal
metallic
Valence Shell Electron Pair Repulsion (VSEPR)
heats of formation
43. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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44. 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.
specific heat
first law of thermodynamics
Le Chatelier's principle
10 degrees
45. In an exothermic process - energy is released and ^E of reaction is ________.
melting point
decreases
negative
positive charge
46. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
pressure
isopiestic process (thermodynamics)
kinetic molecular theory
47. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
Avogrados law
melting point
second law of thermodynamics
48. A hypothetical gas would follow Boyles law under all conditions and is called?
vapor pressure
change in enthalpy
ideal gas
decreases
49. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
increases
absorbs (in atomic spectra)
electrolytic cells
zero
50. 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.
bohr model
electromotive force (emf)/ cell
reversible reaction
Daltons law