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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 law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
valence
wave mechanical model
anode rays
Charles law
2. A process that occurs whent eh system is maintained at constant pressure.
upper right corner
...
isopiestic process (thermodynamics)
Boyles law
3. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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4. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
cathode rays
kinetic molecular theory
decreases
hybridyzation
5. 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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6. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Avogrados law
wave mechanical model
increases
reversible
7. 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.
Van der Waals
pi bonds
Raoults law
increasing
8. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
bohr model
negative
activation energy barrier (Le Chatelier's principle)
9. 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
zero
bohr model
ideal gas
Van der Waals
10. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
melting point
sublimation
reversible
point particles
11. The temperature at which a substance's solid and liquid phases are in equilibrium.
standard atmospheric pressure
Le Chatelier's principle
...
melting point
12. 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
hydrolysis
non-ideal
left - right (Le Chatelier's principle)
13. When the electron moves from the ground state to an excited state - it ______ energy.
metallic
electromotive force (emf)/ cell
activation energy
absorbs (in atomic spectra)
14. 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.
kinetic molecular theory
isopiestic process (thermodynamics)
first law of thermodynamics
anode rays
15. The energy required to remove an electron from an isolated atom in its ground state.
wave mechanical model
ionization energy
positive charge
valence
16. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
electronegativity
base - acid
Boyles law
17. Electronegativities _______ as you go down a group.
single replacement/displacement
decomposition
electromotive force (emf)/ cell
decreases
18. A chemical reaction formed from the union of its elements.
combination
moles (Le Chatelier's principle)
colligative property law
vapor pressure
19. 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 _____ _
boiling point
combined gas law
limiting law
hybridyzation
20. 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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21. 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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22. Metals have electronegativities less than ____
2
emits (in atomic spectra)
phase equilibrium
Charles law
23. Heat added to a system and work done by a system are considered _________ quantities.
limiting law
decomposition
first law of thermodynamics
positive
24. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
kinetic molecular theory
Nernst equation
ideal gas
increasing
25. Liquids with strong attractive forces have ______ boiling points.
high
left (Le Chatelier's principle)
moles (Le Chatelier's principle)
irreversible and reversible processes
26. Rays made up of electrons in basic electron charges.
decomposition
cathode rays
zero
emits (in atomic spectra)
27. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
Van der Waals
crystallizes
colligative property law
decreases
28. **Proceeding across a period from left to right - the ionization energy _______.
increases
point particles
entropy
electrolytic reactions
29. 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.
catalysts
equilibrium
wave mechanical model
zero
30. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
decreases
zero
Avogrados law
31. 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.
titration
state functions (thermodynamics)
decreases
Charles law
32. In an exothermic process - energy is released and ^E of reaction is ________.
emits (in atomic spectra)
reversible
left - right (Le Chatelier's principle)
negative
33. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
Le Chatelier's principle
negative
pressure
34. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
crystallizes
Boyles law
freezing point depression
anode rays
35. 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
upper right corner
Boyles law
left (Le Chatelier's principle)
36. Cells that convert electrical energy into chemical energy.
pressure
pi bonds
molar heat of sublimation
electrolytic cells
37. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
isothermal process (thermodynamics)
decreases
boiling point
catalysts
38. A state function in which it is the heat content of a substance.
activation energy barrier (Le Chatelier's principle)
enthalpy
zero
isothermal process (thermodynamics)
39. The change in enthalpy of an endothermic reaction is ________.
boiling point elevation
positive
vapor pressure
moles (Le Chatelier's principle)
40. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
sublimation
heat capacity
cathode rays
moles (Le Chatelier's principle)
41. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
partial
non-ideal
combined gas law
boiling point elevation
42. The action of salts of weak acids or bases with water to form acidic or basic solutions.
moles (Le Chatelier's principle)
hydrolysis
electrolytic reactions
Boyles law
43. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
boiling point
Le Chatelier's principle
entropy
kinetic molecular theory
44. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
hybridyzation
Charles law
kinetic molecular theory
decomposition
45. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
kinetic molecular theory
...
hybridyzation
46. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
system (thermodynamics)
kinetic molecular theory
wave mechanical model
total pressure (Le Chatelier's principle)
47. 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
heats of formation
reversible reaction
vapor pressure
48. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
heat capacity
Raoult's law
electrolytic cells
...
49. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
vapor pressure
...
increases
state (thermodynamics)
50. The most active nonmetals are found in what corner of the periodic table?
saturated solution
point particles
upper right corner
system (thermodynamics)