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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. In an exothermic process - energy is released and ^E of reaction is ________.
high
negative
combined gas law
base - acid
2. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
...
combined gas law
left - right (Le Chatelier's principle)
activation energy barrier (Le Chatelier's principle)
3. 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.
Van der Waals
VSEPR
ionization energy
dynamic equilibrium
4. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
emits (in atomic spectra)
boiling point elevation
equivalent point
5. 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
bohr model
...
point particles
anode rays
6. 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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7. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
melting point
equilibrium
positive charge
entropy
8. Cells that convert electrical energy into chemical energy.
electrolytic cells
positive
electronegativity
third law of thermodynamics
9. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
catalysts
crystallizes
bohr model
cathode rays
10. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
valence
left (Le Chatelier's principle)
right (Le Chatelier's principle)
11. 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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12. Electronegativities ________ from left to right in a period.
molar heat of sublimation
temperature
kinetic molecular theory
increases
13. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
positive charge
increases
electronegativity
metallic
14. Heat added to a system and work done by a system are considered _________ quantities.
state functions (thermodynamics)
wave mechanical model
reversible reaction
positive
15. 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.
Charles law
colligative property law
irreversible and reversible processes
Daltons law
16. 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.
electrolytic reactions
base - acid
electronegativity
temperature
17. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
...
electrolytic cells
wave mechanical model
Van der Waals
18. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
sublimation
double replacement/displacement
vapor pressure
Charles law
19. 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.
kinetic molecular theory
system (thermodynamics)
Raoults law
activation energy barrier (Le Chatelier's principle)
20. 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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21. *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.
...
Avogrados law
high
reversible reaction
22. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
reversible
increases
phase equilibrium
standard atmospheric pressure
23. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.
heat capacity
colligative property law
emits (in atomic spectra)
Le Chatelier's principle
24. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
Charles law
system (thermodynamics)
negative
crystallizes
25. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
base - acid
kinetic molecular theory
state (thermodynamics)
increases
26. 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.
reversible
titration
left (Le Chatelier's principle)
boiling point elevation
27. In titration - this is the point at which a particular indicator changes color.
point particles
boiling point elevation
end point
kinetic molecular theory
28. Deviations from Boyles law that occur with real gases represent _______ behavior.
Van der Waals
boiling point
saturated solution
non-ideal
29. A state function in which it is the heat content of a substance.
valence
positive charge
Daltons law
enthalpy
30. Metals have electronegativities less than ____
Charles law
anode rays
combination
2
31. In an endothermic process - energy is absorbed and ^E is _______.
positive
limiting law
non-ideal
melting point
32. Liquids with strong attractive forces have ______ boiling points.
boiling point elevation
high
anode rays
saturated solution
33. The vapor pressure increases with increasing _____.
anode rays
Van der Waals
Van der Waals
temperature
34. A process that occurs whent eh system is maintained at constant pressure.
change in enthalpy
end point
isopiestic process (thermodynamics)
melting point
35. 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.
Daltons law
dynamic equilibrium
first law of thermodynamics
kinetic molecular theory
36. 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 _____ _
decomposition
equivalent point
limiting law
combination
37. When the rate of evaporation equals the rate of condensation - the system is in __________.
ideal gas
boiling point
bohr model
equilibrium
38. _____ bonds are present in molecules containing double or triple bonds.
decreases
pi bonds
negative
decreases
39. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
...
system (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
40. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
right (Le Chatelier's principle)
Le Chatelier's principle
first law of thermodynamics
41. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
ionization energy
freezing point depression
heats of formation
end point
42. *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
ideal gas
catalysts
equilibrium
43. 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.
...
increases
partial
kinetic molecular theory
44. 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
sublimation
reversible reaction
end point
45. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
first law of thermodynamics
activation energy barrier (Le Chatelier's principle)
equilibrium
Van der Waals
46. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
ionization energy
vapor pressure
...
pressure
47. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
emits (in atomic spectra)
boiling point elevation
Boyles law
10 degrees
48. 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).
negative
Van der Waals
moles (Le Chatelier's principle)
equation of state
49. **Proceeding across a period from left to right - the ionization energy _______.
Raoults law
increases
hydrolysis
adiabatic process (thermodynamics)
50. 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.
state functions (thermodynamics)
negative
system (thermodynamics)
Boyles law