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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. 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)
catalysts
molar heat of sublimation
high
2. 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).
Le Chatelier's principle
2
equilibrium
Van der Waals
3. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
pi bonds
irreversible and reversible processes
boiling point elevation
Avogrados law
4. 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.
bohr model
Valence Shell Electron Pair Repulsion (VSEPR)
positive charge
emits (in atomic spectra)
5. 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.
6. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
increases
change in enthalpy
Charles law
7. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
8. 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
non-ideal
equilibrium
pressure
9. 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.
10. The most active nonmetals are found in what corner of the periodic table?
upper right corner
negative
first law of thermodynamics
electronegativity
11. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
combination
temperature
point particles
12. 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.
heats of formation
equilibrium
decomposition
equivalent point
13. Electronegativities ________ from left to right in a period.
entropy
limiting law
standard atmospheric pressure
increases
14. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
boiling point
metallic
entropy
positive
15. **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.
kinetic molecular theory
...
Van der Waals
wave mechanical model
16. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
specific heat
kinetic molecular theory
Van der Waals
single replacement/displacement
17. Deviations from Boyles law that occur with real gases represent _______ behavior.
adiabatic process (thermodynamics)
valence
non-ideal
change in enthalpy
18. 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.
19. 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).
end point
state (thermodynamics)
activation energy barrier (Le Chatelier's principle)
saturated solution
20. Electronegativities _______ as you go down a group.
right (Le Chatelier's principle)
decreases
increasing
positive
21. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
...
end point
...
22. The pressure exerted by each gas in a mixture is called its _____ pressure.
vapor pressure
partial
positive charge
Raoults law
23. 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.
heats of formation
VSEPR
Van der Waals
Raoults law
24. When the electron moves from the ground state to an excited state - it ______ energy.
phase equilibrium
absorbs (in atomic spectra)
increasing
ionization energy
25. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
enthalpy
temperature
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.
Raoult's law
base - acid
heats of formation
titration
27. This process occurs when the system is maintained at the same temperature throughout an experiment.
reversible
isothermal process (thermodynamics)
specific heat
sublimation
28. 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.
Le Chatelier's principle
reversible
Avogrados law
increases
29. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
hydrolysis
bohr model
end point
30. 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 _______.
31. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
partial
end point
ionization energy
32. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
reversible reaction
...
sublimation
Nernst equation
33. The temperature at which a substance's solid and liquid phases are in equilibrium.
Le Chatelier's principle
reversible reaction
increases
melting point
34. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
vapor pressure
phase equilibrium
Valence Shell Electron Pair Repulsion (VSEPR)
activation energy
35. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
pi bonds
Nernst equation
2
crystallizes
36. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
negative
increasing
electrolytic reactions
Van der Waals
37. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
increasing
phase equilibrium
state (thermodynamics)
38. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
activation energy
positive
kinetic molecular theory
39. In an endothermic process - energy is absorbed and ^E is _______.
...
kinetic molecular theory
positive
freezing point depression
40. 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
kinetic molecular theory
standard atmospheric pressure
Van der Waals
41. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
negative
dynamic equilibrium
Van der Waals
entropy
42. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
second law of thermodynamics
increases
heats of formation
third law of thermodynamics
43. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
cathode rays
wave mechanical model
pressure
positive
44. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.
left - right (Le Chatelier's principle)
equation of state
ideal gas
Van der Waals
45. 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
melting point
electrolytic reactions
second law of thermodynamics
irreversible and reversible processes
46. In titration - this is the point at which a particular indicator changes color.
decreases
end point
irreversible and reversible processes
bohr model
47. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
combination
Charles law
change in enthalpy
non-ideal
48. The energy required to remove an electron from an isolated atom in its ground state.
Charles law
ionization energy
...
combination
49. A hypothetical gas would follow Boyles law under all conditions and is called?
VSEPR
Le Chatelier's principle
ideal gas
increases
50. When the rate of evaporation equals the rate of condensation - the system is in __________.
specific heat
kinetic molecular theory
VSEPR
equilibrium