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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. Deviations from Boyles law that occur with real gases represent _______ behavior.
crystallizes
Le Chatelier's principle
kinetic molecular theory
non-ideal
2. Electronegativities ________ from left to right in a period.
Le Chatelier's principle
increases
boiling point elevation
decreases
3. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
equilibrium
Van der Waals
Charles law
reversible reaction
4. The temperature at which a substance's solid and liquid phases are in equilibrium.
left (Le Chatelier's principle)
increases
melting point
negative
5. The most active metals are found in what corner of the periodic table?
lower left corner
catalysts
moles (Le Chatelier's principle)
bohr model
6. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
wave mechanical model
kinetic molecular theory
Raoults law
equilibrium
7. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
reversible reaction
base - acid
saturated solution
high
8. 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
equation of state
irreversible and reversible processes
standard atmospheric pressure
kinetic molecular theory
9. A state function in which it is the heat content of a substance.
single replacement/displacement
molar heat of sublimation
specific heat
enthalpy
10. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
isothermal process (thermodynamics)
Van der Waals
third law of thermodynamics
11. A chemical reaction formed from the union of its elements.
irreversible and reversible processes
combination
total pressure (Le Chatelier's principle)
Van der Waals
12. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
increases
reversible reaction
electromotive force (emf)/ cell
bohr model
13. 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.
colligative property law
entropy
boiling point elevation
Boyles law
14. 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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15. **Proceeding across a period from left to right - the ionization energy _______.
2
increases
catalysts
end point
16. 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
decreases
VSEPR
electromotive force (emf)/ cell
17. The action of salts of weak acids or bases with water to form acidic or basic solutions.
heat capacity
electromotive force (emf)/ cell
hydrolysis
first law of thermodynamics
18. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
electrolytic reactions
heat capacity
system (thermodynamics)
valence
19. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
Daltons law
crystallizes
saturated solution
kinetic molecular theory
20. In titration - this is the point at which a particular indicator changes color.
Avogrados law
end point
pi bonds
decreases
21. 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.
first law of thermodynamics
isothermal process (thermodynamics)
Charles law
Daltons law
22. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
anode rays
equivalent point
equation of state
entropy
23. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
anode rays
dynamic equilibrium
total pressure (Le Chatelier's principle)
24. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
emits (in atomic spectra)
partial
specific heat
decreases
25. The heat change during a process carried out at a constant pressure.
valence
Van der Waals
change in enthalpy
activation energy barrier (Le Chatelier's principle)
26. *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.
kinetic molecular theory
hydrolysis
equation of state
left (Le Chatelier's principle)
27. *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.
non-ideal
system (thermodynamics)
electronegativity
...
28. Rays made up of positive electrodes in basic electron charges.
reversible reaction
Raoult's law
anode rays
Van der Waals
29. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
increasing
Avogrados law
...
metallic
30. Rays made up of electrons in basic electron charges.
adiabatic process (thermodynamics)
pi bonds
increases
cathode rays
31. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.
double replacement/displacement
system (thermodynamics)
wave mechanical model
increases
32. 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.
freezing point depression
catalysts
point particles
heats of formation
33. 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 _____ _
limiting law
sublimation
end point
electrolytic cells
34. **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.
Avogrados law
electronegativity
...
metallic
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.
absorbs (in atomic spectra)
hybridyzation
first law of thermodynamics
adiabatic process (thermodynamics)
36. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
standard atmospheric pressure
positive
Raoults law
37. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
negative
crystallizes
zero
38. 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
metallic
negative
electrolytic reactions
bohr model
39. 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.
titration
standard atmospheric pressure
vapor pressure
valence
40. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
melting point
double replacement/displacement
system (thermodynamics)
second law of thermodynamics
41. 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.
catalysts
total pressure (Le Chatelier's principle)
...
Valence Shell Electron Pair Repulsion (VSEPR)
42. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
boiling point
Van der Waals
colligative property law
43. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
vapor pressure
electronegativity
first law of thermodynamics
44. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
kinetic molecular theory
dynamic equilibrium
Avogrados law
cathode rays
45. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
molar heat of sublimation
positive
boiling point elevation
negative
46. *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
cathode rays
electronegativity
valence
metallic
47. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
Charles law
left (Le Chatelier's principle)
VSEPR
double replacement/displacement
48. 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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49. 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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50. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
equilibrium
increases
Le Chatelier's principle
metallic