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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. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
10 degrees
second law of thermodynamics
isopiestic process (thermodynamics)
entropy
2. Rays made up of positive electrodes in basic electron charges.
anode rays
kinetic molecular theory
crystallizes
increases
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.
combined gas law
Valence Shell Electron Pair Repulsion (VSEPR)
total pressure (Le Chatelier's principle)
electrolytic cells
4. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
reversible
Raoult's law
single replacement/displacement
kinetic molecular theory
5. 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
Raoult's law
right (Le Chatelier's principle)
6. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
increases
phase equilibrium
electrolytic reactions
metallic
7. The freezing point is always lowered by addition of solute.
freezing point depression
Raoult's law
Avogrados law
melting point
8. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
VSEPR
pressure
Boyles law
...
9. 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
positive
entropy
negative
10. When the electron moves from the ground state to an excited state - it ______ energy.
hybridyzation
negative
absorbs (in atomic spectra)
saturated solution
11. Electronegativities _______ as you go down a group.
double replacement/displacement
colligative property law
decreases
second law of thermodynamics
12. 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.
lower left corner
VSEPR
electromotive force (emf)/ cell
non-ideal
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.
pressure
ionization energy
colligative property law
end point
14. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
equivalent point
ideal gas
boiling point
absorbs (in atomic spectra)
15. A hypothetical gas would follow Boyles law under all conditions and is called?
activation energy barrier (Le Chatelier's principle)
boiling point
2
ideal gas
16. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
isothermal process (thermodynamics)
metallic
Van der Waals
17. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
emits (in atomic spectra)
temperature
phase equilibrium
heat capacity
18. 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).
state (thermodynamics)
Van der Waals
molar heat of sublimation
combination
19. The energy required to remove an electron from an isolated atom in its ground state.
Le Chatelier's principle
ionization energy
melting point
Van der Waals
20. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
ideal gas
activation energy
enthalpy
standard atmospheric pressure
21. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
double replacement/displacement
kinetic molecular theory
irreversible and reversible processes
22. 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).
Van der Waals
wave mechanical model
increases
titration
23. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge
Le Chatelier's principle
...
positive charge
increasing
24. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
...
kinetic molecular theory
electromotive force (emf)/ cell
decreases
25. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
reversible reaction
upper right corner
decreases
26. 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
increases
adiabatic process (thermodynamics)
27. 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.
colligative property law
Van der Waals
10 degrees
Avogrados law
28. 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.
29. In an endothermic process - energy is absorbed and ^E is _______.
state (thermodynamics)
positive
electrolytic reactions
activation energy
30. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
freezing point depression
vapor pressure
valence
dynamic equilibrium
31. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
negative
heat capacity
adiabatic process (thermodynamics)
melting point
32. 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
Daltons law
electrolytic reactions
...
33. A process that occurs whent eh system is maintained at constant pressure.
left (Le Chatelier's principle)
isopiestic process (thermodynamics)
kinetic molecular theory
boiling point
34. *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.
pi bonds
wave mechanical model
Valence Shell Electron Pair Repulsion (VSEPR)
increases
35. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
10 degrees
emits (in atomic spectra)
Van der Waals
combined gas law
36. Cells that convert electrical energy into chemical energy.
kinetic molecular theory
Charles law
electrolytic cells
isopiestic process (thermodynamics)
37. The pressure exerted by each gas in a mixture is called its _____ pressure.
Le Chatelier's principle
change in enthalpy
partial
equation of state
38. When the rate of evaporation equals the rate of condensation - the system is in __________.
specific heat
increasing
equilibrium
cathode rays
39. *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.
entropy
bohr model
equation of state
non-ideal
40. 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.
41. The vapor pressure increases with increasing _____.
increases
combination
temperature
non-ideal
42. The change in enthalpy of an exothermic reaction is ________.
increases
Avogrados law
negative
combination
43. **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
pressure
combination
...
44. 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.
45. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
vapor pressure
pressure
electromotive force (emf)/ cell
combined gas law
46. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
negative
non-ideal
positive
47. *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.
limiting law
right (Le Chatelier's principle)
...
catalysts
48. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hydrolysis
hybridyzation
system (thermodynamics)
double replacement/displacement
49. _____ bonds are present in molecules containing double or triple bonds.
Boyles law
decomposition
positive
pi bonds
50. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
combination
Van der Waals
system (thermodynamics)
decreases