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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. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
decreases
standard atmospheric pressure
dynamic equilibrium
2. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
Van der Waals
combined gas law
isothermal process (thermodynamics)
3. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
4. 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 _______.
5. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
left - right (Le Chatelier's principle)
activation energy
boiling point elevation
increasing
6. 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
hybridyzation
absorbs (in atomic spectra)
isothermal process (thermodynamics)
7. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
activation energy barrier (Le Chatelier's principle)
Van der Waals
second law of thermodynamics
system (thermodynamics)
8. 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.
decreases
positive
Charles law
catalysts
9. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
electromotive force (emf)/ cell
system (thermodynamics)
state functions (thermodynamics)
activation energy barrier (Le Chatelier's principle)
10. This process occurs when the system is maintained at the same temperature throughout an experiment.
limiting law
pi bonds
Charles law
isothermal process (thermodynamics)
11. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
lower left corner
emits (in atomic spectra)
kinetic molecular theory
right (Le Chatelier's principle)
12. 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.
heats of formation
titration
metallic
positive
13. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
standard atmospheric pressure
limiting law
right (Le Chatelier's principle)
14. The most active nonmetals are found in what corner of the periodic table?
upper right corner
freezing point depression
Le Chatelier's principle
Raoult's law
15. The temperature at which a substance's solid and liquid phases are in equilibrium.
kinetic molecular theory
melting point
adiabatic process (thermodynamics)
Daltons law
16. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
boiling point elevation
valence
electrolytic reactions
standard atmospheric pressure
17. 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
positive charge
molar heat of sublimation
reversible reaction
end point
18. In an endothermic process - energy is absorbed and ^E is _______.
melting point
Charles law
positive
titration
19. Electronegativities _______ as you go down a group.
decreases
wave mechanical model
base - acid
molar heat of sublimation
20. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
valence
heats of formation
Charles law
positive
21. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
equivalent point
emits (in atomic spectra)
pressure
kinetic molecular theory
22. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
10 degrees
end point
standard atmospheric pressure
crystallizes
23. In titration - this is the point at which a particular indicator changes color.
saturated solution
upper right corner
end point
Raoult's law
24. *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.
equation of state
decreases
kinetic molecular theory
dynamic equilibrium
25. **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.
...
activation energy barrier (Le Chatelier's principle)
metallic
ionization energy
26. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
single replacement/displacement
reversible reaction
electrolytic reactions
27. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
Daltons law
metallic
specific heat
point particles
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. 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.
activation energy barrier (Le Chatelier's principle)
reversible
Daltons law
pi bonds
30. This process occurs when the system is thermally isolated so that no heat enters or leaves.
standard atmospheric pressure
metallic
single replacement/displacement
adiabatic process (thermodynamics)
31. 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.
first law of thermodynamics
Van der Waals
system (thermodynamics)
saturated solution
32. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
10 degrees
2
single replacement/displacement
Raoults law
33. A solution in which solid solute is in equilibrium with dissolved solute.
heat capacity
colligative property law
saturated solution
increases
34. 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
pi bonds
isothermal process (thermodynamics)
positive charge
bohr model
35. *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
kinetic molecular theory
increasing
increases
valence
36. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
valence
emits (in atomic spectra)
kinetic molecular theory
decomposition
37. The most active metals are found in what corner of the periodic table?
lower left corner
Valence Shell Electron Pair Repulsion (VSEPR)
cathode rays
decreases
38. Rays made up of electrons in basic electron charges.
cathode rays
Le Chatelier's principle
Van der Waals
state functions (thermodynamics)
39. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
freezing point depression
decreases
positive
bohr model
40. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
heat capacity
increases
sublimation
41. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
decomposition
crystallizes
melting point
metallic
42. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
standard atmospheric pressure
reversible reaction
double replacement/displacement
positive charge
43. A hypothetical gas would follow Boyles law under all conditions and is called?
kinetic molecular theory
single replacement/displacement
ideal gas
colligative property law
44. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
third law of thermodynamics
metallic
boiling point
dynamic equilibrium
45. 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.
46. 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.
ionization energy
negative
base - acid
reversible
47. The energy required to remove an electron from an isolated atom in its ground state.
ionization energy
increasing
isopiestic process (thermodynamics)
titration
48. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
state (thermodynamics)
enthalpy
pressure
Avogrados law
49. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
50. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
wave mechanical model
vapor pressure
Van der Waals
reversible reaction