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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. *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.
emits (in atomic spectra)
wave mechanical model
entropy
heat capacity
2. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Van der Waals
kinetic molecular theory
Charles law
total pressure (Le Chatelier's principle)
3. 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.
positive charge
first law of thermodynamics
increases
2
4. 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
electromotive force (emf)/ cell
state (thermodynamics)
increases
positive charge
5. 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
kinetic molecular theory
activation energy barrier (Le Chatelier's principle)
high
6. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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7. In an endothermic process - energy is absorbed and ^E is _______.
positive
enthalpy
2
electrolytic cells
8. 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)
kinetic molecular theory
increases
phase equilibrium
9. The vapor pressure increases with increasing _____.
kinetic molecular theory
state functions (thermodynamics)
temperature
increases
10. A state function in which it is the heat content of a substance.
electrolytic cells
enthalpy
titration
Le Chatelier's principle
11. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
non-ideal
sublimation
kinetic molecular theory
left (Le Chatelier's principle)
12. When the rate of evaporation equals the rate of condensation - the system is in __________.
isothermal process (thermodynamics)
equilibrium
boiling point elevation
vapor pressure
13. A hypothetical gas would follow Boyles law under all conditions and is called?
2
10 degrees
cathode rays
ideal gas
14. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
temperature
state functions (thermodynamics)
left - right (Le Chatelier's principle)
standard atmospheric pressure
15. Liquids with strong attractive forces have ______ boiling points.
positive
kinetic molecular theory
combined gas law
high
16. 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.
Van der Waals
equation of state
kinetic molecular theory
change in enthalpy
17. A chemical reaction formed from the union of its elements.
state (thermodynamics)
combination
hydrolysis
reversible reaction
18. 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.
state (thermodynamics)
single replacement/displacement
Daltons law
standard atmospheric pressure
19. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
...
ionization energy
change in enthalpy
Avogrados law
20. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
single replacement/displacement
adiabatic process (thermodynamics)
base - acid
zero
21. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
total pressure (Le Chatelier's principle)
double replacement/displacement
electronegativity
22. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
catalysts
double replacement/displacement
change in enthalpy
state (thermodynamics)
23. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
point particles
combination
limiting law
electromotive force (emf)/ cell
24. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
combination
activation energy
VSEPR
activation energy barrier (Le Chatelier's principle)
25. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
right (Le Chatelier's principle)
wave mechanical model
metallic
26. 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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27. The temperature at which a substance's solid and liquid phases are in equilibrium.
right (Le Chatelier's principle)
melting point
sublimation
Avogrados law
28. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
double replacement/displacement
phase equilibrium
titration
temperature
29. The energy required to remove an electron from an isolated atom in its ground state.
ionization energy
state functions (thermodynamics)
valence
hydrolysis
30. The heat change during a process carried out at a constant pressure.
...
Le Chatelier's principle
change in enthalpy
Van der Waals
31. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
base - acid
right (Le Chatelier's principle)
melting point
increases
32. 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.
increases
saturated solution
titration
Nernst equation
33. 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
hydrolysis
boiling point
bohr model
Boyles law
34. *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.
isothermal process (thermodynamics)
standard atmospheric pressure
equation of state
ionization energy
35. The change in enthalpy of an endothermic reaction is ________.
zero
ideal gas
positive
saturated solution
36. 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
Charles law
boiling point
irreversible and reversible processes
negative
37. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
limiting law
ionization energy
decreases
titration
38. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Boyles law
activation energy
combination
absorbs (in atomic spectra)
39. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
decomposition
VSEPR
system (thermodynamics)
positive
40. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
melting point
combination
kinetic molecular theory
41. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
combined gas law
kinetic molecular theory
increases
42. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
state functions (thermodynamics)
Van der Waals
third law of thermodynamics
valence
43. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
pressure
10 degrees
single replacement/displacement
positive
44. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Nernst equation
kinetic molecular theory
reversible reaction
adiabatic process (thermodynamics)
45. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
Nernst equation
second law of thermodynamics
specific heat
sublimation
46. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
moles (Le Chatelier's principle)
decreases
kinetic molecular theory
47. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
colligative property law
pi bonds
electronegativity
48. 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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49. The molecules in a gas are in constant - continueous - random - and straight-line motion.
electrolytic cells
kinetic molecular theory
negative
Charles law
50. In an exothermic process - energy is released and ^E of reaction is ________.
point particles
decreases
negative
cathode rays