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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. Metals have electronegativities less than ____
positive
2
Daltons law
Raoult's law
2. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
positive
single replacement/displacement
valence
3. **Proceeding across a period from left to right - the ionization energy _______.
increases
kinetic molecular theory
VSEPR
Daltons law
4. 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.
left (Le Chatelier's principle)
catalysts
sublimation
point particles
5. *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
Nernst equation
total pressure (Le Chatelier's principle)
...
valence
6. A hypothetical gas would follow Boyles law under all conditions and is called?
boiling point elevation
kinetic molecular theory
Van der Waals
ideal gas
7. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
heats of formation
phase equilibrium
Nernst equation
melting point
8. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
saturated solution
wave mechanical model
dynamic equilibrium
freezing point depression
9. 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.
VSEPR
enthalpy
equivalent point
adiabatic process (thermodynamics)
10. A state function in which it is the heat content of a substance.
lower left corner
enthalpy
Daltons law
Charles law
11. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Van der Waals
heat capacity
...
adiabatic process (thermodynamics)
12. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
freezing point depression
boiling point
moles (Le Chatelier's principle)
13. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
high
decomposition
reversible reaction
cathode rays
14. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
pi bonds
partial
high
specific heat
15. 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
kinetic molecular theory
decreases
absorbs (in atomic spectra)
positive charge
16. When the rate of evaporation equals the rate of condensation - the system is in __________.
decreases
total pressure (Le Chatelier's principle)
kinetic molecular theory
equilibrium
17. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
increases
first law of thermodynamics
electrolytic reactions
Le Chatelier's principle
18. 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
Van der Waals
phase equilibrium
pressure
19. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
kinetic molecular theory
decreases
absorbs (in atomic spectra)
left - right (Le Chatelier's principle)
20. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
third law of thermodynamics
standard atmospheric pressure
state functions (thermodynamics)
21. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
base - acid
increasing
sublimation
dynamic equilibrium
22. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pi bonds
pressure
hydrolysis
increasing
23. A solution in which solid solute is in equilibrium with dissolved solute.
boiling point elevation
saturated solution
electronegativity
non-ideal
24. Cells that convert electrical energy into chemical energy.
equilibrium
electrolytic cells
Boyles law
electromotive force (emf)/ cell
25. The freezing point is always lowered by addition of solute.
third law of thermodynamics
positive
freezing point depression
Charles law
26. The molecules in a gas are in constant - continueous - random - and straight-line motion.
ionization energy
kinetic molecular theory
lower left corner
bohr model
27. The temperature at which a substance's solid and liquid phases are in equilibrium.
point particles
activation energy barrier (Le Chatelier's principle)
melting point
kinetic molecular theory
28. The most active metals are found in what corner of the periodic table?
double replacement/displacement
pi bonds
lower left corner
decreases
29. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
enthalpy
change in enthalpy
dynamic equilibrium
30. 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
decreases
reversible
non-ideal
bohr model
31. Rays made up of positive electrodes in basic electron charges.
electrolytic reactions
anode rays
first law of thermodynamics
decreases
32. Deviations from Boyles law that occur with real gases represent _______ behavior.
entropy
combined gas law
non-ideal
single replacement/displacement
33. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
right (Le Chatelier's principle)
decomposition
decreases
titration
34. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
positive
electrolytic cells
heats of formation
10 degrees
35. 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.
irreversible and reversible processes
reversible
point particles
pi bonds
36. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
molar heat of sublimation
emits (in atomic spectra)
anode rays
kinetic molecular theory
37. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
change in enthalpy
non-ideal
single replacement/displacement
temperature
38. 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.
39. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
metallic
hybridyzation
increasing
Van der Waals
40. 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.
kinetic molecular theory
Charles law
electronegativity
isothermal process (thermodynamics)
41. 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.
sublimation
Daltons law
isopiestic process (thermodynamics)
decreases
42. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Avogrados law
left - right (Le Chatelier's principle)
VSEPR
electronegativity
43. The heat change during a process carried out at a constant pressure.
left (Le Chatelier's principle)
Avogrados law
state (thermodynamics)
change in enthalpy
44. 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.
45. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
Raoults law
electrolytic reactions
second law of thermodynamics
decomposition
46. *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.
Daltons law
...
sublimation
pressure
47. The change in enthalpy of an endothermic reaction is ________.
Raoults law
ideal gas
Van der Waals
positive
48. *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
first law of thermodynamics
standard atmospheric pressure
...
49. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
equation of state
sublimation
base - acid
...
50. 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
isothermal process (thermodynamics)
zero
irreversible and reversible processes
Van der Waals