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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 energy required to remove an electron from an isolated atom in its ground state.
2
boiling point elevation
ionization energy
kinetic molecular theory
2. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
freezing point depression
VSEPR
Charles law
3. Electronegativities ________ from left to right in a period.
phase equilibrium
decreases
increases
Raoult's law
4. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
single replacement/displacement
vapor pressure
temperature
titration
5. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
Valence Shell Electron Pair Repulsion (VSEPR)
non-ideal
...
kinetic molecular theory
6. The action of salts of weak acids or bases with water to form acidic or basic solutions.
combined gas law
phase equilibrium
hydrolysis
irreversible and reversible processes
7. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
base - acid
equation of state
activation energy barrier (Le Chatelier's principle)
8. *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.
increasing
right (Le Chatelier's principle)
non-ideal
wave mechanical model
9. A chemical reaction formed from the union of its elements.
negative
positive
anode rays
combination
10. The heat change during a process carried out at a constant pressure.
Boyles law
hybridyzation
Le Chatelier's principle
change in enthalpy
11. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.
Avogrados law
specific heat
Raoults law
total pressure (Le Chatelier's principle)
12. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
...
adiabatic process (thermodynamics)
vapor pressure
Charles law
13. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
electromotive force (emf)/ cell
Boyles law
irreversible and reversible processes
Daltons law
14. The change in enthalpy of an exothermic reaction is ________.
10 degrees
negative
electrolytic reactions
vapor pressure
15. 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
electrolytic reactions
boiling point
temperature
16. Cells that convert electrical energy into chemical energy.
Le Chatelier's principle
moles (Le Chatelier's principle)
Raoult's law
electrolytic cells
17. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
left - right (Le Chatelier's principle)
point particles
increases
state (thermodynamics)
18. *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.
colligative property law
Daltons law
equation of state
sublimation
19. When the rate of evaporation equals the rate of condensation - the system is in __________.
Raoult's law
equilibrium
Le Chatelier's principle
lower left corner
20. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.
equivalent point
freezing point depression
Nernst equation
Boyles law
21. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
isopiestic process (thermodynamics)
ideal gas
combination
22. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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23. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
melting point
positive
kinetic molecular theory
24. A state function in which it is the heat content of a substance.
electronegativity
enthalpy
...
negative
25. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
Boyles law
freezing point depression
metallic
increases
26. 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.
increases
temperature
activation energy
kinetic molecular theory
27. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.
standard atmospheric pressure
electronegativity
activation energy barrier (Le Chatelier's principle)
anode rays
28. 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.
Charles law
dynamic equilibrium
catalysts
double replacement/displacement
29. This process occurs when the system is thermally isolated so that no heat enters or leaves.
dynamic equilibrium
single replacement/displacement
isothermal process (thermodynamics)
adiabatic process (thermodynamics)
30. 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 _____ _
total pressure (Le Chatelier's principle)
left (Le Chatelier's principle)
change in enthalpy
limiting law
31. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
kinetic molecular theory
upper right corner
VSEPR
increasing
32. 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).
increases
left - right (Le Chatelier's principle)
state (thermodynamics)
ideal gas
33. A process that occurs whent eh system is maintained at constant pressure.
equilibrium
crystallizes
standard atmospheric pressure
isopiestic process (thermodynamics)
34. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
electromotive force (emf)/ cell
decreases
kinetic molecular theory
35. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
increases
increases
combined gas law
36. 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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37. 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).
electronegativity
vapor pressure
Boyles law
Van der Waals
38. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
equilibrium
Nernst equation
specific heat
Valence Shell Electron Pair Repulsion (VSEPR)
39. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.
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40. 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
pi bonds
positive charge
adiabatic process (thermodynamics)
catalysts
41. Electronegativities _______ as you go down a group.
melting point
decreases
vapor pressure
limiting law
42. This process occurs when the system is maintained at the same temperature throughout an experiment.
ionization energy
state functions (thermodynamics)
isothermal process (thermodynamics)
non-ideal
43. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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44. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
third law of thermodynamics
increases
catalysts
anode rays
45. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
total pressure (Le Chatelier's principle)
upper right corner
anode rays
46. 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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47. The pressure exerted by each gas in a mixture is called its _____ pressure.
left (Le Chatelier's principle)
partial
combination
hybridyzation
48. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
electrolytic reactions
irreversible and reversible processes
pressure
49. In an endothermic process - energy is absorbed and ^E is _______.
valence
positive
electronegativity
electromotive force (emf)/ cell
50. 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.
kinetic molecular theory
Van der Waals
Daltons law
vapor pressure