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Test your basic knowledge |
CLEP Chemistry 1
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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. 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
heats of formation
activation energy
bohr model
2. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
positive charge
absorbs (in atomic spectra)
single replacement/displacement
equation of state
3. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
Valence Shell Electron Pair Repulsion (VSEPR)
first law of thermodynamics
pressure
4. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
equation of state
change in enthalpy
catalysts
metallic
5. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
equilibrium
zero
boiling point
standard atmospheric pressure
6. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
positive
10 degrees
Nernst equation
combined gas law
7. *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
Le Chatelier's principle
ideal gas
valence
increasing
8. When the electron moves from the ground state to an excited state - it ______ energy.
Nernst equation
absorbs (in atomic spectra)
crystallizes
metallic
9. 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.
10. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
phase equilibrium
boiling point
cathode rays
11. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
saturated solution
upper right corner
specific heat
electrolytic reactions
12. The pressure exerted by each gas in a mixture is called its _____ pressure.
equation of state
high
VSEPR
partial
13. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Charles law
base - acid
left - right (Le Chatelier's principle)
increasing
14. 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.
electromotive force (emf)/ cell
vapor pressure
Raoults law
Van der Waals
15. 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.
decomposition
phase equilibrium
electronegativity
Van der Waals
16. A process that occurs whent eh system is maintained at constant pressure.
Nernst equation
isopiestic process (thermodynamics)
high
reversible
17. 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.
18. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
titration
crystallizes
heats of formation
second law of thermodynamics
19. A hypothetical gas would follow Boyles law under all conditions and is called?
electromotive force (emf)/ cell
point particles
10 degrees
ideal gas
20. Liquids with strong attractive forces have ______ boiling points.
high
zero
colligative property law
reversible
21. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
total pressure (Le Chatelier's principle)
negative
Charles law
third law of thermodynamics
22. The heat required to change 1mole of solid completely to vapor.
Boyles law
positive
molar heat of sublimation
heats of formation
23. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
right (Le Chatelier's principle)
Avogrados law
cathode rays
crystallizes
24. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
point particles
crystallizes
adiabatic process (thermodynamics)
electromotive force (emf)/ cell
25. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
10 degrees
isothermal process (thermodynamics)
positive charge
26. The vapor pressure increases with increasing _____.
Raoults law
system (thermodynamics)
temperature
hybridyzation
27. 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.
28. Electronegativities ________ from left to right in a period.
boiling point elevation
limiting law
positive
increases
29. A state function in which it is the heat content of a substance.
enthalpy
sublimation
electronegativity
Le Chatelier's principle
30. 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.
boiling point elevation
Daltons law
colligative property law
kinetic molecular theory
31. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
base - acid
kinetic molecular theory
heats of formation
Van der Waals
32. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
Charles law
second law of thermodynamics
increases
equilibrium
33. A solution in which solid solute is in equilibrium with dissolved solute.
Avogrados law
high
saturated solution
increases
34. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
left - right (Le Chatelier's principle)
wave mechanical model
first law of thermodynamics
35. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
enthalpy
Le Chatelier's principle
activation energy
36. The temperature at which a substance's solid and liquid phases are in equilibrium.
isothermal process (thermodynamics)
kinetic molecular theory
melting point
metallic
37. The most active nonmetals are found in what corner of the periodic table?
ionization energy
Nernst equation
kinetic molecular theory
upper right corner
38. **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.
point particles
freezing point depression
Avogrados law
...
39. In titration - this is the point at which a particular indicator changes color.
end point
colligative property law
phase equilibrium
irreversible and reversible processes
40. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
...
state (thermodynamics)
wave mechanical model
41. 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)
Van der Waals
titration
valence
42. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
double replacement/displacement
Charles law
reversible reaction
right (Le Chatelier's principle)
43. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
kinetic molecular theory
Boyles law
pressure
specific heat
44. 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.
45. 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.
46. 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
titration
melting point
Van der Waals
positive charge
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.
isothermal process (thermodynamics)
activation energy barrier (Le Chatelier's principle)
...
Van der Waals
48. 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.
colligative property law
emits (in atomic spectra)
VSEPR
melting point
49. 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.
increases
catalysts
dynamic equilibrium
positive charge
50. 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
...
temperature
bohr model
pressure