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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 temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
first law of thermodynamics
upper right corner
boiling point
2
2. Deviations from Boyles law that occur with real gases represent _______ behavior.
cathode rays
equation of state
second law of thermodynamics
non-ideal
3. Electronegativities ________ from left to right in a period.
Charles law
electromotive force (emf)/ cell
left - right (Le Chatelier's principle)
increases
4. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
dynamic equilibrium
cathode rays
boiling point
5. A hypothetical gas would follow Boyles law under all conditions and is called?
combination
ideal gas
heats of formation
...
6. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
10 degrees
boiling point elevation
...
hybridyzation
7. 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.
8. 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 _______.
9. 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.
metallic
heats of formation
colligative property law
enthalpy
10. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
equation of state
third law of thermodynamics
colligative property law
high
11. In titration - this is the point at which a particular indicator changes color.
Avogrados law
Van der Waals
reversible
end point
12. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
melting point
Boyles law
point particles
increases
13. 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.
14. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
boiling point elevation
boiling point
third law of thermodynamics
15. The temperature at which a substance's solid and liquid phases are in equilibrium.
total pressure (Le Chatelier's principle)
melting point
absorbs (in atomic spectra)
activation energy
16. 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).
combined gas law
electronegativity
state (thermodynamics)
electrolytic reactions
17. 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.
base - acid
combination
molar heat of sublimation
Daltons law
18. A solution in which solid solute is in equilibrium with dissolved solute.
standard atmospheric pressure
entropy
saturated solution
...
19. Cells that convert electrical energy into chemical energy.
electrolytic cells
cathode rays
...
metallic
20. **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.
pi bonds
crystallizes
...
reversible
21. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
...
Van der Waals
Van der Waals
second law of thermodynamics
22. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
increases
left (Le Chatelier's principle)
base - acid
entropy
23. The change in enthalpy of an endothermic reaction is ________.
catalysts
negative
positive
reversible reaction
24. 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.
electronegativity
Raoults law
crystallizes
melting point
25. 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.
26. Electronegativities _______ as you go down a group.
positive
decreases
reversible
point particles
27. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.
catalysts
state functions (thermodynamics)
hybridyzation
Le Chatelier's principle
28. The energy required to remove an electron from an isolated atom in its ground state.
system (thermodynamics)
enthalpy
bohr model
ionization energy
29. 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.
sublimation
Raoults law
Charles law
VSEPR
30. *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.
equation of state
left - right (Le Chatelier's principle)
combination
wave mechanical model
31. The heat change during a process carried out at a constant pressure.
metallic
positive charge
change in enthalpy
base - acid
32. Rays made up of electrons in basic electron charges.
standard atmospheric pressure
combined gas law
cathode rays
Raoult's law
33. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
Nernst equation
Charles law
partial
34. 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.
decomposition
total pressure (Le Chatelier's principle)
anode rays
titration
35. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
kinetic molecular theory
hybridyzation
metallic
increases
36. The change in enthalpy of an exothermic reaction is ________.
negative
Raoults law
kinetic molecular theory
Charles law
37. The molecules in a gas are in constant - continueous - random - and straight-line motion.
double replacement/displacement
...
kinetic molecular theory
non-ideal
38. *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
increases
non-ideal
temperature
valence
39. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
Van der Waals
single replacement/displacement
pressure
hybridyzation
40. In an exothermic process - energy is released and ^E of reaction is ________.
electrolytic cells
moles (Le Chatelier's principle)
Avogrados law
negative
41. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
melting point
valence
crystallizes
phase equilibrium
42. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
...
metallic
cathode rays
43. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
Van der Waals
boiling point
crystallizes
electronegativity
44. Heat added to a system and work done by a system are considered _________ quantities.
positive
equation of state
state functions (thermodynamics)
point particles
45. 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.
46. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
upper right corner
boiling point elevation
VSEPR
kinetic molecular theory
47. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
anode rays
activation energy
third law of thermodynamics
48. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
enthalpy
first law of thermodynamics
change in enthalpy
Avogrados law
49. A state function in which it is the heat content of a substance.
enthalpy
adiabatic process (thermodynamics)
kinetic molecular theory
base - acid
50. When the rate of evaporation equals the rate of condensation - the system is in __________.
phase equilibrium
equilibrium
cathode rays
base - acid