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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. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
end point
left - right (Le Chatelier's principle)
sublimation
dynamic equilibrium
2. This process occurs when the system is maintained at the same temperature throughout an experiment.
positive
boiling point elevation
10 degrees
isothermal process (thermodynamics)
3. Rays made up of electrons in basic electron charges.
specific heat
VSEPR
valence
cathode rays
4. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Raoult's law
increasing
total pressure (Le Chatelier's principle)
pressure
5. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Le Chatelier's principle
limiting law
standard atmospheric pressure
heat capacity
6. 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
2
freezing point depression
standard atmospheric pressure
7. Rays made up of positive electrodes in basic electron charges.
anode rays
saturated solution
left - right (Le Chatelier's principle)
standard atmospheric pressure
8. In an exothermic process - energy is released and ^E of reaction is ________.
...
partial
titration
negative
9. In an endothermic process - energy is absorbed and ^E is _______.
right (Le Chatelier's principle)
left (Le Chatelier's principle)
high
positive
10. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
kinetic molecular theory
cathode rays
Avogrados law
11. 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 _______.
12. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
13. **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.
total pressure (Le Chatelier's principle)
increases
...
sublimation
14. *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
anode rays
positive
valence
electrolytic reactions
15. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
base - acid
activation energy barrier (Le Chatelier's principle)
boiling point
reversible reaction
16. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
kinetic molecular theory
hybridyzation
heat capacity
isothermal process (thermodynamics)
17. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
second law of thermodynamics
colligative property law
state (thermodynamics)
entropy
18. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Van der Waals
standard atmospheric pressure
bohr model
base - acid
19. When the electron moves from the ground state to an excited state - it ______ energy.
Valence Shell Electron Pair Repulsion (VSEPR)
absorbs (in atomic spectra)
saturated solution
kinetic molecular theory
20. 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.
21. 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.
melting point
heats of formation
10 degrees
Valence Shell Electron Pair Repulsion (VSEPR)
22. 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
decreases
irreversible and reversible processes
equivalent point
activation energy barrier (Le Chatelier's principle)
23. 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.
upper right corner
Le Chatelier's principle
Van der Waals
Le Chatelier's principle
24. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
anode rays
electromotive force (emf)/ cell
decreases
25. The most active metals are found in what corner of the periodic table?
lower left corner
electrolytic reactions
isopiestic process (thermodynamics)
bohr model
26. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
state (thermodynamics)
specific heat
wave mechanical model
27. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
saturated solution
decomposition
Boyles law
hydrolysis
28. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
Raoults law
boiling point
decreases
third law of thermodynamics
29. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
decreases
Raoults law
boiling point elevation
dynamic equilibrium
30. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
freezing point depression
electrolytic reactions
...
Van der Waals
31. The molecules in a gas are in constant - continueous - random - and straight-line motion.
decomposition
kinetic molecular theory
boiling point elevation
activation energy
32. 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.
33. *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.
pi bonds
irreversible and reversible processes
...
phase equilibrium
34. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
isopiestic process (thermodynamics)
equilibrium
Van der Waals
phase equilibrium
35. In titration - this is the point at which a particular indicator changes color.
electrolytic reactions
partial
end point
point particles
36. 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.
third law of thermodynamics
titration
lower left corner
decreases
37. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
third law of thermodynamics
double replacement/displacement
Van der Waals
38. A process that occurs whent eh system is maintained at constant pressure.
system (thermodynamics)
isopiestic process (thermodynamics)
decreases
emits (in atomic spectra)
39. 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.
high
increases
Raoults law
dynamic equilibrium
40. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
melting point
increases
left (Le Chatelier's principle)
41. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
single replacement/displacement
ideal gas
Avogrados law
positive
42. 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.
43. Cells that convert electrical energy into chemical energy.
electrolytic cells
third law of thermodynamics
irreversible and reversible processes
increasing
44. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
negative
Le Chatelier's principle
electrolytic cells
vapor pressure
45. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
state (thermodynamics)
Daltons law
Raoults law
46. Metals have electronegativities less than ____
2
valence
Charles law
VSEPR
47. The pressure exerted by each gas in a mixture is called its _____ pressure.
kinetic molecular theory
single replacement/displacement
boiling point elevation
partial
48. 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.
state functions (thermodynamics)
hydrolysis
temperature
2
49. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
limiting law
point particles
Valence Shell Electron Pair Repulsion (VSEPR)
valence
50. 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.
first law of thermodynamics
second law of thermodynamics
kinetic molecular theory
positive charge