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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. Deviations from Boyles law that occur with real gases represent _______ behavior.
third law of thermodynamics
saturated solution
state functions (thermodynamics)
non-ideal
2. 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
adiabatic process (thermodynamics)
isothermal process (thermodynamics)
Nernst equation
3. 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.
kinetic molecular theory
crystallizes
sublimation
Van der Waals
4. 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.
titration
VSEPR
10 degrees
decomposition
5. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
point particles
high
isopiestic process (thermodynamics)
system (thermodynamics)
6. Rays made up of positive electrodes in basic electron charges.
electronegativity
dynamic equilibrium
Van der Waals
anode rays
7. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
pressure
kinetic molecular theory
change in enthalpy
hybridyzation
8. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
electromotive force (emf)/ cell
second law of thermodynamics
lower left corner
Raoult's law
9. 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.
cathode rays
VSEPR
moles (Le Chatelier's principle)
electronegativity
10. 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
10 degrees
Daltons law
isopiestic process (thermodynamics)
11. 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.
Daltons law
partial
colligative property law
vapor pressure
12. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
anode rays
negative
freezing point depression
13. 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).
hydrolysis
Van der Waals
electrolytic reactions
Raoult's law
14. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
kinetic molecular theory
base - acid
dynamic equilibrium
15. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
adiabatic process (thermodynamics)
specific heat
single replacement/displacement
Le Chatelier's principle
16. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
equation of state
hybridyzation
right (Le Chatelier's principle)
sublimation
17. 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.
positive
Van der Waals
ionization energy
kinetic molecular theory
18. 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.
Van der Waals
first law of thermodynamics
moles (Le Chatelier's principle)
decreases
19. The heat required to change 1mole of solid completely to vapor.
increases
bohr model
boiling point elevation
molar heat of sublimation
20. 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.
hybridyzation
standard atmospheric pressure
Raoults law
Le Chatelier's principle
21. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
moles (Le Chatelier's principle)
left (Le Chatelier's principle)
...
22. The molecules in a gas are in constant - continueous - random - and straight-line motion.
Charles law
Van der Waals
kinetic molecular theory
standard atmospheric pressure
23. 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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24. The change in enthalpy of an exothermic reaction is ________.
equivalent point
negative
freezing point depression
kinetic molecular theory
25. 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.
reversible
Charles law
catalysts
positive
26. The change in enthalpy of an endothermic reaction is ________.
ionization energy
boiling point
negative
positive
27. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
enthalpy
point particles
electronegativity
kinetic molecular theory
28. **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.
combined gas law
...
hydrolysis
equilibrium
29. 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
combined gas law
total pressure (Le Chatelier's principle)
colligative property law
bohr model
30. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
...
melting point
single replacement/displacement
31. 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
wave mechanical model
combination
bohr model
32. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
electromotive force (emf)/ cell
entropy
moles (Le Chatelier's principle)
heats of formation
33. Metals have electronegativities less than ____
kinetic molecular theory
Raoults law
ionization energy
2
34. The most active metals are found in what corner of the periodic table?
bohr model
increases
lower left corner
melting point
35. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
entropy
high
adiabatic process (thermodynamics)
isothermal process (thermodynamics)
36. A chemical reaction formed from the union of its elements.
...
combination
positive
bohr model
37. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
valence
increasing
colligative property law
Nernst equation
38. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
state functions (thermodynamics)
isopiestic process (thermodynamics)
decomposition
39. A process that occurs whent eh system is maintained at constant pressure.
wave mechanical model
isopiestic process (thermodynamics)
10 degrees
Raoult's law
40. **Proceeding across a period from left to right - the ionization energy _______.
increases
...
standard atmospheric pressure
increasing
41. Electronegativities ________ from left to right in a period.
point particles
combined gas law
Le Chatelier's principle
increases
42. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
state functions (thermodynamics)
...
combination
43. Rays made up of electrons in basic electron charges.
left (Le Chatelier's principle)
temperature
kinetic molecular theory
cathode rays
44. The heat change during a process carried out at a constant pressure.
negative
ionization energy
change in enthalpy
Nernst equation
45. In an exothermic process - energy is released and ^E of reaction is ________.
positive
vapor pressure
ideal gas
negative
46. The energy required to remove an electron from an isolated atom in its ground state.
isothermal process (thermodynamics)
ionization energy
pressure
kinetic molecular theory
47. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
ideal gas
decreases
combined gas law
pi bonds
48. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Raoult's law
pi bonds
phase equilibrium
Charles law
49. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
base - acid
catalysts
boiling point
titration
50. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
high
VSEPR
positive
phase equilibrium