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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. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
dynamic equilibrium
base - acid
kinetic molecular theory
point particles
2. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
zero
vapor pressure
combined gas law
3. 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)
decreases
Raoults law
electrolytic reactions
4. Heat added to a system and work done by a system are considered _________ quantities.
base - acid
state functions (thermodynamics)
positive
electrolytic reactions
5. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
Nernst equation
Valence Shell Electron Pair Repulsion (VSEPR)
electrolytic reactions
6. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
Charles law
Valence Shell Electron Pair Repulsion (VSEPR)
phase equilibrium
colligative property law
7. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
absorbs (in atomic spectra)
kinetic molecular theory
...
limiting law
8. **Proceeding across a period from left to right - the ionization energy _______.
increases
VSEPR
valence
reversible
9. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
Van der Waals
standard atmospheric pressure
positive
10 degrees
10. **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.
increases
Van der Waals
...
limiting law
11. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
electrolytic reactions
electrolytic cells
heat capacity
increasing
12. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
positive
positive
kinetic molecular theory
hybridyzation
13. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
kinetic molecular theory
second law of thermodynamics
enthalpy
anode rays
14. In an exothermic process - energy is released and ^E of reaction is ________.
negative
Le Chatelier's principle
electrolytic cells
decreases
15. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
specific heat
second law of thermodynamics
isopiestic process (thermodynamics)
16. A state function in which it is the heat content of a substance.
bohr model
...
decreases
enthalpy
17. 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
Van der Waals
zero
18. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
colligative property law
decreases
equilibrium
Boyles law
19. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
partial
reversible reaction
dynamic equilibrium
...
20. This process occurs when the system is maintained at the same temperature throughout an experiment.
Charles law
...
isothermal process (thermodynamics)
standard atmospheric pressure
21. 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
electromotive force (emf)/ cell
Boyles law
metallic
22. The heat change during a process carried out at a constant pressure.
kinetic molecular theory
change in enthalpy
base - acid
Avogrados law
23. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
boiling point elevation
entropy
ideal gas
titration
24. Metals have electronegativities less than ____
2
melting point
point particles
increases
25. 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.
increasing
Nernst equation
reversible
equivalent point
26. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
pressure
increases
partial
combined gas law
27. 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.
bohr model
hybridyzation
kinetic molecular theory
Boyles law
28. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
Boyles law
increases
dynamic equilibrium
29. Rays made up of positive electrodes in basic electron charges.
kinetic molecular theory
combination
positive
anode rays
30. Electronegativities ________ from left to right in a period.
kinetic molecular theory
2
wave mechanical model
increases
31. The change in enthalpy of an exothermic reaction is ________.
specific heat
negative
absorbs (in atomic spectra)
standard atmospheric pressure
32. Liquids with strong attractive forces have ______ boiling points.
change in enthalpy
increasing
high
dynamic equilibrium
33. The energy required to remove an electron from an isolated atom in its ground state.
VSEPR
negative
ionization energy
point particles
34. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
isopiestic process (thermodynamics)
system (thermodynamics)
positive
dynamic equilibrium
35. In an endothermic process - energy is absorbed and ^E is _______.
positive
kinetic molecular theory
positive charge
heat capacity
36. 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.
37. The temperature at which a substance's solid and liquid phases are in equilibrium.
boiling point elevation
melting point
kinetic molecular theory
Nernst equation
38. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
hybridyzation
single replacement/displacement
positive charge
Boyles law
39. The action of salts of weak acids or bases with water to form acidic or basic solutions.
point particles
bohr model
electrolytic cells
hydrolysis
40. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
VSEPR
Nernst equation
decomposition
reversible reaction
41. 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).
decreases
colligative property law
state (thermodynamics)
total pressure (Le Chatelier's principle)
42. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
Van der Waals
...
crystallizes
43. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
44. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
colligative property law
partial
high
45. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
melting point
base - acid
total pressure (Le Chatelier's principle)
kinetic molecular theory
46. When the electron moves from the ground state to an excited state - it ______ energy.
bohr model
negative
absorbs (in atomic spectra)
activation energy
47. 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.
48. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
irreversible and reversible processes
temperature
pressure
vapor pressure
49. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
decreases
isothermal process (thermodynamics)
standard atmospheric pressure
positive
50. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
valence
Van der Waals
limiting law
crystallizes