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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 ______ 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).
positive
standard atmospheric pressure
wave mechanical model
state (thermodynamics)
2. A chemical reaction formed from the union of its elements.
ideal gas
combination
boiling point elevation
Raoult's law
3. Metals have electronegativities less than ____
positive
dynamic equilibrium
2
Daltons law
4. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
moles (Le Chatelier's principle)
boiling point
increasing
5. 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.
Charles law
isopiestic process (thermodynamics)
positive
Van der Waals
6. *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.
decreases
enthalpy
wave mechanical model
VSEPR
7. 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
equilibrium
boiling point
irreversible and reversible processes
first law of thermodynamics
8. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
equivalent point
negative
decomposition
electromotive force (emf)/ cell
9. 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.
positive
dynamic equilibrium
titration
first law of thermodynamics
10. The heat change during a process carried out at a constant pressure.
electrolytic cells
change in enthalpy
wave mechanical model
heats of formation
11. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
decreases
kinetic molecular theory
total pressure (Le Chatelier's principle)
12. The change in enthalpy of an endothermic reaction is ________.
positive
equation of state
boiling point
negative
13. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
reversible reaction
...
increases
heat capacity
14. In an endothermic process - energy is absorbed and ^E is _______.
upper right corner
absorbs (in atomic spectra)
dynamic equilibrium
positive
15. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
titration
left (Le Chatelier's principle)
temperature
16. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
titration
irreversible and reversible processes
molar heat of sublimation
activation energy
17. In an exothermic process - energy is released and ^E of reaction is ________.
melting point
negative
right (Le Chatelier's principle)
Daltons law
18. 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).
Van der Waals
wave mechanical model
end point
Avogrados law
19. 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.
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20. The freezing point is always lowered by addition of solute.
boiling point elevation
Raoult's law
standard atmospheric pressure
freezing point depression
21. Liquids with strong attractive forces have ______ boiling points.
high
VSEPR
electrolytic reactions
Avogrados law
22. The most active metals are found in what corner of the periodic table?
pressure
increases
lower left corner
boiling point
23. The change in enthalpy of an exothermic reaction is ________.
anode rays
titration
upper right corner
negative
24. 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.
Daltons law
VSEPR
isopiestic process (thermodynamics)
dynamic equilibrium
25. 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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26. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
Valence Shell Electron Pair Repulsion (VSEPR)
moles (Le Chatelier's principle)
vapor pressure
zero
27. 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 _______.
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28. 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.
combination
high
Valence Shell Electron Pair Repulsion (VSEPR)
heats of formation
29. 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
positive charge
positive
system (thermodynamics)
30. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
change in enthalpy
double replacement/displacement
...
31. The action of salts of weak acids or bases with water to form acidic or basic solutions.
adiabatic process (thermodynamics)
increasing
hydrolysis
positive
32. *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.
specific heat
end point
...
heats of formation
33. **Proceeding across a period from left to right - the ionization energy _______.
increases
positive
partial
kinetic molecular theory
34. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
entropy
...
single replacement/displacement
total pressure (Le Chatelier's principle)
35. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
titration
sublimation
double replacement/displacement
2
36. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Avogrados law
10 degrees
double replacement/displacement
left - right (Le Chatelier's principle)
37. _____ bonds are present in molecules containing double or triple bonds.
change in enthalpy
boiling point elevation
emits (in atomic spectra)
pi bonds
38. 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.
left (Le Chatelier's principle)
kinetic molecular theory
heat capacity
combination
39. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
kinetic molecular theory
colligative property law
increases
40. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
...
kinetic molecular theory
standard atmospheric pressure
total pressure (Le Chatelier's principle)
41. The pressure exerted by each gas in a mixture is called its _____ pressure.
single replacement/displacement
left (Le Chatelier's principle)
absorbs (in atomic spectra)
partial
42. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
activation energy
kinetic molecular theory
electrolytic reactions
partial
43. 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
decreases
single replacement/displacement
third law of thermodynamics
bohr model
44. 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.
activation energy barrier (Le Chatelier's principle)
entropy
electronegativity
equivalent point
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
temperature
Charles law
standard atmospheric pressure
46. 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.
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47. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
10 degrees
Van der Waals
Daltons law
third law of thermodynamics
48. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
reversible reaction
pressure
heat capacity
10 degrees
49. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
phase equilibrium
limiting law
Nernst equation
Charles law
50. A state function in which it is the heat content of a substance.
combined gas law
Le Chatelier's principle
enthalpy
Daltons law