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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 amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
decreases
kinetic molecular theory
pressure
2. The freezing point is always lowered by addition of solute.
freezing point depression
decreases
first law of thermodynamics
sublimation
3. The change in enthalpy of an exothermic reaction is ________.
lower left corner
Raoults law
hybridyzation
negative
4. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
combination
Daltons law
base - acid
5. 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.
increases
...
single replacement/displacement
electronegativity
6. The most active nonmetals are found in what corner of the periodic table?
upper right corner
limiting law
titration
phase equilibrium
7. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
positive charge
heats of formation
electronegativity
valence
8. 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
Van der Waals
upper right corner
moles (Le Chatelier's principle)
9. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
standard atmospheric pressure
vapor pressure
hybridyzation
Van der Waals
10. 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
decomposition
adiabatic process (thermodynamics)
moles (Le Chatelier's principle)
bohr model
11. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _
limiting law
Le Chatelier's principle
adiabatic process (thermodynamics)
isothermal process (thermodynamics)
12. Metals have electronegativities less than ____
state functions (thermodynamics)
2
hybridyzation
vapor pressure
13. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
Le Chatelier's principle
system (thermodynamics)
electromotive force (emf)/ cell
14. 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.
15. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
negative
vapor pressure
state (thermodynamics)
crystallizes
16. The vapor pressure increases with increasing _____.
single replacement/displacement
temperature
system (thermodynamics)
end point
17. In an exothermic process - energy is released and ^E of reaction is ________.
positive
Van der Waals
negative
freezing point depression
18. Rays made up of electrons in basic electron charges.
zero
Nernst equation
base - acid
cathode rays
19. Liquids with strong attractive forces have ______ boiling points.
increases
...
irreversible and reversible processes
high
20. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.
catalysts
left - right (Le Chatelier's principle)
kinetic molecular theory
combination
21. In an endothermic process - energy is absorbed and ^E is _______.
positive
standard atmospheric pressure
single replacement/displacement
moles (Le Chatelier's principle)
22. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
enthalpy
total pressure (Le Chatelier's principle)
boiling point
23. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
zero
electromotive force (emf)/ cell
saturated solution
24. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
wave mechanical model
non-ideal
combined gas law
25. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
increases
crystallizes
zero
freezing point depression
26. 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.
27. The pressure exerted by each gas in a mixture is called its _____ pressure.
decreases
titration
point particles
partial
28. 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.
29. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
30. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
total pressure (Le Chatelier's principle)
kinetic molecular theory
upper right corner
Valence Shell Electron Pair Repulsion (VSEPR)
31. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
decreases
upper right corner
kinetic molecular theory
metallic
32. Cells that convert electrical energy into chemical energy.
equation of state
kinetic molecular theory
Le Chatelier's principle
electrolytic cells
33. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
34. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
Charles law
electronegativity
cathode rays
35. *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.
left - right (Le Chatelier's principle)
wave mechanical model
hydrolysis
phase equilibrium
36. 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
left (Le Chatelier's principle)
kinetic molecular theory
pressure
irreversible and reversible processes
37. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.
right (Le Chatelier's principle)
positive
equation of state
saturated solution
38. A hypothetical gas would follow Boyles law under all conditions and is called?
activation energy barrier (Le Chatelier's principle)
ideal gas
entropy
combined gas law
39. Electronegativities ________ from left to right in a period.
lower left corner
positive charge
third law of thermodynamics
increases
40. The change in enthalpy of an endothermic reaction is ________.
wave mechanical model
boiling point elevation
positive
electrolytic reactions
41. 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.
Raoults law
ionization energy
negative
first law of thermodynamics
42. 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.
Van der Waals
Raoults law
combination
reversible
43. The most active metals are found in what corner of the periodic table?
lower left corner
entropy
combined gas law
decreases
44. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
Van der Waals
negative
zero
45. *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
ionization energy
Le Chatelier's principle
titration
valence
46. When the rate of evaporation equals the rate of condensation - the system is in __________.
Charles law
increases
melting point
equilibrium
47. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
isothermal process (thermodynamics)
molar heat of sublimation
catalysts
48. The energy required to remove an electron from an isolated atom in its ground state.
cathode rays
ionization energy
zero
kinetic molecular theory
49. 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.
ideal gas
activation energy barrier (Le Chatelier's principle)
Van der Waals
double replacement/displacement
50. The temperature at which a substance's solid and liquid phases are in equilibrium.
system (thermodynamics)
pi bonds
melting point
base - acid