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Test your basic knowledge |
CLEP Chemistry 1
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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. Rays made up of positive electrodes in basic electron charges.
anode rays
wave mechanical model
negative
Avogrados law
2. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
activation energy
metallic
electromotive force (emf)/ cell
heat capacity
3. **Proceeding across a period from left to right - the ionization energy _______.
saturated solution
increases
point particles
reversible
4. 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
increases
temperature
Raoults law
5. A hypothetical gas would follow Boyles law under all conditions and is called?
Raoults law
decreases
ideal gas
base - acid
6. The molecules in a gas are in constant - continueous - random - and straight-line motion.
Van der Waals
kinetic molecular theory
electromotive force (emf)/ cell
high
7. A solution in which solid solute is in equilibrium with dissolved solute.
electrolytic reactions
pi bonds
cathode rays
saturated solution
8. The most active metals are found in what corner of the periodic table?
negative
bohr model
lower left corner
boiling point elevation
9. 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
colligative property law
isopiestic process (thermodynamics)
melting point
10. In an endothermic process - energy is absorbed and ^E is _______.
double replacement/displacement
melting point
positive
isopiestic process (thermodynamics)
11. *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.
activation energy
decreases
phase equilibrium
wave mechanical model
12. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
saturated solution
hydrolysis
kinetic molecular theory
standard atmospheric pressure
13. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
pi bonds
crystallizes
equation of state
14. The vapor pressure increases with increasing _____.
decreases
temperature
10 degrees
Van der Waals
15. A chemical reaction formed from the union of its elements.
decomposition
combination
Boyles law
upper right corner
16. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
Daltons law
Charles law
kinetic molecular theory
17. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
standard atmospheric pressure
pressure
high
Avogrados law
18. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
left - right (Le Chatelier's principle)
upper right corner
absorbs (in atomic spectra)
double replacement/displacement
19. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
Charles law
negative
point particles
ionization energy
20. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
left - right (Le Chatelier's principle)
isothermal process (thermodynamics)
specific heat
Raoults law
21. A state function in which it is the heat content of a substance.
electronegativity
total pressure (Le Chatelier's principle)
kinetic molecular theory
enthalpy
22. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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23. 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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24. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
negative
second law of thermodynamics
negative
...
25. **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.
enthalpy
decreases
upper right corner
...
26. 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.
Daltons law
Charles law
Boyles law
colligative property law
27. When the electron moves from the ground state to an excited state - it ______ energy.
activation energy barrier (Le Chatelier's principle)
absorbs (in atomic spectra)
VSEPR
equation of state
28. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
bohr model
positive charge
zero
heat capacity
29. 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.
total pressure (Le Chatelier's principle)
vapor pressure
system (thermodynamics)
titration
30. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
combined gas law
change in enthalpy
Le Chatelier's principle
31. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
Charles law
...
Le Chatelier's principle
decreases
32. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
heats of formation
metallic
kinetic molecular theory
hybridyzation
33. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
increases
Van der Waals
kinetic molecular theory
decreases
34. 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.
Charles law
enthalpy
limiting law
catalysts
35. The pressure exerted by each gas in a mixture is called its _____ pressure.
Raoults law
pi bonds
activation energy barrier (Le Chatelier's principle)
partial
36. 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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37. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.
reversible
2
system (thermodynamics)
sublimation
38. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
lower left corner
decreases
end point
kinetic molecular theory
39. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
second law of thermodynamics
heats of formation
pi bonds
Daltons law
40. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
freezing point depression
limiting law
activation energy
41. Rays made up of electrons in basic electron charges.
state functions (thermodynamics)
cathode rays
point particles
zero
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.
Le Chatelier's principle
Raoults law
electronegativity
kinetic molecular theory
43. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
single replacement/displacement
titration
pressure
44. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
Charles law
activation energy
kinetic molecular theory
adiabatic process (thermodynamics)
45. 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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46. *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.
Boyles law
...
lower left corner
anode rays
47. Cells that convert electrical energy into chemical energy.
electrolytic cells
boiling point
electrolytic reactions
catalysts
48. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
isopiestic process (thermodynamics)
double replacement/displacement
kinetic molecular theory
phase equilibrium
49. Electronegativities _______ as you go down a group.
hydrolysis
negative
metallic
decreases
50. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
positive
Nernst equation
standard atmospheric pressure
bohr model
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