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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.
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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. 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.
pi bonds
Raoults law
freezing point depression
Le Chatelier's principle
2. *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.
change in enthalpy
positive charge
equation of state
melting point
3. This process occurs when the system is thermally isolated so that no heat enters or leaves.
point particles
positive
anode rays
adiabatic process (thermodynamics)
4. 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.
hydrolysis
combined gas law
Van der Waals
increases
5. When the electron moves from the ground state to an excited state - it ______ energy.
activation energy
...
adiabatic process (thermodynamics)
absorbs (in atomic spectra)
6. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
state (thermodynamics)
base - acid
standard atmospheric pressure
high
7. Cells that convert electrical energy into chemical energy.
Daltons law
electrolytic cells
decreases
limiting law
8. The temperature at which a substance's solid and liquid phases are in equilibrium.
wave mechanical model
Boyles law
standard atmospheric pressure
melting point
9. 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.
Charles law
Le Chatelier's principle
kinetic molecular theory
combined gas law
10. A state function in which it is the heat content of a substance.
catalysts
positive
enthalpy
lower left corner
11. Electronegativities _______ as you go down a group.
decreases
Le Chatelier's principle
boiling point
catalysts
12. In titration - this is the point at which a particular indicator changes color.
Nernst equation
kinetic molecular theory
end point
increases
13. The change in enthalpy of an endothermic reaction is ________.
absorbs (in atomic spectra)
standard atmospheric pressure
left (Le Chatelier's principle)
positive
14. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
positive
increases
pressure
boiling point
15. 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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16. 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
positive charge
...
high
decreases
17. In an exothermic process - energy is released and ^E of reaction is ________.
sublimation
negative
heats of formation
double replacement/displacement
18. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
kinetic molecular theory
electronegativity
activation energy
reversible
19. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
total pressure (Le Chatelier's principle)
combination
pressure
2
20. 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.
point particles
pressure
combination
Daltons law
21. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
negative
heats of formation
Raoult's law
boiling point elevation
22. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
end point
negative
decomposition
boiling point elevation
23. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
decomposition
pi bonds
sublimation
24. The most active metals are found in what corner of the periodic table?
lower left corner
heat capacity
titration
activation energy barrier (Le Chatelier's principle)
25. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
Van der Waals
Charles law
second law of thermodynamics
electromotive force (emf)/ cell
26. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
...
heat capacity
equivalent point
kinetic molecular theory
27. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.
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28. The heat required to change 1mole of solid completely to vapor.
lower left corner
left - right (Le Chatelier's principle)
molar heat of sublimation
reversible reaction
29. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
boiling point elevation
partial
hydrolysis
30. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
melting point
electromotive force (emf)/ cell
Boyles law
equivalent point
31. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
enthalpy
emits (in atomic spectra)
change in enthalpy
32. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
increases
...
hydrolysis
decomposition
33. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
equilibrium
boiling point elevation
system (thermodynamics)
metallic
34. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
activation energy barrier (Le Chatelier's principle)
pressure
kinetic molecular theory
35. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
wave mechanical model
electrolytic reactions
change in enthalpy
heats of formation
36. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
limiting law
entropy
vapor pressure
absorbs (in atomic spectra)
37. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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38. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
metallic
vapor pressure
wave mechanical model
39. 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.
electronegativity
equation of state
VSEPR
saturated solution
40. **Proceeding across a period from left to right - the ionization energy _______.
increases
irreversible and reversible processes
absorbs (in atomic spectra)
limiting law
41. 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.
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42. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
titration
heats of formation
positive
43. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
combined gas law
upper right corner
Avogrados law
positive
44. 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.
combination
anode rays
VSEPR
2
45. Liquids with strong attractive forces have ______ boiling points.
heat capacity
high
valence
first law of thermodynamics
46. The molecules in a gas are in constant - continueous - random - and straight-line motion.
Le Chatelier's principle
kinetic molecular theory
non-ideal
combination
47. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
boiling point elevation
emits (in atomic spectra)
entropy
moles (Le Chatelier's principle)
48. *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
valence
pi bonds
Raoult's law
Nernst equation
49. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
third law of thermodynamics
positive
decreases
enthalpy
50. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
double replacement/displacement
hybridyzation
decreases
Van der Waals
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