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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 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.
combined gas law
2
temperature
equation of state
2. 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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3. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
positive
kinetic molecular theory
decomposition
combination
4. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
wave mechanical model
electromotive force (emf)/ cell
hydrolysis
kinetic molecular theory
5. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
state (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
Avogrados law
negative
6. The molecules in a gas are in constant - continueous - random - and straight-line motion.
single replacement/displacement
kinetic molecular theory
decomposition
freezing point depression
7. The pressure exerted by each gas in a mixture is called its _____ pressure.
VSEPR
partial
decreases
end point
8. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
...
electronegativity
hybridyzation
positive
9. 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.
left (Le Chatelier's principle)
third law of thermodynamics
temperature
titration
10. *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.
Le Chatelier's principle
...
enthalpy
Avogrados law
11. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
adiabatic process (thermodynamics)
heats of formation
kinetic molecular theory
absorbs (in atomic spectra)
12. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
high
first law of thermodynamics
standard atmospheric pressure
upper right corner
13. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
non-ideal
bohr model
electronegativity
base - acid
14. 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.
kinetic molecular theory
metallic
Le Chatelier's principle
limiting law
15. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Nernst equation
increases
increasing
end point
16. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
third law of thermodynamics
negative
...
right (Le Chatelier's principle)
17. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
Van der Waals
2
electrolytic cells
18. The energy required to remove an electron from an isolated atom in its ground state.
freezing point depression
ionization energy
saturated solution
left - right (Le Chatelier's principle)
19. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
third law of thermodynamics
second law of thermodynamics
equilibrium
molar heat of sublimation
20. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
single replacement/displacement
boiling point elevation
Boyles law
equivalent point
21. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
saturated solution
entropy
point particles
combined gas law
22. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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23. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
colligative property law
reversible
dynamic equilibrium
Raoult's law
24. 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.
entropy
increases
anode rays
Daltons law
25. In an endothermic process - energy is absorbed and ^E is _______.
positive
cathode rays
colligative property law
high
26. *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.
increases
hybridyzation
increases
wave mechanical model
27. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Boyles law
positive
dynamic equilibrium
bohr model
28. Electronegativities ________ from left to right in a period.
zero
specific heat
heat capacity
increases
29. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
increases
activation energy
single replacement/displacement
30. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
electrolytic cells
negative
decomposition
31. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
total pressure (Le Chatelier's principle)
Le Chatelier's principle
Charles law
32. Metals have electronegativities less than ____
reversible reaction
activation energy barrier (Le Chatelier's principle)
2
single replacement/displacement
33. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
kinetic molecular theory
boiling point
Nernst equation
crystallizes
34. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
reversible reaction
Le Chatelier's principle
kinetic molecular theory
emits (in atomic spectra)
35. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Nernst equation
Van der Waals
Charles law
hybridyzation
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. A hypothetical gas would follow Boyles law under all conditions and is called?
positive
state (thermodynamics)
increasing
ideal gas
38. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
point particles
positive
phase equilibrium
pi bonds
39. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
isopiestic process (thermodynamics)
colligative property law
metallic
equation of state
40. When the rate of evaporation equals the rate of condensation - the system is in __________.
...
absorbs (in atomic spectra)
equilibrium
hydrolysis
41. 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
Van der Waals
positive charge
ionization energy
Valence Shell Electron Pair Repulsion (VSEPR)
42. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
decreases
equivalent point
Boyles law
vapor pressure
43. Liquids with strong attractive forces have ______ boiling points.
molar heat of sublimation
high
second law of thermodynamics
irreversible and reversible processes
44. A process that occurs whent eh system is maintained at constant pressure.
Charles law
combination
isopiestic process (thermodynamics)
heats of formation
45. Electronegativities _______ as you go down a group.
adiabatic process (thermodynamics)
isothermal process (thermodynamics)
Boyles law
decreases
46. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
Charles law
specific heat
enthalpy
combination
47. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
VSEPR
decomposition
bohr model
kinetic molecular theory
48. 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
electronegativity
freezing point depression
Le Chatelier's principle
49. Rays made up of electrons in basic electron charges.
cathode rays
system (thermodynamics)
combined gas law
decreases
50. The change in enthalpy of an endothermic reaction is ________.
positive
...
kinetic molecular theory
temperature