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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. 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.
2. Metals have electronegativities less than ____
combination
state functions (thermodynamics)
2
Van der Waals
3. 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.
4. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Nernst equation
Charles law
hydrolysis
...
5. The pressure exerted by each gas in a mixture is called its _____ pressure.
state functions (thermodynamics)
combined gas law
increases
partial
6. 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
state (thermodynamics)
irreversible and reversible processes
negative
VSEPR
7. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
metallic
hydrolysis
third law of thermodynamics
...
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.
temperature
boiling point elevation
combination
state functions (thermodynamics)
9. 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.
10. 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
wave mechanical model
sublimation
single replacement/displacement
11. Electronegativities _______ as you go down a group.
isopiestic process (thermodynamics)
combined gas law
activation energy
decreases
12. Cells that convert electrical energy into chemical energy.
isothermal process (thermodynamics)
equation of state
electrolytic cells
limiting law
13. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Boyles law
ideal gas
positive
Le Chatelier's principle
14. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
system (thermodynamics)
first law of thermodynamics
decreases
15. 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.
16. 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.
Van der Waals
irreversible and reversible processes
system (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
17. Heat added to a system and work done by a system are considered _________ quantities.
equation of state
positive
electrolytic cells
isothermal process (thermodynamics)
18. The molecules in a gas are in constant - continueous - random - and straight-line motion.
upper right corner
kinetic molecular theory
ideal gas
isothermal process (thermodynamics)
19. 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.
20. The heat change during a process carried out at a constant pressure.
...
emits (in atomic spectra)
change in enthalpy
reversible reaction
21. When an electron moves from an excited state to the ground state - it _______ energy.
state functions (thermodynamics)
left (Le Chatelier's principle)
zero
emits (in atomic spectra)
22. 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
high
colligative property law
positive charge
Raoult's law
23. The energy required to remove an electron from an isolated atom in its ground state.
increases
ionization energy
adiabatic process (thermodynamics)
molar heat of sublimation
24. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
heat capacity
point particles
Boyles law
positive
25. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
point particles
Boyles law
activation energy
bohr model
26. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Van der Waals
single replacement/displacement
catalysts
Nernst equation
27. This process occurs when the system is maintained at the same temperature throughout an experiment.
activation energy
isothermal process (thermodynamics)
adiabatic process (thermodynamics)
entropy
28. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
boiling point
catalysts
equivalent point
29. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
catalysts
electronegativity
2
30. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
molar heat of sublimation
Valence Shell Electron Pair Repulsion (VSEPR)
single replacement/displacement
emits (in atomic spectra)
31. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
boiling point
heat capacity
entropy
second law of thermodynamics
32. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
system (thermodynamics)
kinetic molecular theory
heats of formation
specific heat
33. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
lower left corner
positive
metallic
boiling point
34. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
positive
electrolytic reactions
equivalent point
metallic
35. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
molar heat of sublimation
reversible
kinetic molecular theory
hybridyzation
36. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
heats of formation
absorbs (in atomic spectra)
electrolytic cells
reversible reaction
37. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
catalysts
electrolytic reactions
equivalent point
38. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
negative
...
hybridyzation
standard atmospheric pressure
39. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
electromotive force (emf)/ cell
Nernst equation
hybridyzation
kinetic molecular theory
40. When the electron moves from the ground state to an excited state - it ______ energy.
negative
absorbs (in atomic spectra)
10 degrees
Van der Waals
41. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
partial
catalysts
bohr model
Van der Waals
42. 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
VSEPR
boiling point
saturated solution
43. The change in enthalpy of an exothermic reaction is ________.
negative
decreases
first law of thermodynamics
kinetic molecular theory
44. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
system (thermodynamics)
positive
heats of formation
45. Rays made up of positive electrodes in basic electron charges.
Raoults law
anode rays
state functions (thermodynamics)
melting point
46. When the rate of evaporation equals the rate of condensation - the system is in __________.
kinetic molecular theory
isopiestic process (thermodynamics)
equilibrium
bohr model
47. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
emits (in atomic spectra)
...
decomposition
48. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Avogrados law
state functions (thermodynamics)
system (thermodynamics)
increases
49. 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.
electrolytic cells
10 degrees
Charles law
reversible reaction
50. Electronegativities ________ from left to right in a period.
system (thermodynamics)
increases
entropy
wave mechanical model