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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. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
decomposition
limiting law
base - acid
2. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
partial
Nernst equation
kinetic molecular theory
sublimation
3. The most active metals are found in what corner of the periodic table?
titration
partial
positive charge
lower left corner
4. The change in enthalpy of an endothermic reaction is ________.
upper right corner
reversible
positive
absorbs (in atomic spectra)
5. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
...
vapor pressure
pressure
reversible reaction
6. 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.
7. 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.
Charles law
system (thermodynamics)
combination
kinetic molecular theory
8. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
crystallizes
state functions (thermodynamics)
third law of thermodynamics
valence
9. Rays made up of electrons in basic electron charges.
cathode rays
ideal gas
colligative property law
positive
10. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
titration
pressure
heats of formation
11. A hypothetical gas would follow Boyles law under all conditions and is called?
positive
combination
left (Le Chatelier's principle)
ideal gas
12. 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.
partial
sublimation
non-ideal
catalysts
13. In titration - this is the point at which a particular indicator changes color.
increases
combination
end point
second law of thermodynamics
14. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
point particles
decreases
sublimation
isopiestic process (thermodynamics)
15. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.
equivalent point
ideal gas
2
molar heat of sublimation
16. 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
bohr model
kinetic molecular theory
vapor pressure
Charles law
17. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
positive
...
pi bonds
point particles
18. The pressure exerted by each gas in a mixture is called its _____ pressure.
left - right (Le Chatelier's principle)
partial
phase equilibrium
metallic
19. 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.
double replacement/displacement
electronegativity
kinetic molecular theory
increases
20. 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.
equation of state
activation energy
first law of thermodynamics
lower left corner
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.
lower left corner
Van der Waals
boiling point elevation
...
22. A state function in which it is the heat content of a substance.
10 degrees
change in enthalpy
enthalpy
...
23. The molecules in a gas are in constant - continueous - random - and straight-line motion.
colligative property law
2
pressure
kinetic molecular theory
24. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
anode rays
Valence Shell Electron Pair Repulsion (VSEPR)
10 degrees
isothermal process (thermodynamics)
25. 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
temperature
combination
positive charge
base - acid
26. **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.
Raoults law
isothermal process (thermodynamics)
cathode rays
...
27. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
28. 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.
melting point
reversible
equivalent point
decreases
29. *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
increases
second law of thermodynamics
positive
valence
30. 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.
31. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
third law of thermodynamics
Avogrados law
kinetic molecular theory
positive
32. Liquids with strong attractive forces have ______ boiling points.
Nernst equation
negative
high
sublimation
33. _____ bonds are present in molecules containing double or triple bonds.
limiting law
equation of state
pi bonds
system (thermodynamics)
34. *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.
2
...
high
freezing point depression
35. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
increases
...
zero
upper right corner
36. The energy required to remove an electron from an isolated atom in its ground state.
Nernst equation
ionization energy
heat capacity
point particles
37. The action of salts of weak acids or bases with water to form acidic or basic solutions.
cathode rays
Le Chatelier's principle
hydrolysis
Van der Waals
38. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
isopiestic process (thermodynamics)
increases
Daltons law
39. 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.
40. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
lower left corner
Van der Waals
second law of thermodynamics
41. *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.
equation of state
Le Chatelier's principle
point particles
enthalpy
42. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
negative
catalysts
...
43. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
...
vapor pressure
molar heat of sublimation
state functions (thermodynamics)
44. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
change in enthalpy
adiabatic process (thermodynamics)
activation energy barrier (Le Chatelier's principle)
Charles law
45. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
vapor pressure
...
combined gas law
activation energy
46. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
Boyles law
reversible
positive
kinetic molecular theory
47. The change in enthalpy of an exothermic reaction is ________.
Van der Waals
negative
standard atmospheric pressure
irreversible and reversible processes
48. Metals have electronegativities less than ____
increasing
2
adiabatic process (thermodynamics)
positive
49. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.
...
hybridyzation
Daltons law
state functions (thermodynamics)
50. 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).
Nernst equation
Van der Waals
positive
limiting law