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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. Metals have electronegativities less than ____
emits (in atomic spectra)
isothermal process (thermodynamics)
2
heats of formation
2. In an endothermic process - energy is absorbed and ^E is _______.
system (thermodynamics)
dynamic equilibrium
catalysts
positive
3. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
equation of state
Avogrados law
positive
kinetic molecular theory
4. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
heat capacity
state functions (thermodynamics)
Van der Waals
temperature
5. A chemical reaction formed from the union of its elements.
combination
electrolytic reactions
crystallizes
wave mechanical model
6. The energy required to remove an electron from an isolated atom in its ground state.
ionization energy
...
left (Le Chatelier's principle)
upper right corner
7. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
left - right (Le Chatelier's principle)
electrolytic reactions
Van der Waals
kinetic molecular theory
8. **Proceeding across a period from left to right - the ionization energy _______.
increases
ionization energy
Daltons law
state (thermodynamics)
9. A hypothetical gas would follow Boyles law under all conditions and is called?
heat capacity
ideal gas
first law of thermodynamics
Nernst equation
10. A state function in which it is the heat content of a substance.
enthalpy
second law of thermodynamics
crystallizes
irreversible and reversible processes
11. 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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12. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Nernst equation
heat capacity
Charles law
hybridyzation
13. The heat required to change 1mole of solid completely to vapor.
...
molar heat of sublimation
entropy
phase equilibrium
14. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).
bohr model
state (thermodynamics)
catalysts
state functions (thermodynamics)
15. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
2
...
heats of formation
zero
16. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
Boyles law
base - acid
point particles
17. 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.
left - right (Le Chatelier's principle)
valence
positive
electronegativity
18. The most active metals are found in what corner of the periodic table?
ideal gas
lower left corner
zero
temperature
19. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
metallic
single replacement/displacement
high
kinetic molecular theory
20. The heat change during a process carried out at a constant pressure.
change in enthalpy
combination
increasing
zero
21. The freezing point is always lowered by addition of solute.
Avogrados law
positive charge
increases
freezing point depression
22. 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.
electrolytic reactions
Van der Waals
equivalent point
enthalpy
23. Rays made up of electrons in basic electron charges.
limiting law
hybridyzation
cathode rays
high
24. 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.
titration
base - acid
activation energy barrier (Le Chatelier's principle)
specific heat
25. *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
sublimation
valence
single replacement/displacement
equivalent point
26. Cells that convert electrical energy into chemical energy.
state (thermodynamics)
emits (in atomic spectra)
Van der Waals
electrolytic cells
27. 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.
Raoults law
decreases
ionization energy
Van der Waals
28. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
dynamic equilibrium
emits (in atomic spectra)
base - acid
valence
29. 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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30. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
pressure
10 degrees
cathode rays
electrolytic reactions
31. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
Charles law
single replacement/displacement
entropy
upper right corner
32. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
wave mechanical model
Van der Waals
right (Le Chatelier's principle)
33. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
high
irreversible and reversible processes
phase equilibrium
boiling point elevation
34. The temperature at which a substance's solid and liquid phases are in equilibrium.
positive
single replacement/displacement
melting point
dynamic equilibrium
35. 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 _____ _
increases
limiting law
left (Le Chatelier's principle)
zero
36. 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.
Raoults law
Charles law
Valence Shell Electron Pair Repulsion (VSEPR)
Van der Waals
37. Heat added to a system and work done by a system are considered _________ quantities.
point particles
positive
third law of thermodynamics
kinetic molecular theory
38. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
catalysts
Nernst equation
titration
kinetic molecular theory
39. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
10 degrees
standard atmospheric pressure
electromotive force (emf)/ cell
2
40. 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.
Le Chatelier's principle
VSEPR
isopiestic process (thermodynamics)
negative
41. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
cathode rays
limiting law
saturated solution
42. The action of salts of weak acids or bases with water to form acidic or basic solutions.
change in enthalpy
hydrolysis
Daltons law
hybridyzation
43. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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44. Rays made up of positive electrodes in basic electron charges.
adiabatic process (thermodynamics)
negative
increases
anode rays
45. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
boiling point
increases
pressure
46. The change in enthalpy of an exothermic reaction is ________.
emits (in atomic spectra)
negative
crystallizes
...
47. 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
Van der Waals
kinetic molecular theory
48. 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
limiting law
temperature
ideal gas
irreversible and reversible processes
49. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
electromotive force (emf)/ cell
Charles law
limiting law
double replacement/displacement
50. 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.
positive
Charles law
first law of thermodynamics
reversible