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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. 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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2. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
temperature
kinetic molecular theory
Avogrados law
increases
3. In an exothermic process - energy is released and ^E of reaction is ________.
bohr model
Avogrados law
third law of thermodynamics
negative
4. 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
titration
state (thermodynamics)
positive charge
boiling point elevation
5. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
combination
titration
Raoult's law
6. 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
kinetic molecular theory
temperature
crystallizes
7. **Proceeding across a period from left to right - the ionization energy _______.
increases
kinetic molecular theory
Avogrados law
moles (Le Chatelier's principle)
8. The most active nonmetals are found in what corner of the periodic table?
upper right corner
absorbs (in atomic spectra)
Van der Waals
catalysts
9. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
heats of formation
double replacement/displacement
enthalpy
sublimation
10. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
emits (in atomic spectra)
ionization energy
Van der Waals
Raoults law
11. In titration - this is the point at which a particular indicator changes color.
temperature
emits (in atomic spectra)
end point
catalysts
12. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
electronegativity
adiabatic process (thermodynamics)
sublimation
combined gas law
13. 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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14. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
heats of formation
electromotive force (emf)/ cell
Daltons law
specific heat
15. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
electronegativity
10 degrees
reversible reaction
reversible
16. Electronegativities ________ from left to right in a period.
saturated solution
system (thermodynamics)
valence
increases
17. Electronegativities _______ as you go down a group.
decreases
10 degrees
positive
electronegativity
18. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
Charles law
system (thermodynamics)
right (Le Chatelier's principle)
19. This process occurs when the system is thermally isolated so that no heat enters or leaves.
decreases
bohr model
boiling point elevation
adiabatic process (thermodynamics)
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.
10 degrees
first law of thermodynamics
Daltons law
equation of state
21. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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22. Metals have electronegativities less than ____
vapor pressure
negative
pressure
2
23. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
crystallizes
10 degrees
specific heat
24. 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.
positive
VSEPR
isothermal process (thermodynamics)
left - right (Le Chatelier's principle)
25. A hypothetical gas would follow Boyles law under all conditions and is called?
isopiestic process (thermodynamics)
electronegativity
sublimation
ideal gas
26. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
right (Le Chatelier's principle)
Boyles law
positive
ideal gas
27. The heat change during a process carried out at a constant pressure.
Boyles law
emits (in atomic spectra)
single replacement/displacement
change in enthalpy
28. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
increases
vapor pressure
kinetic molecular theory
hybridyzation
29. The action of salts of weak acids or bases with water to form acidic or basic solutions.
temperature
system (thermodynamics)
total pressure (Le Chatelier's principle)
hydrolysis
30. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
state functions (thermodynamics)
heats of formation
kinetic molecular theory
31. 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.
freezing point depression
electronegativity
Nernst equation
electrolytic reactions
32. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.
entropy
metallic
equation of state
colligative property law
33. The change in enthalpy of an endothermic reaction is ________.
positive
upper right corner
kinetic molecular theory
moles (Le Chatelier's principle)
34. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
kinetic molecular theory
Charles law
phase equilibrium
35. 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.
kinetic molecular theory
molar heat of sublimation
state (thermodynamics)
state functions (thermodynamics)
36. The energy required to remove an electron from an isolated atom in its ground state.
non-ideal
ionization energy
Raoult's law
third law of thermodynamics
37. 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).
Charles law
Le Chatelier's principle
Van der Waals
dynamic equilibrium
38. The freezing point is always lowered by addition of solute.
Boyles law
freezing point depression
temperature
entropy
39. 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
Daltons law
catalysts
Charles law
40. A state function in which it is the heat content of a substance.
boiling point
enthalpy
entropy
hydrolysis
41. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
crystallizes
vapor pressure
increases
42. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
Charles law
third law of thermodynamics
positive
43. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
positive charge
valence
second law of thermodynamics
44. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
metallic
base - acid
upper right corner
zero
45. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
specific heat
Nernst equation
Charles law
catalysts
46. 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.
positive
entropy
enthalpy
equivalent point
47. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
positive
entropy
partial
irreversible and reversible processes
48. Rays made up of positive electrodes in basic electron charges.
bohr model
molar heat of sublimation
anode rays
entropy
49. 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.
wave mechanical model
negative
phase equilibrium
titration
50. *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
upper right corner
valence
10 degrees
limiting law