SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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 freezing point is always lowered by addition of solute.
kinetic molecular theory
moles (Le Chatelier's principle)
activation energy
freezing point depression
2. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
molar heat of sublimation
catalysts
Boyles law
activation energy barrier (Le Chatelier's principle)
3. 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.
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
4. A state function in which it is the heat content of a substance.
increasing
2
enthalpy
Van der Waals
5. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
increases
zero
phase equilibrium
kinetic molecular theory
6. Electronegativities ________ from left to right in a period.
positive charge
increases
Daltons law
saturated solution
7. In an endothermic process - energy is absorbed and ^E is _______.
...
pressure
positive
electrolytic cells
8. Liquids with strong attractive forces have ______ boiling points.
absorbs (in atomic spectra)
positive charge
...
high
9. The energy required to remove an electron from an isolated atom in its ground state.
Charles law
increases
left - right (Le Chatelier's principle)
ionization energy
10. 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
Boyles law
bohr model
absorbs (in atomic spectra)
Nernst equation
11. *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
equilibrium
Boyles law
valence
electrolytic reactions
12. Cells that convert electrical energy into chemical energy.
electrolytic cells
reversible
increases
Van der Waals
13. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
double replacement/displacement
non-ideal
positive
14. 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.
Nernst equation
Van der Waals
isopiestic process (thermodynamics)
base - acid
15. 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.
titration
VSEPR
enthalpy
negative
16. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
molar heat of sublimation
base - acid
end point
second law of thermodynamics
17. Metals have electronegativities less than ____
phase equilibrium
saturated solution
non-ideal
2
18. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
combination
Le Chatelier's principle
Valence Shell Electron Pair Repulsion (VSEPR)
19. 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.
Charles law
limiting law
positive
reversible
20. 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.
isopiestic process (thermodynamics)
specific heat
catalysts
equivalent point
21. The heat change during a process carried out at a constant pressure.
change in enthalpy
boiling point elevation
Valence Shell Electron Pair Repulsion (VSEPR)
activation energy barrier (Le Chatelier's principle)
22. A solution in which solid solute is in equilibrium with dissolved solute.
decreases
heat capacity
saturated solution
left (Le Chatelier's principle)
23. **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.
...
Van der Waals
first law of thermodynamics
colligative property law
24. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
bohr model
decreases
electromotive force (emf)/ cell
25. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
system (thermodynamics)
decreases
Valence Shell Electron Pair Repulsion (VSEPR)
electrolytic cells
26. Rays made up of electrons in basic electron charges.
cathode rays
hybridyzation
single replacement/displacement
decreases
27. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
decreases
double replacement/displacement
combination
increases
28. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
pi bonds
system (thermodynamics)
standard atmospheric pressure
Raoults law
29. This process occurs when the system is thermally isolated so that no heat enters or leaves.
left - right (Le Chatelier's principle)
equation of state
adiabatic process (thermodynamics)
specific heat
30. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
positive
Nernst equation
right (Le Chatelier's principle)
Avogrados law
31. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
metallic
kinetic molecular theory
Van der Waals
boiling point elevation
32. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Avogrados law
emits (in atomic spectra)
Nernst equation
freezing point depression
33. 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.
electronegativity
colligative property law
titration
heat capacity
34. 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.
...
Valence Shell Electron Pair Repulsion (VSEPR)
zero
emits (in atomic spectra)
35. 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
combined gas law
irreversible and reversible processes
electromotive force (emf)/ cell
boiling point elevation
36. 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.
increases
VSEPR
state functions (thermodynamics)
kinetic molecular theory
37. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
Valence Shell Electron Pair Repulsion (VSEPR)
metallic
...
activation energy barrier (Le Chatelier's principle)
38. The molecules in a gas are in constant - continueous - random - and straight-line motion.
partial
Avogrados law
kinetic molecular theory
Van der Waals
39. 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.
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
40. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
decreases
Raoults law
Van der Waals
41. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
saturated solution
limiting law
state functions (thermodynamics)
increases
42. *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.
Van der Waals
...
Daltons law
titration
43. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
Le Chatelier's principle
Valence Shell Electron Pair Repulsion (VSEPR)
kinetic molecular theory
equivalent point
44. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
Nernst equation
metallic
boiling point elevation
anode rays
45. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
specific heat
kinetic molecular theory
...
moles (Le Chatelier's principle)
46. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
bohr model
negative
hybridyzation
lower left corner
47. 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.
standard atmospheric pressure
electrolytic reactions
colligative property law
double replacement/displacement
48. The most active metals are found in what corner of the periodic table?
wave mechanical model
zero
lower left corner
ionization energy
49. **Proceeding across a period from left to right - the ionization energy _______.
pressure
increases
bohr model
isopiestic process (thermodynamics)
50. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183