Instructions:

• Answer 50 questions in 15 minutes.
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• Match each statement with the correct term.
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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 _____ 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.
change in enthalpy
increases
catalysts
combination


2. 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
electrolytic reactions
Van der Waals
positive charge
crystallizes


3. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
boiling point elevation
left (Le Chatelier's principle)
zero
valence


4. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
double replacement/displacement
increases
vapor pressure


5. 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.
10 degrees
Valence Shell Electron Pair Repulsion (VSEPR)
single replacement/displacement
phase equilibrium


6. 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.

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7. The heat change during a process carried out at a constant pressure.
change in enthalpy
heats of formation
melting point
emits (in atomic spectra)


8. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
end point
increases
melting point
single replacement/displacement


9. *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
valence
change in enthalpy
zero
isopiestic process (thermodynamics)


10. Rays made up of positive electrodes in basic electron charges.
anode rays
saturated solution
molar heat of sublimation
crystallizes


11. In an exothermic process - energy is released and ^E of reaction is ________.
Boyles law
temperature
kinetic molecular theory
negative


12. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
left (Le Chatelier's principle)
limiting law
Van der Waals
positive charge


13. 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.
Daltons law
Avogrados law
irreversible and reversible processes
pressure


14. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
equilibrium
Valence Shell Electron Pair Repulsion (VSEPR)
Daltons law
metallic


15. **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
combination
increases
...


16. A process that occurs whent eh system is maintained at constant pressure.
sublimation
metallic
isopiestic process (thermodynamics)
double replacement/displacement


17. _____ bonds are present in molecules containing double or triple bonds.
increases
pi bonds
first law of thermodynamics
point particles


18. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
sublimation
lower left corner
electromotive force (emf)/ cell
entropy


19. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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20. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.
wave mechanical model
combined gas law
Avogrados law
colligative property law


21. 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).
zero
heat capacity
single replacement/displacement
state (thermodynamics)


22. *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
decreases
molar heat of sublimation


23. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
single replacement/displacement
positive charge
emits (in atomic spectra)


24. 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.
Le Chatelier's principle
kinetic molecular theory
lower left corner
heat capacity


25. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
kinetic molecular theory
boiling point
increases
reversible reaction


26. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
Valence Shell Electron Pair Repulsion (VSEPR)
electronegativity
...


27. A chemical reaction formed from the union of its elements.
combination
Van der Waals
Van der Waals
left - right (Le Chatelier's principle)


28. 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.

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29. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
heat capacity
combination
ideal gas


30. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
bohr model
second law of thermodynamics
total pressure (Le Chatelier's principle)
negative


31. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
third law of thermodynamics
increases
wave mechanical model
heat capacity


32. 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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33. The most active nonmetals are found in what corner of the periodic table?
limiting law
right (Le Chatelier's principle)
upper right corner
Van der Waals


34. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
reversible
10 degrees
Nernst equation
Raoults law


35. 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.
first law of thermodynamics
left (Le Chatelier's principle)
Boyles law
cathode rays


36. The energy required to remove an electron from an isolated atom in its ground state.
kinetic molecular theory
state functions (thermodynamics)
ionization energy
Van der Waals


37. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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38. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
zero
third law of thermodynamics
Charles law
sublimation


39. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
state functions (thermodynamics)
increasing
increases
electromotive force (emf)/ cell


40. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
Charles law
wave mechanical model
total pressure (Le Chatelier's principle)


41. The freezing point is always lowered by addition of solute.
freezing point depression
isothermal process (thermodynamics)
decomposition
positive


42. Cells that convert electrical energy into chemical energy.
electrolytic cells
total pressure (Le Chatelier's principle)
boiling point
Avogrados law


43. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
non-ideal
kinetic molecular theory
Raoults law
absorbs (in atomic spectra)


44. 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 _____ _
electrolytic cells
colligative property law
limiting law
Valence Shell Electron Pair Repulsion (VSEPR)


45. 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.
Van der Waals
first law of thermodynamics
kinetic molecular theory
melting point


46. In an endothermic process - energy is absorbed and ^E is _______.
Avogrados law
state (thermodynamics)
isothermal process (thermodynamics)
positive


47. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
...
crystallizes
catalysts
Daltons law


48. 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
Avogrados law
sublimation


49. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
double replacement/displacement
heat capacity
kinetic molecular theory


50. 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
zero
system (thermodynamics)
point particles