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CLEP Chemistry 1

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 _____ 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.






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






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.






4. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.






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.






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.






8. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






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






10. Rays made up of positive electrodes in basic electron charges.






11. In an exothermic process - energy is released and ^E of reaction is ________.






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.






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.






14. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






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.






16. A process that occurs whent eh system is maintained at constant pressure.






17. _____ bonds are present in molecules containing double or triple bonds.






18. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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.






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).






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.






23. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






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.






25. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






26. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






27. A chemical reaction formed from the union of its elements.






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.






30. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






31. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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?






34. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






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.






36. The energy required to remove an electron from an isolated atom in its ground state.






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.






39. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






40. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






41. The freezing point is always lowered by addition of solute.






42. Cells that convert electrical energy into chemical energy.






43. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






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 _____ _






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.






46. In an endothermic process - energy is absorbed and ^E is _______.






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






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.






49. Deviations from Boyles law that occur with real gases represent _______ behavior.






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.







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