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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. 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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2. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






3. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






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






5. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






7. 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).






8. The change in enthalpy of an endothermic reaction is ________.






9. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






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






11. Metals have electronegativities less than ____






12. The change in enthalpy of an exothermic reaction is ________.






13. **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.






14. 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.






15. 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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16. 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.






17. The most active metals are found in what corner of the periodic table?






18. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






19. 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






20. 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.






21. 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.






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. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






25. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






26. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






27. _______ has very little effect on the solubility of liquids or solids in liquid solvents.






28. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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29. 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.






30. Heat added to a system and work done by a system are considered _________ quantities.






31. The temperature at which a substance's solid and liquid phases are in equilibrium.






32. This process occurs when the system is maintained at the same temperature throughout an experiment.






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






34. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






35. 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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36. This process occurs when the system is thermally isolated so that no heat enters or leaves.






37. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






38. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






39. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






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






41. *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.






42. 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.






43. The heat change during a process carried out at a constant pressure.






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

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






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






47. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






48. When the electron moves from the ground state to an excited state - it ______ energy.






49. 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.






50. Electronegativities _______ as you go down a group.