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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. The molecules in a gas are in constant - continueous - random - and straight-line motion.






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






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






6. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






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






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






9. 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.






10. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






11. 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






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






13. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






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. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






16. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






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






18. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.






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






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






21. Rays made up of electrons in basic electron charges.






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






23. 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 _____ _






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.






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






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






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






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






29. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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






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






32. 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).






33. 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.






34. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






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






36. 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






37. 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.






38. 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.






39. **Proceeding across a period from left to right - the ionization energy _______.






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






41. 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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42. When the rate of evaporation equals the rate of condensation - the system is in __________.






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






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






45. 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






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






47. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






48. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






49. *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






50. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.