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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. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.


2. Metals have electronegativities less than ____






3. 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.


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






5. The pressure exerted by each gas in a mixture is called its _____ pressure.






6. 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






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






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






9. 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.


10. 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 _____ _






11. Electronegativities _______ as you go down a group.






12. Cells that convert electrical energy into chemical energy.






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






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






15. 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.


16. 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.






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






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






19. 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.


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






21. When an electron moves from an excited state to the ground state - it _______ energy.






22. 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






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






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






25. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






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






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






28. 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.






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






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






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






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






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






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






35. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






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






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






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






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






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






41. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.






42. 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.






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






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






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






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






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






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






49. 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.






50. Electronegativities ________ from left to right in a period.