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






2. *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.






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

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4. 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.






5. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






7. 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






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






9. The vapor pressure increases with increasing _____.






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






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






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






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






14. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






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






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






17. 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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18. *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






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






20. 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.






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






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






23. A hypothetical gas would follow Boyles law under all conditions and is called?






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






25. 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.






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






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






28. 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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29. Liquids with strong attractive forces have ______ boiling points.






30. The most active nonmetals are found in what corner of the periodic table?






31. The heat required to change 1mole of solid completely to vapor.






32. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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






34. In titration - this is the point at which a particular indicator changes color.






35. **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.






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






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






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






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






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






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






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






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






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






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






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






47. 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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48. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.






49. 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.






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