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






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






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






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






5. 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.






6. *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






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


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






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






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






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






12. 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.


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






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






16. 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.






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






18. 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.






19. 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.






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






21. A state function in which it is the heat content of a substance.






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






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






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






25. 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.


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






27. 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).






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






29. 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.






30. 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.






31. 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.






32. *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.






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






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






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






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






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






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






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






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






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






42. 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






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






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






45. Liquids with strong attractive forces have ______ boiling points.






46. 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 _____ _






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






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






49. 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






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