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






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






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






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






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






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






7. 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).






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






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






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






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






12. 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.






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






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 thermally isolated so that no heat enters or leaves.






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






17. 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






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






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






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






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






22. 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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23. *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.






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






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






26. The vapor pressure increases with increasing _____.






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






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






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






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






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






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






33. 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.






34. 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.






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






36. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






37. 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.






38. 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.






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






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






41. 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.

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42. 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.






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






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






45. 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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46. 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.






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






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






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






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







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