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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 enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






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






3. A solution in which solid solute is in equilibrium with dissolved solute.






4. 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.






5. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






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






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






8. 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.






9. 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






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






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






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






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






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






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






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






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






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






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






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






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






23. Metals have electronegativities less than ____






24. 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.






25. 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.






26. 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.






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






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






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






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






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






32. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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33. **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.






34. 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






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






36. 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.






37. 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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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 heat change during a process carried out at a constant pressure.






40. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






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






43. 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.

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44. *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.






45. 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.

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






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






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






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






50. 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.