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






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






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






4. 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.






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






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






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






9. Metals have electronegativities less than ____






10. The vapor pressure increases with increasing _____.






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






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






13. 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.






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






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






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






17. 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.






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






19. Electronegativities _______ as you go down a group.






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






21. 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.






22. _______ has very little effect on the solubility of liquids or solids in liquid solvents.






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






24. 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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25. 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.






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






27. 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






28. 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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29. Rays made up of positive electrodes in basic electron charges.






30. 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.






31. 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.






32. 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).






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






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






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






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






37. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.

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






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






40. 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.






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






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






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






44. 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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45. 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.






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






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






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






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






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