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






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






3. **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.






4. 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.


5. 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






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






7. 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).






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






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






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






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






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






13. 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.






14. Rays made up of electrons in basic electron charges.






15. 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.






16. Electronegativities _______ as you go down a group.






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






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






19. 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.






20. 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.






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






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






23. *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.






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






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






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






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


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






29. 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.






30. The vapor pressure increases with increasing _____.






31. 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 _______.


32. 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.






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






34. 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






35. 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.


36. 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






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






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






39. 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.






40. 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.


41. This process occurs when the system is thermally isolated so that no heat enters or leaves.






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






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






44. 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.


45. 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).






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






47. 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.






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






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






50. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____