Test your basic knowledge |

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


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






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






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






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






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






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






8. The vapor pressure increases with increasing _____.






9. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






11. Cells that convert electrical energy into chemical energy.






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






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






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






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






17. 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.






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






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






20. **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.






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






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






23. 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






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






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






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






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






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






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






30. 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.






31. 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






32. 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.






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






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






35. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






36. 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.


37. 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.






38. 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.






39. 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).






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






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






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






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






44. 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






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


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






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






48. 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).






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






50. 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.