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






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






4. 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






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






6. 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.






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






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






9. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






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






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






12. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






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






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






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






17. Electronegativities _______ as you go down a group.






18. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






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






20. 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.






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

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22. Metals have electronegativities less than ____






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






24. 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.






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






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






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






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






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






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






31. 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.






32. 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.






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






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






35. 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.






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






37. 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).






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






39. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _






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






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






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






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






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






45. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






46. 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.






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






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






49. 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.






50. *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