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






2. *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






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






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






6. 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






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






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






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






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






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






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






13. 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.






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






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

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






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






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






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






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






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






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






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






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






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






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






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






28. **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.






29. 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






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






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






32. 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.






33. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






34. 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).






35. 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.






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






37. The change in enthalpy of an exothermic reaction is ________.






38. 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.






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






40. 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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41. Metals have electronegativities less than ____






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






43. Cells that convert electrical energy into chemical energy.






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






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






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






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






48. *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.






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






50. 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.