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






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






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






4. 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.






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






6. *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.






7. 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.






8. 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.






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






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






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






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






13. *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






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






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






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






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






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






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






20. Metals have electronegativities less than ____






21. 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.


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






23. Cells that convert electrical energy into chemical energy.






24. 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.


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






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






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






28. 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.






29. 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.






30. The vapor pressure increases with increasing _____.






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






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






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


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






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






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






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






38. 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.






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






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. 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).






42. 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.






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






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






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






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






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






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






49. 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.






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