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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. 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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2. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






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






4. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






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






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






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






9. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.






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






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






12. 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.






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






14. 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.






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






16. 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






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






18. 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.






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






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






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






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






23. *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






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






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






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






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






28. A process that occurs whent eh system is maintained at constant pressure.






29. 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






30. **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.






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






32. 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 _____ _






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

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34. 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.






35. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






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






37. 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.






38. 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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39. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






40. 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.






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






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






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






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






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






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






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






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






49. 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.






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







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