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






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






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






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






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






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






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






8. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.






9. 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.






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






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






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






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






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






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






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






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






19. 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.






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






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






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






23. 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.






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






25. 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






26. *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






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






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






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

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






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






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 _____ 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.






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






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






36. **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.






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






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






39. The vapor pressure increases with increasing _____.






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






41. Metals have electronegativities less than ____






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






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






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






46. 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 _____ _






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






48. 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).






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






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







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