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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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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. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






2. Elements in the middle of the periodic table - in groups 3-12.






3. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






4. A solid made up of particles that are not arranged in a regular pattern.






5. A horizontal row of elements in the periodic table






6. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






7. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






8. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






9. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






10. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






11. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






12. The energy required to break a chemical bond and form neutral isolated atoms






13. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






14. Two or more atoms held together by covalent bonds






15. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






16. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






17. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






18. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






19. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






20. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






21. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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22. The process of decomposing a chemical compound by the passage of an electric current.






23. Small discrete increments of energy.






24. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






25. The lowest allowable energy state of an atom






26. A dynamic condition in which two opposing changes occur at equal rates in a closed system






27. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






28. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






29. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






30. The area of chemistry that is concerned with reaction rates and reaction mechanisms






31. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






32. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






33. E=hc/?






34. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






35. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






36. The Percent by mass of each element in a compound.






37. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






38. The percent by mass of each element in a compound






39. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






40. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






41. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






42. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






43. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






44. (chemistry) p(otential of) H(ydrogen)






45. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






46. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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47. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






48. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






49. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






50. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules