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MCAT Chemistry

Subjects : mcat, science
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. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






2. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






3. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






5. Numbers that specify the properties of atomic orbitals and of their electrons






6. Tells you how much solute is present compared to the amount of solvent






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






8. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






9. The process by which one or more substances change to produce one or more different substances






10. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






11. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






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






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






15. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






16. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






18. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






19. Property of the elements that can be predicted from the arrangement of the periodic table






20. The average distance between the nuclei of two bonded atoms






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






22. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






23. 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.






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






25. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






26. 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.






27. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






28. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






29. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






30. 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






31. 5 different orbitals shaped like clover leaves and max electrons is 10






32. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






33. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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






35. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






36. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






37. 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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38. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






39. The lowest allowable energy state of an atom






40. An atom or group of atoms that has a positive or negative charge






41. A reaction in which atoms of one element take the place of atoms of another element in a compound






42. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






43. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






44. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






45. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






46. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






47. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






48. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






49. 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.






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







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