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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 process by which one or more substances change to produce one or more different substances






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






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






5. The maximum amount of product that can be produced from a given amount of reactant






6. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






7. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






8. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






9. 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






10. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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11. 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.






12. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






13. 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






14. Redox reaction - in which the same species is both oxidized and reduced.






15. E=hc/?






16. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






18. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






19. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






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






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






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






23. Sum of the protons and neutrons in an element often denoted by the letter A






24. 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.






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






26. Acids defined as electron - pair acceptors and bases as electron - pair donors.






27. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






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






29. In a solution - the substance that dissolves in the solvent






30. An elementary particle with 0 charge and mass about equal to a proton






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. 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.






33. 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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34. Gram equivalent weight of solute per liter of solution - often denoted by N.






35. A horizontal row of elements in the periodic table






36. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






37. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






38. 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.






39. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






41. 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






42. 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






43. 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






44. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






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






47. 2.18 x 10^-18 J/electron






48. 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






49. 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






50. Chalcogens - - Oxide O







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