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


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






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






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






5. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






6. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






7. Named after their cation and anion






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






9. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






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






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






12. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






14. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






15. 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.






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






17. Slightly less reactive than alkali metals - comprise group II






18. 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.






19. Rare earth element group (elements 58-71)






20. 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






21. Small discrete increments of energy.






22. PH of a molecule at which it contains no net electric charge - isoelectric point.






23. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






24. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






25. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






26. 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






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






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






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






30. 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






31. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






32. 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.






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






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






35. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






36. A horizontal row of elements in the periodic table






37. 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-






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






39. Substance in which a solute is dissolved to form a solution






40. 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.






41. A base that can accept two moles of H+ per mole of itself (ex: SO4






42. 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






43. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






45. Common definition of acids as proton (H+) donors and bases as proton acceptors






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






47. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






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






49. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






50. The slowest elementary step which is the limit for the rate of the other steps