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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. An ionic compound that resists changes in its pH






2. E=hc/?






3. 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






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






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






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






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






8. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






10. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






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






13. Small discrete increments of energy.






14. 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.






15. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






16. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






17. Named after their cation and anion






18. Simplest whole # ration of atoms in a compound






19. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






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






21. 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.






22. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin


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






24. 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.






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






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






27. 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


28. A definite stable energy that a physical system can have






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






30. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






32. 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






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






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






35. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






36. 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






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






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


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






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 solution in which water is the solvent






42. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






43. 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.






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






45. Having characteristics of both an acid and a base and capable of reacting as either






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






47. 2.18 x 10^-18 J/electron






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






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






50. 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