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






2. 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.






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






5. 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






6. 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






7. 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






8. 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






9. 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






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






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






12. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






14. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






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






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






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






19. 2.18 x 10^-18 J/electron






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






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






22. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






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






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






26. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






28. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






29. 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.






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






31. A reaction where a compound does Not change its molecular structure.






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






33. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






34. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






36. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






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






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






39. Chalcogens - - Oxide O






40. 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.






41. 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






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






43. 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






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






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






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






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






48. 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.






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






50. 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.