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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. Simplest whole # ration of atoms in a compound






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






3. 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






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






5. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






6. 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.






7. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






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






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






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






11. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






12. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






15. 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.






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






17. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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

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






21. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






22. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






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






25. 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






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






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






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






29. 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






30. 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.






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






32. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






33. 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






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






35. Small discrete increments of energy.






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






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 lowest allowable energy state of an atom






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






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






41. 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.






42. The percent by mass of each element in a compound






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






44. 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.






45. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






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






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






49. An ionic compound that resists changes in its pH






50. 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







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