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






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






3. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






4. 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






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






6. 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.






7. 5 different orbitals shaped like clover leaves and max electrons is 10






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






9. 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






10. 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






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






12. 2.18 x 10^-18 J/electron






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






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






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






16. 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.






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






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






19. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






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






21. 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






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

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






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






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






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






27. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






28. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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






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






31. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






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






34. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






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






37. 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






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






39. 5 valence electrons -3 ions - Nitride N






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






41. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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






43. 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.






44. 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.






45. 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.






46. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






47. 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






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






49. 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






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







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