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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. A dynamic condition in which two opposing changes occur at equal rates in a closed system






2. 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






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






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






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






6. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






8. The maximum amount of product that can be produced from a given amount of reactant






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






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






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






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






13. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






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






15. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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






17. 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

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

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19. 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






20. 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






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






22. 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






23. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






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






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






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






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






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






29. 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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30. 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






31. 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.






32. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






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






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






35. 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






36. Chalcogens - - Oxide O






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






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






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






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






42. 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






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






44. 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

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






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






47. 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






48. A substance that - when dissolved in water - results in a solution that can conduct electricity






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






50. A subdivision of an energy level in an atom. They are divided into orbitals.







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