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






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






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






4. 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






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






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






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






8. 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.






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






10. 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






11. 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






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






13. 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.






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






15. 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






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






17. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






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






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






21. 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.






22. 2.18 x 10^-18 J/electron






23. 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.






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






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






26. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






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






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






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






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






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






33. 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






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






35. 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






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






37. 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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38. 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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39. 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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40. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






41. 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






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






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






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






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






46. 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






47. 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






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






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






50. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms