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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. The energy required to break a chemical bond and form neutral isolated atoms






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






3. 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.






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






5. 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






6. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






8. Named after their cation and anion






9. 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






10. A horizontal row of elements in the periodic table






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






12. 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






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






14. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






15. 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






16. 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






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






18. Small discrete increments of energy.






19. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






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






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






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

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






26. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






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

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28. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






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






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






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






32. 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






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






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






35. 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






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






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






38. Redox reaction - in which the same species is both oxidized and reduced.






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






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






41. Rare earth element group (elements 58-71)






42. 2.18 x 10^-18 J/electron






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






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






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






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






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






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






49. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






50. 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.