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

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






3. 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.






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






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






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

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






8. 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






9. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






10. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






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






12. 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






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






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






15. Named after their cation and anion






16. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






17. 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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18. 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






19. A horizontal row of elements in the periodic table






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






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






22. E=hc/?






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






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






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






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






27. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






28. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






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






30. Simplest whole # ration of atoms in a compound






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






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






33. Chalcogens - - Oxide O






34. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






35. Small discrete increments of energy.






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






37. The lowest allowable energy state of an atom






38. 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.






39. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






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






42. 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.






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






44. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






45. 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






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






47. 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






48. Two or more atoms held together by covalent bonds






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






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