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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 chemical formula showing the ratio of elements in a compound rather than the total number of 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. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






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






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






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






7. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






8. 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.






9. 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






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






11. 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






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






13. 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.






14. 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.






15. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






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






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






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






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






21. 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






22. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






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






26. 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






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






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






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






30. 5 valence electrons -3 ions - Nitride N






31. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






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






34. 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






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






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






37. 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






38. Named after their cation and anion






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






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






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






42. 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






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






44. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






45. 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.






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






47. 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






48. The slowest elementary step which is the limit for the rate of the other steps






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






50. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt