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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 set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






2. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






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






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






7. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






8. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






9. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






11. A reaction where a compound does Not change its molecular structure.






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






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






14. An ionic compound that resists changes in its pH






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






16. 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






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






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






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






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






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






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






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






24. 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






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






26. 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.






27. 2.18 x 10^-18 J/electron






28. 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.






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






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






31. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






33. 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






34. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






36. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






37. 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






38. The area of chemistry that is concerned with reaction rates and reaction mechanisms






39. 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.






40. Chalcogens - - Oxide O






41. 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






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






43. Simplest whole # ration of atoms in a compound






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






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






46. PH of a molecule at which it contains no net electric charge - isoelectric point.






47. 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.






48. Named after their cation and anion






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






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