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






2. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






3. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






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






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






8. 5 different orbitals shaped like clover leaves and max electrons is 10






9. 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.






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






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






12. Having characteristics of both an acid and a base and capable of reacting as either






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






14. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






15. 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.






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






17. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






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






19. 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






20. 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






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






22. 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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23. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






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






25. The lowest allowable energy state of an atom






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






27. 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






28. Gram equivalent weight of solute per liter of solution - often denoted by N.






29. 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






30. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






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






32. 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






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






34. Named after their cation and anion






35. 5 valence electrons -3 ions - Nitride N






36. 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.






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






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






39. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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






41. 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.






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






43. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






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






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






46. 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






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






48. 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






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






50. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.