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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.
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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 maximum amount of product that can be produced from a given amount of reactant






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






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






4. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






5. 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






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






7. 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.






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






9. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






10. 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.






11. 2.18 x 10^-18 J/electron






12. 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.






13. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






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






16. 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






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






18. 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.






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






20. 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






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






22. 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






23. 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






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






25. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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

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






29. 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






30. 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






31. 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






32. Property of the elements that can be predicted from the arrangement of the periodic table






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






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






35. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






38. Small discrete increments of energy.






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






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






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






42. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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






44. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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. E=hc/?






49. 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.






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