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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 base that can accept two moles of H+ per mole of itself (ex: SO4






2. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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






4. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






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






6. A reaction in which atoms of one element take the place of atoms of another element in a compound






7. Small discrete increments of energy.






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






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






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






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






12. 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






13. 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.






14. 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.






15. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






17. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






18. A solution in which water is the solvent






19. 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






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






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






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






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






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






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






26. 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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27. The average distance between the nuclei of two bonded atoms






28. Sum of the protons and neutrons in an element often denoted by the letter A






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






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






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






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






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






34. 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






35. Named after their cation and anion






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






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






38. 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






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






41. 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.






42. 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






43. 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






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






45. 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.






46. 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






47. 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.






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






49. 2.18 x 10^-18 J/electron






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