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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. 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.






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






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






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






5. 2.18 x 10^-18 J/electron






6. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






8. 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






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






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






11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






13. 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






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






15. Slightly less reactive than alkali metals - comprise group II






16. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






17. 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






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






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






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






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






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






23. 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.






24. The energy required to break a chemical bond and form neutral isolated atoms






25. Chalcogens - - Oxide O






26. Common definition of acids as proton (H+) donors and bases as proton acceptors






27. The Percent by mass of each element in a compound.






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






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






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






31. 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






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






33. 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-






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






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






36. 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






37. (chemistry) p(otential of) H(ydrogen)






38. 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






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






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






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






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






43. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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. 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






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