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






2. 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






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






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






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






6. 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






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






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






9. A solution in which water is the solvent






10. 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-






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






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






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






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






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






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






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






18. 2.18 x 10^-18 J/electron






19. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






21. 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






22. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






24. 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






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






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






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






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. 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






30. 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






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






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






33. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






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






35. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






36. Any sample of a given compound will contain the same elements in the identical mass ratio.






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






38. 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.






39. The process by which one or more substances change to produce one or more different substances






40. 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.






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






42. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






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






45. 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






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






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






48. Small discrete increments of energy.






49. 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






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