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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. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






2. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






3. 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






4. 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.






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






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






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






8. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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






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






11. E=hc/?






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






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






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






15. 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.






16. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






17. Simplest whole # ration of atoms in a compound






18. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






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






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






21. 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






22. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






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






25. 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.






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






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






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






29. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






31. 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.






32. 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






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






34. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






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






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






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






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






41. 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






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






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






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






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






47. The process of decomposing a chemical compound by the passage of an electric current.






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






49. 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.






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