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






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






3. 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






4. 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.






5. 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






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






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






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






9. 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






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






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






12. 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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13. Slightly less reactive than alkali metals - comprise group II






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






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






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






17. A solution in which water is the solvent






18. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






19. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






20. 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-






21. 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.






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






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






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






25. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






26. 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.






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






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






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






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






32. 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.






33. 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






34. 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






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






36. 2.18 x 10^-18 J/electron






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






38. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






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






41. 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






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






43. 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






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






45. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






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






47. Two or more atoms held together by covalent bonds






48. 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






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






50. An ionic compound that resists changes in its pH