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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. 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.






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






3. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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






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






6. 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






7. 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






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






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






10. 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






11. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






12. The slowest elementary step which is the limit for the rate of the other steps






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






14. A solution in which water is the solvent






15. 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.






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






17. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






18. 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






19. A definite stable energy that a physical system can have






20. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






22. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






23. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






24. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






26. A subdivision of an energy level in an atom. They are divided into orbitals.






27. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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28. 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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29. 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






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






31. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






32. 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






33. An ionic compound that resists changes in its pH






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






35. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






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






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






38. 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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39. Slightly less reactive than alkali metals - comprise group II






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






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






42. 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.






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






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






45. 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






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






47. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






48. A reaction where a compound does Not change its molecular structure.






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






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