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






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






3. 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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4. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






5. 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






6. 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






7. 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.






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






9. 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.






10. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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






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






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






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






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






17. 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






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






19. 5 different orbitals shaped like clover leaves and max electrons is 10






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






21. A horizontal row of elements in the periodic table






22. 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.






23. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






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






25. 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






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






27. 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






28. 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.






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






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






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






32. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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 formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






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






37. 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






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. A definite stable energy that a physical system can have






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






41. Simplest whole # ration of atoms in a compound






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






43. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






45. 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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46. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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






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






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






50. 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