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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. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






3. 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.






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






5. 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.






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






7. 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.






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






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






11. 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.






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






13. 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






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






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






16. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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






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






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






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






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






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






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






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






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






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






27. 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






28. 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






29. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






30. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






31. A horizontal row of elements in the periodic table






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






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






34. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






35. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






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






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






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






42. 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






43. Two or more atoms held together by covalent bonds






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






45. 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






46. 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






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






48. 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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49. A solution in which water is the solvent






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