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






2. 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.






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






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






5. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






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






8. Slightly less reactive than alkali metals - comprise group II






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






10. Rare earth element group (elements 58-71)






11. 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






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






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






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






15. 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






16. An ionic compound that resists changes in its pH






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






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






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






20. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






22. E=hc/?






23. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






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






25. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






26. 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






27. 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.






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






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






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






31. Named after their cation and anion






32. 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.






33. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






35. 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.






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






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






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

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






40. 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






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






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






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






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






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






46. 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






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






48. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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 average distance between the nuclei of two bonded atoms