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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.
  • 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. 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






2. Simplest whole # ration of atoms in a compound






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






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






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






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






7. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






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






10. 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.






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






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






13. 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






14. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






15. 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






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






17. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






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






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






20. 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






21. Tells you how much solute is present compared to the amount of solvent






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






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






24. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






27. 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.






28. (chemistry) p(otential of) H(ydrogen)






29. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






30. The energy required to break a chemical bond and form neutral isolated atoms






31. 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






32. 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






33. 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






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






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






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






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






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






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






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






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






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






43. A reaction in which atoms of one element take the place of atoms of another element in a compound






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






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






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






47. The lowest allowable energy state of an atom






48. 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






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






50. 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.