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






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






3. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






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






5. 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






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






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






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






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






10. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






13. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






14. 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.






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






17. 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






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






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






20. 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.






21. 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.






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






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






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






25. 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






26. 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






27. 2.18 x 10^-18 J/electron






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






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






31. 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.






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






33. 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






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






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






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






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






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






39. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






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






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






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






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






46. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






47. 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.






48. 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






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






50. 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.







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