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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. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






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






6. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






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






8. 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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9. 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






10. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






11. 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






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






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






14. 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






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






16. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






18. 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.






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






20. 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.






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






22. 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.






23. PH of a molecule at which it contains no net electric charge - isoelectric point.






24. 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.






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






26. A horizontal row of elements in the periodic table






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






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






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

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






31. 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






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






34. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






35. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






37. 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






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






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






40. Simplest whole # ration of atoms in a compound






41. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






42. A solution in which water is the solvent






43. 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.






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






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






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






47. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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48. The average distance between the nuclei of two bonded atoms






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






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







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