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

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2. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






3. 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.






4. In a solution - the substance that dissolves in the solvent






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






6. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






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






8. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






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






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






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






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






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






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






15. 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.






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






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






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






19. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






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






22. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






23. A horizontal row of elements in the periodic table






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






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






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






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






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






29. 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.






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






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






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






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






34. 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.






35. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






37. Simplest whole # ration of atoms in a compound






38. Redox reaction - in which the same species is both oxidized and reduced.






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






40. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






43. Named after their cation and anion






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






45. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






46. 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.






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






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






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






50. 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