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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 Percent by mass of each element in a compound.






2. 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.






3. 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.






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






5. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






6. A horizontal row of elements in the periodic table






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






8. 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






9. 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.






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






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






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






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






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






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






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






17. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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






19. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






20. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






21. 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






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






23. 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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24. 2.18 x 10^-18 J/electron






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






26. 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.






27. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






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






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






31. 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






32. Simplest whole # ration of atoms in a compound






33. 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.






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






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






36. 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






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






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






39. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






41. 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.






42. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






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






44. A solution in which water is the solvent






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






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






47. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






48. 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






49. 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






50. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq