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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 solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid


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






3. 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






4. Simplest whole # ration of atoms in a compound






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






6. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






7. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






9. 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






10. 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.






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






12. E=hc/?






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






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






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






16. The process of decomposing a chemical compound by the passage of an electric current.






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






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






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






20. 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.






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






22. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






23. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






24. An ionic compound that resists changes in its pH






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






26. 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






27. 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.






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






29. Slightly less reactive than alkali metals - comprise group II






30. 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






31. Sum of the protons and neutrons in an element often denoted by the letter A






32. The lowest allowable energy state of an atom






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






34. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






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






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


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






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






39. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






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






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






45. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






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






48. 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.






49. Named after their cation and anion






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