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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • 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 weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






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






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






5. 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.






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






7. 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.






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






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






10. 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






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






12. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






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






15. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






16. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






17. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






18. 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.






19. 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.






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






21. 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






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






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






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






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






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


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






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






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






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






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






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






33. 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






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






35. An ionic compound that resists changes in its pH






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






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






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






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






40. Named after their cation and anion






41. 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.






42. 5 valence electrons -3 ions - Nitride N






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






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






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






46. Simplest whole # ration of atoms in a compound






47. 2.18 x 10^-18 J/electron






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






49. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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