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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. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






3. Any sample of a given compound will contain the same elements in the identical mass ratio.






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






5. Two or more atoms held together by covalent bonds






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






8. 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






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






10. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






12. Named after their cation and anion






13. Small discrete increments of energy.






14. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






17. 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.






18. 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






19. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






21. 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






22. E=hc/?






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






24. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






26. An ionic compound that resists changes in its pH






27. 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-






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






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






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






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






32. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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






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






35. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






36. 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






37. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






38. 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.






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






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






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






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

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43. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






45. 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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46. In a solution - the substance that dissolves in the solvent






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

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48. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






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