Test your basic knowledge |

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 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






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






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






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






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


6. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






7. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






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






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






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






11. E=hc/?






12. 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






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






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






15. A solid made up of particles that are not arranged in a regular pattern.






16. 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






17. 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






18. 5 valence electrons -3 ions - Nitride N






19. 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






20. 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


21. 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






22. 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.






23. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






25. 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






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






27. 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






28. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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






33. Named after their cation and anion






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






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






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






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






38. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






39. 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






40. 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.






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






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






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






44. 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






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






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






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






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






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






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