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






2. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






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






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






5. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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






7. 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.






8. 5 valence electrons -3 ions - Nitride N






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






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






11. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






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






14. 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






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






16. 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.






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






18. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






20. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






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






22. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






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






24. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






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






29. Named after their cation and anion






30. E=hc/?






31. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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






33. Two or more atoms held together by covalent bonds






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






35. A substance that - when dissolved in water - results in a solution that can conduct electricity






36. 5 different orbitals shaped like clover leaves and max electrons is 10






37. 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.






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






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






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






41. 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-






42. The lowest allowable energy state of an atom






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






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






45. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






46. 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






47. 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






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






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






50. An ionic compound that resists changes in its pH