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






2. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






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






5. 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






6. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






7. The maximum amount of product that can be produced from a given amount of reactant






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






9. Tells you how much solute is present compared to the amount of solvent






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






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






12. E=hc/?






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






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






15. Named after their cation and anion






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






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

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18. 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






19. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






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






21. Common definition of acids as proton (H+) donors and bases as proton acceptors






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






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






24. 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






25. 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.






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

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






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






29. 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.






30. 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.






31. 5 valence electrons -3 ions - Nitride N






32. 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






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






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






35. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






37. 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






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






39. Simplest whole # ration of atoms in a compound






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

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






42. The lowest allowable energy state of an atom






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






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






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






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






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






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






50. 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.