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






2. 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.






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






4. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






5. 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.






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






7. 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






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






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






10. The Percent by mass of each element in a compound.






11. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






12. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






13. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






14. Small discrete increments of energy.






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






16. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






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






18. 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






19. 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






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






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






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






23. 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






24. An ionic compound that resists changes in its pH






25. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






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






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






28. 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






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






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

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31. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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. 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.






34. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






35. 2.18 x 10^-18 J/electron






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






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






38. The lowest allowable energy state of an atom






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






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






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

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42. 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






43. 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






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






45. The process by which one or more substances change to produce one or more different substances






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






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






48. 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






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






50. Named after their cation and anion