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






2. 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






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






4. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






6. 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






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






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






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






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






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






12. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






13. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






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






15. 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.






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






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






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






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






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






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






22. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






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

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26. 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.






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






28. 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






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






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






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






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

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






36. 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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37. 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






38. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






39. 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






40. 5 valence electrons -3 ions - Nitride N






41. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






42. 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.






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






44. 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






45. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






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






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






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






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