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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. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






2. Sum of the protons and neutrons in an element often denoted by the letter A






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






4. Elements in the middle of the periodic table - in groups 3-12.






5. 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.






6. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






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






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






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






11. 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-






12. 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






13. 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






14. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






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






17. 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






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






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






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






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






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. A solution in which water is the solvent






24. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






25. Chalcogens - - Oxide O






26. Property of the elements that can be predicted from the arrangement of the periodic table






27. An ionic compound that resists changes in its pH






28. 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.






29. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






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






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






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






33. 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.






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






35. 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






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






37. The percent by mass of each element in a compound






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






39. 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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40. 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.






41. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






43. 5 different orbitals shaped like clover leaves and max electrons is 10






44. 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






45. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






47. 5 valence electrons -3 ions - Nitride N






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






49. Two or more atoms held together by covalent bonds






50. 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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