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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. 5 valence electrons -3 ions - Nitride N






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






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






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






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






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






7. Simplest whole # ration of atoms in a compound






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






9. 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






10. 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






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






12. 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






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






14. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






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






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






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






19. 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.






20. 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.






21. 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-






22. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






24. 2.18 x 10^-18 J/electron






25. 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.






26. 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






27. 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






28. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






30. Any sample of a given compound will contain the same elements in the identical mass ratio.






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






32. Small discrete increments of energy.






33. (chemistry) p(otential of) H(ydrogen)






34. 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.






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






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






37. 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






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






39. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






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






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






44. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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






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






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






48. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






50. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound