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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. 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.






2. In a solution - the substance that dissolves in the solvent






3. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






4. Two or more atoms held together by covalent bonds






5. 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






6. 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






7. 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






8. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






9. Simplest whole # ration of atoms in a compound






10. 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.






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






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






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






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






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






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






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






19. 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






20. 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.






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






22. Small discrete increments of energy.






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






24. 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.






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






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






27. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






28. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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

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






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






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






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






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






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






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






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






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






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






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






41. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






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






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






44. 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.






45. 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.






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






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






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






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






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