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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. 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. 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.






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






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






5. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






6. 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






7. 5 different orbitals shaped like clover leaves and max electrons is 10






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






9. 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.






10. Simplest whole # ration of atoms in a compound






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






12. Named after their cation and anion






13. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






14. A substance that - when dissolved in water - results in a solution that can conduct electricity






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






16. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






17. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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






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






20. 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.






21. Small discrete increments of energy.






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






23. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






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






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






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






27. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






29. Redox reaction - in which the same species is both oxidized and reduced.






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






31. 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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32. 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.






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






34. A subdivision of an energy level in an atom. They are divided into orbitals.






35. 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.






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






37. The maximum amount of product that can be produced from a given amount of reactant






38. 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






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






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






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






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






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






44. 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






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






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






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






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

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49. 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






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