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






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






3. 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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4. 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






5. 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.






6. 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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7. The process of decomposing a chemical compound by the passage of an electric current.






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






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






10. 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






11. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






12. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






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






14. 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.






15. The area of chemistry that is concerned with reaction rates and reaction mechanisms






16. 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






17. 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.






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






19. 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






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. 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.






22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






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






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






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






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






28. 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






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






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






31. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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






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






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






36. 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






37. Named after their cation and anion






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






40. 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.






41. 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.






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






43. 2.18 x 10^-18 J/electron






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






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






46. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






47. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






48. A solution in which water is the solvent






49. 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






50. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group