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






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






3. 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






4. 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






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






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


7. E=hc/?






8. 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






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






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






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






12. 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.






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






14. 5 valence electrons -3 ions - Nitride N






15. An ionic compound that resists changes in its pH






16. 2.18 x 10^-18 J/electron






17. 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






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






19. 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






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






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






22. 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.






23. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






24. 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.






25. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






27. Simplest whole # ration of atoms in a compound






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






29. 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






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






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






32. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






33. A solid made up of particles that are not arranged in a regular pattern.






34. 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.






35. 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


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






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






38. 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






39. 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.






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






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






42. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






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






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






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






46. An atom or group of atoms that has a positive or negative charge






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






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






49. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


50. 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