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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 definite stable energy that a physical system can have






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






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






4. Simplest whole # ration of atoms in a compound






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






6. 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






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






8. An ionic compound that resists changes in its pH






9. Elements in the middle of the periodic table - in groups 3-12.






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






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






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






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






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






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






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






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






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






19. 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.






20. 5 different orbitals shaped like clover leaves and max electrons is 10






21. 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






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






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






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






25. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






27. 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.






28. 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.






29. 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.






30. 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.






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






32. 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






33. 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






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






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






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






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






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






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






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






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






44. Rare earth element group (elements 58-71)






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






46. PH of a molecule at which it contains no net electric charge - isoelectric point.






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






48. Chalcogens - - Oxide O






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






50. E=hc/?