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






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






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






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






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






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






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






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






9. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






10. A solution in which water is the solvent






11. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






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






13. A definite stable energy that a physical system can have






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. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






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






17. 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






18. Chalcogens - - Oxide O






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






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






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






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






23. 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






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






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






26. 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






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






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






29. 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






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






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






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






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






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






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






37. E=hc/?






38. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






39. 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.






40. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






41. 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






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






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






44. 5 different orbitals shaped like clover leaves and max electrons is 10






45. The energy required to break a chemical bond and form neutral isolated atoms






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






47. The lowest allowable energy state of an atom






48. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






49. Slightly less reactive than alkali metals - comprise group II






50. Numbers that specify the properties of atomic orbitals and of their electrons