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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. An elementary particle with 0 charge and mass about equal to a proton






2. 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






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






4. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






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






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






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






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






9. Sum of the protons and neutrons in an element often denoted by the letter A






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


11. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






13. 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.






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






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






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






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






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






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






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






21. Simplest whole # ration of atoms in a compound






22. A horizontal row of elements in the periodic table






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






24. Having characteristics of both an acid and a base and capable of reacting as either






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






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






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






28. E=hc/?






29. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T


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






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






32. 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






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






34. The lowest allowable energy state of an atom






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






36. Chalcogens - - Oxide O






37. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






39. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






40. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






43. 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






44. Named after their cation and anion






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






46. 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


47. 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.






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






49. 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.






50. 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