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






2. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






4. The lowest allowable energy state of an atom






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






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






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






8. 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






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






10. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






11. 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






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






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






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






15. Tells you how much solute is present compared to the amount of solvent






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






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. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






19. 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.






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






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






22. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






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






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






25. 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.






26. 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.






27. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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






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






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






31. 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.






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






33. An ionic compound that resists changes in its pH






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






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






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






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






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






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






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






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






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

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43. 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






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






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






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






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






48. 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






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






50. Named after their cation and anion