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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.
  • 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. 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






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






3. 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






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






5. 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






6. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






7. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






8. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






10. A substance that - when dissolved in water - results in a solution that can conduct electricity






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






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. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






14. 2.18 x 10^-18 J/electron






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






16. The lowest allowable energy state of an atom






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






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






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






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






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






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






23. A horizontal row of elements in the periodic table






24. Chalcogens - - Oxide O






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






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






27. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






28. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






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






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






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






33. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






34. 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






35. 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






36. E=hc/?






37. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






38. 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.






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






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 nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






42. 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






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






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






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






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






47. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






49. 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.






50. 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