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






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






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






4. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






5. 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.






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






7. Named after their cation and anion






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






9. 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






10. A reaction where a compound does Not change its molecular structure.






11. 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






12. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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






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






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






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






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






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






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






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






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






22. A solution in which water is the solvent






23. 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.






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






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






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

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27. A horizontal row of elements in the periodic table






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






29. Chalcogens - - Oxide O






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






31. 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






32. The process by which one or more substances change to produce one or more different substances






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






34. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






38. 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-






39. 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






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






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






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






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






45. The Percent by mass of each element in a compound.






46. 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.






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






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






49. 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






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