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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. The slowest elementary step which is the limit for the rate of the other steps






2. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






3. 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






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






5. 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.






6. 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






7. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






8. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






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






11. A solution in which water is the solvent






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






13. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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






15. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






16. 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






17. 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

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18. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






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






21. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






23. 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






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






25. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






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






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






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






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






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






32. 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-






33. 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






34. 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.






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






36. E=hc/?






37. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






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






39. 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






40. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






41. The lowest allowable energy state of an atom






42. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






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






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






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






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






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






48. 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.






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






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