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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. 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.






2. Chalcogens - - Oxide O






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






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






5. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






6. The lowest allowable energy state of an atom






7. 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






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






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






10. A solution in which water is the solvent






11. Small discrete increments of energy.






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






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






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






15. 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






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






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






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






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






20. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






21. 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






22. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






24. 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-






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






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






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






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






29. 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






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






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






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






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






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






35. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






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






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






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






39. The maximum amount of product that can be produced from a given amount of reactant






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






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






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






43. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






45. E=hc/?






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






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






48. 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






49. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






50. 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.