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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. 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






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






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






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






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






6. An ionic compound that resists changes in its pH






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






8. The lowest allowable energy state of an atom






9. 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






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






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






13. 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.






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






15. 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






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






17. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






18. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






19. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






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






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






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






23. 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






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






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






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






27. 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.






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






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






30. 2.18 x 10^-18 J/electron






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






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






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






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






35. A horizontal row of elements in the periodic table






36. Simplest whole # ration of atoms in a compound






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






38. Two or more atoms held together by covalent bonds






39. 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






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






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






42. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






44. 5 valence electrons -3 ions - Nitride N






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






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






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






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






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






50. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds