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






2. (chemistry) p(otential of) H(ydrogen)






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






4. 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






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






6. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






7. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






8. A reaction in which atoms of one element take the place of atoms of another element in a compound






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






10. In a solution - the substance that dissolves in the solvent






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






12. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






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






15. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






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






17. 2.18 x 10^-18 J/electron






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






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






20. 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






21. An ionic compound that resists changes in its pH






22. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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23. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






25. 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






26. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






28. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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






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






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






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






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






37. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






38. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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






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






41. 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






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






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






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






45. 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-






46. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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47. 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






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






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






50. 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







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