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






2. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






3. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






5. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






7. 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






8. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






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






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






11. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






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






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






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






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






17. Named after their cation and anion






18. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






19. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






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






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






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






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






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






26. 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






27. 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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28. 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.






29. 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.






30. 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






31. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






32. 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






33. 2.18 x 10^-18 J/electron






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






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






36. 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.






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






38. 5 valence electrons -3 ions - Nitride N






39. 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






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






41. A horizontal row of elements in the periodic table






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






43. 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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44. The average distance between the nuclei of two bonded atoms






45. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






46. Two or more atoms held together by covalent bonds






47. 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






48. 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.






49. Chalcogens - - Oxide O






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






Can you answer 50 questions in 15 minutes?



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