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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. 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






2. 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.






3. E=hc/?






4. 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






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






7. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






8. Small discrete increments of energy.






9. 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






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






11. 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






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






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






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






16. 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






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






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






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






20. Chalcogens - - Oxide O






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






22. A subdivision of an energy level in an atom. They are divided into orbitals.






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






24. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






25. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






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






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






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






30. 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






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






32. 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






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






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






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






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






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






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






39. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






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






42. Named after their cation and anion






43. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






44. 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






45. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






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






47. 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






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






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






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







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