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






2. 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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3. 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






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






5. 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.






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






7. 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






8. 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.






9. 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.






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






11. Small discrete increments of energy.






12. 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






13. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






16. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






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






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






19. 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.






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






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






22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






23. 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






24. 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.






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






26. 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.






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






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






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






31. Named after their cation and anion






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






33. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






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






35. E=hc/?






36. 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






37. Simplest whole # ration of atoms in a compound






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






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






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






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






42. Chalcogens - - Oxide O






43. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






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






45. The energy required to break a chemical bond and form neutral isolated atoms






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






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






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






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






50. 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