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






2. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






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






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






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






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






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






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






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






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






11. 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.






12. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






15. 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.






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






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






18. Chalcogens - - Oxide O






19. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






20. Small discrete increments of energy.






21. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






23. Redox reaction - in which the same species is both oxidized and reduced.






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






25. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






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






27. The lowest allowable energy state of an atom






28. 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






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






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






32. The percent by mass of each element in a compound






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






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






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






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






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






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






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






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






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






42. The average distance between the nuclei of two bonded atoms






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






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






45. A horizontal row of elements in the periodic table






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






47. 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






48. 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






49. 5 different orbitals shaped like clover leaves and max electrons is 10






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