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






2. Gram equivalent weight of solute per liter of solution - often denoted by N.






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






4. Named after their cation and anion






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






6. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






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






8. 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






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






10. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






11. 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-






12. PH of a molecule at which it contains no net electric charge - isoelectric point.






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






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






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






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






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






18. 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






19. 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






20. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






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






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






23. 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.






24. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






25. Any sample of a given compound will contain the same elements in the identical mass ratio.






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






27. 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






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






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






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






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






32. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






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






34. 5 different orbitals shaped like clover leaves and max electrons is 10






35. 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.






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






37. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






38. 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.






39. A solution in which water is the solvent






40. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






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






43. An ionic compound that resists changes in its pH






44. A horizontal row of elements in the periodic table






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






46. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






48. 5 valence electrons -3 ions - Nitride N






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






50. 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.