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






2. 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






3. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






4. 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.






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






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






7. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






8. 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






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






10. 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






11. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






12. 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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13. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






14. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






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






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






17. 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






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






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






20. 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.






21. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






22. 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






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






24. 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






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






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






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






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






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






30. Substance in which a solute is dissolved to form a solution






31. 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






32. 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






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






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






35. 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.






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






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






38. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






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






40. Named after their cation and anion






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






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






43. 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






44. E=hc/?






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






46. 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






47. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






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






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