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






2. 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.






3. An elementary particle with 0 charge and mass about equal to a proton






4. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






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






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






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






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






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






12. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






13. 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






14. Named after their cation and anion






15. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






16. 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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17. E=hc/?






18. 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






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






20. The lowest allowable energy state of an atom






21. 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






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






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






24. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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






26. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






28. 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.






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






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






31. 5 valence electrons -3 ions - Nitride N






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






33. 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






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






35. 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






36. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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






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






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






40. 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






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






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






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






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






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






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






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






48. 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






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






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