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






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






3. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






4. 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






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






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






7. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






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

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9. Small discrete increments of energy.






10. Named after their cation and anion






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






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. 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






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






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






16. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






17. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






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






19. 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






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






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






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






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






24. 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






25. 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






26. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






27. 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






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






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






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






31. The slowest elementary step which is the limit for the rate of the other steps






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






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






34. Chalcogens - - Oxide O






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






36. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






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






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






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






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






42. 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






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






44. (chemistry) a substance that changes color to indicate the presence of some ion or substance






45. 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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46. 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






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






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






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






50. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points







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