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






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






3. Two or more atoms held together by covalent bonds






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






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






6. 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






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






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






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






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






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






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






14. 2.18 x 10^-18 J/electron






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






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






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






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






19. 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






20. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






21. The maximum amount of product that can be produced from a given amount of reactant






22. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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






24. 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






25. Simplest whole # ration of atoms in a compound






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






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






28. 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






29. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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






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






32. 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






33. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






34. 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






35. E=hc/?






36. Chalcogens - - Oxide O






37. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






39. A horizontal row of elements in the periodic table






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






41. 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






42. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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






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






46. 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-






47. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






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






50. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu