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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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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 lowest allowable energy state of an atom






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






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






5. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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. 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






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






9. Two or more atoms held together by covalent bonds






10. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






11. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






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






13. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






15. 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.






16. 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.






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






18. 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.






19. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






21. 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






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






23. Named after their cation and anion






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






25. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






27. 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






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






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






30. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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31. 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






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






33. 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






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






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






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






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






38. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






40. 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.






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






42. 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.






43. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






45. Rare earth element group (elements 58-71)






46. Chalcogens - - Oxide O






47. 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






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






49. The process by which one or more substances change to produce one or more different substances






50. 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.