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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 physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






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






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






4. Named after their cation and anion






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






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






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






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






9. 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






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






11. A definite stable energy that a physical system can have






12. 5 different orbitals shaped like clover leaves and max electrons is 10






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






14. 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






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






16. 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






17. 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






18. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






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






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






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






22. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






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






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






25. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






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






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






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






30. 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.






31. Property of the elements that can be predicted from the arrangement of the periodic table






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. A subdivision of an energy level in an atom. They are divided into orbitals.






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






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






36. 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






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






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






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






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






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






42. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






43. The lowest allowable energy state of an atom






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






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






46. 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.






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






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






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






50. 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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