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






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






3. 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.






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






5. 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-






6. Redox reaction - in which the same species is both oxidized and reduced.






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






8. 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.






9. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






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






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






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






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






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






15. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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. 2.18 x 10^-18 J/electron






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






19. 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.






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






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






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






23. 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.






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






25. 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






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






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






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






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






30. 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






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






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






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






34. 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


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






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






37. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






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






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






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






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


43. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






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






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






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






47. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






49. 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






50. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge