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






2. 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.






3. Small discrete increments of energy.






4. 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.






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






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






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






8. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






11. A substance that - when dissolved in water - results in a solution that can conduct electricity






12. An atom or group of atoms that has a positive or negative charge






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






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






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






16. A solution in which water is the solvent






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






18. Sum of the protons and neutrons in an element often denoted by the letter A






19. 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.






20. Chalcogens - - Oxide O






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






22. 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






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






24. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






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






26. 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.






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






28. 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






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






30. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






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






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






34. Simplest whole # ration of atoms in a compound






35. 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






36. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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37. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






40. 5 valence electrons -3 ions - Nitride N






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. Numbers that specify the properties of atomic orbitals and of their electrons






43. Any sample of a given compound will contain the same elements in the identical mass ratio.






44. 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-






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






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






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






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






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






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