Test your basic knowledge |

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






2. 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.






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






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






5. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






7. 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.






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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


9. Elements in the middle of the periodic table - in groups 3-12.






10. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






12. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






13. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






14. 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






15. 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.






16. 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






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






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






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






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






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






22. 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






23. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






25. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






26. The percent by mass of each element in a compound






27. 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






28. A solution in which water is the solvent






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






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






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






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






33. 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.






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






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






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






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






38. Common definition of acids as proton (H+) donors and bases as proton acceptors






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






40. 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.






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






42. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






43. 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






44. 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






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






46. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






47. 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






48. 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






49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






50. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.