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. 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






2. 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.






3. 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






4. A reaction in which atoms of one element take the place of atoms of another element in a compound






5. 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






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






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






8. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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






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






11. 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






12. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






13. 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






14. 5 valence electrons -3 ions - Nitride N






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






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

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


17. 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






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






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






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






21. 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

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


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






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






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






25. 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.






26. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






27. The area of chemistry that is concerned with reaction rates and reaction mechanisms






28. 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.






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






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






31. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






32. E=hc/?






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






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






35. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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






37. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






38. 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






39. A reaction in which atoms of one element take the place of atoms of another element in a compound






40. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






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






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






43. 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






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






45. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






46. 5 different orbitals shaped like clover leaves and max electrons is 10






47. Simplest whole # ration of atoms in a compound






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






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






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