Conceptual Chemistry - Naming Compounds Lecture Notes PDF

Section 3.5 There Is a System for Naming Compounds Conceptual Chemistry Fourth Edition...

Section 3.5 There Is a System for Naming Compounds Conceptual Chemistry Fourth Edition John Suchocki © 2011 Pearson Education, Inc. Chapter 3 The Periodic Table  A system for naming the countless number of possible compounds has been developed by the International Union for Pure and Applied Chemistry (IUPAC). This system is designed so that a compound’s name reflects the elements it contains and how those elements are joined. © 2011 Pearson Education, Inc. Chapter 3  The following four guidelines will acquaint you with the way the system works for many simple compounds consisting of only a few elements. © 2011 Pearson Education, Inc. Chapter 3  Guideline 1 Start with the element farthest to the left in the periodic table… © 2011 Pearson Education, Inc. Chapter 3  Guideline 1 …for the element farthest to the right, add the suffix -ide © 2011 Pearson Education, Inc. Chapter 3  The Periodic Table © 2011 Pearson Education, Inc. Chapter 3  Example NaCl © 2011 Pearson Education, Inc. Chapter 3  Example NaCl Sodium Chlor ine © 2011 Pearson Education, Inc. Chapter 3  Example NaCl Sodium Chlor ide © 2011 Pearson Education, Inc. Chapter 3  Example NaCl sodium chloride © 2011 Pearson Education, Inc. Chapter 3  Guideline 2 With different possible combinations of elements… © 2011 Pearson Education, Inc. Chapter 3  Guideline 2 …use prefixes to remove any ambiguity. © 2011 Pearson Education, Inc. Chapter 3  mono- 1 di- 2 tri- 3 tetra- 4 © 2011 Pearson Education, Inc. Chapter 3  Example CO CO2 © 2011 Pearson Education, Inc. Chapter 3  Example CO carbon monoxide CO2 carbon dioxide © 2011 Pearson Education, Inc. Chapter 3  Example H 2O dihydrogen monoxide H 2O2 dihydrogen dioxide © 2011 Pearson Education, Inc. Chapter 3  Guideline 3 Atoms can clump together to form a molecular unit that acts as a single electrically charged group, called a polyatomic ion. © 2011 Pearson Education, Inc. Chapter 3 © 2011 Pearson Education, Inc. Chapter 3  Positively charged polyatomic ions are listed first within the name (without the word ion). Ammonium chloride, NH44Cl © 2011 Pearson Education, Inc. Chapter 3  Negatively charged polyatomic ions are placed at the end of the name. Lithium nitrate, LiNO33 © 2011 Pearson Education, Inc. Chapter 3  Guideline 4 Common names are also sometimes used for convenience. © 2011 Pearson Education, Inc. Chapter 3  Example H 2O dihydrogen monoxide H 2O2 dihydrogen dioxide © 2011 Pearson Education, Inc. Chapter 3  H 2O dihydrogen monoxide (water) H 2O2 dihydrogen dioxide (hydrogen peroxide) © 2011 Pearson Education, Inc. Chapter 3  Quiz Time Li3N Lithium nitride CaF2 Calcium fluoride Li2O Lithium oxide Sr3P2 Strontium phosphide © 2011 Pearson Education, Inc. Chapter 3  Quiz Time NO2 Nitrogen dioxide N2O Dinitrogen monoxide N2O5 Dinitrogen pentaoxide CCl4 Carbon tetrachloride © 2011 Pearson Education, Inc. Chapter 3  Section 4.8 The Shell Model Helps to Explain the Periodic Table Conceptual Chemistry Fourth Edition John Suchocki © 2011 Pearson Education, Inc. Chapter 4  What does an electron wave look like? Although electrons are too small to be seen, we can get a reliable sense of the nature of an electron wave from some very advanced mathematics. Briefly, the nature of the wave depends upon how much energy the electron has. Furthermore, this wave is 3-dimensional. The next slide shows a set of overlapping electron waves as calculated by these mathematics. © 2011 Pearson Education, Inc. Chapter 4  Overlapping Overlapping electron electron waveswaves of of similar similar energy energy levels. levels. © 2011 Pearson Education, Inc. Chapter 4  These These waves waves can can be be simplified simplified into into a a single single shell. shell..... © 2011 Pearson Education, Inc. Chapter 4...... or or ring. ring. © 2011 Pearson Education, Inc. Chapter 4 © 2011 Pearson Education, Inc. Chapter 4  According to the shell model, electrons behave as though they are arranged in a series of concentric shells. A shell is defined as a region of space about the atomic nucleus within which electrons may reside. An important aspect of this model is that there are at least seven shells and each shell can hold only a limited number of electrons. © 2011 Pearson Education, Inc. Chapter 4 © 2011 Pearson Education, Inc. Chapter 4  These shells explain the organization of the periodic table. © 2011 Pearson Education, Inc. Chapter 4  Periodic Table © 2011 Pearson Education, Inc. Chapter 4  Section 4.9 The Periodic Table Helps Us Predict Properties of Elements Conceptual Chemistry Fourth Edition John Suchocki © 2011 Pearson Education, Inc. Chapter 4  Atomic size © 2011 Pearson Education, Inc. Chapter 4  Ionization energy © 2011 Pearson Education, Inc. Chapter 4  Electronegativity © 2011 Pearson Education, Inc. Chapter 4  Density © 2011 Pearson Education, Inc. Chapter 4  Inner-shell shielding Effective nuclear charge © 2011 Pearson Education, Inc. Chapter 4  Inner-shell shielding The tendency of inner-shell electrons to partially shield outer-shell electrons from the nuclear charge © 2011 Pearson Education, Inc. Chapter 4  Effective nuclear charge The nuclear charge experienced by outer-shell electrons Z* © 2011 Pearson Education, Inc. Chapter 4  First First shell shell Helium © 2011 Pearson Education, Inc. Chapter 4 © 2011 Pearson Education, Inc. Chapter 4  First First shell shell Second Second shell shell Lithium © 2011 Pearson Education, Inc. Chapter 4 © 2011 Pearson Education, Inc. Chapter 4  +17 -10 Chlorine © 2011 Pearson Education, Inc. Chapter 4  +17 -10 Z* = +7 Chlorine © 2011 Pearson Education, Inc. Chapter 4  Chlorine Chlorine +17 +17 Actual Actual nuclear nuclear charge charge -10 -10 Inner Inner shell shell electrons electrons +7 +7 Effective Effective nuclear nuclear charge charge © 2011 Pearson Education, Inc. Chapter 4  +19 -18 Z* = +1 Potassium © 2011 Pearson Education, Inc. Chapter 4  Potassium Potassium +19 +19 Actual Actual nuclear nuclear charge charge -18 -18 Inner Inner shell shell electrons electrons +1 +1 Effective Effective nuclear nuclear charge charge © 2011 Pearson Education, Inc. Chapter 4  Atomic size © 2011 Pearson Education, Inc. Chapter 4  Group Group 1 1 © 2011 Pearson Education, Inc. Chapter 4  Group Group 1 1 Increasing atomic size © 2011 Pearson Education, Inc. Chapter 4  Period 2 © 2011 Pearson Education, Inc. Chapter 4  Period 2 Z* Z* = = +1 +1 Z* Z* = = +2 +2 Z* Z* = = +3 +3 +3 +3 +4 +4 +5 +5 © 2011 Pearson Education, Inc. Chapter 4  Period 2 Z* Z* = = +3 +3 Z* Z* = = +4 +4 Z* Z* = = +5 +5 Z* Z* = = +6 +6 +5 +5 +6 +6 +7 +8 +7 +8 © 2011 Pearson Education, Inc. Chapter 4  Period 2 Z* Z* = = +5 +5 Z* Z* = = +6 +6 +7 +7 +8 +8 +9 +9 +10 +10 © 2011 Pearson Education, Inc. Chapter 4  Period 2 Z* Z* = = +5 +5 Z* Z* = = +6 +6 Z* Z* = = +7 +7 Z* Z* = = +8 +8 +7 +7 +8 +8 +9 +9 +10 +10 © 2011 Pearson Education, Inc. Chapter 4  Period 2 Z* Z* = = +6 +6 Z* Z* = = +7 +7 Z* Z* = = +8 +8 Z* Z* = = +1 +1 +8 +8 +9 +9 +10 +10 +11 +11 Sodium Sodium © 2011 Pearson Education, Inc. Chapter 4  Period 2 Decreasing Decreasing atomic atomic size size © 2011 Pearson Education, Inc. Chapter 4  Ionization energy The amount of energy required to pull an electron away from an atom © 2011 Pearson Education, Inc. Chapter 4  Ionization energy © 2011 Pearson Education, Inc. Chapter 4  Lithium Lithium © 2011 Pearson Education, Inc. Chapter 4  Z* Z* = = +1 +1 Lithium Lithium © 2011 Pearson Education, Inc. Chapter 4  Z* Z* = = +1 +1 Lithium Lithium © 2011 Pearson Education, Inc. Chapter 4  Z* Z* = = +1 +1 Lithium Lithium © 2011 Pearson Education, Inc. Chapter 4  Z* Z* = = +1 +1 Small Small distance, distance, Stronger Stronger force force Lithium Lithium © 2011 Pearson Education, Inc. Chapter 4  Z* Z* = = +1 +1 Cesium Cesium © 2011 Pearson Education, Inc. Chapter 4  Z* Z* = = +1 +1 Greater Greater distance, distance, weaker weaker force force Cesium Cesium © 2011 Pearson Education, Inc. Chapter 4  Ionization energy © 2011 Pearson Education, Inc. Chapter 4  Period 2 Z*= Z*= +1 +1 Z*= Z*= +2 +2 Z*= Z*= +3 +3 Z*= Z*= +4 +4 Z*= Z*= +5 +5 Z*= Z*= +6 +6 Z*= Z*= +7 +7 Z*= Z*= +8 +8 © 2011 Pearson Education, Inc. Chapter 4  Chapter 4 Subatomic Particles Part 2: Sections 4.7 – 4.9 Conceptual Chemistry Fourth Edition John Suchocki © 2011 Pearson Education, Inc. Chapter 4