Lewis Structures Notes Draw the dot diagram for each atom. Make sure you place the electrons in the correct order.
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1 Lewis Structures Notes Draw the dot diagram for each atom. Make sure you place the electrons in the correct order. Draw the dot diagrams for Carbon, Nitrogen and Oxygen. Steps for drawing Lewis Structures: o Order the atoms- the atom with the most unpaired electrons will be the central atom (Carbon is always the central atom). o Draw the dot diagram for each element in the compound. o Pair up all unpaired electrons. Examples: o Phosphorous and Chlorine (PCl 3 ) o Carbon and Bromine (CBr 4 ) Ionic Dot Diagrams- the electrons are gained and lost, not shared. Put each atom in a bracket with its balance electrons around it. The charge of the atom goes outside of the bracket. o Ex: Sodium Chloride (NaCl) Unit 6: Bonding and Nomenclature Page 12
2 Ionic Lewis Structure Activity In this activity we will be modeling what an Ionic Bond is using cereal to represent the valence electrons. Please follow the following steps for modeling what occurs in the following ionic compounds: 1. Draw the element s symbols in the designated box. 2. Assign the proper number of valance electrons (Cereal) to each original element 3. Make an ionic bond to create a balanced neutral compound by moving a valence electron (Cereal) 4. Draw the correct Lewis Structure in the box below. 5. Write the formula or name of the compound. KBr Magnesium chloride CaO Lithium oxide Mg 3 N 2 Sodium Sulfide Fe 2 O 3 Silver Nitrate PbS 2 Unit 6: Bonding and Nomenclature Page 13
3 Covalent Bonding Notes Covalent bonds are between. Covalent bonds are formed when electrons are between two atoms. If two atoms share 4 electrons, they form a. If two atoms share 6 electrons, they form a. There are two types of covalent bonds: polar and non-polar. Polar bonds have an electronegativity difference between. Non-polar bonds have an electronegativity difference less than. In polar bonds, the electrons are shared. In non-polar bonds, the electrons are shared. Covalent compounds can exist in any state (solid, liquid or gas). They have melting and boiling points. Write the correct formulas for each covalent compound: Compound Name Oxidation States Covalent Formula water O (-2) H (+1) Carbon Dioxide C (+4) O (-2) Chlorine (Diatomic Element) Cl (-1) Methane (5 total atoms) Ammonia (4 total atoms) Carbon tetrabromide (5 total atoms) Phosphorous trichloride (4 total atoms) Diphosphorous trioxide (5 total atoms) C (-4) H (+1) N (-3) H (+1) C (+4) Br (-1) P (-3) Cl (-1) P (-3) O (-2) Unit 6: Bonding and Nomenclature Page 14
4 Polyatomic Ions Ions formed from a single atom are known as ions. You wrote formulas for ionic compounds using monoatomic ions. Many ionic and covalent compounds found in chemistry contain polyatomic ions, which are ions made up of. Practice writing ionic formulas using polyatomic ions: BaCO 3 Al 2 (SO 4 ) 3 Zn(ClO) 2 Pb(C 2 H 3 O 2 ) 2 Cobalt (III) Nitrate Ammonium Chloride Silver Chlorate Barium Phosphate How would you write the formula for calcium hydroxide?. Is there a difference between CaOH 2 & Ca(OH) 2? Circle the correct formula. When more than one polyatomic ion is present, the formula for the polyatomic ion is surrounded by. Unit 6: Bonding and Nomenclature Page 15
5 Covalent Lewis Activity In this activity we will be modeling what a Covalent Bond is using cereal to represent the valence electrons. Please follow the following steps for modeling what occurs in the following ionic compounds: 1. Draw the element s symbols in the designated box. 2. Assign the proper number of valance electrons (cereal) to each original element 3. Make a covalent bond to create a balanced neutral compound. 4. Draw the correct Lewis Structure in the box below. 5. Mark with stars the compounds that are diatomic. CO 2 H 2 O NH 3 F 2 O 2 N 2 ClO 3 PO 3 SO 2 Unit 6: Bonding and Nomenclature Page 16
6 Lewis Dot Structure Worksheet Here are the basic steps involved in drawing the Lewis dot structure for a molecule: a) Calculate the total number of valence electrons in the molecule (take the number of valence electrons for each atom and add them together). b) Draw the electrons around each atom. Put the atom that normally forms the most bonds in the center. c) Each single bond contains 2 electrons. In the spaces below, draw the Lewis structure for each molecule. Each molecule contains only single bonds. Write the total number of electrons for each molecule in the upper right corner. H 2 O NH 3 CCl 4 electrons electrons electrons CH 4 O C 2 H 6 OF 2 electrons electrons electrons Unit 6: Bonding and Nomenclature Page 17
7 Now we are going to look at molecules that contain at least one double or triple bond. In the spaces below, draw the Lewis structure for each molecule. Write the total number of electrons for each molecule in the upper right corner. O 2 N 2 CO 2 electrons electrons electrons SO 3 PO 4 electrons electrons Some chemical substances represent EXCEPTIONS to the octet rule. For example, boron trichloride has a Lewis dot structure that only has three single bonds. The boron atom is surrounded by only 6 electrons instead of 8. Draw the Lewis structure for BCl 3 BCl 3 electrons Unit 6: Bonding and Nomenclature Page 18
8 Covalent Naming Notes Binary covalent compounds are characterized by having two nonmetals. Naming these compounds involves the use of numerical prefixes: Prefix Number Prefix Number If there is only ONE atom of the first element, you DON T need a prefix. The FIRST element is named as a normal element. The SECOND element has an IDE ending. o N 2 O 4 o XeF 4 o N 2 O 5 o CO o CBr 4 o Diarsenic pentoxide o Phosphorous pentabromide o Carbon tetraiodide o Trisilicon tetranitride o Tetraphosphorous decoxide Unit 6: Bonding and Nomenclature Page 19
9 Covalent Naming Worksheet CO 2 NI 3 CO SiBr 4 PCl 5 SF 6 N 2 O As 2 O 5 N 2 O 3 Cl 2 S 7 B 2 Cl 4 P 4 O 10 nitrogen dioxide carbon diselenide silicon tetrachloride phosphorus trifluoride dinitrogen tetrasulfide sulfur hexabromide diphosphorus trioxide arsenic pentafluoride dibromine heptaoxide xenon hexafluoride Unit 6: Bonding and Nomenclature Page 20
10 Naming Acids If the compound begins with Hydrogen, it is an acid. If the acid does not contain a polyatomic ion, write the prefix hydro-, then name the second element and change the ending to ic. o HCl o HBr o H 2 S Naming Acids with Polyatomic Ions The polyatomic ions you have memorized have ate as the ending, so you name the polyatomic ion and change the ending to ic. Use sulfate (SO 4 2- ) as the example H 2 SO 4 is sulfuric acid If the ion has one more oxygen atom than the base (SO 4 2- ), then the ion is named by adding the prefix per- and the suffix ic o H 2 SO 5 is persulfuric acid If the ion has one less oxygen atom than the base (SO 4 2- ), then the ion is named with the suffix ous. o H 2 SO 3 is sulfurous acid If the ion has two less oxygen atoms than the base (SO 4 2- ), then the ion is named with the prefix hypo- and the suffix ous. o H 2 SO 2 is hyposulfurous acid Name the following: 1. H 2 CO 3 2. H 3 PO 2 3. HClO 4 4. H 3 PO 3 Unit 6: Bonding and Nomenclature Page 21
11 VSPER- Valence Shell Electron Pair Repulsion VSPER is used to describe the of molecules Single, double, or triple bonds act. Unbonded electrons, of electrons take up more space than bonded pairs of electrons. Electron densities (lone pairs and bonds) will arrange themselves around an atom to minimize repulsive forces. Steps to determine geometry: 1. Draw the Lewis Structure 2. Count up the number of bonds on the central atom. 3. Look on the chart to find the shape (You will NOT have the chart on the test). Bonds Lone Pairs Shape Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral Unit 6: Bonding and Nomenclature Page 22
12 VSEPR Complete the table with the requested information. Molecule Structural Diagram Oxidation State of each element Molecular Geometry CClF 3 SF 2 BF 3 SiBr 4 NH 3 Unit 6: Bonding and Nomenclature Page 23
13 Shapes and Bonding Orbitals Activity Unit 6: Bonding and Nomenclature Page 24
14 Unit 6: Bonding and Nomenclature Page 25
15 Unit 6: Bonding and Nomenclature Page 26
16 VSEPR Worksheet 1) What is the main idea behind VSEPR theory? 2) For each of the following compounds, determine the bond angles, molecular shapes, and hybridizations for all atoms: a) carbon tetrachloride b) BH 3 c) silicon disulfide d) C 2 H 2 e) PF 3 Unit 6: Bonding and Nomenclature Page 27
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