Table 3 Molecules with Multiple Central Atoms Molecule C2H4 H2O2 CH3OH CH3NH2 Number of Bond Pairs / / / / Number of Lone Pairs / / / / Number of Electron

NH3 vs BH3 NH3 BH3               polar nonpolar polar nonpolar Molecular Geometry   Molecular Geometry   Question 1b: How does the molecular geometry (trigonal pyramidal vs trigonal planar) affect the polarity?

Predict the ideal bond angles around each central atom in this molecule. H H -H oxygen: carbon: :O: -I -H O O

Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CHCH20H) give the structure around the bold atom.

6. Predict the geometries of PCI, using the VSSPR method with the following steps Step 1) Draw the skeletal structure and finish Lewis structure Valence:5(7)+1(5)=40 ー10 30 Step 2: Write the general form (Abx or ABXEY): Step 3) Table number to use (10.1 or 10.2): Step 4: Predict the geometry Steps) dletermine polarity:

Can you please do the first 3 rows of the table?

For each, draw the lewis structure, a 3D Structure including Angles, Electron Pair Geometry, Molecular Geometry, and whether it is "Polar or Non/Polar" A)   SF6 B)   CH2O

1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table.   1.2 Describe the type of bonding that exists in F2 (g) molecule. How does this type of bonding differ from that found in the HF (g) molecule?   1.3 Define hydrogen bonding using examples.   1.4 PH3 and NH3 moleculea are the same shape but the molecules are non-polar and polar respectively. Explain why this is so.   1.5 Give an example of molecule that has a coordinate covalent bond.   1.6 Draw a Lewis structure for each of the following molecules of ions: a) HF3 b) CIO3-

Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CH,CH,0H) give the structure around the bold atom. Molecule ЕPG Hyb (circle if polar) 2D Lewis Structure 3D Lewis Structure MG ВА CH,S GeO2 CF4

Provide the Lewis, structure, Molecule/Ion type (i.e. AX3E, AX5, etc), Molecular Geometry, bond angle (the ideal/pure bond angle, not the bond angle as affect by lone pairs), and Polarity (a 3-d representation with bond and molecular dipoles annotated)