n your lab notebook, draw the "correct" (or best) Lewis structure for the molecule CH2CO. Now, answer the following questions about this molecule.   What is the total number of valence electrons represented in the Lewis structure of this molecule (or molecular ions)? How many lone-pairs of electrons are on the C atom? How many (σ) sigma bonds does this molecule have?

organize the page that will show a geometrically-accurate Lewis dot structure for each of these covalent compounds. Write the name of the compound , geometric shape and indicate if it is polar or nonpolar.  PF3         HCN         H2S         CCl4         CO2         CH4         CH2O     HF

Write the Lewis structure for the following molecule. State the electronic structure (shape based on electron pairs or bonds) AND the geometric structure (shape based on the atoms only). Include all valence electrons in your structure. State how many electrons are used to form covalent bonds in the molecule. Is the molecule polar? H_2S

II. Complete the table below. Compound Molecular Geometry Molecule Polarity 1. НCСI 2. H2S 3. CH4 4. N2 Dipole moment of CO2 5. Н2О Take note that bond polarity and molecule polarity are not the same. The presence of polar bonds does not automatically make a molecule polar. The geometry of the molecule also plays an important role. This can be seen in CO2 wherein the electronegativity difference of C and O is 1.0. This equal distribution of polar bonds makes the molecule non- polar.

Answer the questions in the table below about the shape of the chlorine trifluoride (ClF,) molecule. How many electron groups are around the central chlorine atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central chlorine atom? (You may need to use the scrollbar to see all the choices.) |(choose one)

Draw the Lewis Structure for NH2CH2CO2H. Now answer the following questions based on your Lewis structure: (Enter an integer value only.) # single bonds in the entire molecule # double bonds in the entire molecule # lone pairs in the entire molecule

For the molecule NO-2, draw the 3D Lewis structure then, give the electronic geometry (EG), the molecular geometry (MG), and the bond angle (BA). Finally, determine if the molecule is polar.

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Answer the following questions about the Lewis structure for calcium hydrogen carbonate, Ca(HCO3)2 There are calcium ions and hydrogen carbonate ions. There are ionic bonds in the molecule. The calcium ion has electron dots. Each hydrogen carbonate ion has central atoms and valence electrons. Each hydrogen carbonate ion has single covalent bonds, double covalent bonds, and triple covalent bonds. In each hydrogen carbonate ion, the central C has REDS, the shape is y and the bond angles are about In each hydrogen carbonate ion, the central O has REDS and the shape is а. О b. 1 С. 2 d. 3 е. 4 f. 5 g. 8 h. 10 i. 12 j. 14 k. 16 I. 18 m. 20 n. 24 О. 26 р. 30 q. 32 r. 34 S. 36 t. diatomic u. pyramidal v. linear z. bent y. trigonal planar w. monoatomic ions x. tetrahedral aа. 1200 bb. 180° Cc. no bond angles, no central atom nonpolar dd. 109.5° ее. polar ff. gg. ionic hh. O and O

H20 CO2 Both molecules pictured have 3 atoms but different molecular geometry and different molecular polarity. Identify the shape and molecular polarity for each. Then explain what causes the difference in molecular geometry and molecular polarity. Answer in 5-8 complete sentences, in your own words, with proper grammar and spelling. HTML Editor I A 工三 三目 E E x' ¶ ¶ 12pt Paragraph !!!