I. Determine the molecular geometry of the encircled atom in the following organic molecules by giving the required information in the table below: (Type your answers except for the Lewis structure. Draw the Lewis structure in a sheet of paper, scan copy or shot a picture of it and paste it next page.) LEWIS ELECTRON PAIR MOLECULAR MOLECULE STRUCTURE GEOMETRY SHAPE CH3 CH3-CH2 CC-C-CH3 CH3 (1) (2) CH3 -(CH2), CO-CH(CH3)-CH3 (3) CH3 -(CH2)3-CO-CH(CH3)-CH3 ATOM' S VALENCE ELECTRON NO. OF BONDING PAIRS NO. OF NON- BONDING PAIRS TOTAL ELECTRON PAIRS GENERAL FORMULA BOND ANGLE HYBRID ORBITAL

I. Determine the molecular geometry of the encircled atom in the following organic molecules by giving the required information in the table below: (Type your answers except for the Lewis structure. Draw the Lewis structure in a sheet of paper, scan copy or shot a picture of it and paste it next page.) LEWIS ELECTRON PAIR MOLECULAR MOLECULE STRUCTURE GEOMETRY SHAPE CH3 CH3-CH2 CC-C-CH3 CH3 (1) (2) CH3 -(CH2), CO-CH(CH3)-CH3 (3) CH3 -(CH2)3-CO-CH(CH3)-CH3 ATOM' S VALENCE ELECTRON NO. OF BONDING PAIRS NO. OF NON- BONDING PAIRS TOTAL ELECTRON PAIRS GENERAL FORMULA BOND ANGLE HYBRID ORBITAL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Draw a Lewis structure for the given skeletal molecule. Note: Multiple bonds and lone pairs are not shown in the skeletal molecule. H. H H HHH | | | + H-C-C-N-H II H H I C-H How many lone pairs of electrons are found in the Lewis structure of your molecule?
ructions tiple Attempts Not allowed. This test can only be taken once. ce Completion This test can be saved and resumed later. Your answers are saved automatically. Jestion Completion Status: 1 2 3 4 QUESTION 1 Enter the number of valence electrons and number of possible bonds for each of the following element CARBON: Valence electrons: 4 ; Bonds needed: 4 OXYGEN: Valence electrons: 6 ; Bonds needed: 2 HYDROGEN: Valence electrons: 1 NITROGEN: Valence electrons: 5 SULFUR: Valence electrons: PHOSPHORUS: Valence electrons: CHLORINE: Valence electrons: FLUORINE: Valence electrons: I For Blank 9 ; Bonds needed: 1 ; Bonds needed: 3 ; Bonds needed: ; Bonds needed: ; Bonds needed: ; Bonds needed: Click Save and Submit to save and submit. Click Save All Answers to suve all answers,
Following is a molecule with polar bonds whose shape was obtained using the VSEPR theory. Specify the molecular shape of this molecule, and whether the molecule is polar or nonpolar. (Hint: In terms of polarity, see whether the dipoles in the molecule cancel or not. A molecule containing polar bonds can be nanpolar if the dipoles cancel each other. You can imagine the dipoles as ropes pulling on the central atom–If the pulls cancel each other, that is, the central atom cannot move, then the molecule is nonpolar. If on the other hand the opposite is true, then the molecule is polar.) O trigonal pyramidal shape, nonpolar O trigonal planar shape, nonpolar O tetrahedral shape, polar O trigonal pyramidal shape, polar O trigonal planar shape, polar
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1. Classify the following compound as metallic, ionic, polar covalent, or nonpolar. Additionally, predict 3 properties of the compound based on the type of bonds it presents and/or the intermolecular forces present. Remember to justify your answer. C3H3N Answer:
Chem. 065 Ionic and covalent bonds 1. Complete the following worksheet: Compound Ionic bond or covalent bond: which applies NO CrO CaCO3 PC13 NaCl CS₂ 2. Complete the following work sheet Compound Number of Number of Number of triple bonds single bonds double bonds HCN CHCI, -2 SO₂-² SO₂ HCOCI CO₂ SC₁₂ CIO, Number of lone Molecular pair of shape electrons on the central atom.
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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-
Pls helo ASAP. Pls help in all asked questions.
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