2. Use the atomic skeleton of a molecule below to answer the following questions.FFS FN₁ C₁-C2 HH-O-C N₂HCANHC5F₁- CC6-H-CC₁-HHFa) How many valence electrons are in the molecule?b) Use these valence electrons to complete the above structure so that EVERY atom has zeroformal charge (this will mean adding lone electrons and multiple bonds to some atoms). Besure to show how you know the formal charge of each atom in the structure.c) Give the electron domain geometry and the molecular geometry for: (a) Carbons labeled 1-8,(b) Nitrogens labeled 1-3, (c) Oxygen and (d) Sulfur. Explain how you came to your answer.

Valence electrons of a molecule can be calculated by the group member of each atom present molecule…

Answered: 2. Use the atomic skeleton of a…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 5QRT

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a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.
The valence shell of an atom in a legitimate Lewis structure (see Figure 2.3) has what in commonwith the valence shell of a noble gas? (Noble gases are stable elements found in the last column ofthe periodic table, e.g., He, Ne, Ar, etc.)
hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.
Decide whether the Lewis structure proposed for each molecule is reasonable or not. molecule proposed Lewis structure BeH₂ :O || :0 || :F: :F: H- Be H Is this a reasonable structure? If not, why not? Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary.…
cide whether the Lewis structure proposed for each molecule is reasonable or not. molecule 13 proposed Lewis I Br₂ structure [1-3] BH [H-B-H]* Br-I- Br: Is this a reasonable structure? If not, why not? Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For…
Around Central Atom Draw Vector for Polar Bonds Formula Molecular Drawing Electron group arrangement (name) Total Molecule Polar? Lewis Structure # lone Bond Inst. (atoms + lone pairs) bonded pairs angle Init. # Valence Electrons atoms Molecular Shape Name (y/n) CH2CI2 NH4* HCN (C is the central atom)
Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for CO₂ that obeys the octet rule if possible and answer the following questions based on your drawing. 1. For the central carbon atom: The number of lone pairs The number of single bonds= The number of double bonds = 2. The central carbon atom
Write a Lewis structure for each of the following molecules. H2CO (carbon is central) Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.
For Nitrogen atom answer the following questions: 1) How many protons does it have? 7 protons 2) How many electrons does it have? 7 electrons 3) How many valence electrons does it have? 5 valence electrons 4) Show full electron configuration (use format similar to this example: 1s2 2s2 2p6 3s2) 1s2 25 2 2p 3 5) The number of dots on the Lewis structure 5 6) How many electrons does it need to lose or gain to achieve the stable octet? (lose/gain) electrons 7) What is the net charge after losing/gaining some electrons? 2 8) Did it become a cation or an anion? neither 9) Show electron configuration after transformation to cation or anion? (use format similar to this example: 1s2 2s2 2p6 3s2) 10) Now which noble gas has an electron configuration identical to electron configuration this ion? Helium
The compound XeCl2F2 can exist in two different forms. One form is polar and the other form is non-polar. Draw a valid Lewis structure of XeCl2F2. Then, draw two 3-dimensional representations of this molecule (including all lone pairs); one that shows the polar form with a correct dipole arrow and the other that shows the non-polar form of the molecule.
Part E: Polarity of Molecules After watching the video on Polarity of Molecules, determine if the entire molecule for each structure shown below is polar or nonpolar. In addition, be sure to indicate polar bonds using arrows or partial charge (delta ō signs) as shown in the first example. Remember, a C-H bond is nonpolar and nonpolar bonds would not require an arrow in this process. 3D Sketch of Molecule Polar or Nonpolar? Formula Molecular Geometry Tetrahedral &- CH2Cl2 Polar CH3CI Tetrahedral CI H. CC14 Tetrahedral CI Co Cl CI CI NH3 Trigonal pyramidal H. H. SO2 Bent CO2 Linear 180° 0=C=0 H2CO Trigonal planar H. H.
5. NO₂-¹ Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) 3-D Model Sketch Any polar bonds in the molecule? Yes No Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No 6. H30*¹ — use a yellow ball for oxygen (not red) when constructing this model Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar

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