the first image shows instructions. please answer For each of the following molecules or polyatomic ions, fill out all the columns using thefollowing instructions:1.Calculate the total number of valence electrons.2. Draw the Lewis structure.3. Build the model.4. Determine the molecular geometry (tetrahedral, trigonal pyramid, bent, linear, ortrigonal planar).5. Determine the bond angle.6. Using the electronegativity table, determine the type of the bonds in the structure.7. Determine if the molecule is polar (dipole moment) or nonpolar.Study Assignment E Lewis Structures and M olecular Geometry Polar orNumberBondBondnonpolarmoleculeLewisMolecularof valenceanglepolaritystructuregeometryelectronsC,H,CO,SO,N,H,OCHIFBR

The Valence Shell Electron Pair Repulsion (VSEPR) theory provides insights into molecular geometry…

Answered: CH₁ CO₂ SO₂ N₂ H₂O CHIFBr Number of…

CH₁ CO₂ SO₂ N₂ H₂O CHIFBr Number of valence electrons Polar or Lewis Molecular structure geometry Bond angle Bond polarity nonpolar molecule

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU1: Alchemy: Matter, Atomic Structure, And Bonding

Section: Chapter Questions

Problem 22STP

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19. Soz? 20. NOZ 21. H;О* 22. NH,+
Steps for Lewis Structures: 1. Determine the total number of valence electrons. Add electrons for negative charges, subtract electrons for positive charges. 2. Place least electronegative atom (except H) as central atom in structure. 3. Connect atoms by singles bonds. Each single bond = 2 electrons. 4. “Sprinkle” remaining electrons around outside atoms first to complete octets. Don’t use more electrons than the total found in step 1. Then complete the central atom’s octet last if you have enough electrons. 5. Make double or triple bonds as needed to complete octets. 6. Place brackets and charge for ions. For the central atom in each formula, draw the Lewis Structure with all valence electrons shown. 1. PH3 2. H2O 3. CO2 4. CHCl3 5. O2 6. N2 7. CF4 8. C3H8 9. CH3COOH 10. N2O 11. OCN-
Answer each of the following questions correctly. Choose the correct answer. 1. It is a measure of how equally the electrons in a bond are distributed between the two atoms involved in a covalent bond. a. Polarity b. Octet rule c. Ionization energy d. Electron affinity 2. The shape of bonding molecular orbital shows that the greatest electron density is in the region. a. Between the two nuclei b. Close to the more atom electronegative c. Close to the bigger atom d. Uniformly around the two nuclei 3. In which compound is the bond that has the most ionic character found? a. HCl b. Kl c. MgS d. NO
or ion: 1. Draw the complete Lewis structure of the molecule or ion. 2. Determine the total number of electron groups (clouds) surrounding the central atom. 3. Determine the electron geometry of the groups around the central atom (linear, trigonal planar, etc.) 4. Determine the molecular shape of the molecule (linear, bent, trigonal planar, etc.) 5. Determine the molecular polarity (polar vs, nonpolar) 6. SCN-, thiocyanate ion (carbon central atom) Lewis structure Total number of electron groups around the central atom Electron geometry Molecular shape Molecular polarity
1. The electron pair in a H - Cl bond could be considered... a. closer to H because Hydrogen has a larger radius and thus exerts greater control over the shared electron pair b. closer to Cl because Chlorine has a higher electronegativity than Hydrogen c. closer to H because Hydrogen has a lower electronegativity than Chlorine d. an inadequate model since the bond is ionic 2. It is important to know the geometry of a molecule because the geometry _______. a. will give the Lewis structure of the molecule b. affects the physical and chemical properties of the substance c. will determine whether the molecule is ionic or covalent d. Both B, and C
ionic character of the bond is less than 51% percent so the bond is covalent. (Think and check the periodic table) Multiple Choice. 20. In the molecule models of HF, HCI, and HBr on page 10, the respective numbers (1.0cm, 1.2 cm, and 1.5 cm) represent the a. protons in the atom c. repulsive force between the atoms b. molecular distance between nuclei d. actual distance between atoms 21. The halogen element that has the most attraction for the hydrogen electron is a. fluorine b. chlorine c. bromine
I need very short answers they dont have to in complete sentence solve all of them if you cant do all of them dont do anything
The molecular drawing tool provides a canvas and tools for drawing molecules in Sapling Learning. The main toolbar Drawing single bonds, double bonds, and triple bonds. Draw C-C, C=C and C=C. consists of several menus. 1. Click on the Draw menu and select the single bond The Select menu allows you to select bonds, atoms, (the single line). electrons, and charges to be moved or rotated. 2. Click on the drawing canvas to draw the single bond. 3. Next, draw a double bond, Select the double bond The Draw menu is used to draw bonds and atoms. • The Rings menu allows you to quickly draw rings of (two lines) from the Draw menu. Then, click on a various sizes and includes the most commonly separate area on the drawing canvas. 4. Lastly, draw the triple bond. Select the triple bond (three lines) from the Draw menu and click on a used rings. The More menu is used to add charges, nonbonding electrons (optional), and curved arrows (optional). Also present is the "reset drawing" button, which will…
1. Draw the best Lewis dot structure for the anion CCl, in the correct molecular geometry (Include formal charges and lone pair electrons, and use dashed and solid wedge bonds if necessary) 2. How many electron groups are present around the central atom and what is the electron group geometry? 3. What is the molecular geometry and ideal bond angles? 4. Is the molecule polar or honpolar? If it is polar, draw a dipole moment arrow next to your structure to indicate the directionality of the dipole moment. Answers: Edit View Insert Formuat Tools Table 12pt Paragraph BIUA 2 of Bons O words IMG4Sg IMG 3449 og IMG 344 jpg IMG 3447 jp De
Which description below correctly describes polar molecules? a. Have polar bonds present. b. The polar bonds are arranged so that they do not cancel. c. Lone pairs on the central atom are arranged so that they do not cancel. d. Lone pairs on the central atom are arranged so that they can be cancelled out.
Please help me answer all blank of Bond type