Identify the type of bond that would likely form between each of the following pairs of atoms.circle one: non-polar covalent polar covalent ioniccircle one: non-polar covalent polar covalent ioniccircle one: non-polar covalent polar covalent ionica. Be & Fb. Be & Pc. Fe & P

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Answered: Identify the type of bond that would…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 34A

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Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure for aspartame is shown below. Aspartame can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure above to give each atom a formal charge of zero when drawing the Lewis structure. Also note that the six-sided ring is shorthand notation for a benzene ring (C6H5). Benzene is discussed in Section 4-7. Complete the Lewis structure for aspartame. How many C and N atoms exhibit sp1 hybridization? How many C and O atoms exhibit sp3 hybridization? How many and bonds are in aspartame?
Which one of the following bonds is polar? a. a bond between two identical atoms b. a bond between two atoms with the same electronegativity c. a bond between two atoms with different electronegativities
In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.
a model of each of the following molecules: a. Based on your model, draw a bond-line representation with as many atoms as possible in the plane of the paper. Use wedge and dash bonds to represent any atoms that do not lie in the plane of the paper. b. Indicate each unique bond angle and the shape of each unique central atom.
WCJC:: Single Sign-On to all you X macmillanlearning.com/sac/7598972#/7598972/8/0 ✪ Assignment Score: 8- ! 82.9% Ei O C—0 Ch 9 Homework: Covalent Bondi X 0—F C-N O—CI 8- Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta notation next to each end of the bond. S-H 8- S-CI CI—C 8- 6- ö + hp 8- Question 9 of 12 - Ch 9 Homewo X + Resources Answer Bank E N Ex Give Up? 8 + Feedback A { Resume Attempt 1 78°F Haze ( Sig 2 2/
Part ADraw the Lewis structure for HCCH (ethyne).Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all hydrogen atoms and all lone pairs of electrons. Part BDraw the Lewis structure for CS2 (where C is the central atom).Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.
Draw the resonance structure indicated by the curved arrows. Assign formal charges. H H/:O: H H-C-C-C-Ċ—H H H H Draw the molecule by placing atoms on the canvas and connecting them with bonds. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms in the correct structure.
2. Circle the following pairs are not resonance structures of one another. Draw in all implied lone pairs on the structures. All formal charges have been included. A D $a G B E OH H to C F F
10. Molecule: CzHj0 Indicate the number of available electrons that are in the molecule. ae = Trial Structure: in the space to the right connect all of the atoms to the central atoms (all Cs in a chain) and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization:
3. Draw structural formulas for the following covalently bonded molecules, representingeach covalent bond by a line. НССH HCN HC1 CH;CH2OH CCI4
Please note that "geometry" refers to the molecular or ionic geometry. A. The Lewis diagram for H₂O is: The electron-pair geometry around the O atom in H₂O is There are B. The Lewis diagram for NH4+ is: HỘ–H There are lone pair(s) around the central atom, so the geometry of H₂O is H H-N-H H The electron-pair geometry around the N atom in NH4+ is lone pair(s) around the central atom, so the geometry of NH4+ is
9. Molecule: SF6 indicate the number of available electrons that are ae = in the molecule. in the space to the right connect all of the atoms Trial Structure: to the central atom and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization:

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Identify the type of bond that would likely form between each of the following pairs of atoms. circle one: non-polar covalent polar covalent ionic circle one: non-polar covalent polar covalent ionic circle one: non-polar covalent polar covalent ionic a. Be & F b. Be & P c. Fe & P