Which of the following bonds would be classified as nonpolar covalent bonds? [Select all that apply.] С-С O C-C O C-F F-F O P-H O N-H C-H O Li-CI O C-N
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![Which of the following bonds would be
classified as nonpolar covalent bonds?
[Select all that apply.]
O C-C
O C-F
O F-F
O P-H
O N-H
O C-H
O Li-CI
O C-N](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fde326383-8b00-4076-b3f6-1f860c5e4029%2Fa5651a8c-0d95-41ee-bcb2-5d2c32ce470d%2Ffnoj7ua_processed.jpeg&w=3840&q=75)
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- A) Which of the following bonds are nonpolar? Choose all that apply Choices: O=O double bond C=O double bond C-O single bond C=C double bond C-H single bond N-H single bond O-H single bond H-H single bond B) Which of the following bonds are polar covalent? Choices: N-H single bond C=O double bond C-O single bond C-H single bond C-C single bond N-F single bond S-H single bond O=O double bond Thank you so Much!!Which of the following are ionic compounds? Select all that apply.Answer the following question about acetonitrile (CH3C≡N:). Question: Label all bonds as polar or nonpolar ?
- Predict which of these compounds are ionic and which are covalent. State your reasoning.(a) SF6(b) KBr(c) N2O3(d) BaS(e) CaCO3(f) C6H5ClQuestion: Consider a hypothetical molecule, X₄Y₃, composed of four atoms of element X and three atoms of element Y. The molecule is in a gaseous state. a) According to the octet rule, which elements are likely to form multiple bonds in this molecule? Explain your reasoning. b) Calculate the total number of valence electrons in X₄Y₃. c) Based on the total number of valence electrons, determine the formal charge on each atom in X₄Y₃.Resonance Forms Question (b) Draw two resonance forms for nitrite ion, NO2−. What can yousay about the geometry of this molecule (linear or bent)? (Hint: Consider the effect of electron repulsion exerted by the lone pair on nitrogen.) (c) The possibility of valence-shell expansion increases the number of feasibleresonance forms, and it is often difficult to decide on one that is “best.” Onecriterion that is used is whether the Lewis structure predicts bond lengths andbond angles with reasonable accuracy. Draw Lewis octet and valence-shellexpanded resonance forms for SO2(OSO). Considering the Lewis structure for SO (Exercise 1-8), its experimental bond length of1.48Å, and the measured S–O distance in SO2 of 1.43Å, which one of the various structures would you consider “best”. Explain your answer in depth, clarity and with details and in a step-by-step fashion.
- I got the net charge -1 but the system shows it wrong. The formula I used: Formal charge= Valence electron-(bonding electrons +individual lone pair)For each of the given below, compute for the electronegativity difference (2 decimal places) and identify the bond type of the compound write PC for polar covalent, and NPC for nonpolar covalent, and IB for ionic bond. Refer to the sample shown belowWhich of the following has nonpolar bonds? Group of answer choices I2 OF2 HF All are nonpolar H2S
- Question: The vanillin molecule depicted below is a flavor in vanilla beans. What is the molecular formula for this molecule? Also, consider the bonds indicated with arrows below. What types of covalent bonds are these? What types of orbitals overlap to make each of these bonds?Question: Two pairs of shared electrons are:A. single bond.B. double bond.C. triple bond.D. resonance forms of bonding.Reset SelectionMark for Review What’s This?Which of the following Lewis Dot Structures is definitely incorrect? Group of answer choices C A B D E
