fno lewis structure molecular geometry fno lewis structure molecular geometry

For N: Total number of the valence electrons in Free State = 5, Putting these values in above formula, Formal Charge = 5 [ 2 6/2] = 0, For O: Total number of valence electron in Free State = 6, Putting these values in above formula, Formal Charge = 6 [ 4 4/2] = 0, Similarly for F: Total number of valence electron in Free State = 7, Putting these values in above formula, Formal Charge = 7 [ 6 2/2] = 0. A) 2 double bonds and 8 nonbonding electrons. Use Figure \(\PageIndex{3}\) to determine the molecular geometry around each carbon atom and then deduce the structure of the molecule as a whole. wetransfer we're nearly ready stuck hcn atom closest to negative side. 2003-2023 Chegg Inc. All rights reserved. A) PCl3 and LiBr NO, or nitric oxide has two atoms: one N atom, and one O atom. Explain. This theory is very simplistic and does not account for the subtleties of orbital interactions that influence molecular shapes; however, the simple VSEPR counting procedure accurately predicts the three-dimensional structures of a large number of compounds, which cannot be predicted using the Lewis electron-pair approach. This is not the ultimate solution, since there are debates regarding the hybridization value which is considered to be sometimes sp2 and in other times, sp. Answers to these will be posted on the web late Friday afternoon. There are six electron groups around the central atom, each a bonding pair. If we look at this sketch, we will find out that the oxygen atom now has eight electrons surrounding it and nitrogen only has five. Polarity refers to the presence of two opposite charges viz. B) Ionic compounds contain oxygen, and molecular compounds do not. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. B) ditellerium monoxide A) H2, F2, and HF are nonpolar covalent molecules The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. To confirm, whether the above-mentioned Lewis structure sketch is the most suitable formation for NO, there is one more thing we need to check. D) Li, Si, O. Electronegativity is a concept that is useful along with other concepts in are also correct formulas for molecular compounds involving X? This article will help you have a summarized viewpoint about nitric oxide and its internal bonding state so that it becomes easy for you to comprehend the various features and reactions that NO exhibits. All positions are chemically equivalent, so all electronic interactions are equivalent. Smith, Michael Abbott. In this case you want the lowest formal charges for each of the elements. Step 5. A) B2 However, Helium is an exception to this rule which is satisfied with two valence electrons and also derives the basis of stability of the H2 atom. This is known as electron dot structure, another name for Lewis Structure. We can therefore predict the CH3N portion of the molecule to be roughly tetrahedral, similar to methane: The nitrogen atom is connected to one carbon by a single bond and to the other carbon by a double bond, producing a total of three bonds, CN=C. Lewis structure of which of the following molecules? Im a mother of two crazy kids and a science lover with a passion for sharing the wonders of our universe. 1. Also indicate the molecular geometry around the central atom the Hybridization around the central atom, and approximate bond angles BH,CN Molecular Geometry around Central Atom hybridi- zation bond angle * HBC BCN NF,OH Molecular Geometry around Central Atom hybridi- zation bond angle A FNO- I. This designation has a total of four electron pairs, three X and one E. We expect the LPBP interactions to cause the bonding pair angles to deviate significantly from the angles of a perfect tetrahedron. C) NO2 not. E) no correct response, The number of nonbonding electrons exceeds the number of bonding electrons in the Answer and Explanation: 1 If one lone pair is axial and the other equatorial, we have one LPLP repulsion at 90 and three LPBP repulsions at 90: Structure (c) can be eliminated because it has a LPLP interaction at 90. 1. The structure of \(\ce{CO2}\) is shown in Figure \(\PageIndex{1}\). We expect the concentration of negative charge to be on the oxygen, the more electronegative atom, and positive charge on the two hydrogens. C) they occur only between atoms containing 2 valence electrons. C) atoms involved must always also possess nonbonding electron pairs. Transcribed Image Text: a) FNO Total valence electrons AXE notation 2D Lewis structure Electron-group geometry Molecular geometry 3D molecular geometry Ideal bond angle around center atom: In SO2, we have one BPBP interaction and two LPBP interactions. Techiescientist is a Science Blog for students, parents, and teachers. Mathematically, dipole moments are vectors; they possess both a magnitude and a direction. In ammonia, the central atom, nitrogen, has five valence electrons and each hydrogen donates one valence electron, producing the Lewis electron structure. With two bonding pairs and three lone pairs, I3 has a total of five electron pairs and is designated as AX2E3. 3. Step 6: Finally, by completing the octet of all the atoms, the lewis structure appears to be like this: From the above structure, it is clear that the octet for all the atoms involved in the formation of the molecule is satisfied. Therefore, the electron pair geometry here would be trigonal planar with a bond angle of about 120. C) diarsenic pentaselenide All electron groups are bonding pairs (BP). Take your NO molecule. The lewis structure of OF2 is very easy to . We also expect a deviation from ideal geometry because a lone pair of electrons occupies more space than a bonding pair. Assign an AX m E n designation; then identify the LP-LP, LP-BP, or BP-BP interactions and predict deviations from ideal bond angles. In which of the following pairs of compounds are both members of the pair molecular E) no correct response, In which of the following triatomic molecules or ions are both of the bonds multiple You previously learned how to calculate the dipole moments of simple diatomic molecules. 4. dr amy hutcheson vet. As you learned previously, the Lewis electron structure of one of three resonance forms is represented as. ), Re: Fall 2009 Final Exam Question 3A Part C, How to make a New Post (submit a question) and use Equation Editor (click for details), How to Subscribe to a Forum, Subscribe to a Topic, and Bookmark a Topic (click for details), Multimedia Attachments (click for details), Accuracy, Precision, Mole, Other Definitions, Bohr Frequency Condition, H-Atom , Atomic Spectroscopy, Heisenberg Indeterminacy (Uncertainty) Equation, Wave Functions and s-, p-, d-, f- Orbitals, Electron Configurations for Multi-Electron Atoms, Polarisability of Anions, The Polarizing Power of Cations, Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding), *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids), *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism), Coordination Compounds and their Biological Importance, Shape, Structure, Coordination Number, Ligands, *Molecular Orbital Theory Applied To Transition Metals, Properties & Structures of Inorganic & Organic Acids, Properties & Structures of Inorganic & Organic Bases, Acidity & Basicity Constants and The Conjugate Seesaw, Calculating pH or pOH for Strong & Weak Acids & Bases, Chem 14A Uploaded Files (Worksheets, etc. Therefore, understanding how a molecule is formed, the types of bonds that are exhibited, and in what state the molecules are positioned, is important for a thorough description of any given molecule, in this case, we will talk about NO or nitric oxide. + and NO2 Yes/No Molecular Polarity: Polar/Non-Polar 12. N 2 Total \# of Valence Electrons: Lewis Structure: NOTE: There is no bond angle in this . This is because the non-bonding orbitals give rise to partial + and charges on O and N sides. Experts are tested by Chegg as specialists in their subject area. Use the VSEPR model to predict the molecular geometry of propyne (H3CCCH), a gas with some anesthetic properties. Your email address will not be published. The FaxialBrFaxial angle is 172, less than 180 because of LPBP repulsions (Figure \(\PageIndex{2}\).1). Posted at 02:28h in espace o diner saint joseph by who has authority over the sheriff in texas combien de fois le mot pardon dans la bible Likes 4. electronegativity? 4. C) HF is a nonpolar covalent compound and F2 is a polar covalent molecule Well, they really do and electrons are no exception to this. Understanding the molecular structure of a compound can help determine the polarity, reactivity, phase of matter, color, magnetism, as well as the biological activity. A) hydrogen telluride 4. Coming back to NO, we are going to describe its bonding nature in a broad manner here. Thus both F atoms are in the axial positions, like the two iodine atoms around the central iodine in I3. In addition, there was significant damage to livestock and crops. My aim is to uncover unknown scientific facts and sharing my findings with everyone who has an interest in Science. H2O molecule also has a bent-shaped structure. Nitrosyl fluoride | FNO | CID 123261 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety/hazards/toxicity information, supplier lists, and more. 4. Step 4. The molecular geometry is described only by the positions of the nuclei, not by the positions of the lone pairs. ), *Thermodynamics and Kinetics of Organic Reactions, *Free Energy of Activation vs Activation Energy, *Names and Structures of Organic Molecules, *Constitutional and Geometric Isomers (cis, Z and trans, E), *Identifying Primary, Secondary, Tertiary, Quaternary Carbons, Hydrogens, Nitrogens, *Alkanes and Substituted Alkanes (Staggered, Eclipsed, Gauche, Anti, Newman Projections), *Cyclohexanes (Chair, Boat, Geometric Isomers), Stereochemistry in Organic Compounds (Chirality, Stereoisomers, R/S, d/l, Fischer Projections). By shifting the electron dots from the lateral side towards the center shared by nitrogen and oxygen, we now get nitrogen valency to be 7. So before directly going over it. From Figure \(\PageIndex{3}\) we see that with two bonding pairs, the molecular geometry that minimizes repulsions in BeH2 is linear. 4. ____________is characterized by a severe reaction to foods containing gluten. This usually occurs due to the difference in electronegativity of combining atoms resulting in the formation of polar bonds. In the SF2 lewis structure, there is a single bond between sulfur and two fluorine atoms. Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. NOF is actually ONF, since nitrogen has a higher bonding capacity than both oxygen and fluorine.The Nitrogen is double bonded to the oxygen atom on one sideA. Using this information, we can describe the molecular geometry, the arrangement of the bonded atoms in a molecule or polyatomic ion. The VSEPR model can be used to predict the shapes of many molecules and polyatomic ions, but it gives no information about bond lengths and the presence of multiple bonds. Therefore, we do not expect any deviation in the ClICl bond angles. B) Cl2 In contrast, the H2O molecule is not linear (Figure \(\PageIndex{8b}\)); it is bent in three-dimensional space, so the dipole moments do not cancel each other. Science Chemistry The Lewis diagram for SiH4 is: H 1 H-Si-H H The electron-pair geometry around the Si atom in SiH4 is There is/are lone pair(s) around the central atom, so the geometry of SiH4 is The Lewis diagram for BeI is: :I-Be-I: The electron-pair geometry around the Be atom in BeI is There is/are lone pair(s) around the central atom, so the geometry of Bel2 is NO 2 is, in fact, bent (the bond angle is 136). Well, thats for today. 1. Step 4: Looking at the structure and distribution of electrons in the molecule it can be seen that the octet of both fluorine and oxygen is complete, however, Nitrogen is in short of two electrons. 1. The rainwater is so unusually acidic that it can cause toxicity and poses to be really harmful to life on earth. 2. There are two nuclei about the central atom, so the molecular shape is bent, or V shaped, with an HOH angle that is even less than the HNH angles in NH3, as we would expect because of the presence of two lone pairs of electrons on the central atom rather than one. Each group around the central atom is designated as a bonding pair (BP) or lone (nonbonding) pair (LP). First . Once again, we have a compound that is an exception to the octet rule. D) silicon dioxide, The correct name for the compound H2Te is Step 3: Thereafter, the valence electrons of all the three atoms inside the molecule are placed around them in the form of dots, each dot in the structure represents an electron, and the three atoms are connected with the single bonds. This will lead a diatomic molecule to form a linear structure, farthest from each other to minimize the repulsion effects. It is a trigonal bipyramid with three missing equatorial vertices. All electron groups are bonding pairs, so the structure is designated as AX5. What are the relative cross-sections of the two types of collision? 1. B) dihydrogen telluride Consequently, molecules with these geometries always have a nonzero dipole moment. These are majorly responsible for the characteristics displayed by any atom and play a very important role in chemical bonding. The structure for which formal charge is closest to zero is considered correct. B) OX2 As with SO2, this composite model of electron distribution and negative electrostatic potential in ammonia shows that a lone pair of electrons occupies a larger region of space around the nitrogen atom than does a bonding pair of electrons that is shared with a hydrogen atom. View the full answer. This concept has a name to it: Valence Shell Electron Pair Repulsion model theory or VSEPR theory. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. This is essentially a trigonal bipyramid that is missing two equatorial vertices. Required fields are marked *. If you are wondering whether nitric oxide has only harmful effects, be ready to be surprised. Save my name, email, and website in this browser for the next time I comment. The lewis structure of OF2 contains 8 lone pairs (2 lone pairs on oxygen (O) atom and 3 lone pairs on each fluorine (F) atom). 1. 4. With fewer 90 LPBP repulsions, we can predict that the structure with the lone pair of electrons in the equatorial position is more stable than the one with the lone pair in the axial position. With three bonding groups around the central atom, the structure is designated as AX3. For some highly symmetrical structures, the individual bond dipole moments cancel one another, giving a dipole moment of zero. Looking at the above structure it is clear that the octet of all the three atoms involved is satisfied and the lone pairs are placed as far apart as possible, indicating this to be the most precise lewis structure for NOF. With five electron groups, the lowest energy arrangement is a trigonal bipyramid, as shown in Figure \(\PageIndex{2}\). Structure and BondingThank you so much! Therefore, since they are in their least possible formal charge values, we can conclude that the appropriate LS for NO is: Nitrogen forms several oxides, each combination with different ratios of oxygen atoms. In the following molecules, draw the correct Lewis structure. A) predicting the polarity of a bond. ), Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams, Work, Gibbs Free Energy, Cell (Redox) Potentials, Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH), Interesting Applications: Rechargeable Batteries (Cell Phones, Notebooks, Cars), Fuel Cells (Space Shuttle), Photovoltaic Cells (Solar Panels), Electrolysis, Rust, Kinetics vs. Thermodynamics Controlling a Reaction, Method of Initial Rates (To Determine n and k), Arrhenius Equation, Activation Energies, Catalysts, Chem 14B Uploaded Files (Worksheets, etc. The total number of valence electrons available for drawing the nitrous acid (HNO2) Lewis structure is 18. With four electron groups, we must learn to show molecules and ions in three dimensions. Difluoroamine has a trigonal pyramidal molecular geometry. D) they always involve the sharing of 4 electrons. SF2 molecule is polar in nature. It is also a proposed oxidizer for rocket propellants. Select from the following choices: (a) producers (b) primary consumers (c) secondary consumers (d) tertiary consumers. Also, the p-orbital is perpendicular to the plane which is a characteristic of sp2 hybridization. With no lone pair repulsions, we do not expect any bond angles to deviate from the ideal. The Lewis dot structure of HNO nitrogen contains one electron pair while oxygen contains two pairs of electrons. C) trigonal pyramidal Consequently, the bond dipole moments cannot cancel one another, and the molecule has a dipole moment. The electronic configuration of Nitrogen is 1s2 2s2 2p3. c. two single bonds, two double bonds, and no lone pairs. Legal. I am Savitri,a science enthusiast with a passion to answer all the questions of the universe. C) SO2 NO is a diatomic molecule having unpaired electrons. A) F, Br, As Once again, both groups around the central atom are bonding pairs (BP), so CO2 is designated as AX2. C) H2O You, as I expect, are already familiar with valence shell and valence electrons, right? Thus a molecule such as H2O has a net dipole moment. more elements. C) ClF Now, when we consider the double bond, as we checked in the lewis structure sketch, we found out that nitrogen doesnt really fulfill its octet and sticks to seven valence electrons. Groups are positioned around the central atom in a way that produces the molecular structure with the lowest energy, as illustrated in Figures \(\PageIndex{1}\) and \(\PageIndex{2}\). B) CF4 The theory of hybridization was first proposed by Linus Pauling in 1931. The terminal carbon atoms are trigonal planar, the central carbon is linear, and the CCC angle is 180. When drawing the Lewis structure for nitrosyl fluoride, FNO, why is there a double bond between the nitrogen and oxygen molecules instead of there being a double bond between the nitrogen and fluorine molecules? (6 dots)F--(four dots)O--(6 dots)F. Analysis of an unknown substance showed that it has a high boiling point and is brittle. Till then, keep enjoying and learning chemistry! 1. E) no correct response, Coordinate covalent bonds differ from normal covalent bonds in that Placing them in the axial positions eliminates 90 LPLP repulsions and minimizes the number of 90 LPBP repulsions. 3. With three bonding pairs and one lone pair, the structure is designated as AX3E. A) Molecular compounds contain two elements, and ionic compounds contain three or In which of the following molecular compounds are all the bonds single bonds? The central atom, carbon, has four valence electrons, and each oxygen atom has six valence electrons. National Institutes of Health. HNO2 Lewis Structure, Molecular Geometry, Hybridization, Bond Angle, and Shape. - The total number of nonbonding electron pairs present in the Lewis structure of GeH4 is. Owing to the presence of an unpaired electron, it acts as a free radical and is reactive in nature. The VSEPR model can be used to predict the structure of somewhat more complex molecules with no single central atom by treating them as linked AXmEn fragments. the same geometry? When atoms combine to form molecules, every constituent atom already has a number of electrons surrounding it. This is because a multiple bond has a higher electron density than a single bond, so its electrons occupy more space than those of a single bond. Carbon monoxide is made of two elements: carbon and oxygen. Nitrogen has five valence electrons in its outermost shell and Oxygen has six valence electrons. solon high school swimming; dennison funeral home viola, il; fno lewis structure molecular geometry Now, if we come back to our molecule NO, do you notice one thing that this molecule has only two atoms in it. My aim is to uncover unknown scientific facts and sharing my findings with everyone who has an interest in Science. The O-S-O bond angle is expected to be less than 120 because of the extra space taken up by the lone pair. - [citation needed] It has also been proposed as an oxidizer in rocket propellants. In more complex molecules with polar covalent bonds, the three-dimensional geometry and the compounds symmetry determine whether there is a net dipole moment. celiac disease \hspace{1cm}Crohns disease. As we discussed before, NO is polar. The theory of hybridization was first proposed by Linus Pauling in 1931. In molecular geometries that are highly symmetrical (most notably tetrahedral and square planar, trigonal bipyramidal, and octahedral), individual bond dipole moments completely cancel, and there is no net dipole moment. NO Hybridization and Molecular Orbital (MO) Diagram, SF4 Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram, HNO2 Lewis Structure, Molecular Geometry, Hybridization, and Polarity. Im a mother of two crazy kids and a science lover with a passion for sharing the wonders of our universe. A Lewis structure is the pictorial representation of bond formation in a molecule. So, let us learn about this molecule in a detailed format to have an elaborate comprehension of the internal bonding nature and several other characteristics. If you want me to write on any specific topic, your suggestions are always welcomed. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Because there is one hydrogen and two fluorines, and because of the lone pair of electrons on nitrogen, the molecule is not symmetrical, and the bond dipoles of NHF. As a result, the CO2 molecule has no net dipole moment even though it has a substantial separation of charge. Given the following electronegativites: Li = 1.0, H = 2.1, F = 4.0 which of the B) polar covalent. So totally it has 3 electron pairs. Here, oxygen has attained a valency of eight but the nitrogen hasnt yet. D) more than one correct response E) no correct response, For which of the following pairs of compounds do both members of the pair have names 1. We will work with and here, so before we go direct, heres just a quick view: Sigma orbitals are found to be symmetric across the bond axis and Pi orbitals are found along a nodal plane with the bond axis. Check out the article I wrote on lewis structure, hybridization, geometry of H2O. 3. lewis structure, hybridization, geometry of H2O, 11 Uses of Platinum Laboratory, Commercial, and Miscellaneous, CH3Br Lewis Structure, Geometry, Hybridization, and Polarity. D) more than one correct response 120 . Because a multiple bond is counted as a single bond in the VSEPR model, each carbon atom behaves as if it had two electron groups. The three nuclei in BrF3 determine its molecular structure, which is described as T shaped. The carbon atom forms two double bonds. Using the VSEPR model, predict the molecular geometry of each molecule or ion. Now, let us draw these electrons as dots surrounding the nitrogen and oxygen atoms. B) two bonds and one nonbonding electron group. Question: Chem 3A Chapter 10 Exercise 3: Draw the Lewis and VSEPR structures of the following: a) FNO (N in middle) (Draw Lewis on left) (Draw VSEPR with vectors on right) - What is the approximate bond angle in FNO? Each double bond is a group, so there are two electron groups around the central atom. It was first reported in 1930 by Ruff and Krug who prepared it by fluorination of chlorine; this also produced ClF (chlorine monofluoride) and the mixture was separated by distillation.. 3 F 2 + Cl 2 2 ClF 3. There are five groups around sulfur, four bonding pairs and one lone pair. We see from Figure \(\PageIndex{2}\) that the geometry that minimizes repulsions is octahedral. paul mcfadden rochester ny February 20, 2023 | | 0 Comment | 5:38 am The next two carbon atoms share a triple bond, and each has an additional single bond. I am Savitri,a science enthusiast with a passion to answer all the questions of the universe. Which of the following Step 2: Now counting the number of valence electrons in the molecule: For Nitrogen (Group 15 element), number of valence electron = 5, For Oxygen (Group 16 element), number of valence electron = 6, For Fluorine (Group 17 element), number of valence electron = 7, Now counting total number of valence electron= 5 + 6 + 7. Recognizing similarities to simpler molecules will help you predict the molecular geometries of more complex molecules. Both groups around the central atom are bonding pairs (BP). It has a bent molecular shape: this can be rationalized in the VSEPR model in terms of the lone-pair of electrons located on the N atom. The three fragments combine to give the following structure: Certain patterns are seen in the structures of moderately complex molecules. With four bonding pairs, the molecular geometry of methane is tetrahedral (Figure \(\PageIndex{3}\)). Produced in laboratories via ammonia oxidation or nitric acid reduction, this is also formed naturally during lightning and thunderstorms. In MO theory, we will come across certain terms called. 2. Also indicate the molecular geometry around the central atom the Hybridization around the central atom, and approximate bond angles BH,CN Molecular Geometry around Central Atom hybridi- zation bond angle * HBC BCN NF,OH Molecular Geometry around Central Atom hybridi- zation bond angle A FNO- I * NOH- CH NF . Like NH3, repulsions are minimized by directing each hydrogen atom and the lone pair to the corners of a tetrahedron. , Using Standard Molar Entropies), Gibbs Free Energy Concepts and Calculations, Environment, Fossil Fuels, Alternative Fuels, Biological Examples (*DNA Structural Transitions, etc. C) Molecular compounds possess a molecular structural unit, and ionic compounds do Atoms of different nature combine together in different ratios to form different compounds and this combination leads to the rise of several properties that the resultant molecule exhibits. 3. D) determining the charge on a polyatomic ion. E) no correct response, In which of the following pairs of bonds is the first listed bond more polar than the It helps us to understand the valence electrons and the arrangement of atoms in the molecule. D) more than one correct response The sulfur atom has six valence electrons and each fluorine has seven valence electrons, so the Lewis electron structure is. Placing five F atoms around Br while minimizing BPBP and LPBP repulsions gives the following structure: 3. D) more than one correct response This VESPR procedure is summarized as follows: We will illustrate the use of this procedure with several examples, beginning with atoms with two electron groups. E) no correct response, A period 2 nonmetal, X, forms the molecular compound NX3. 2. The first and foremost step towards understanding chemical bonds inside a molecule is to draw the Lewis Structure. Many of the physical and chemical properties of a molecule or ion are determined by its three-dimensional shape (or molecular geometry). All LPBP interactions are equivalent, so we do not expect a deviation from an ideal 180 in the FXeF bond angle. Not only a major participant in acid rain deposition, but NO can also cause ozone layer depletion and badly affect the human respiratory system in general. 2. With a double bond on fluorine, oxygen has a formal charge of -1, nitrogen has a formal charge of 0, and fluorine has a formal charge of +1. NO2 Lewis structure molecular geometry. that contain the prefix di-? In the following molecules, draw the correct Lewis structure. D) F2 is a nonpolar covalent molecule and HF is a polar covalent molecule, D) F2 is a nonpolar covalent molecule and HF is a polar covalent molecule, Which of the following diatomic molecules contains the bond of greatest polarity?