Very strong silicon-oxygen covalent bonds have to be broken throughout the structure before melting occurs. Covalent bonds are commonly found in carbon-based organic molecules, such as DNA and proteins. The giant covalent structure of silicon dioxide. The planar configuration for the ethene molecule occurs because it is the most stable bonding arrangement. ... exothermic - Exothermic describes a process that gives off heat. In diamond, each carbon shares electrons with four other carbon atoms - forming four single bonds. The giant covalent structure of diamond. ... covalent bond - A covalent bond is a chemical bond formed when two atoms share two electrons. Electrons shared in pure covalent bonds have an equal probability of being near each nucleus. … Rotation about the internuclear axis is much more difficult for multiple bonds; however, this would drastically alter the off-axis overlap of the π bonding orbitals, essentially breaking the π bond. hydrogen bonds. In this chapter, we will consider another type of bonding—covalent bonding. is insoluble in water and organic solvents. A σ bond is stronger than a π bond due to greater overlap. These molecules are attracted to each other by a) coordinate covalent bonds c) ionic bonds b) electrovalent bonds d) hydrogen bonds 14) The bond between hydrogen and oxygen in a water molecule is classified as a) covalent and nonpolar c) ionic and polar you may look at a periodic table that doesn't have electronegativities. Electrons shared in pure covalent bonds have an equal probability of being near each nucleus. For example, molecule benzene has two resonance forms (Figure 5). It does not consist of discrete molecules. Assignment of Hybridization Involving Resonance The σ bonds are usually formed by the overlap of hybridized atomic orbitals, while the π bonds are formed by the side-by-side overlap of unhybridized orbitals. The three bonding regions form a trigonal planar electron-pair geometry. The two unhybridized p orbitals per carbon are positioned such that they overlap side by side and, hence, form two π bonds. doesn't conduct electricity. Equilibria of Other Reaction Classes, 16.3 The Second and Third Laws of Thermodynamics, 17.1 Balancing Oxidation-Reduction Reactions, Chapter 18. The term covalent bond describes the bonds in compounds that result … We find this situation in acetylene, H−C≡C−H, which is a linear molecule. Ion exchange usually describes a processes of purification of aqueous solutions using solid polymeric ion exchange resin.More precisely, the term encompasses a large variety of processes where ions are exchanged between two electrolytes. Chemistry by Rice University is licensed under a Creative Commons Attribution 4.0 International License, except where otherwise noted. oxygen bonds. To describe the number of electron pairs shared by neighbouring atoms, … Neither resonance structure completely describes the electrons in the π bonds. (c) Describe the atomic orbitals that form the π bonds in the molecule. In the case of Cl 2, each atom starts off with seven valence electrons, and each Cl shares one … Covalent bonds within molecules are strong. alkane - An alkane is an organic molecule that only contains single carbon-carbon bonds. However the forces between the molecules themselves (intermolecular forces) are weak. As we learned in the previous topic, ionic structures have high melting and boiling points … The atoms within a sheet are held together by strong covalent bonds - stronger, in fact, than in diamond because of the additional bonding caused by the delocalised electrons. 5. The molecules are bigger than phosphorus molecules, and thus the van der Waals attractions are stronger, leading to a higher melting and boiling point. For instance, H-bonds can form between NH 3 and H 2 O, between HF and H 2 O, but not between F 2 and H 2 O since the F atoms in F 2 are not slightly negative or positive since the bond between them is nonpolar covalent. The structure of diamond. We will examine how atoms share electrons to form these bonds, and we will begin to explore how the resulting compounds, such as cholesterol, … The other halogen molecules (F 2, Br 2, I 2, and At 2) form bonds like those in the chlorine molecule: one single bond between atoms and three lone pairs of electrons per atom. 1. We can use either of these forms to determine that each of the carbon atoms is bonded to three other atoms with no lone pairs, so the correct hybridization is sp2. Elements. Member States may allow for exemptions from this Regulation in specific cases for certain substances or mixtures, where necessary in the interests of defence. However, it also has some features of covalent bonding: it is directional, stronger than a van … Because breaking a chemical bond requires energy, homolysis occurs under the addition of heat or light. These bonds are stronger and much more common than are ionic bonds in the molecules of living organisms. You can tell from its formula that it is not an ionic compound; it is not composed of a metal and a nonmetal. For example, in water each hydrogen and oxygen share a pair of electrons to make a molecule of two hydrogen atoms single bonded to a single oxygen atom. Describe how a covalent bond forms. Q. Multiple bonds consist of a σ bond located along the axis between two atoms and one or two π bonds. Very strong carbon-carbon covalent bonds have to be broken throughout the structure before sublimation occurs. If a piece of graphite is connected into a circuit, electrons can fall off one end of the sheet and be replaced with new ones at the other end. When looking at a compound and trying to determine whether it is an ionic compound or a covalent … water bonds. You have to break the covalent bonding throughout the whole structure. Each bond type differs in the way atom share This page describes the structures of giant covalent substances like diamond, graphite and silicon dioxide (silicon(IV) oxide), and relates those structures to the physical properties of the substances. The octet rule can be satisfied by the sharing of electrons between atoms to form covalent bonds. Eating, putting gas in a car and throwing a log on a campfire all involve adding energy to a system. answer choices . The sp hybrid orbitals of the two carbon atoms overlap end to end to form a σ bond between the carbon atoms (Figure 4). Polarization of Covalent Bonds. That leaves a fourth electron in the bonding level. Most molecules in living things are covalently bonded, for instance. All the electrons are held tightly between the atoms, and aren't free to move. When you use a pencil, sheets are rubbed off and stick to the paper. However, many structures also include resonance forms. Attractions between solvent molecules and carbon atoms will never be strong enough to overcome the strong covalent bonds in graphite. (Figure 2.3.1) illustrates why this bond is formed. The term covalent bond describes the bonds in compounds that result from the sharing of one or more pairs of electrons. Water molecules form which type of bond with other water molecules? ionic bonds. . A. Covalent bonds form from the attraction of positive… Check Your Learning Sulfur: Elemental sulfur forms S 8 rings of atoms. has a high melting point - varying depending on what the particular structure is (remember that the structure given is only one of three possible structures), but around 1700°C. The hydrogen bond is often described as a strong electrostatic dipole–dipole interaction. Bonding in molecules with resonance forms is better described by molecular orbital theory. This page describes the structures of giant covalent substances like diamond, graphite and silicon dioxide (silicon(IV) oxide), and relates those structures to the physical properties of the substances. So what holds the sheets together? Is it also capable of describing molecules containing double and triple bonds? Example, Nonpolar Covalent Bond is found in gas molecules like Hydrogen gas, Nitrogen gas, etc. covalent bonds. The important thing is that the delocalised electrons are free to move anywhere within the sheet - each electron is no longer fixed to a particular carbon atom. A covalent bond, also called a molecular bond[citation needed], is a chemical bond that involves the sharing of electron pairs between atoms. 1.5 Measurement Uncertainty, Accuracy, and Precision, 1.6 Mathematical Treatment of Measurement Results, Chapter 3. If the atoms that form a covalent bond are identical, as in H 2, Cl 2, and other diatomic molecules, then the electrons in the bond must be shared equally.We refer to this as a pure covalent bond.Electrons shared in pure covalent bonds have an equal probability of being near each nucleus. The resonance structures of SO2 are. ions are molecules that have a can charge an ionic bond is many times made between a metallic and a nonmetal (like Na and Cl forming NaCl) and covalent bonds are made between nonmetals. If the atoms that form a covalent bond are identical, as in H 2, Cl 2, and other diatomic molecules, then the electrons in the bond must be shared equally. 60 seconds . These "spare" electrons in each carbon atom become delocalised over the whole of the sheet of atoms in one layer. These orbitals form the C–H single bonds … (Note: the lone electron on nitrogen occupies a hybridized orbital just as a lone pair would.). To the atomic structure and bonding menu . any bond with a hydrogen. (c) Each of the two π bonds is formed by overlap of a 2p orbital on carbon and a nitrogen 2p orbital. Melting phosphorus breaks no covalent bonds; instead, it disrupts the much weaker van der Waals forces between the molecules. Polar Covalent Bonds: Covalent bonds are formed when two atoms each donate one of their valence electrons to form a bond. Therefore, the electron-pair geometry is trigonal planar, and the hybridization of the sulfur atom is sp2. The distance between the layers is about 2.5 times the distance between the atoms within each layer. The other three are ionic bonds, metallic bonds and hydrogen bonds. We refer to this as a pure covalent bond. Covalent network solids have high melting points by virtue of their network of covalent bonds, all of which would have to be broken for them to transform into a liquid. Covalent bonds are much weaker than the ionic bonds and, therefore, most of the covalent compounds exist in the gaseous phase. Homolysis makes two new radicals from a spin-paired molecule by breaking a covalent bond, leaving each of the fragments with one of the electrons in the bond. There is, however, no direct contact between the delocalised electrons in one sheet and those in the neighbouring sheets. In a single bond, one pair of electrons is shared between two atoms. A double bond shares two pairs of electrons; it is stronger than a single bond, but it also creates a less stable molecule because it is more reactive. A well-known example is BF 3: Identify the statement that correctly describes hydrogen bonds. Covalent compounds form from bonds, such as polar bonds from polar molecules. In Chemistry, covalent bonds are formed between two atoms or ions in which the electron pairs are shared between them; they are also known as molecular bonds. The π bond in the C=C double bond results from the overlap of the third (remaining) 2p orbital on each carbon atom that is not involved in hybridization. Solution Advanced Theories of Covalent Bonding, 9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law, 9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions, 10.6 Lattice Structures in Crystalline Solids, Chapter 13. Note that it is not necessary to hybridize the nitrogen atom. For example, the hydrogen molecule, H 2, contains a covalent bond between its two hydrogen atoms. A)both solids contain only ionic bonds B)both solids contain only covalent bonds C)solid A contains only covalent bonds and solid B contains only ionic bonds D)solid A contains only ionic bonds and solid B contains only covalent bonds 2.A chemist performs the same tests on two homogeneous white crystalline solids, A … In graphite you have the ultimate example of van der Waals dispersion forces. To form ionic bonds, Carbon molecules must either gain or lose 4 electrons. This is due to the need to break the very strong covalent bonds. SURVEY . Composition of Substances and Solutions, 3.2 Determining Empirical and Molecular Formulas, 3.4 Other Units for Solution Concentrations, Chapter 4. Pure vs. Polar Covalent Bonds. The two carbon atoms of acetylene are thus bound together by one σ bond and two π bonds, giving a triple bond. Don't forget that this is just a tiny part of a giant structure extending on all 3 dimensions. Waste as defined in Directive 2006/12/EC of the European Parliament and of the Council of 5 April 2006 on waste (2) is not a substance, mixture or article within the meaning of Article 2 of this Regulation.4. In the case of Cl 2, each atom starts off with seven valence electrons, and each Cl shares one … There are no possible attractions which could occur between solvent molecules and carbon atoms which could outweigh the attractions between the covalently bound carbon atoms. Example: Water decomposes into a mixture of hydrogen and oxygen when an electric current is passed through the liquid. Electrons shared in pure covalent bonds have an equal probability of being near each nucleus. your answer o n … One substance mentioned in Chapter 3 "Ionic Bonding and Simple Ionic Compounds" was water (H 2 O). Non-polar Covalent Compounds. has a high melting point, similar to that of diamond. The diagram below shows the arrangement of the atoms in each layer, and the way the layers are spaced. Don't try to be too clever by trying to draw too much of the structure! Which of the following elements is most likely to form covalent bonds? attraction between a slightly positive atom of one molecule and a … They are no longer associated directly with any particular atom or pair of atoms, but are free to wander throughout the whole sheet. Capping off an era marred by drug development failures and punctuated by waning interest and presumed intractability toward direct targeting of KRAS, new technologies and strategies are aiding in the target’s resurgence. In that case, it is important to give some idea of the distances involved. In practice, a real piece of graphite isn't a perfect crystal, but a host of small crystals stuck together at all sorts of angles. Valence and covalent bonds link together atoms to make molecules. Notice that each silicon atom is bridged to its neighbours by an oxygen atom. A non-polar covalent bond can occur between two identical non-metal atoms or between different atoms. The two electrons involved in the bond … Covalent bonds are also found in inorganic molecules such as H 2 … Any substance that contains only one kind of an atom is known as an element.Because atoms cannot be created or destroyed in a chemical reaction, elements such as phosphorus (P 4) or sulfur (S 8) cannot be broken down into simpler substances by these reactions.. Representative Metals, Metalloids, and Nonmetals, 18.2 Occurrence and Preparation of the Representative Metals, 18.3 Structure and General Properties of the Metalloids, 18.4 Structure and General Properties of the Nonmetals, 18.5 Occurrence, Preparation, and Compounds of Hydrogen, 18.6 Occurrence, Preparation, and Properties of Carbonates, 18.7 Occurrence, Preparation, and Properties of Nitrogen, 18.8 Occurrence, Preparation, and Properties of Phosphorus, 18.9 Occurrence, Preparation, and Compounds of Oxygen, 18.10 Occurrence, Preparation, and Properties of Sulfur, 18.11 Occurrence, Preparation, and Properties of Halogens, 18.12 Occurrence, Preparation, and Properties of the Noble Gases, Chapter 19. doesn't conduct electricity. Pure vs. Polar Covalent Bonds. We refer to this as a pure covalent bond. has a lower density than diamond. Double and triple bonds offer added stability to compounds, and … 3.15 (b), (d) and (e) are molecular substances. The most common examples are the covalent compounds of beryllium and boron. The three bonding regions form a trigonal planar electron-pair geometry. This unhybridized p orbital (lobes shown in red and blue in Figure 2) is perpendicular to the plane of the sp2 hybrid orbitals. Carbon has an electronic arrangement of 2,4. Starting on the far right, we have two separate hydrogen atoms with a particular potential energy, indicated by the red line. Thus we expect the σ bonds from each carbon atom are formed using a set of sp 2 hybrid orbitals that result from hybridization of two of the 2p orbitals and the 2s orbital . Each carbon atom uses three of its electrons to form simple bonds to its three close neighbours. (a) sp2; (b) sp; (c) sp2; (d) sp3; (e) sp3; (f) sp3d; (g) sp3, 7. Covalent compounds in which there is no electronegativity difference are known as non-polar covalent compounds. Valence bond theory does not easily address delocalization. In general ionic bonds occur between elements that are far apart on the periodic … Chapter 3 "Ionic Bonding and Simple Ionic Compounds" discussed ionic bonding, which results from the transfer of electrons among atoms or groups of atoms. Covalent compounds are a diverse group of molecules, so there are several exceptions to each 'rule'. As the delocalised electrons move around in the sheet, very large temporary dipoles can be set up which will induce opposite dipoles in the sheets above and below - and so on throughout the whole graphite crystal. The forces of attraction or repulsion between two atoms (when they share an electron pair or bonding pair) are called Covalent Bonding. Covalent Compounds: Covalent compound is the chemical compound which contains covalent bond in between their constituent's elements. The tendency of main group atoms to form enough bonds to obtain eight valence electrons is known as the The physical properties of silicon dioxide. In molecules with sp hybrid orbitals, two unhybridized p orbitals remain on the atom (Figure 3). Do it in the following stages: Practise until you can do a reasonable free-hand sketch in about 30 seconds. You might argue that carbon has to form 4 bonds because of its 4 unpaired electrons, whereas in this diagram it only seems to be forming 3 bonds to the neighbouring carbons. By the end of this section, you will be able to: The hybrid orbital model appears to account well for the geometry of molecules involving single covalent bonds. (a) sp2, delocalized; (b) sp, localized; (c) sp2, delocalized; (d) sp3, delocalized. (a) H3PO4, phosphoric acid, used in cola soft drinks, (b) NH4NO3, ammonium nitrate, a fertilizer and explosive, (c) S2Cl2, disulfur dichloride, used in vulcanizing rubber, (d) K4[O3POPO3], potassium pyrophosphate, an ingredient in some toothpastes, (b) carbon dioxide (CO2) central C hybridization, (c) nitrogen dioxide (NO2) central N hybridization, (d) phosphate ion (PO43−) central P hybridization, Answers to Chemistry End of Chapter Exercises. Next we can consider how we visualize these components and how they relate to hybrid orbitals. This is a significant difference between σ and π bonds; rotation around single (σ) bonds occurs easily because the end-to-end orbital overlap does not depend on the relative orientation of the orbitals on each atom in the bond. This is often the result of a stronger electronegative atom drawing the electrons closer than a weaker … You can think of graphite rather like a pack of cards - each card is strong, but the cards will slide over each other, or even fall off the pack altogether. 3. Chemical Bonding and Molecular Geometry, 7.5 Strengths of Ionic and Covalent Bonds, Chapter 8. The sulfur atom is surrounded by two bonds and one lone pair of electrons in either resonance structure. Stoichiometry of Chemical Reactions, 4.1 Writing and Balancing Chemical Equations, Chapter 6. Ion-dipole bonds (ionic species to covalent molecules) are formed between ions and polar molecules. This is because of the relatively large amount of space that is "wasted" between the sheets. Learn to draw the diagram given above. We are only showing a small bit of the whole structure. This is a giant covalent structure - it continues on and on in three dimensions. If the two planes of sp2 hybrid orbitals tilted relative to each other, the p orbitals would not be oriented to overlap efficiently to create the π bond. Tags: Question 29 . Covalent or molecular compounds contain atoms held together by covalent bonds. In the diagram some carbon atoms only seem to be forming two bonds (or even one bond), but that's not really the case. The third way of obtaining this (apart from giving away and accepting electrons as mentioned in the case of the ionic bonds) is … These orbitals form the C–H single bonds and the σ bond in the C=C double bond (Figure 2). This diagram is something of a simplification, and shows the arrangement of atoms rather than the bonding. (b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds. Carbon cannot gain or donate electrons, so to complete its nearest noble gas configuration, it shares electron to form a covalent bond. Please remember that this … In order to melt graphite, it isn't enough to loosen one sheet from another. Formation of Covalent Bonds. Hint: they all form single covalent bonds) Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds. If the atoms that form a covalent bond are identical, as in H 2, Cl 2, and other diatomic molecules, then the electrons in the bond must be shared equally. answer choices . In an ethene molecule, the four hydrogen atoms and the two carbon atoms are all in the same plane. Each of the four electrons is in a separate orbital and overlaps with an electron on an oxygen atom. 13) Oxygen, nitrogen, and fluorine bond with hydrogen to form molecules. In other words, rotation around the internuclear axis does not change the extent to which the σ bonding orbitals overlap because the bonding electron density is symmetric about the axis. Play this game to review Chemical Bonds. Transition Metals and Coordination Chemistry, 19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds, 19.2 Coordination Chemistry of Transition Metals, 19.3 Spectroscopic and Magnetic Properties of Coordination Compounds, 20.3 Aldehydes, Ketones, Carboxylic Acids, and Esters, Appendix D: Fundamental Physical Constants, Appendix F: Composition of Commercial Acids and Bases, Appendix G: Standard Thermodynamic Properties for Selected Substances, Appendix H: Ionization Constants of Weak Acids, Appendix I: Ionization Constants of Weak Bases, Appendix K: Formation Constants for Complex Ions, Appendix L: Standard Electrode (Half-Cell) Potentials, Appendix M: Half-Lives for Several Radioactive Isotopes. Some elements are unlikely to lose or gain electrons, but share electrons to form covalent bonds. Sulfur dioxide, SO2, is a major component of volcanic gases as well as a product of the combustion of sulfur-containing coal. Covalent bonding extends throughout a lattice giving the material exceptional strength. All the electrons are held tightly between the atoms, and aren't free to move. The layers, of course, extend over huge numbers of atoms - not just the few shown above. Since the arrangement of π bonds involves only the unhybridized orbitals, resonance does not influence the assignment of hybridization. To turn it into silicon dioxide, all you need to do is to modify the silicon structure by including some oxygen atoms. Structures that account for these features describe the correct hybridization of the atoms. You have already seen examples of substances that contain covalent bonds. If this is the first set of questions you have done, please read the introductory page before you start. (a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule. The remaining sp orbitals form σ bonds with hydrogen atoms. A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms.These electron pairs are known as shared pairs or bonding pairs, and the stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding. An unsaturated fatty acid occurs when a double covalent bond replaces a single covalent bond and two hydrogen atoms (Figure 2). Some acid rain results from the reaction of sulfur dioxide with atmospheric water vapor, followed by the formation of sulfuric acid. Remember that resonance forms occur when various arrangements of π bonds are possible. 1.Which statement describes a multiple covalent bond? Solution for Which statement describes the difference between covalent bonds and Van der Waals forces? For many molecules, the sharing of electrons allows each atom to attain the … is very hard. is insoluble in water and organic solvents. It is not a molecule, because the number of atoms joined up in a real diamond is completely variable - depending on the size of the crystal. We have already discussed that multiple bonds consist of σ and π bonds. Nonmetal atoms frequently form covalent bonds with other nonmetal atoms. There aren't any delocalised electrons. Electrons will be able to find a route through the large piece of graphite in all directions by moving from one small crystal to the next. A triple bond consists of one σ bond and two π bonds. Indeed, covalent network solids are among the highest-melting substances known: the melting point of diamond is over 3,500°C, while the melting point of SiO 2 is around 1,650°C. This is again due to the need to break very strong covalent bonds operating in 3-dimensions. Electronic Structure and Periodic Properties of Elements, 6.4 Electronic Structure of Atoms (Electron Configurations), 6.5 Periodic Variations in Element Properties, Chapter 7. The sharing of electrons can be done in … Covalent bonds … (b) The terminal carbon atom uses sp3 hybrid orbitals, while the central carbon atom is sp hybridized. The Lewis structure of ethene, C2H4, shows us that each carbon atom is surrounded by one other carbon atom and two hydrogen atoms. There are three different crystal forms of silicon dioxide. For example: carbon does not form ionic bonds because it has 4 valence electrons, half of an octet. It is observed that in the sigma bonds between two different atoms, the electron cloud is always closer to the … A hydrogen bond is the attraction between the lone pair of an electronegative atom and a hydrogen atom that is bonded to an electronegative atom, usually nitrogen, oxygen, or fluorine. Polar bonds usually consist of different atoms unequally sharing electrons. Notice that you can't really draw the side view of the layers to the same scale as the atoms in the layer without one or other part of the diagram being either very spread out or very squashed. The delocalised electrons are free to move throughout the sheets. Graphite has a layer structure which is quite difficult to draw convincingly in three dimensions. There are five kinds of intermolecular forces described below; the bond strengths described range from strongest to weakest (the latter 3 are examples of van der Waals forces). Up to three covalent bonds can form at one time in a molecule. Thus the unhybridized 2p orbitals overlap in a side-by-side fashion, above and below the internuclear axis (Figure 2) and form a π bond. See answer freemankellie freemankellie Answer:they usually occur between nonmetals. H-bonds can from between an H on a(n) F, O, or N on one molecule, and a partially negative F, O, or N on another molecule. The triple bond shares three pairs of electrons, making it the least stable covalent bond. conducts electricity. Another acid in acid rain is nitric acid, HNO3, which is produced by the reaction of nitrogen dioxide, NO2, with atmospheric water vapor. In each case, the energy is added in the form of covalent bonds that hold atoms together in molecules. The electrons in the unhybridized p orbitals form π bonds. This allows each halogen atom to have a noble gas electron configuration. Double and triple covalent bonds are stronger than single covalent bonds and they are characterized by the sharing of four or six electrons between atoms, respectively. Ionic bonds, where electrons transfer between atoms, occur when atoms with just a few electrons in their outer shell give the electrons to atoms with just a few missing from their outer shell. We refer to this as a pure covalent bond. © Jim Clark 2000 (modified September 2019). They are not located in one position or the other, but in reality are delocalized throughout the ring. Which substances form covalent bonds? Fundamental Equilibrium Concepts, 13.3 Shifting Equilibria: Le Châtelier’s Principle, 14.3 Relative Strengths of Acids and Bases, Chapter 15. is hard. Creative Commons Attribution 4.0 International License, Describe multiple covalent bonding in terms of atomic orbital overlap, Relate the concept of resonance to π-bonding and electron delocalization, The bond energy of a C–C single bond averages 347 kJ mol, A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H. Identify the hybridization of the central atom in each of the following molecules and ions that contain multiple bonds: Describe the molecular geometry and hybridization of the N, P, or S atoms in each of the following compounds.
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