ParticleLewis DotAByXz formulaMolecular Shapesulfur trioxide
SO3
carbon tetrachloride
CCl4
phosphate ion
arsenic trichloride
AsCl3
ammonium ion
oxygen difluoride
OF2
phosphorus pentachloride
PCl5
hydrogen selenide
H2Se
nitrogen triiodide
NI3
WKS 6.6 VSEPR Shapes of Molecules (continued)
ParticleLewis DotAByXz formulaMolecular Shapesulfate ion
bromate ion
sulfur dichloride
SCl2
selenium hexafluoride
SeF6
arsenic pentabromide
AsBr5
boron trichloride
BCl3
water
carbonate ion
nitrate ion
WKS 6.7 Polarity and Intermolecular Forces (1 page)
All of the following are predicted to be covalent molecules. Ionic Compound Properties. 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"source@https://openstax.org/details/books/chemistry-2e" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FChemistry_1e_(OpenSTAX)%2F07%253A_Chemical_Bonding_and_Molecular_Geometry%2F7.5%253A_Strengths_of_Ionic_and_Covalent_Bonds, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Using Bond Energies to Approximate Enthalpy Changes, Example \(\PageIndex{1}\): Using Bond Energies to Approximate Enthalpy Changes, Example \(\PageIndex{2}\): Lattice Energy Comparisons, source@https://openstax.org/details/books/chemistry-2e, status page at https://status.libretexts.org, \(\ce{Cs}(s)\ce{Cs}(g)\hspace{20px}H=H^\circ_s=\mathrm{77\:kJ/mol}\), \(\dfrac{1}{2}\ce{F2}(g)\ce{F}(g)\hspace{20px}H=\dfrac{1}{2}D=\mathrm{79\:kJ/mol}\), \(\ce{Cs}(g)\ce{Cs+}(g)+\ce{e-}\hspace{20px}H=IE=\ce{376\:kJ/mol}\), \(\ce{F}(g)+\ce{e-}\ce{F-}(g)\hspace{20px}H=EA=\ce{-328\:kJ/mol}\), \(\ce{Cs+}(g)+\ce{F-}(g)\ce{CsF}(s)\hspace{20px}H=H_\ce{lattice}=\:?\), Describe the energetics of covalent and ionic bond formation and breakage, Use the Born-Haber cycle to compute lattice energies for ionic compounds, Use average covalent bond energies to estimate enthalpies of reaction. Study with Quizlet and memorize flashcards containing terms like Is the following sentence true or false? Ionic bonds are caused by electrons transferring from one atom to another. The name of an ionic compound must distinguish the compound from other ionic compounds containing the same elements., What information is provided by the formula for an ionic compound?, Circle the letter of the word that describes a compound made from only two elements. Now that you've learned about the structure of an atom and the properties of electrons, we have to discuss how to draw molecules! The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. What is an ionic bond? is associated with the stability of the noble gases. Nomenclature of Ionic Compounds Ionic compounds are composed of ions. When. Using the bond energy values in Table \(\PageIndex{2}\), we obtain: \[\begin {align*} From the answers we derive, we place the compound in an appropriate category and then name it accordingly. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The total energy involved in this conversion is equal to the experimentally determined enthalpy of formation, \(H^\circ_\ce f\), of the compound from its elements. Most of the transition metals can form two or more cations with different charges. The energy required to break these bonds is the sum of the bond energy of the HH bond (436 kJ/mol) and the ClCl bond (243 kJ/mol). These lewis dot structures get slightly more complex in the next key topic, but practice makes perfect! ALSO - there may be more than one!!! The enthalpy change in this step is the negative of the lattice energy, so it is also an exothermic quantity. (1 page)
Draw the Lewis structure for each of the following. Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. Stable molecules exist because covalent bonds hold the atoms together. Although the four CH bonds are equivalent in the original molecule, they do not each require the same energy to break; once the first bond is broken (which requires 439 kJ/mol), the remaining bonds are easier to break. Instead you must learn some and work out others.
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