ions. The name of a binary compound containing monatomic ions consists of the name of the cation (the name of the metal) followed by the name of the anion (the name of the nonmetallic element with its ending replaced by the suffix ide). It also defines polyatomic ion and gives the, Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion, Naming Ionic Compounds Answer Key Give the name of the following ionic compounds: Name 1) Na 2 CO 3 sodium carbonate 2) NaOH sodium hydroxide 3) MgBr 2 magnesium bromide 4) KCl potassium chloride 5) FeCl. \(H=H^\circ_f=H^\circ_s+\dfrac{1}{2}D+IE+(EA)+(H_\ce{lattice})\), \(\ce{Cs}(s)+\dfrac{1}{2}\ce{F2}(g)\ce{CsF}(s)=\ce{-554\:kJ/mol}\). WKS 6.3 - LDS for Ionic Compounds (2 pages) Fill in the chart below. 2023 Fiveable Inc. All rights reserved. Predict the common oxidation numbers (CHARGE) for each of the following elements when they form. Circle your answers: C, Na, F, Cs, Ba, Ni Which metal in the list above has the most metallic character? Y o u w i l l n e e d t o d e t e r m i n e h o w m a n y o f e a c h i o n y o u w i l l n e e d t o f o r m a n e u t r a l f o r m u l a u n i t ( c o m p o u n d )
C a t i o n L D S A n i o n L D S A l g e b r a f o r n e u t r a l c o m p o u n d I O N I C C O M P O U N D L D S
N a + C l
N a " ( [ N a ] +
C l ( [ C l ] % ( + 1 ) + ( - 1 ) = 0
[ N a ] + [ C l ] % K + F
M g + I
B e + S
N a + O
G a + S
R b + N
W K S 6 . Ionic compounds form when atoms connect to one another by ionic bonds. 3.5: Ionic Compounds- Formulas and Names is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. For example, if the relevant enthalpy of sublimation \(H^\circ_s\), ionization energy (IE), bond dissociation enthalpy (D), lattice energy Hlattice, and standard enthalpy of formation \(H^\circ_\ce f\) are known, the Born-Haber cycle can be used to determine the electron affinity of an atom. The energy required to break a specific covalent bond in one mole of gaseous molecules is called the bond energy or the bond dissociation energy. Particles with a positive or negative charge are called ions. Lewis diagrams are used to predict the shape of a molecule and the types of chemical reactions it can undergo. The charge of the metal ion is determined from the formula of the compound and the charge of the anion. You will need to determine how many of each ion you will need to form a neutral formula unit (compound) Cation LDS Anion LDS Algebra for neutral compound IONIC COMPOUND LDS Na + Cl Na ( [Na]+ Cl ( [ Cl ] (+1) + (-1) = 0 [Na]+ [ Cl ] K + F Mg + I Be + S Na + O In electron transfer, the number of electrons lost must equal the number of electrons gained. A good example is the ammonium ion made up of one nitrogen atom and four hydrogen atoms. Ion Definition in Chemistry. 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). Matter tends to exist in its ______________________________ energy state. Ionic compounds include salts, oxides, hydroxides, sulphides, and the majority of inorganic compounds. Hydrogen can have a maximum of two valence electrons, beryllium can have a maximum of four valence electrons, and boron can have a maximum of six valence electrons. When one mole each of gaseous Na+ and Cl ions form solid NaCl, 769 kJ of heat is released. \end {align*} \nonumber \]. Keep in mind, however, that these are not directly comparable values. However, the lattice energy can be calculated using the equation given in the previous section or by using a thermochemical cycle. Lattice energy increases for ions with higher charges and shorter distances between ions. Don't confuse the term "coefficient" with "subscript" or "superscript.". IDENTIFY each first as being a simple ion, polyatomic ion, ionic compound (with or without a polyatomic ion), or covalent compound. 7. Because opposite charges attract (while like charges repel), cations and anions attract each other, forming ionic bonds. \end {align*} \nonumber \]. Ionic bonds are caused by electrons transferring from one atom to another. Here are some examples of the first two bullets: Let's go over some relatively straightforward compounds first! 2 0 obj
Chapter 6.3 : Ionic Bonding and Ionic Compounds 1. Periodic table 1. WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. Table T2 gives a value for the standard molar enthalpy of formation of HCl(g), \(H^\circ_\ce f\), of 92.307 kJ/mol. Describe ionic and covalent bonding.. 4. A(n) __________________________ bond is a bond in which one atom donates electrons to another atom. Bonding pairs: pairs of electrons found in the shared space between atoms (often represented by a dash), Ionic Lewis dot structures are very easy to draw out since ionic bonds form due to a transfer of electrons!. Legal. Ionic compounds are solids that typically melt at high temperatures and boil at even higher temperatures. H&= \sum \mathrm{D_{bonds\: broken}} \sum \mathrm{D_{bonds\: formed}}\\[4pt] The enthalpy change, H, for a chemical reaction is approximately equal to the sum of the energy required to break all bonds in the reactants (energy in, positive sign) plus the energy released when all bonds are formed in the products (energy out, negative sign). Thus, FeCl2 is iron(II) chloride and FeCl3 is iron(III) chloride. 3 0 obj
3) Model covalent, Decomposition 1. For example, the bond energy of the pure covalent HH bond, \(\Delta_{HH}\), is 436 kJ per mole of HH bonds broken: \[H_{2(g)}2H_{(g)} \;\;\; D_{HH}=H=436kJ \label{EQ2} \]. The periodic table can help us recognize many of the compounds that are ionic: When a metal is combined with one or more nonmetals, the compound is usually ionic. 7: Chemical Bonding and Molecular Geometry, { "7.0:_Prelude_to_Chemical_Bonding_and_Molecular_Geometry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.1:_Ionic_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.2:_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.3:_Lewis_Symbols_and_Structures" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.4:_Formal_Charges_and_Resonance" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.5:_Strengths_of_Ionic_and_Covalent_Bonds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.6:_Molecular_Structure_and_Polarity" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7.E:_Chemical_Bonding_and_Molecular_Geometry_(Exercises)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Essential_Ideas" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_Molecules_and_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Composition_of_Substances_and_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Stoichiometry_of_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Electronic_Structure_and_Periodic_Properties_of_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Chemical_Bonding_and_Molecular_Geometry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Advanced_Theories_of_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Liquids_and_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Solutions_and_Colloids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Fundamental_Equilibrium_Concepts" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Acid-Base_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Equilibria_of_Other_Reaction_Classes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Representative_Metals_Metalloids_and_Nonmetals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Transition_Metals_and_Coordination_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Organic_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_Nuclear_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Appendices : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 7.5: Strengths of Ionic and Covalent Bonds, [ "article:topic", "Author tag:OpenStax", "bond energy", "Born-Haber cycle", "Lattice Energy", "authorname:openstax", "showtoc:no", "license:ccby", "autonumheader:yes2", "licenseversion:40", "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.
Worklife Boeing From Home,
Articles L
