Ionic compounds are solids that typically melt at high temperatures and boil at even higher temperatures. Look at the empirical formula and count the number of valence electrons there should be total. Examples include SF6, sulfur hexafluoride, and N2O4, dinitrogen tetroxide. WKS 6.5 - LDS for All Kinds of Compounds! Matter tends to exist in its ______________________________ energy state. \end {align*} \nonumber \]. IDENTIFY each first as being a simple ion, polyatomic ion, ionic compound (with or without a polyatomic ion), or covalent compound. We can express this as follows (via Equation \ref{EQ3}): \[\begin {align*} Since there are only two oxygen atoms, we could just draw them side by side (there is technically no central atom here). Covalent bonds are a little more difficult to draw out because the electrons are shared. We will limit our attention here to inorganic compounds, compounds that are composed principally of elements other than carbon, and will follow the nomenclature guidelines proposed by IUPAC. The Molecular Formula for Water. For example, we can compare the lattice energy of MgF2 (2957 kJ/mol) to that of MgI2 (2327 kJ/mol) to observe the effect on lattice energy of the smaller ionic size of F as compared to I. Draw full octets on each atom. Unit 1: Lesson 3. Lewis diagrams, or Lewis structures, are a way of drawing molecular structures and showing the present valence electrons and bonds. This excess energy is released as heat, so the reaction is exothermic. Aluminum ion
Silicon ionPotassium ionFluoride ion
Sulfide ionCarbide ionHydrogen ion
Cesium ionBromide ionChloride ion
Gallium ionZinc ionSilver ion
Oxide ion
Barium ion
Predict the common oxidation numbers (CHARGE) for each of the following elements when they form ions. If the compound is ionic, does the metal form ions of only one type (fixed charge) or more than one type (variable charge)? Solid ammonium carbonate is heated. Out-of-date nomenclature used the suffixes ic and ous to designate metals with higher and lower charges, respectively: Iron(III) chloride, FeCl3, was previously called ferric chloride, and iron(II) chloride, FeCl2, was known as ferrous chloride. When. You can see a. Since Xe has an atomic number of 54, which is much greater than 14, we can break the octet rule and add the necessary number of electrons to Xe. Na + sodium ion, K + potassium ion, Al 3+ aluminum, Noble gases Period alogens Alkaline earth metals Alkali metals TRENDS IN TE PERIDI TABLE Usual charge +1 + +3-3 - -1 Number of Valence e - s 1 3 4 5 6 7 Electron dot diagram X X X X X X X X X 8 Group 1, Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. For example, you may see the words stannous fluoride on a tube of toothpaste. If there is a prefix, then the prefix indicates how many of that element is in the compound. Molecular compounds can form compounds with different ratios of their elements, so prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. cyanide ion
bromide ionsulfur dioxide
SO2
ammonium phosphate
sulfur hexafluoride
SF6
bromine pentachloride
BrCl5chlorate ion
carbon monoxide
CO carbonate ion chlorine tribromide
ClBr3
WKS 6.6 VSEPR Shapes of Molecules (2 pages)
Predict the AByXz and molecular shape of each of the following. Draw the central atom (in most cases it is carbon or the atom that is not hydrogen). Hence, the ionic compound potassium chloride with the formula KCl is formed. Most of the transition metals can form two or more cations with different charges. First, we need to write the Lewis structures of the reactants and the products: From this, we see that H for this reaction involves the energy required to break a CO triple bond and two HH single bonds, as well as the energy produced by the formation of three CH single bonds, a CO single bond, and an OH single bond. Binary acids are named using the prefix hydro-, changing the ide suffix to ic, and adding acid; HCl is hydrochloric acid. &=\mathrm{[D_{HH}+D_{ClCl}]2D_{HCl}}\\[4pt] 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. Transfer valence electrons to the nonmetal (could be done mentally as well). Some atoms have fewer electrons than a full octet of 8. Course Hero is not sponsored or endorsed by any college or university. 3: Molecules, Compounds and Chemical Equations, { "3.01:_Hydrogen_Oxygen_and_Water" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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H&= \sum \mathrm{D_{bonds\: broken}} \sum \mathrm{D_{bonds\: formed}}\\[4pt] The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. Most atoms have 8 electrons when most stable. ZnO would have the larger lattice energy because the Z values of both the cation and the anion in ZnO are greater, and the interionic distance of ZnO is smaller than that of NaCl. Converting one mole of fluorine atoms into fluoride ions is an exothermic process, so this step gives off energy (the electron affinity) and is shown as decreasing along the y-axis. Stability is achieved for both atoms once the transfer of electrons has occurred. Thus, in calculating enthalpies in this manner, it is important that we consider the bonding in all reactants and products. Now to check our work, we can count the number of valence electrons. 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.