{"id":2798,"date":"2016-08-24T18:31:54","date_gmt":"2016-08-24T18:31:54","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2798"},"modified":"2017-08-28T22:55:39","modified_gmt":"2017-08-28T22:55:39","slug":"coordination-numbers","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/coordination-numbers\/","title":{"raw":"Physical Properties of Ionic Compounds","rendered":"Physical Properties of Ionic Compounds"},"content":{"raw":"<h1 id=\"x-ck12-SW9uaWMgYW5kIE1ldGFsbGljIEJvbmRpbmc.-chapter\">Ionic and Metallic Bonding<\/h1>\r\n<div class=\"x-ck12-data\"><\/div>\r\n<h1 id=\"x-ck12-RWxlY3Ryb24gRG90IERpYWdyYW1z\">Physical Properties of Ionic Compounds<\/h1>\r\n<div class=\"x-ck12-data-objectives\">\r\n<ul id=\"x-ck12-Zjk3YmU0MmVkYzM3MGE5ODg4Y2NmYjZhZDVlZDk5ZDc.-vk0\">\r\n \t<li>List and describe the physical properties of ionic compounds.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div id=\"x-ck12-ZGI1MjgxOGE5MjUzMjJmYjJhOTZkNjFlZDkxOWQ0Yjk.-tx1\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n<p id=\"x-ck12-lkv\"><img id=\"x-ck12-OTgwNDUtMTM2MjAwOTkwMC0zNy02NC1JbnRDaC0wOC0wNy1Db2xvcmZ1bC1pb25pYy1jb21wb3VuZHM.\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211408\/20140811155233093570.png\" alt=\"Pictures of amethyst, cinnabar, azurite, and vanadinite\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/In%20nature%2C%20the%20ordered%20arrangement%20of%20ionic%20solids%20gives%20rise%20to%20beautiful%20crystals.%20(A)%20Amethyst%20%E2%80%93%20a%20form%20of%20quartz%2C%20SiO%3Csub%3E2%3C%2Fsub%3E%2C%20whose%20purple%20color%20comes%20from%20iron%20ions.%20(B)%20Cinnabar%20%E2%80%93%20the%20primary%20ore%20of%20mercury%20is%20mercury(II)%20sulfide%2C%20HgS.%20(C)%20Azurite%20%E2%80%93%20a%20copper%20mineral%2C%20Cu%3Csub%3E3%3C%2Fsub%3E(CO%3Csub%3E3%3C%2Fsub%3E)%3Csub%3E2%3C%2Fsub%3E(OH)%3Csub%3E2%3C%2Fsub%3E.%20D)%20Vanadinite%20%E2%80%93%20the%20primary%20ore%20of%20vanadium%2C%20Pb%3Csub%3E5%3C%2Fsub%3E(VO%3Csub%3E4%3C%2Fsub%3E)%3Csub%3E3%3C%2Fsub%3ECl.\" \/><\/p>\r\n<strong>Figure 8.12<\/strong>\r\n<p id=\"x-ck12-YjVlMzMxZjFjY2FmYzg4OTBhOTUzOTVhZDM2MDkwM2I.-6hi\">In nature, the ordered arrangement of ionic solids gives rise to beautiful crystals. (A) Amethyst \u2013 a form of quartz, SiO <sub>2 <\/sub>, whose purple color comes from iron ions. (B) Cinnabar \u2013 the primary ore of mercury is mercury(II) sulfide, HgS. (C) Azurite \u2013 a copper mineral, Cu <sub>3 <\/sub>(CO <sub>3 <\/sub>) <sub>2 <\/sub>(OH) <sub>2 <\/sub>. D) Vanadinite \u2013 the primary ore of vanadium, Pb <sub>5 <\/sub>(VO <sub>4 <\/sub>) <sub>3 <\/sub>Cl.<\/p>\r\n\r\n<\/div>\r\n<p id=\"x-ck12-NDlhNGJlMDAyNDRiNDAwZWNjMzg4YjYzNjY2MzQ4YTM.-npp\"><strong>What produces colored crystals?<\/strong><\/p>\r\n<p id=\"x-ck12-NzliZTVjYmRhZTc2OWQ4YTZhYTFkODdlOGE0NmQ2MTg.-39f\">The figure above shows just a few examples of the color and brilliance of naturally occurring ionic crystals. The regular and orderly arrangement of ions in the crystal lattice is responsible for the various shapes of these crystals, while transition metal ions give rise to the colors.<\/p>\r\n\r\n<h3>Physical Properties of Ionic Compounds<\/h3>\r\n<h4>Melting Points<\/h4>\r\n<p id=\"x-ck12-YjNlZWNmNDk5NjNjMWIzNjMwZTE4ZTNhNGRkZDU0MDM.-8te\">Because of the many simultaneous attractions between cations and anions that occur, ionic crystal lattices are very strong.\u00a0 The process of melting an ionic compound requires the addition of large amounts of energy in order to break all of the ionic bonds in the crystal.\u00a0 For example, sodium chloride has a melting temperature of about 800\u00b0C.<\/p>\r\n\r\n<h4>Shattering<\/h4>\r\n<p id=\"x-ck12-YjVhNTUwMTViZjYwM2YzNGIwMmQ1YTJlZjc5NTMzNmQ.-vcj\">Ionic compounds are generally hard, but <strong>brittle.\u00a0 <\/strong>Why?\u00a0 It takes a large amount of mechanical force, such as striking a crystal with a hammer, to force one layer of ions to shift relative to its neighbor.\u00a0 However, when that happens, it brings ions of the same charge next to each other (see <strong>Figure <\/strong>below ).\u00a0 The repulsive forces between like-charged ions cause the crystal to shatter.\u00a0 When an ionic crystal breaks, it tends to do so along smooth planes because of the regular arrangement of the ions.<\/p>\r\n\r\n<div id=\"x-ck12-MDE3MDkxNGUxNDAxZDBhMjY5NGI0YzYzMWRkODM4MzU.-dkn\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n<p id=\"x-ck12-tfw\"><img id=\"x-ck12-OTgwNDUtMTM2MjAxMDE1MC00OS0xMDAtSW50Q2gtMDgtMDgtTmFDbC1TaGF0dGVy\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211410\/20140811155233259022.png\" alt=\"Diagram of a shattering sodium chloride crystal\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/%28A%29%20The%20sodium%20chloride%20crystal%20is%20shown%20in%20two%20dimensions.%20%28B%29%20When%20struck%20by%20a%20hammer%2C%20the%20negatively-charged%20chloride%20ions%20are%20forced%20near%20each%20other%20and%20the%20repulsive%20force%20causes%20the%20crystal%20to%20shatter.\" \/><\/p>\r\n<strong>Figure 8.13<\/strong>\r\n<p id=\"x-ck12-NmFjNDYyNjYzZTc4MjdkN2UzOTdiNmI5YWY3ODBhZTQ.-use\">(A) The sodium chloride crystal is shown in two dimensions. (B) When struck by a hammer, the negatively-charged chloride ions are forced near each other and the repulsive force causes the crystal to shatter.<\/p>\r\n\r\n<\/div>\r\n<h4>Conductivity<\/h4>\r\n<p id=\"x-ck12-ZTM1MzM2Y2E2M2U1ZjkzZmExMDc2MDkwZWVlMThhYmQ.-asq\">Another characteristic property of ionic compounds is their <strong>electrical conductivity.\u00a0 <\/strong>The figure below shows three experiments in which two electrodes that are connected to a light bulb are placed in beakers containing three different substances.<\/p>\r\n\r\n<div id=\"x-ck12-Y2YzOTYyZmFiYzYwMDU0MzJkNjZjNmRlYTFlNDhlOTk.-mob\" class=\"x-ck12-img-fullpage x-ck12-nofloat\">\r\n\r\n<img id=\"x-ck12-OTgwNDUtMTM2MjAxMDMwMi00Mi00My1JbnRDaC0wOC0wOS1Db25kdWN0aXZpdHk.\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211411\/20140811155233388212.png\" alt=\"Electrical conductivity of pure water, a solid ionic compound, and an ionic solution\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/%28A%29%20Distilled%20water%20does%20not%20conduct%20electricity.%20%28B%29%20A%20solid%20ionic%20compound%20also%20does%20not%20conduct.%20%28C%29%20A%20water%20solution%20of%20an%20ionic%20compound%20conducts%20electricity%20well.\" \/>\r\n\r\n<strong>Figure 8.14<\/strong>\r\n<p id=\"x-ck12-NTBlMjA2NmI0ZDExM2RmY2Y4ZmNmNWIzZjMwZjZhOTc.-jxs\">(A) Distilled water does not conduct electricity. (B) A solid ionic compound also does not conduct. (C) A water solution of an ionic compound conducts electricity well.<\/p>\r\n\r\n<\/div>\r\n<p id=\"x-ck12-ZjU5NDU3MzU0YjA5YTBkNjhhM2EwYTAzN2Y4NTRhZTA.-vgy\">In the first beaker, distilled water does not conduct a current because water is a molecular compound.\u00a0 In the second beaker, solid sodium chloride also does not conduct a current.\u00a0 Despite being ionic and thus composed of charges particles, the solid crystal lattice does not allow the ions to move between the electrodes.\u00a0 Mobile charged particles are required for the circuit to be complete and the light bulb to light up.\u00a0 In the third beaker, the NaCl has been dissolved into the distilled water.\u00a0 Now the crystal lattice has been broken apart and the individual positive and negative ions can move.\u00a0 Cations move to one electrode, while anions move to the other, allowing electricity to flow (see <strong>Figure <\/strong>below ).\u00a0 Melting an ionic compound also frees the ions to conduct a current.\u00a0 Ionic compounds conduct an electric current when melted or dissolved in water.<\/p>\r\n\r\n<div id=\"x-ck12-NzNhOTM1ODVlYjNhNmQ0MDkzMDljYWFiNGI2NjMwOGE.-8ot\" class=\"x-ck12-img-thumbnail x-ck12-nofloat\">\r\n<p id=\"x-ck12-mfl\"><img id=\"x-ck12-OTgwNDUtMTM2MjAxMDQ2MS0xNC05NC1DaGVtSlJTX0NoMTBfSW9uaWNfQ29uZHVjdGlvbl9DQQ..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211413\/20140811155233505392.png\" alt=\"Diagram of ions in an ionic solution when an electrical current is applied\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/In%20an%20ionic%20solution%2C%20the%20A%3Csup%3E%2B%3C%2Fsup%3E%20ions%20migrate%20toward%20the%20negative%20electrode%2C%20while%20the%20B%3Csup%3E%E2%88%92%3C%2Fsup%3E%20ions%20migrate%20toward%20the%20positive%20electrode.\" \/><\/p>\r\n<strong>Figure 8.15<\/strong>\r\n<p id=\"x-ck12-YTdiOGJkZDZmOTU0OTNkOTRmNmIyMDYwZjU3NWQ5MTY.-gzv\">In an ionic solution, the A <sup>+ <\/sup>ions migrate toward the negative electrode, while the B <sup>\u2212 <\/sup>ions migrate toward the positive electrode.<\/p>\r\n\r\n<\/div>\r\n<h4>Summary<\/h4>\r\n<ul id=\"x-ck12-ZTBmODg1MWU4ZGI0YjkzODEyMTA5ZjA5Yzg0Zjk3YWQ.-b7z\">\r\n \t<li>Ionic compounds have high melting points.<\/li>\r\n \t<li>Ionic compounds are hard and brittle.<\/li>\r\n \t<li>Solutions of ionic compounds and melted ionic compounds conduct electricity, but solid materials do not.<\/li>\r\n<\/ul>\r\n<h4>Practice<\/h4>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-jew\"><em>Questions<\/em><\/p>\r\n<p id=\"x-ck12-YmMzM2NmMmUyYzQ1NmUxNTQ2YTNmYjA2MWZlY2FkODA.-d7m\">Watch the video at the link below and answer the following questions:<\/p>\r\nhttps:\/\/youtu.be\/buWrSgs_ZHk\r\n<ol id=\"x-ck12-YmY3MjY5MjA3NzAwZWYxM2NiZWU0MDQ3MGM2ODU0MTM.-sj3\">\r\n \t<li>Do all ionic compounds form crystals?<\/li>\r\n \t<li>Will melted ionic compounds conduct electricity?<\/li>\r\n \t<li>What are the melting and boiling points of KI?<\/li>\r\n<\/ol>\r\n<h4>Review<\/h4>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-0a5\"><em>Questions<\/em><\/p>\r\n\r\n<ol id=\"x-ck12-OTAxZjU2MmJkOWNmMTRkZDU1YzM5ODM3Yjg2OWY5NmY.-wkp\">\r\n \t<li>Why are ionic compounds brittle?<\/li>\r\n \t<li>Why are melting points high for ionic compounds?<\/li>\r\n \t<li>What happens when an electric current is passed through a solution of an ionic compound?<\/li>\r\n<\/ol>\r\n<div class=\"x-ck12-data-problem-set\"><\/div>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-YTU1YzU3NGVmMDM5OWMwOGZkYWNjZjY3NjI2YTA5N2I.-zsh\">\r\n \t<li><strong>brittle: <\/strong>Easily broken, cracked, or snapped.<\/li>\r\n \t<li><strong>electrical conductivity: <\/strong>The ability to conduct an electric current.<\/li>\r\n<\/ul>\r\n<\/div>\r\n[reveal-answer q=\"836080\"]Show References[\/reveal-answer]\r\n[hidden-answer a=\"836080\"]\r\n<h2>References<\/h2>\r\n<ol>\r\n \t<li>(A) Mauro Cateb; (B) Parent G\u00e9ry; (C) Parent G\u00e9ry; (D) User:vassil\/Wikimedia Commons. (A) <a href=\"http:\/\/www.flickr.com\/photos\/mauroescritor\/6544460363\/\" target=\"_blank\" rel=\"noopener\">http:\/\/www.flickr.com\/photos\/mauroescritor\/6544460363\/<\/a>; (B) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Cinabre_macl%C3%A9_%28Chine%29_.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Cinabre_macl%C3%A9_%28Chine%29_.jpg<\/a>; (C) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Azurite_cristallis%C3%A9e_%28Chine%29_2_.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Azurite_cristallis%C3%A9e_%28Chine%29_2_.jpg<\/a>; (D) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Vanadinite_21207.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Vanadinite_21207.jpg<\/a>.<\/li>\r\n \t<li>CK-12 Foundation - Christopher Auyeung.<\/li>\r\n \t<li>CK-12 Foundation - Christopher Auyeung.<\/li>\r\n \t<li>CK-12 Foundation - Christopher Auyeung.<\/li>\r\n<\/ol>\r\n[\/hidden-answer]","rendered":"<h1 id=\"x-ck12-SW9uaWMgYW5kIE1ldGFsbGljIEJvbmRpbmc.-chapter\">Ionic and Metallic Bonding<\/h1>\n<div class=\"x-ck12-data\"><\/div>\n<h1 id=\"x-ck12-RWxlY3Ryb24gRG90IERpYWdyYW1z\">Physical Properties of Ionic Compounds<\/h1>\n<div class=\"x-ck12-data-objectives\">\n<ul id=\"x-ck12-Zjk3YmU0MmVkYzM3MGE5ODg4Y2NmYjZhZDVlZDk5ZDc.-vk0\">\n<li>List and describe the physical properties of ionic compounds.<\/li>\n<\/ul>\n<\/div>\n<div id=\"x-ck12-ZGI1MjgxOGE5MjUzMjJmYjJhOTZkNjFlZDkxOWQ0Yjk.-tx1\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<p id=\"x-ck12-lkv\"><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MjAwOTkwMC0zNy02NC1JbnRDaC0wOC0wNy1Db2xvcmZ1bC1pb25pYy1jb21wb3VuZHM.\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211408\/20140811155233093570.png\" alt=\"Pictures of amethyst, cinnabar, azurite, and vanadinite\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/In%20nature%2C%20the%20ordered%20arrangement%20of%20ionic%20solids%20gives%20rise%20to%20beautiful%20crystals.%20(A)%20Amethyst%20%E2%80%93%20a%20form%20of%20quartz%2C%20SiO%3Csub%3E2%3C%2Fsub%3E%2C%20whose%20purple%20color%20comes%20from%20iron%20ions.%20(B)%20Cinnabar%20%E2%80%93%20the%20primary%20ore%20of%20mercury%20is%20mercury(II)%20sulfide%2C%20HgS.%20(C)%20Azurite%20%E2%80%93%20a%20copper%20mineral%2C%20Cu%3Csub%3E3%3C%2Fsub%3E(CO%3Csub%3E3%3C%2Fsub%3E)%3Csub%3E2%3C%2Fsub%3E(OH)%3Csub%3E2%3C%2Fsub%3E.%20D)%20Vanadinite%20%E2%80%93%20the%20primary%20ore%20of%20vanadium%2C%20Pb%3Csub%3E5%3C%2Fsub%3E(VO%3Csub%3E4%3C%2Fsub%3E)%3Csub%3E3%3C%2Fsub%3ECl.\" \/><\/p>\n<p><strong>Figure 8.12<\/strong><\/p>\n<p id=\"x-ck12-YjVlMzMxZjFjY2FmYzg4OTBhOTUzOTVhZDM2MDkwM2I.-6hi\">In nature, the ordered arrangement of ionic solids gives rise to beautiful crystals. (A) Amethyst \u2013 a form of quartz, SiO <sub>2 <\/sub>, whose purple color comes from iron ions. (B) Cinnabar \u2013 the primary ore of mercury is mercury(II) sulfide, HgS. (C) Azurite \u2013 a copper mineral, Cu <sub>3 <\/sub>(CO <sub>3 <\/sub>) <sub>2 <\/sub>(OH) <sub>2 <\/sub>. D) Vanadinite \u2013 the primary ore of vanadium, Pb <sub>5 <\/sub>(VO <sub>4 <\/sub>) <sub>3 <\/sub>Cl.<\/p>\n<\/div>\n<p id=\"x-ck12-NDlhNGJlMDAyNDRiNDAwZWNjMzg4YjYzNjY2MzQ4YTM.-npp\"><strong>What produces colored crystals?<\/strong><\/p>\n<p id=\"x-ck12-NzliZTVjYmRhZTc2OWQ4YTZhYTFkODdlOGE0NmQ2MTg.-39f\">The figure above shows just a few examples of the color and brilliance of naturally occurring ionic crystals. The regular and orderly arrangement of ions in the crystal lattice is responsible for the various shapes of these crystals, while transition metal ions give rise to the colors.<\/p>\n<h3>Physical Properties of Ionic Compounds<\/h3>\n<h4>Melting Points<\/h4>\n<p id=\"x-ck12-YjNlZWNmNDk5NjNjMWIzNjMwZTE4ZTNhNGRkZDU0MDM.-8te\">Because of the many simultaneous attractions between cations and anions that occur, ionic crystal lattices are very strong.\u00a0 The process of melting an ionic compound requires the addition of large amounts of energy in order to break all of the ionic bonds in the crystal.\u00a0 For example, sodium chloride has a melting temperature of about 800\u00b0C.<\/p>\n<h4>Shattering<\/h4>\n<p id=\"x-ck12-YjVhNTUwMTViZjYwM2YzNGIwMmQ1YTJlZjc5NTMzNmQ.-vcj\">Ionic compounds are generally hard, but <strong>brittle.\u00a0 <\/strong>Why?\u00a0 It takes a large amount of mechanical force, such as striking a crystal with a hammer, to force one layer of ions to shift relative to its neighbor.\u00a0 However, when that happens, it brings ions of the same charge next to each other (see <strong>Figure <\/strong>below ).\u00a0 The repulsive forces between like-charged ions cause the crystal to shatter.\u00a0 When an ionic crystal breaks, it tends to do so along smooth planes because of the regular arrangement of the ions.<\/p>\n<div id=\"x-ck12-MDE3MDkxNGUxNDAxZDBhMjY5NGI0YzYzMWRkODM4MzU.-dkn\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<p id=\"x-ck12-tfw\"><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MjAxMDE1MC00OS0xMDAtSW50Q2gtMDgtMDgtTmFDbC1TaGF0dGVy\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211410\/20140811155233259022.png\" alt=\"Diagram of a shattering sodium chloride crystal\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/%28A%29%20The%20sodium%20chloride%20crystal%20is%20shown%20in%20two%20dimensions.%20%28B%29%20When%20struck%20by%20a%20hammer%2C%20the%20negatively-charged%20chloride%20ions%20are%20forced%20near%20each%20other%20and%20the%20repulsive%20force%20causes%20the%20crystal%20to%20shatter.\" \/><\/p>\n<p><strong>Figure 8.13<\/strong><\/p>\n<p id=\"x-ck12-NmFjNDYyNjYzZTc4MjdkN2UzOTdiNmI5YWY3ODBhZTQ.-use\">(A) The sodium chloride crystal is shown in two dimensions. (B) When struck by a hammer, the negatively-charged chloride ions are forced near each other and the repulsive force causes the crystal to shatter.<\/p>\n<\/div>\n<h4>Conductivity<\/h4>\n<p id=\"x-ck12-ZTM1MzM2Y2E2M2U1ZjkzZmExMDc2MDkwZWVlMThhYmQ.-asq\">Another characteristic property of ionic compounds is their <strong>electrical conductivity.\u00a0 <\/strong>The figure below shows three experiments in which two electrodes that are connected to a light bulb are placed in beakers containing three different substances.<\/p>\n<div id=\"x-ck12-Y2YzOTYyZmFiYzYwMDU0MzJkNjZjNmRlYTFlNDhlOTk.-mob\" class=\"x-ck12-img-fullpage x-ck12-nofloat\">\n<p><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MjAxMDMwMi00Mi00My1JbnRDaC0wOC0wOS1Db25kdWN0aXZpdHk.\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211411\/20140811155233388212.png\" alt=\"Electrical conductivity of pure water, a solid ionic compound, and an ionic solution\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/%28A%29%20Distilled%20water%20does%20not%20conduct%20electricity.%20%28B%29%20A%20solid%20ionic%20compound%20also%20does%20not%20conduct.%20%28C%29%20A%20water%20solution%20of%20an%20ionic%20compound%20conducts%20electricity%20well.\" \/><\/p>\n<p><strong>Figure 8.14<\/strong><\/p>\n<p id=\"x-ck12-NTBlMjA2NmI0ZDExM2RmY2Y4ZmNmNWIzZjMwZjZhOTc.-jxs\">(A) Distilled water does not conduct electricity. (B) A solid ionic compound also does not conduct. (C) A water solution of an ionic compound conducts electricity well.<\/p>\n<\/div>\n<p id=\"x-ck12-ZjU5NDU3MzU0YjA5YTBkNjhhM2EwYTAzN2Y4NTRhZTA.-vgy\">In the first beaker, distilled water does not conduct a current because water is a molecular compound.\u00a0 In the second beaker, solid sodium chloride also does not conduct a current.\u00a0 Despite being ionic and thus composed of charges particles, the solid crystal lattice does not allow the ions to move between the electrodes.\u00a0 Mobile charged particles are required for the circuit to be complete and the light bulb to light up.\u00a0 In the third beaker, the NaCl has been dissolved into the distilled water.\u00a0 Now the crystal lattice has been broken apart and the individual positive and negative ions can move.\u00a0 Cations move to one electrode, while anions move to the other, allowing electricity to flow (see <strong>Figure <\/strong>below ).\u00a0 Melting an ionic compound also frees the ions to conduct a current.\u00a0 Ionic compounds conduct an electric current when melted or dissolved in water.<\/p>\n<div id=\"x-ck12-NzNhOTM1ODVlYjNhNmQ0MDkzMDljYWFiNGI2NjMwOGE.-8ot\" class=\"x-ck12-img-thumbnail x-ck12-nofloat\">\n<p id=\"x-ck12-mfl\"><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MjAxMDQ2MS0xNC05NC1DaGVtSlJTX0NoMTBfSW9uaWNfQ29uZHVjdGlvbl9DQQ..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211413\/20140811155233505392.png\" alt=\"Diagram of ions in an ionic solution when an electrical current is applied\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/In%20an%20ionic%20solution%2C%20the%20A%3Csup%3E%2B%3C%2Fsup%3E%20ions%20migrate%20toward%20the%20negative%20electrode%2C%20while%20the%20B%3Csup%3E%E2%88%92%3C%2Fsup%3E%20ions%20migrate%20toward%20the%20positive%20electrode.\" \/><\/p>\n<p><strong>Figure 8.15<\/strong><\/p>\n<p id=\"x-ck12-YTdiOGJkZDZmOTU0OTNkOTRmNmIyMDYwZjU3NWQ5MTY.-gzv\">In an ionic solution, the A <sup>+ <\/sup>ions migrate toward the negative electrode, while the B <sup>\u2212 <\/sup>ions migrate toward the positive electrode.<\/p>\n<\/div>\n<h4>Summary<\/h4>\n<ul id=\"x-ck12-ZTBmODg1MWU4ZGI0YjkzODEyMTA5ZjA5Yzg0Zjk3YWQ.-b7z\">\n<li>Ionic compounds have high melting points.<\/li>\n<li>Ionic compounds are hard and brittle.<\/li>\n<li>Solutions of ionic compounds and melted ionic compounds conduct electricity, but solid materials do not.<\/li>\n<\/ul>\n<h4>Practice<\/h4>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-jew\"><em>Questions<\/em><\/p>\n<p id=\"x-ck12-YmMzM2NmMmUyYzQ1NmUxNTQ2YTNmYjA2MWZlY2FkODA.-d7m\">Watch the video at the link below and answer the following questions:<\/p>\n<p><iframe loading=\"lazy\" id=\"oembed-1\" title=\"ionic compound properties.flv\" width=\"500\" height=\"375\" src=\"https:\/\/www.youtube.com\/embed\/buWrSgs_ZHk?feature=oembed&#38;rel=0\" frameborder=\"0\" allowfullscreen=\"allowfullscreen\"><\/iframe><\/p>\n<ol id=\"x-ck12-YmY3MjY5MjA3NzAwZWYxM2NiZWU0MDQ3MGM2ODU0MTM.-sj3\">\n<li>Do all ionic compounds form crystals?<\/li>\n<li>Will melted ionic compounds conduct electricity?<\/li>\n<li>What are the melting and boiling points of KI?<\/li>\n<\/ol>\n<h4>Review<\/h4>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-0a5\"><em>Questions<\/em><\/p>\n<ol id=\"x-ck12-OTAxZjU2MmJkOWNmMTRkZDU1YzM5ODM3Yjg2OWY5NmY.-wkp\">\n<li>Why are ionic compounds brittle?<\/li>\n<li>Why are melting points high for ionic compounds?<\/li>\n<li>What happens when an electric current is passed through a solution of an ionic compound?<\/li>\n<\/ol>\n<div class=\"x-ck12-data-problem-set\"><\/div>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-YTU1YzU3NGVmMDM5OWMwOGZkYWNjZjY3NjI2YTA5N2I.-zsh\">\n<li><strong>brittle: <\/strong>Easily broken, cracked, or snapped.<\/li>\n<li><strong>electrical conductivity: <\/strong>The ability to conduct an electric current.<\/li>\n<\/ul>\n<\/div>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q836080\">Show References<\/span><\/p>\n<div id=\"q836080\" class=\"hidden-answer\" style=\"display: none\">\n<h2>References<\/h2>\n<ol>\n<li>(A) Mauro Cateb; (B) Parent G\u00e9ry; (C) Parent G\u00e9ry; (D) User:vassil\/Wikimedia Commons. (A) <a href=\"http:\/\/www.flickr.com\/photos\/mauroescritor\/6544460363\/\" target=\"_blank\" rel=\"noopener\">http:\/\/www.flickr.com\/photos\/mauroescritor\/6544460363\/<\/a>; (B) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Cinabre_macl%C3%A9_%28Chine%29_.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Cinabre_macl%C3%A9_%28Chine%29_.jpg<\/a>; (C) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Azurite_cristallis%C3%A9e_%28Chine%29_2_.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Azurite_cristallis%C3%A9e_%28Chine%29_2_.jpg<\/a>; (D) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Vanadinite_21207.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Vanadinite_21207.jpg<\/a>.<\/li>\n<li>CK-12 Foundation &#8211; Christopher Auyeung.<\/li>\n<li>CK-12 Foundation &#8211; Christopher Auyeung.<\/li>\n<li>CK-12 Foundation &#8211; Christopher Auyeung.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n","protected":false},"author":1507,"menu_order":10,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-2798","chapter","type-chapter","status-publish","hentry"],"part":2329,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2798","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/users\/1507"}],"version-history":[{"count":7,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2798\/revisions"}],"predecessor-version":[{"id":3643,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2798\/revisions\/3643"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2329"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2798\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=2798"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=2798"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=2798"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=2798"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}