{"id":871,"date":"2010-05-12T23:42:51","date_gmt":"2010-05-12T10:42:51","guid":{"rendered":"http:\/\/science4all.blogtown.co.nz\/?p=871"},"modified":"2010-05-12T23:42:51","modified_gmt":"2010-05-12T10:42:51","slug":"ionic-bonding-and-covalent-bonding","status":"publish","type":"post","link":"https:\/\/science4all.blogtown.co.nz\/?p=871","title":{"rendered":"Ionic bonding and Covalent bonding"},"content":{"rendered":"<h3><span style=\"color: #33cccc\">Ionic bonding<\/span><\/h3>\n<p><img decoding=\"async\" src=\"http:\/\/www.chm.bris.ac.uk\/pt\/harvey\/gcse\/pics\/na_cl_e_trans.gif\" alt=\"\" \/><\/p>\n<p>Ionic bonding usually happens from reaction between metal and non-metal elements. You can see ionic bonding from a compound like NaCl (Sodium chloride). The forces of attraction between oppositely charged ions are called\u00a0ionic bonds. As you can see in the diagram, Na+(Sodium ion) is a positive and Cl-(Chloride ion) is a negative ion. This is because sodium has lost one of its electron on it&#8217;s outer shell and chlorine has gained one electron from sodium element.<\/p>\n<p>Sodium is an element but it becomes ion when it loses it&#8217;s electron from the outer shell. Chlorine is also an element &#8211; so it becomes negative ion as it gains a electron from the sodium.<\/p>\n<p>An\u00a0ionic bond (or electrovalent bond) is a type of chemical bond based on electrostatic forces between two oppositely-charged ions.<\/p>\n<p style=\"text-align: center\"><span style=\"color: #ffff99\"> &#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;&#8230;<\/span><\/p>\n<h3><span style=\"color: #33cccc\">Covalent bonding<\/span><\/h3>\n<p><span style=\"color: #33cccc\"><span style=\"color: #333333\">Covalent bonds are forces that hold non-metal <\/span><span style=\"color: #333333\">atoms<\/span><span style=\"color: #333333\"> together. The forces are formed when the atoms of a molecule share electrons.<\/span><\/span><\/p>\n<p><span style=\"color: #33cccc\"><span style=\"color: #333333\"><img decoding=\"async\" src=\"http:\/\/www.cem.msu.edu\/~reusch\/VirtualText\/Images\/lewstrc1.gif\" alt=\"\" \/><\/span><\/span><\/p>\n<p><strong><span style=\"font-weight: normal\">As you may know, an atom is made of a tiny core called a <\/span><span style=\"font-weight: normal\">nucleus<\/span><span style=\"font-weight: normal\">, with tiny particles called electrons traveling about the nucleus. Sometimes when atoms come together, two electrons will start to travel about the nuclei of <\/span><span style=\"font-weight: normal\">both<\/span><span style=\"font-weight: normal\"> atoms. The two atoms then share the pair of electrons.<\/span><\/p>\n<p><\/strong><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Ionic bonding Ionic bonding usually happens from reaction between metal and non-metal elements. You can see ionic bonding from a compound like NaCl (Sodium chloride). The forces of attraction between oppositely charged ions are called\u00a0ionic bonds. As you can see in the diagram, Na+(Sodium ion) is a positive and Cl-(Chloride ion) is a negative ion. &hellip; <\/p>\n<p class=\"link-more\"><a href=\"https:\/\/science4all.blogtown.co.nz\/?p=871\" class=\"more-link\">Continue reading<span class=\"screen-reader-text\"> &#8220;Ionic bonding and Covalent bonding&#8221;<\/span><\/a><\/p>\n","protected":false},"author":1509,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"slim_seo":{"title":"Ionic bonding and Covalent bonding - science4all","description":"Ionic bonding Ionic bonding usually happens from reaction between metal and non-metal elements. You can see ionic bonding from a compound like NaCl (Sodium chlo"},"footnotes":""},"categories":[6328,6306,6305,6303],"tags":[],"class_list":["post-871","post","type-post","status-publish","format-standard","hentry","category-year-6-8-science","category-year10-science","category-year11-chemistry","category-year11-science"],"_links":{"self":[{"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=\/wp\/v2\/posts\/871","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=\/wp\/v2\/users\/1509"}],"replies":[{"embeddable":true,"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=%2Fwp%2Fv2%2Fcomments&post=871"}],"version-history":[{"count":1,"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=\/wp\/v2\/posts\/871\/revisions"}],"predecessor-version":[{"id":872,"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=\/wp\/v2\/posts\/871\/revisions\/872"}],"wp:attachment":[{"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=%2Fwp%2Fv2%2Fmedia&parent=871"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=%2Fwp%2Fv2%2Fcategories&post=871"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/science4all.blogtown.co.nz\/index.php?rest_route=%2Fwp%2Fv2%2Ftags&post=871"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}