{"id":318,"date":"2015-01-29T16:20:22","date_gmt":"2015-01-29T16:20:22","guid":{"rendered":"https:\/\/oduhsadvising.wordpress.com\/?p=277"},"modified":"2015-01-29T16:20:22","modified_gmt":"2015-01-29T16:20:22","slug":"277","status":"publish","type":"post","link":"https:\/\/sites.wp.odu.edu\/hsadvising\/2015\/01\/29\/277\/","title":{"rendered":"Guest Blog: Chemistry Tips Chapters 3 &amp; 5"},"content":{"rendered":"<h3 style=\"text-align:center\"><span style=\"color:#000080\">Our guest blogger Rachel is back with tips from CHEM 105 Chapters 3 &amp; 5!<\/span><\/h3>\n<p><a href=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2015\/01\/get-a-tutor-pass-all-chemistry-tests.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter size-medium wp-image-278\" src=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2015\/01\/get-a-tutor-pass-all-chemistry-tests.jpg?w=300\" alt=\"get-a-tutor-pass-all-chemistry-tests\" width=\"300\" height=\"225\" \/><\/a><\/p>\n<p style=\"text-align:left\"><span style=\"text-decoration:underline\"><strong><a href=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2014\/10\/tucker_headshot.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"alignleft  wp-image-197\" src=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2014\/10\/tucker_headshot.jpg?w=233\" alt=\"Tucker_headshot\" width=\"153\" height=\"197\" \/><\/a>Diagnosing Your Chemistry Problems (Continued) by: Rachel Tucker<\/strong><\/span><\/p>\n<p><strong>Now let\u2019s take a look at the next set of concepts including Chapters 3 &amp; 5 dealing with Elements and Compounds. <\/strong><\/p>\n<p>&nbsp;<\/p>\n<p>&nbsp;<\/p>\n<ul>\n<li>Elements on the periodic table read with the atomic number above the symbol and the atomic mass below the symbol<a href=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2014\/10\/blog-picture-1.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter size-full wp-image-194\" src=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2014\/10\/blog-picture-1.jpg\" alt=\"Blog (Picture 1)\" width=\"300\" height=\"163\" \/><\/a><\/li>\n<li>Verses single <span style=\"text-decoration:underline\">isotopes<\/span> are read with the mass number (protons + neutrons) to the top left and atomic number below the symbol<\/li>\n<\/ul>\n<p><a href=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2014\/10\/blog-picture-2.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter size-full wp-image-195\" src=\"http:\/\/sites.wp.odu.edu\/hsadvising\/wp-content\/uploads\/sites\/19909\/2014\/10\/blog-picture-2.png\" alt=\"Blog Picture 2\" width=\"245\" height=\"176\" \/><\/a><\/p>\n<ul>\n<li>When given a <span style=\"text-decoration:underline\">periodic table<\/span>, label the columns (groups) from left to right as #1-8 skipping over the transition metals. These group numbers give you all kinds of clues for finding valence electrons and typical charges.\n<ul>\n<li>Group number tells you how many valence electrons the element has.\n<ul>\n<li>Na = 1 valence electron<\/li>\n<\/ul>\n<\/li>\n<li>Group numbers 1-3 have positive charges and the group # tells you what that charge is.\n<ul>\n<li>Mg (group 2) = 2+ charge because when Mg bonds to other atoms, it loses 2 electrons<\/li>\n<\/ul>\n<\/li>\n<li>Group numbers 5-7 have negative charges and 8 \u2013 the group number = the charge.\n<ul>\n<li>S (group 6) = 2- charge because 8 \u2013 6 = 2, S gains 2 electrons when it bonds to other atoms<\/li>\n<\/ul>\n<\/li>\n<li>Elements in one group have similar bonding and chemical properties<\/li>\n<\/ul>\n<\/li>\n<li><span style=\"text-decoration:underline\">Electron configurations<\/span>\n<ul>\n<li>READ THE PERIODIC TABLE LIKE A BOOK FROM LEFT TO RIGHT BEGINNING WITH HYDROGEN.<\/li>\n<li>Visualize how the periodic table is blocked out\n<ul>\n<li>Groups 1-2 are the s block<\/li>\n<li>Groups 3-8 are the p block<\/li>\n<li>The transition metals are the d block<\/li>\n<li>The inner transition metals are the f block (which you do not need to worry about for this class)<\/li>\n<li>Read from left to right on each row (period), filling in the s, p, or d orbital until you have reached the end of the block<\/li>\n<\/ul>\n<\/li>\n<li>Think of electron configurations as a blue print for building blocks \u2013 if you are given the element Cu (copper), which is element 29, every element coming before Cu (1-28) should be included in its electron configuration<\/li>\n<\/ul>\n<\/li>\n<li>Memorize your <span style=\"text-decoration:underline\">polyatomic ions<\/span>\n<ul>\n<li>These interact and form compounds acting as \u201cone unit\u201d or \u201cone element\u201d<\/li>\n<li>The \u201cate\u201d form of a family of polyatomic ions has more oxygen than the \u201cite\u201d form\n<ul>\n<li>Sulf<em>ate<\/em> = SO4^-2<\/li>\n<li>Sulf<em>ite<\/em> = SO3^-2<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n<p>I wish you all the best in applying for your individual programs and please come by the <a href=\"http:\/\/sci.odu.edu\/msrc\/\">chemistry-tutoring center <\/a>in <a href=\"https:\/\/www.odu.edu\/about\/visitors\/campus-map\">OCNPS 146<\/a> for help with any homework or study questions! We are open from 10am \u2013 5pm M-F.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Our guest blogger Rachel is back with tips from CHEM 105 Chapters 3 &amp; 5! Diagnosing Your <a class=\"more-link\" href=\"https:\/\/sites.wp.odu.edu\/hsadvising\/2015\/01\/29\/277\/\">Continue reading <span class=\"screen-reader-text\">  Guest Blog: Chemistry Tips Chapters 3 &amp; 5<\/span><span class=\"meta-nav\">&rarr;<\/span><\/a><\/p>\n","protected":false},"author":10585,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":"","wds_primary_category":0},"categories":[3,5,6,10,11,12],"tags":[],"_links":{"self":[{"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/posts\/318"}],"collection":[{"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/users\/10585"}],"replies":[{"embeddable":true,"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/comments?post=318"}],"version-history":[{"count":0,"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/posts\/318\/revisions"}],"wp:attachment":[{"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/media?parent=318"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/categories?post=318"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/sites.wp.odu.edu\/hsadvising\/wp-json\/wp\/v2\/tags?post=318"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}