{"id":1820,"date":"2023-10-02T06:31:29","date_gmt":"2023-10-02T06:31:29","guid":{"rendered":"http:\/\/localhost\/ecole9ja\/?p=1820"},"modified":"2023-10-02T06:32:11","modified_gmt":"2023-10-02T06:32:11","slug":"week-10-ss1-first-term-chemistry-notes","status":"publish","type":"post","link":"https:\/\/ecolebooks.com\/nigeria\/posts\/week-10-ss1-first-term-chemistry-notes\/","title":{"rendered":"Week 10 &#8211; SS1 First Term Chemistry Notes"},"content":{"rendered":"<p>\u00a0<br \/>\n\u00a0<strong>WEEK TEN<br \/>\n<\/strong><strong>TOPIC: STRUCTURE OF THE ATOM<br \/>\n<\/strong><strong>CONTENT<br \/>\n<\/strong><\/p>\n<ul>\n<li>\n<div>Orbitals of The Atom\n<\/div>\n<\/li>\n<li>\n<div>Electronic Structure Of the Atom\n<\/div>\n<\/li>\n<li>\n<div>Filling Of Electrons in to Orbitals\n<\/div>\n<\/li>\n<li>\n<div>Quantum Numbers\n<\/div>\n<\/li>\n<\/ul>\n<p><strong>ORBITALS OF THE ATOM<br \/>\n<\/strong>The region in space within which there is maximum possibility of finding an electron in an atom is called an ATOMIC ORBITAL. We have s, p, d, and f orbitals.<strong><br \/>\n\t\t\t<\/strong>Shapes of s and p orbitals are as follows<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F1.png\" alt=\"\"\/><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F2.png\" alt=\"\"\/><strong>:              \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<\/strong><br \/>\n\t\t<strong>\u00a0\u00a0\u00a0\u00a0<br \/>\n<\/strong><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F3.png\" alt=\"\"\/><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F4.png\" alt=\"\"\/><strong><br \/>\n\t\t\t<\/strong><strong>                       s-orbital<br \/>\n<\/strong><br \/>\n\u00a0<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F5.png\" alt=\"\"\/><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F6.png\" alt=\"\"\/><strong>p<sub>x<\/sub> orbital<\/strong><\/p>\n<p>\u00a0<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F7.png\" alt=\"\"\/><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100223_0631_Week10SS1F8.png\" alt=\"\"\/><strong>                                               p<sub>y<\/sub> orbital                                 \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0                                p<sub>z    <\/sub>orbital<br \/>\n<\/strong><br \/>\n\u00a0<strong>EVALUATION<\/strong><\/p>\n<ol>\n<li>\n<div>Define atomic orbital\n<\/div>\n<\/li>\n<li>\n<div>State the shape of (i) S-orbital (ii) P-orbital.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>ELECTRONIC STRUCTURE OF THE ATOM<br \/>\n<\/strong>With the knowledge of atomic orbital the spectra of more complex atoms than hydrogen atom can be explained as follows:<\/p>\n<p>\u00a0a) that within a given principal quantum number or energy level, there are sub energy levels, i.e. energy levels otherwise called K,L,M,N,O,P AND Q shells have sub-energy levels otherwise called s,p,d and f orbitals <\/p>\n<p>\u00a0(b) The total number of sub-shells within a shell is given by n<sup>2<\/sup><br \/>\n\t\twhile the total maximum number of  electrons is given by 2n<sup>2<\/sup> where n is  the number of  enregy level.<br \/>\nEnergy Level                             Number of orbitals                    Maximum No of electrons<br \/>\nn = 1(K- shell)                              1<sup>2<\/sup> =1                                         2\u00b41<sup>2 =2<br \/>\n<\/sup><sup><br \/>\n\t\t\t\t<\/sup>n =2 (L- shell)                              2<sup>2 <\/sup>= 4                                       2\u00b42<sup>2 = 8<\/sup><br \/>\n\t\t\t n = 3 (M- shell)                          3<sup>2<\/sup> = 9                                       2\u00b43<sup>2<\/sup> = 18<br \/>\n n = 4 (N- shell)                           4<sup>2<\/sup> =16                                      2\u00b4 4<sup>2<\/sup> = 32<br \/>\nn = 5 (O- shell)                            5<sup>2<\/sup> = 25                                     2\u00b4 5<sup>2<\/sup> =50<br \/>\nn = 6 (P-shell)                              6<sup>2<\/sup> = 36                                     2\u00b46<sup>2 <\/sup>=72<br \/>\nn = 7 (Q &#8211; shell)                           7<sup>2  <\/sup>= 49                                      2\u00b47<sup>2<\/sup> = 98                     <\/p>\n<p>\u00a0(c) In a given orbital there could be a maximum of only two electrons and electron in all orbitals of the same type within a principal quantum number possess equal energies.<\/p>\n<p>\u00a0(d) The electrons in the different sub- shells or orbitals within a principal quantum number do not all have equal energies.<br \/>\nThe gradation of energies of orbitals is as follows:<br \/>\n1s&lt; 2s&lt;2p&lt;3s&lt;3p&lt;3d&lt;4s&lt;4p&lt;4d&#8212; <\/p>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>State the first five energy levels.\n<\/div>\n<\/li>\n<li>\n<div>Calculate the total no of electrons when n is equal to (i) 2 (ii) 4.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>FILLING OF ELECTRONS IN ORBITALS<br \/>\n<\/strong>In filling electrons into the atoms of elements, considerations are given to the conditions laid down by Aufbau Principle, Pauli exclusion principle and Hund&#8217;s rule of maximum multiplicity.<\/p>\n<p>\u00a0AUFBAU PRINCIPLE states that electrons go in to fill orbitals of lower energy first before filling orbitals of higher energy and each orbital may hold up to two electrons.<\/p>\n<p>\u00a0PAULI EXCLUSION PRINCIPLE states that no two electrons have identical sets of the four quantum numbers {n, l, m and s in an atom}.<\/p>\n<p>\u00a0HUND&#8217;S RULE OF MAXIMUM MULTIPLICITY state that in filling degenerate orbitals with electrons, electrons go in singly first before pairing up occurs.<\/p>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong>State the following principle<br \/>\n{a} Aufbau Principle {b} Hund&#8217;s rule.<\/p>\n<p>\u00a0<strong>QUANTUM NUMBERS<br \/>\n<\/strong>Studies show that the energy of an electron may be characterized by four quantum numbers. These are<br \/>\n{1}The principal quantum number represented by n with integral values of 1,2,3,4 e.t.c.<br \/>\n{2}The subsidiary or Azimuthal quantum number represented by l with integral values<br \/>\n      ranging from O to (n-1).<br \/>\n(3) The magnetic quantum number represented by m with integral values ranging<br \/>\n      from \u2013l to +l.<br \/>\n4. The spin quantum number represented by s with integral values \u2013 <sup>1<\/sup>\/<sub>2<\/sub> and = <sup>1<\/sup>\/<sub>2<\/sub>.<br \/>\n<strong>Element           Atomic Number         Electronic configuration.<br \/>\n<\/strong>H                           1                               1S<sup>1<\/sup><br \/>\n\t\tHe                          2                              1S<sup>2<\/sup><br \/>\n\t\tLi                           3                              1S<sup>2 <\/sup>2S<sup>1<\/sup><br \/>\n\t\tBe                          4                              1S<sup>2<\/sup> 2S<sup>2<\/sup><br \/>\n\t\tB                            5                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>1<\/sup><br \/>\n\t\tC                            6                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>2<\/sup><br \/>\n\t\tN                            7                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>3<\/sup><br \/>\n\t\tO                            8                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>4 <\/sup><br \/>\n\t\tF                             9                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>5 <\/sup><br \/>\n\t\tNe                         10                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup><br \/>\n\t\tNa                         11                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>1<\/sup><br \/>\n\t\tMg                         12                              1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2<\/sup><br \/>\n\t\tAl                           13                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2 <\/sup>3P<sup>1<\/sup><br \/>\n\t\tSi                            14                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2 <\/sup>3P<sup>2<\/sup><br \/>\n\t\tP                             15                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6<\/sup>3S<sup>23<\/sup>3P<sup>3<\/sup><br \/>\n\t\tS                             16                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6<\/sup>3S<sup>2 <\/sup>3P<sup>4<\/sup><br \/>\n\t\tCl                            17                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2 <\/sup>3P<sup>5<\/sup><br \/>\n\t\tAr                            18                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2<\/sup>3P<sup>6<\/sup><br \/>\n\t\tK                             19                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2<\/sup>3P<sup>6 <\/sup>4S<sup>1<\/sup><br \/>\n\t\tCa                            20                             1S<sup>2<\/sup> 2S<sup>2 <\/sup>2P<sup>6 <\/sup>3S<sup>2<\/sup>3P<sup>6 <\/sup>4S<sup>2<br \/>\n<\/sup><br \/>\n\u00a0<strong>GENERAL EVALUATION<\/strong><sup><br \/>\n\t\t\t<\/sup><\/p>\n<ol>\n<li>\n<div>State the four quantum numbers.\n<\/div>\n<\/li>\n<li>\n<div>Write the electronic configuration of the following a) Mg b) S<sup>2-<\/sup> c) Ca<sup>2+<\/sup> d) Si\n<\/div>\n<p>\u00a0<strong>READING ASSIGNMENT<br \/>\n<\/strong><\/li>\n<\/ol>\n<ul>\n<li>\n<div>New School Chemistry By O.Y. Ababio pg 49-54.\n<\/div>\n<\/li>\n<\/ul>\n<p>\u00a0<strong>WEEKEND ASSIGNMENT<\/strong><br \/>\n\t\t1.  Which of the following orbitals is spherical in shape?<\/p>\n<ol>\n<li>\n<div>s (b) p (c) d (d) f\n<\/div>\n<\/li>\n<\/ol>\n<p>2. Which of the following shells have a maximum of eight electrons ?<\/p>\n<ol>\n<li>\n<div>k (b) l (c) m (d) n\n<\/div>\n<\/li>\n<\/ol>\n<p>3. 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3p<sup>1<\/sup> is the electronic configuration of <\/p>\n<ol>\n<li>\n<div>potassium (b) calcium (c) sodium  (d) aluminum.\n<\/div>\n<\/li>\n<\/ol>\n<p>4. &#8220;No two electrons have identical sets of four quantum numbers&#8221;. This statement is <\/p>\n<ol>\n<li>\n<div>Aufbau principle (b) Pauli exclusion (c) Hund&#8217;s rule (d) Rutherford&#8217;s model.\n<\/div>\n<\/li>\n<\/ol>\n<p>5. Which of the quantum number is represented by L?<\/p>\n<ol>\n<li>\n<div>principal quantum no (b) subsidiary quantum no (c) magnetic quantum\n<\/div>\n<\/li>\n<\/ol>\n<p>(d) spin quantum.<\/p>\n<p>\u00a0<strong>THEORY<\/strong><\/p>\n<ol>\n<li>\n<div>State the following principle (a) Pauli exclusion principle. (b) Aufbau principle.\n<\/div>\n<\/li>\n<li>\n<div>Write the electronic configuration of\n<\/div>\n<p>(a) Oxygen<br \/>\n(b) Calcium (c) Chloride ion (Cl<sup>&#8211;<\/sup>) (d) Aluminum ion (Al<sup>3+<\/sup>)\n<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"<p>\u00a0 \u00a0WEEK TEN TOPIC: STRUCTURE OF THE ATOM CONTENT Orbitals of The Atom Electronic Structure&#8230;<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1,167],"tags":[],"class_list":["post-1820","post","type-post","status-publish","format-standard","hentry","category-posts","category-first-term-ss1-chemistry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/1820","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/comments?post=1820"}],"version-history":[{"count":1,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/1820\/revisions"}],"predecessor-version":[{"id":1821,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/1820\/revisions\/1821"}],"wp:attachment":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/media?parent=1820"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/categories?post=1820"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/tags?post=1820"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}