{"id":68,"date":"2017-08-18T08:54:40","date_gmt":"2017-08-18T08:54:40","guid":{"rendered":"http:\/\/americanboard.org\/Subjects\/chemistry\/?page_id=68"},"modified":"2017-09-18T15:54:35","modified_gmt":"2017-09-18T15:54:35","slug":"the-structure-of-the-atom","status":"publish","type":"page","link":"https:\/\/americanboard.org\/Subjects\/chemistry\/the-structure-of-the-atom\/","title":{"rendered":"The Structure of the Atom"},"content":{"rendered":"<div class=\"twelve columns\" style=\"margin-top: 10%;\">\n<div class=\"advance\">\n<p><a class=\"button button-primary\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/development-of-the-atomic-theory\">\u2b05 Previous Lesson<\/a>\u00a0<a class=\"button\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/atomic-structure-periodicity-and-matter\">Workshop Index<\/a>\u00a0<a class=\"button button-primary\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/the-periodic-table\">Next Lesson \u27a1<\/a><\/p>\n<\/div>\n<p><!-- UPDATE NEXT\/PREVIOUS ABOVE --><\/p>\n<p><!-- CONTENT STARTS HERE --><\/p>\n<h1 id=\"title\">Atomic Structure, Periodicity, and Matter:The Structure of the Atom<\/h1>\n<h4>Objective<\/h4>\n<p>In this lesson, we will study the structure and properties of the atom .<\/p>\n<h4>Previously we covered&#8230;<\/h4>\n<ul>\n<li>The ancient and early atomic theories of Democritus and Dalton.<\/li>\n<li>The work of Faraday, Crookes, Roentgen, Thomson and Rutherford toward the discovery of electrically charged particles within atoms.<\/li>\n<li>The discovery of radioactivity and the differences between alpha, beta and gamma rays.<\/li>\n<li>Different models of the atom leading up to the currently accepted model.<\/li>\n<\/ul>\n<section>\n<h3>Introduction<\/h3>\n<div class=\"figures u-pull-left\">\n<p><img decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/chemistry\/wp-content\/uploads\/sites\/3\/2017\/08\/structureofatom2.helium.png\" alt=\"Helium atom\" \/><\/p>\n<p class=\"figcaption\">Helium atom<\/p>\n<\/div>\n<p>All matter consists of elements, of which there are more than 100. Each element has its own unique properties, and the atoms of each element are the smallest parts that retain the properties of that element. Since most atoms consist of the same three basic particles: protons, neutrons, and electrons, then the question becomes &#8220;what makes the atoms of one element different from another?&#8221; The answer lies in the number and arrangement of these three basic subatomic particles. For this reason, it is important to understand the fundamental structure of an atom and the characteristics of its protons, neutrons and electrons.<\/p>\n<p>Early experiments studying the relationship between matter and electricity during the late 1800&#8217;s led scientists to the discovery of the first subatomic particle, the <abbr title=\"A negatively charged subatomic particle\">electron<\/abbr>. Electrons are negatively charged particles, found in <abbr title=\"Regions around the nucleus of an atom where an electron is likely to be moving\">energy levels<\/abbr> surrounding the center or nucleus of the atom, and are in constant motion.<\/p>\n<p>Further investigations identified the <abbr title=\"The dense central portion of an atom, composed of protons and neutrons\">nucleus<\/abbr> as being composed of two types of particles, <abbr title=\"A positively charged subatomic particle found in the nucleus of an atom\">protons<\/abbr> and <abbr title=\"A subatomic particle with zero charge and a mass of one amu found in the nucleus of the atom\">neutrons<\/abbr>. The proton is a positively charged particle, and the neutron is a particle with no electric charge.<\/p>\n<h3>The Nucleus: Protons<\/h3>\n<p>In 1920, Ernest Rutherford refined the concept of the nucleus and concluded that the nucleus contained positively charged particles called protons. The proton is a subatomic particle carrying a charge equal but opposite to the negative charge of the electron. That is, the proton has a charge of +1, and the electron has a charge of -1. Therefore, an atom is electrically neutral as long as it has an equal number of protons and electrons.<\/p>\n<p>However, when the number of protons does not equal the number of electrons, the atom becomes charged and is known as an <abbr title=\"Atoms or group of atoms that have a positive or negative charge\">ion<\/abbr>. Ions will be covered in\u00a0more detail in this lesson; but it is important to note, at this time, that it\u00a0is the movement of the electrons, and not the protons, that creates the\u00a0positive or negative charge which changes an atom into an ion.<\/p>\n<p>Although\u00a0the number of electrons\u00a0and neutrons can vary in individual atoms of an element, the number of\u00a0protons\u00a0cannot. Each and every atom or ion of an element must have exactly the\u00a0same\u00a0number of protons. All carbon atoms, for example, must have 6 protons.\u00a0If a\u00a0proton were added to a carbon atom, then the atom would become an atom\u00a0of\u00a0nitrogen, having only the properties of nitrogen. Similarly, if a\u00a0proton were\u00a0removed from a carbon atom, it would become an atom of boron with the\u00a0properties of boron.<\/p>\n<p>Since\u00a0the number of protons in an\u00a0atom of an element is unique to that element, this number is\u00a0significant and is\u00a0known as the element&#8217;s <abbr title=\"The number of protons in the nucleus of an atom of an element\">atomic number<\/abbr>.\u00a0In the section of this lesson dealing with the <abbr title=\"An arrangement of elements into rows and columns according to similarities in their properties\">periodic table<\/abbr>, you will see that the elements are arranged by\u00a0increasing atomic number. Additionally, the proton has approximately\u00a0the same\u00a0mass as a <abbr title=\"A subatomic particle with zero charge and a mass of one amu found in the nucleus of the atom\">neutron<\/abbr>,\u00a0and the combined\u00a0mass of these two nuclear particles is known as the <abbr title=\"The total number of protons and neutrons in the nucleus of an atom\">mass number<\/abbr>.<\/p>\n<p>Although,\u00a0the proton is often\u00a0discussed as a single indivisible subatomic particle, it is important\u00a0to\u00a0recognize recent theories that no longer consider the proton as an\u00a0elementary\u00a0particle. The proton is referred to as a <abbr title=\"The protons and neutrons that make up a nucleus\">nucleon<\/abbr> which is made up of three <abbr title=\"Particles of which neutrons and protons are composed\">quarks<\/abbr>. As in\u00a0most\u00a0theories, the concept of\u00a0the proton is in a constant condition of being refined.<\/p>\n<h3>The Nucleus: Neutrons<\/h3>\n<p>In 1932, James Chadwick was credited with the discovery of a second subatomic particle contained in the nucleus of\u00a0the atom. Chadwick described this particle as having no electrical charge and the approximate mass of a proton. This\u00a0particle is the neutron. Unlike the protons, the number of neutrons can and do vary in the atoms of an element.\u00a0Atoms of the same element with differing numbers of neutrons are called <abbr title=\" Atoms of the same element that have the same atomic number but different atomic masses due to a different number of neutrons\">isotopes<\/abbr>.\u00a0Because neutrons are electrically neutral, a variation in the number of neutrons in the nucleus has no effect on the charge of the atom. However, the number of neutrons will affect the mass of an atom and the atomic mass of an element, and may affect the stability of the nucleus.<\/p>\n<p>Since the number of neutrons plus the number of protons in an atom is equal to the <abbr title=\" The total number of protons and neutrons in the nucleus of an atom\">mass number<\/abbr> of that atom, the neutrons are an important factor in the determination of the mass of any particular atom. In addition, the naturally occurring isotopes of an element determine the <abbr title=\"The weighted average of the masses of the isotopes of an element\">atomic mass<\/abbr> of that element. The atomic mass is the average of the mass numbers of the naturally occurring isotopes of an element. For example, naturally occurring copper consists of 69.17% copper atoms with a mass number of 63 <abbr title=\"Atomic mass unit - A unit of mass equal to one-twelfth the mass of a carbon-12 atom\">amu<\/abbr> and 30.83% copper atoms with a mass number of 65 amu. By multiplying the atomic mass of each isotope by its relative abundance and adding the two products, the average atomic mass of naturally occurring copper is calculated to be 63.55 amu.<\/p>\n<p>The neutrons also play an important role in the stability of the nucleus. There is a significant correlation between the neutron to proton ratio (n\/p) and the stability of the nucleus. Atoms with low atomic numbers (less than 20) are most stable when the neutron to proton ratio is 1:1. However, as the atomic number increases, more and more neutrons are needed to produce a strong nuclear force sufficient to hold the nucleus together. Thus, the neutron to proton ratio gradually increases in stable atoms to a maximum ratio of approximately 1.5 neutrons to 1 proton. This neutron to proton ratio range of 1.5 to 1 is known as the <abbr title=\"The region on a graph within which all stable nuclei are found when plotting their number of neutrons versus their number of protons\">band of stability<\/abbr>. Atoms with an n\/p ratio within this band have stable nuclei, and atoms with a ratio outside the band of stability contain nuclei that are radioactive.<\/p>\n<h3>The Mass Spectrometer<\/h3>\n<p>A <abbr title=\"A device used to separate electrically charged particles according to their masses\">mass spectrometer<\/abbr> is a device used to separate atoms of slightly different masses, thereby proving that many samples of naturally occurring elements are actually composed of a mixture of isotopes.<\/p>\n<div class=\"figures u-pull-right\">\n<p><img decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/chemistry\/wp-content\/uploads\/sites\/3\/2017\/08\/structureofAtom5.Mass_spectrom2.gif\" \/><\/p>\n<p class=\"figcaption\">Diagram of a typical mass spectrometer<\/p>\n<\/div>\n<p>In a mass spectrometer, a sample is placed in a vacuum chamber, where it is vaporized. There, the vaporized sample of\u00a0the element is bombarded with high energy electrons coming from a heated filament. When a particle in the sample is\u00a0hit by one of these electrons, it becomes ionized, usually to a positive ion (cation) due to the loss of an\u00a0electron. The ions are then focused into a narrow beam of particles and accelerated by an electric field. Because of\u00a0their charge, the particles can be deflected by magnetic fields. The amount of deflection depends on the speed,\u00a0charge, and mass of the particles.<\/p>\n<p>The ions are deflected in an arc whose radius is inversely proportional to the mass of the ion. Lighter ions are\u00a0deflected more than heavier ions. By varying the strength of the magnetic field, ions of different masses can be\u00a0focused on a detector fixed at the end of a curved tube. If a sample contains particles of several different masses,\u00a0each different mass corresponds to a different deflection. The resulting information is stored in and analyzed by a\u00a0computer. This information will usually be presented as a bar graph or line graph. Once the mass number and percent\u00a0of naturally occurring isotopes of an element is known, it is a relatively simple mathematical process to determine\u00a0the atomic mass of an element as we shall see in the next section.<\/p>\n<h3>How to Calculate an Atomic Mass<\/h3>\n<p>In order to calculate the atomic mass of an element, two values must be known:<br \/>\nThe <abbr title=\"The mass of an atom weighed in atomic mass units; An atomic mass unit is one-twelfth the mass of a carbon-12 atom. With the exception of carbon-12, the exact mass of an atom differs slightly from its mass number\">exact mass<\/abbr> for each naturally occurring stable isotope of the element and the percent<br \/>\nabundance of each isotope. These values can be found in chemistry and physics reference books. To find the atomic<br \/>\nmass of an element, multiply the exact mass of each isotope times the percent abundance (expressed as a decimal) of<br \/>\nthe isotope. Then add the results for each isotope together, and the sum will be the atomic mass for the<br \/>\nelement.<\/p>\n<section class=\"question\">\n<h4>Question<\/h4>\n<p>What is the atomic mass of the element silicon?<\/p>\n<table class=\"q_table\" border=\"1\" cellspacing=\"0\" cellpadding=\"2\" align=\"center\">\n<thead>\n<tr>\n<th colspan=\"3\">Silicon<\/th>\n<\/tr>\n<tr>\n<td>Mass number<\/td>\n<td>Exact mass<\/td>\n<td>Percent abundance<\/td>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>28<\/td>\n<td>27.976927<\/td>\n<td>92.23%<\/td>\n<\/tr>\n<tr>\n<td>29<\/td>\n<td>28.976495<\/td>\n<td>4.67%<\/td>\n<\/tr>\n<tr>\n<td>30<\/td>\n<td>29.973770<\/td>\n<td>3.10%<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<ol>\n<li>29.845<\/li>\n<li>27.589<\/li>\n<li>28.086<\/li>\n<li>30.009<\/li>\n<\/ol>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<div class=\"q-reveal\">The correct answer is C.<br \/>\n(27.976927)(0.9223) + (28.976495)(0.0467) + (29.973770)(0.031)\u00a0= 28.086<\/div>\n<\/section>\n<hr \/>\n<h3>Electrons<\/h3>\n<p>The subatomic particle of most importance to the chemist is the electron, because of its involvement in chemical<br \/>\nreactions. Electrons are subatomic, negatively charged particles that surround the nucleus of an atom. The electrons<br \/>\neach have a single fundamental unit of negative electric charge, or \u20131. It is much lighter than either the proton or<br \/>\nneutron. One electron&#8217;s mass is approximately 1\/1840<sup>th<\/sup> of the mass of either a proton or neutron.<\/p>\n<p>Scientists no longer think of electrons as following the fixed orbits as described by Bohr&#8217;s planetary model of the<br \/>\natom. Instead, electrons form regions of negative charge around the nucleus which are referred to as <abbr title=\"Regions around the nucleus of an atom where an electron is likely to be moving\">energy levels<\/abbr>. There are seven principal energy levels or regions around the nucleus where electrons are likely to be moving. Each principle energy level is divided into sublevels. Each sublevel is composed of a number of <abbr title=\"A three-dimensional region about the nucleus in which a particular electron can be located; an orbital can contain only one or two electrons\">orbitals<\/abbr> (not to be confused with the Bohr model\u2019s planetary orbit) which can hold one or two electrons.<\/p>\n<p>Obviously, the radii of the energy levels increase as they get further from the nucleus. The outer energy levels,<br \/>\nbeing larger, can contain more sublevels with a greater number of electrons. The maximum number of electrons for the<br \/>\nfirst four principle energy levels, as their distance from the nucleus increases, is summarized in the chart<br \/>\nbelow.<\/p>\n<table>\n<tbody>\n<tr>\n<td><strong>Principal energy level<\/strong><\/td>\n<td>1<\/td>\n<td>2<\/td>\n<td>3<\/td>\n<td>4<\/td>\n<\/tr>\n<tr>\n<td><strong>Maximum number of electrons<\/strong><\/td>\n<td>2<\/td>\n<td>8<\/td>\n<td>18<\/td>\n<td>32<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3>Electron Orbitals<\/h3>\n<p>In 1926, Erwin Schr\u00f6dinger took the electron arrangement one giant step further based on the <abbr title=\" A mathematical description of the wave properties of electrons and other small particle\">quantum theory<\/abbr>. He developed mathematical equations describing the probable location and energy of an\u00a0electron in a hydrogen atom. From his calculations, the <abbr title=\"The modern description, primarily mathematical, of the behavior of electrons in atoms\">quantum mechanical model<\/abbr> of the atom was developed. Previous models, although very useful in providing a visual image of the basic atomic structure, were based on the observations of large objects in motion. The quantum\u00a0mechanical model is not based on visual analogies, but rather on mathematical calculations. The quantum mechanical\u00a0model agrees with the Bohr model that there are seven principal energy levels, but does not define the exact path of\u00a0an electron around the nucleus. Instead, it describes the probability of finding an electron in a certain position\u00a0which may be depicted as a blurry cloud of negative charge. In addition, within each principal energy level, the\u00a0quantum mechanical model gives us one or more electron cloud shapes. This is because the mathematics of the quantum theory divides the principal energy levels into <abbr title=\"The energy levels contained within a principal energy level\">energy sublevels<\/abbr>, labeled <em>s, p, d<\/em>, and <em>f<\/em>. Each <abbr title=\"A three-dimensional region about the nucleus in which a particular electron can be located; an orbital can contain only one or two electrons\">orbital<\/abbr> in each sublevel has its own unique cloud shape. All <em>s<\/em> orbitals are spherical and all <em>p<\/em> orbitals are dumbbell shaped. However, not all <em>d<\/em> or <em>f <\/em>orbitals have the same shape.<\/p>\n<p><center><img decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/chemistry\/wp-content\/uploads\/sites\/3\/2017\/08\/structureofatom6.eorbitals.jpg\" \/><\/center>The quantum mechanical model assigns <abbr title=\" The quantum number (usually designated n) that indicates the main energy levels surrounding a nucleus\">principal quantum numbers<\/abbr> (<em>n<\/em>) to indicate the relative sizes and energies of the energy levels. As\u00a0<em>n<\/em> increases, the energy level becomes larger, the electrons are located farther from the nucleus, and the\u00a0atom&#8217;s energy level increases. Recall that seven energy levels have been described called principal energy levels.\u00a0Thus, <em>n<\/em> =1 for the energy level closest to the nucleus, <em>n <\/em>= 2 for the next energy level and\u00a0continuing to the outermost principal energy level in which <em>n <\/em>= 7. Principal energy levels contain energy\u00a0sublevels. The sublevels contain one, three, five or seven orbitals. An orbital is an area that can contain only one\u00a0or two electrons. The first sublevel is called the <em>s <\/em>sublevel and contains one orbital with a maximum of\u00a0two electrons. The second sublevel is called <em>p<\/em> and contains three orbitals and a maximum of six total\u00a0electrons. The third sublevel is called <em>d <\/em>containing five orbitals with a maximum of ten total electrons.\u00a0The fourth sublevel is called <em>f<\/em> and contains seven orbitals and a maximum of fourteen total electrons.<\/p>\n<table class=\"gas_law_table\" border=\"1\" cellspacing=\"0\" cellpadding=\"1\">\n<thead>\n<tr>\n<td colspan=\"5\" width=\"99%\">\n<p class=\"center\">Orbitals and Electron Capacity of the First Four Principle Energy Levels<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\">Principle energy level (<em>n<\/em>)<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">Type of sublevel<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">Number of orbitals per type<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">Number of orbitals per level (<em>n<\/em><sup>2<\/sup>)<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">Maximum number of electrons (2<em>n<\/em><sup>2<\/sup>)<\/p>\n<\/td>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td width=\"19%\">\n<p class=\"center\">1<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\"><em> s <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">1<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">1<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">2<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td rowspan=\"2\" width=\"19%\">\n<p class=\"center\">2<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\"><em> s <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">1<\/p>\n<\/td>\n<td rowspan=\"2\" width=\"19%\">\n<p class=\"center\">4<\/p>\n<\/td>\n<td rowspan=\"2\" width=\"19%\">\n<p class=\"center\">8<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\"><em> p <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">3<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td rowspan=\"3\" width=\"19%\">\n<p class=\"center\">3<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\"><em> s <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">1<\/p>\n<\/td>\n<td rowspan=\"3\" width=\"19%\">\n<p class=\"center\">9<\/p>\n<\/td>\n<td rowspan=\"3\" width=\"19%\">\n<p class=\"center\">18<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\"><em> p <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">3<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\"><em> d <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">5<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td rowspan=\"4\" width=\"19%\">\n<p class=\"center\">4<\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\"><em> s <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">1<\/p>\n<\/td>\n<td rowspan=\"4\" width=\"19%\">\n<p class=\"center\">16<\/p>\n<\/td>\n<td rowspan=\"4\" width=\"19%\">\n<p class=\"center\">32<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\"><em> p <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">3<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\"><em> d <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">5<\/p>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"19%\">\n<p class=\"center\"><em> f <\/em><\/p>\n<\/td>\n<td width=\"19%\">\n<p class=\"center\">7<\/p>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<section class=\"question\">\n<h4>Question 1<\/h4>\n<p>Which of the following is <strong> not<\/strong> a similarity between the proton and neutron of an atom?<\/p>\n<ol>\n<li>Both particles are believed to be approximately the same size.<\/li>\n<li>Both particles are located in the nucleus of the atom.<\/li>\n<li>Both particles have a mass of approximately 1 atomic mass unit.<\/li>\n<li>Both particles follow a curved path when moving through a magnetic field.<\/li>\n<\/ol>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<div class=\"q-reveal\">\n<p>The correct answer is D. The path of a proton is affected by a magnetic field due to its positive charge. The\u00a0path of a neutron is unaffected by a magnetic field because it has no charge.<\/p>\n<\/div>\n<\/section>\n<section class=\"question\">\n<h4>Question 2<\/h4>\n<p>The mass spectrometer can be used to__________________<\/p>\n<ol>\n<li>determine the relative masses of protons, neutrons, and electrons.<\/li>\n<li>determine the number of protons in the atoms of an element.<\/li>\n<li>determine the number of isotopes in naturally occurring elements.<\/li>\n<li>determine the elements that are found in an unknown mass.<\/li>\n<\/ol>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<div class=\"q-reveal\">\n<p>The correct answer is C. The mass spectrometer is a device used to separate charged particles of varying\u00a0masses.<\/p>\n<\/div>\n<\/section>\n<section class=\"question\">\n<h4>Question 3<\/h4>\n<p>Which of the following statements concerning the energy sublevels are true?<\/p>\n<ol>\n<li>The sublevel that is present in all principal energy levels is the <em>s <\/em> sublevel.<\/li>\n<li>Sublevels may be described as having different shapes.<\/li>\n<li>There are four different types of sublevels labeled <em>s<\/em>, <em>p<\/em>, <em>d<\/em>, and <em>f.<\/em><\/li>\n<li>All choices are correct.<\/li>\n<\/ol>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<div class=\"q-reveal\">\n<p>The correct answer is D. All statements concerning sublevels are correct.<\/p>\n<\/div>\n<\/section>\n<p><!-- CONTENT ENDS HERE --><\/p>\n<p><!-- UPDATE NEXT\/PREVIOUS BELOW --><\/p>\n<div class=\"advance\">\n<p><a class=\"button button-primary\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/development-of-the-atomic-theory\">\u2b05 Previous Lesson<\/a>\u00a0<a class=\"button\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/atomic-structure-periodicity-and-matter\">Workshop Index<\/a>\u00a0<a class=\"button button-primary\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/the-periodic-table\">Next Lesson\u27a1<\/a><\/p>\n<\/div>\n<p><a class=\"backtotop\" href=\"#title\">Back to Top<\/a><\/p>\n<\/section>\n<\/div>\n","protected":false},"excerpt":{"rendered":"<p>\u2b05 Previous Lesson\u00a0Workshop Index\u00a0Next Lesson \u27a1 Atomic Structure, Periodicity, and Matter:The Structure of the Atom Objective In this lesson, we will study the structure and properties of the atom . Previously we covered&#8230; The ancient and early atomic theories of Democritus and Dalton. The work of Faraday, Crookes, Roentgen, Thomson and Rutherford toward the discovery [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-68","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages\/68","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/comments?post=68"}],"version-history":[{"count":20,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages\/68\/revisions"}],"predecessor-version":[{"id":789,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages\/68\/revisions\/789"}],"wp:attachment":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/media?parent=68"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}