the value of n is 4 then there are 4 different subshells. What is the Pauli Exclusion Principle? With chemicals, its shoot first and ask questions later. Al Meyerhoff. 2) Using Octet Rule, arrange the electrons to its orbital shells based on electron configuration. For example: let us learn the abbreviated and unabbreviated form of Gold metal in the periodic table. Electron configurations of atoms follow a standard notation in which all electron-containing atomic subshells (with the number of electrons they hold written in superscript) are placed in a sequence. Call Us Today! We have already learnt that each period starts with the element having general outer electronic configuration ns 1 and ends with ns 2, np 6 where n is the period number. In the third period the 3s subshell is filling for Na and Mg, and therefore Al, Si, P, S, Cl, and Ar. noble gases. The existence of these exceptions to the Aufbau principle is due to the fact that atomic orbitals are affected by the charge of the nucleus of the atom and the presence of electrons in other orbitals of the atom. Period 1: K shell (1 st energy level) filling. 6) Check out for every atom whether it possess octet configuration. Therefore, the noble gas element Xe denotes the completely filled outermost shells and becomes [Xe] 4f145d106s1. The electron: May it never be of any use to anybody! Joseph John Thomson. Adding up all the superscript numbers gives us 5, and boron has 5 electrons. More important. A half-filled 4s orbital and a fully filled 3d orbital is more stable than a full 4s orbital and a 3d orbital with only 9 electrons, so the atom opts for the former state. Follow the Aufbau rule and write the full electron configuration. The electrons are arranged in four subshells namely s,p, d and f. The electron configuration of each atom is represented by following a standard notation. Consider Bromine element located in the Group VII, Period 4 of the periodic table. 3) In case of cation, subtract the electrons around the element from the total number of valence electrons while drawing the dot diagram. This last electron is called the distinguishing electron because it distinguishes an atom from the one immediately preceding it in the periodic table. For ex: 7s, 5f, 6d and 7p subshells will not be filled up without the occupation of electrons in 1s to 6p subshells. Zip. He was awarded a Nobel prize for his work. All Rights Reserved. answer . ISSN: 2639-1538 (online). Iodine is the stable halogen with atomic number 53 and has symbol I. d) Y. e) La. Thus, they play a crucial role in determining the important role in carrying out chemical reactions which involve the atom. What are shells in an electronic configuration? Answers to the questions appear at the end of the test. That is where the role of abbreviated and unabbreviated electron configurations come into the picture. DETAILS - Comprehensive review of every chemistry topic to appear on the SAT II subject test - Flexible study schedule tailored to your needs - Packed The atomic number is the number of electrons in that element. Step-by-step guide to drawing electron configuration diagrams By Kirsty Patterson2021-09-06T07:06:00+01:00 4comments Boost your 14-16 students' confidence drawing electron configuration diagrams with these easy to follow steps An electron configuration diagram is a model that depicts the position of electrons as they orbit the nucleus of an atom. answer choices. Thats it! Using our rules for deriving electron configurations (Example 1) we have Thus the similarities of chemical behavior and valence noted earlier for these elements correlate with the similarities of their outermost electron clouds. Free practice questions for AP Chemistry - Atomic Structure and Electron Configuration. It can be alternatively explained as "two electrons in the same atom do not have the same values for all 4 quantum numbers present". Electron Configuration Chart Let's try using this chart to fill out an example electron configuration for a selenium (Se) atom. The maximum number of electrons that can be acclimated by a subshell is allotted by the formula 2*(2l + 1). If two orbitals have the same value for n+l, the orbital with lower value of n will have the lower energy and so the electrons will occupy that first. Apart from electrons and protons, an atom also has neutrons which may or may not be equal to the number of the protons. I am Angela. the large, bulky nuclei of heavy elements exert a significant force on the surrounding orbitals, which can make the atom take on electron configurations at odds with the Aufbau principle. Here, the n is the shell number. A: Solution of question 3 Given, The abundance of 69Ga = 62.1% The abundance of 71Ga = 37.9% Formula. a) Na. 4) The least possible electronegative atom or ion is placed in the middle of the molecule and connect the atoms using single bonds only. This handy chart compiles the electron configurations of the elements up through number 104. I.e. Valence electrons. Therefore the distinguishing electron must occupy either the 5s or 5p subshell. The modern periodic table is based on Dmitri Mendeleev's 1896 observations that chemical elements can be grouped according to chemical properties they exhibit. text explanation. Accordingly, shell 1 can hold a total of 2 electrons, shell 2 can hold a total of 8 electrons, shell three a total of 18, etc. At this point, we all are aware of that an electrons location is uncertain and only reveal their probability of exact location around the nucleus. Electronic configuration of an atom defines the precise distribution of electrons in an atom and this distribution helps in understanding the reasons for the chemical reactions that the atom or its corresponding molecules get involved in. Legal. Electronic configuration is defined as the distribution of electrons into the orbitals of an atom. The letters in the electronic configuration of any element i.e. In this chart, the numbers (1, 2, 3,) are referred to as theprincipal quantum number, referred to as n,which corresponds to an electron shell. Have the students place the markers (bingo chips, etc) on the map in numerical order to show students how electrons are configured. The values of n, shells and total number of electrons are accommodated differently. If the value of ms is +1/2 for an electron, then that electron is alpha electron while the electron with -1/2 spin value is beta electron. It is the very strong attractive force of this small fraction of the total 4s electron density that lowers the energy of the 4s electron below that of the 3d. Every shell is designated a value which is basically the principal quantum number. As we all already know, electrons bear charge i.e. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. As an example, consider hydrogen. It has 35 electrons and among which 7 electrons are valence electrons. In general, atoms will completely fill a lower level orbital before filling a higher one. Electron configurations of atoms adhere to a standard . Follow up your study with REA's proven test-taking strategies, powerhouse drills and study schedule that get you ready for test day. Each atomic orbital can just accommodate only 2 electrons that are in opposite spin only. 4) Make use of periodic table rows and determine orbital shells. H 1s1. In an atom, the protons and the neutrons lie in the nucleus and have almost negligible role in governing any chemical reaction. Spin quantum number, s: The electrons in an atom have a particle property; it spins on its own axis at a particular speed. 4) Make use of periodic table rows and determine orbital shells. The formula that derives the value of magnetic quantum number is ml = (2+ 1)! On the other hand, the electrons lie outside the nucleus of the atom and have precise distribution inside an atom. So, overall values of quantum numbers based on this formula could be; For = 0; m1 = 0 and For = 1; m1 = -1, 0, +1. Moreover, the chart also describes how electrons are arranged within energy. Every shall has a fixed number of subshells/sublevels. This agrees with the valence rules derived from the periodic table, and results in formulas for chlorides of the first dozen elements that show the periodic variation of valence. Thus, they play a crucial role in determining the important role in carrying out chemical reactions which involve the atom. The unabbreviated electron configuration of Gold is: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d10 6s1 while the abbreviated electron configuration of Gold is [Xe] 4f145d106s1, You might have observed that the unabbreviated electron configuration of Gold is long, tedious and takes time to write it completely. 3) Trace out the number of electrons present in the outer most shell. This website uses cookies and similar technologies to deliver its services, to analyse and improve performance and to provide personalised content and advertising. Hence, unabbreviated electron configuration remains much longer, confused and time-taking. 2. Thus, an s orbital can hold a total of two electrons, a p orbital can hold a total of 6 electrons, a d orbital 10 and an f orbital 14. Kirsty Patterson is the assistant editor for teaching resources at the Royal Society of Chemistry. Their movement from one energy state to another completely depends on the attractive and repulsive forces between the positive and negative charges. Find the table representation of possible subshells based on the principal energy levels below: Here we have included the values of n up to 4 and the rest of the values follows the same method. According to the rules of electronic configuration, two electrons can locate in the same orbital but with opposite spin directions. The electron configuration of an element describes how electrons are distributed in its atomic orbitals. For any given element, that elements electron configuration can be represented as some sequence of shell labels and orbital labels. The chemistry of the transition metals is more complicated and a wider variety of formulas for transition-metal compounds is possible because of this variable valence. 2) Using Octet Rule, arrange the electrons to its orbital shells based on electron configuration. The spin quantum number, denoted by s, indicates the orientation of the electrons angular momentum. Therefore, a cadmium atom will have two electrons in the first shell, eight in the 2nd orbit, and eighteen electrons in the 3rd shell. The protons and neutrons lie inside the nucleus in an atom and have a negligible role in regulating any chemical reactions. The spin quantum number, denoted by s, indicates the orientation of the electrons angular momentum. 2s subshell can have only one atomic orbital (2*0+1=1 so only 1 orbital) and the corresponding value for m is 0. However, they are basically the orbital angular momentum or subsidiary quantum number. Then, the number of electrons located in each orbital is denoted in the superscript of the orbital symbol i.e. The 3rd shell has 3 subshells i.e. The number of electrons in the atom is. The oxygen atom consists of 6 valence electrons and 2 lone pairs. Likewise, the p-block is 6 wide because it takes 6 electrons to fill up p orbitals. To find out elements that show similar chemical and physical properties. Relate electron configurations to element classifications in the periodic table Having introduced the basics of atomic structure and quantum mechanics, we can use our understanding of quantum numbers to determine how atomic orbitals relate to one another. 1) Pick a periodic table where you will find all the variety of elements in the boxes. Molecules with a linear geometry have hybridized sp orbitals, molecules with a trigonal planar geometry have an sp hybridization, and molecules with a tetrahedral geometry have an sp hybridization. Hydrogens (H) electron configuration notation is 1s. The electrons which do not participate in any type of chemical bonding and do not refer to valence electrons are core electrons. For each electron shell atom diagram, the element symbol is listed in the nucleus. For n=3, i.e. The number of shells shows which period, or row, its in and the number of electrons in the outer shell shows which group its in. For electronic configuration we must know about shells and subshells. 1. Electron configuration chart of all Elements is mentioned in the table below. Obtain the electron configuration for (a) Nb; (b) Pr. Although the 3d electron clouds do not extend farther from the nucleus than 3s and 3p (and hence do not constitute another shell as the 4s electrons do), they are thoroughly shielded from the nuclear charge and thus often act as valence electrons. Hence, the electron dot configuration is otherwise popular with the names Lewis diagram or Lewis structure or Lewis Electron Dot Diagram in his honour. Writing electronic configurations for the elements present in the initial periods and groups of the periodic table is easy and simple. Number of electrons that can be in 3p orbitals? For example, iodine is a representative element in the fifth period. Keeping the uncertain behaviour of electrons in mind, our scientists discovered different energy levels around the nucleus of an atom. Francium is a radioactive element with very low half-life. (Choose two.) a) Nb, element number 41, is found in the fifth period and in a region of the periodic table where a d subshell is filling (the second transition series). 49. Correlate the valence orbital of an atom with the atom's placement on the periodic table. Valence electrons and ionic compounds. So, the order of filling of the electrons goes this way: 1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,4f,5d,6p,7s. So, 1 refers to the first shell, 2 the second shell, and so on. But writing electronic configuration of elements in the periodic table that come after noble gas group is lengthy and tedious. The values = 0, 1, 2, 3 correspond to the orbitals s, p, d, and f, respectively. 3. Electronegativity - yes. Taken together, the lanthanoids and actinoids are called inner transition elements because the f subshells being filled lie so deep within the remaining electronic structure of their atoms. Paramagnetism and diamagnetism. The values remains between zero and n-1 while depending on the values of principal quantum number. Essentially, this notation means that the electron configuration of calcium is equal to the configuration of Argon, the noble gas from the preceding period, plus the valence electrons of calcium (4s). The first example occurs in the case of the lanthanoids (elements having atomic numbers between 57 and 71).The lanthanoids have the general electron configuration. This module explains the arrangement of elements in the period table. For example, consider the alkaline-earth elements (group IIA). Identify the neutral element represented by this excited-state electron configuration, then write the ground-state electron configuration for that element. Want other step-by-step guides to drawing bonds? Similarly, the notation for helium (He) is 1s because helium has 2 electrons in the s orbital of itsfirst shell. Electron configuration can be defined as the distribution of electrons across the orbitals of an atom. The fact that the 4s electron cloud is more extensive than the 3d has an important influence on the chemistry of the transition elements. So, we can say that every subshell is assigned an Azimuthal quantum number, and for every subshell we have a corresponding symbol in order to designate the subshell. S, P, D and F are the four different atomic orbitals located around the nucleus of an atom with different energy levels. To make it easy and convenience to write, we can write the electronic configuration of Aluminium using noble gas notation as [Ne] 3s2 3p1. did mike boone lone star law retire Menu. Required fields are marked *. In an atom of copper, 1 electron from the 4s orbital migrates to the 3d orbital, leaving a half-filled 4s orbital. The electronic configuration of an element is defined as the arrangement of electrons in the orbital of the subshells of the atom. To determine the electronic configuration of an element, one must follow three important principles from quantum mechanics. A set of three rules can be used to determine the electron arrangement of 90% of the elements. by. Atomic Structure and Electron Configuration - AP Chemistry Sign In Tutor Bios Test Prep HIGH SCHOOL ACT Tutoring SAT Tutoring PSAT Tutoring ASPIRE Tutoring SHSAT Tutoring STAAR Tutoring GRADUATE SCHOOL MCAT Tutoring Atomic structure and electron configuration. e) Ar. Li 1s22s1. Students will love learning from this step by step activity that will increase their accuracy, inspire collaboration, and will create a fun learning environment.There are two versions depending on the level of prep time you have:A nearly no prep version-You will need to print game boards and score cards. As the name proposes, n is the chief energy level where the electron is easily detectable. They have opposite spins. Accordingly, the s, p, d, and f subshells can have a maximum of 2, 6, 10, and 14 electrons, respectively. All of the tables will print on a single 8 x 11 page, though some may require color to retain their appearance. Electron configuration Chart Template is a type of code that describes how many electrons are in energy level of atom. These shells, in turn, have orbitals regions of the shell where electrons inhabit. In the first period the distinguishing electrons for H and He are in the 1s subshell. Therefore, it can bond to oxygen atom using double bond. Thus in the building-up process for the lanthanoids, electrons are being added to a subshell (4f) whose principal quantum number is two less than that of the outermost orbital (6s). The atoms of elements in the same vertical column of the table have similar electron configurations. The value of n, the principal quantum number for the distinguishing electron, can be quickly determined by counting down from the top of the periodic table. Well, using the periodic table, anyone can easily write the electronic configuration of any element. You might have observed the standardized notation while writing electron configuration. Bohr observed that bursts of energy emitted from hydrogen atoms, visible as light, only occurred at specific wavelengths. This Jekyll and Hyde behavior of 3d electrons makes life more complicated (and often far more interesting) for chemists who study the transition elements. Which of the following properties is not shown by Z? So, 1st shell, n=1 has 1 subshell i.e. However, Hunds rule strictly follows the theory of atomic spectra. We have grown leaps and bounds to be the best Online Tuition Website in India with immensely talented Vedantu Master Teachers, from the most reputed institutions. 2022 Science Trends LLC. Group 3: Possibility of 3 valence electrons, Group 4: Possibility of 2-4 valence electrons, Group 5: Possibility of 2-5 valence electrons, Group 6: Possibility of 2-6 valence electrons, Group 7: Possibility of 2-7 valence electrons, Group 8: Possibility of 2-3 valence electrons, Group 9: Possibility of 2-3 valence electrons, Group 10: Possibility of 2-3 valence electrons, Group 11: Possibility of 1 or 2 valence electrons, Group 12: Possibility of 2 valence electrons. The electron configuration of an atom is 1s 2 2s 2 2p 6. And then they can start double occupying of orbitals of subshell. mri resident connect login 1) Find out the element symbol using periodic table. For example, consider the alkaline-earth elements (group IIA). Have a look! 1) Choose an element and write its electronic configuration. For ex: If the value is 0, then it represents the s orbital; = 1, then it is p orbital; = 2, it is f orbital and if = 3, it is f orbital. the total no. The tendency for an electron to fill in its lower level orbitals before higher-level ones is sometimes referred to as the Aufbau principle. Selenium has an atomic number of 34, and therefore has 34. The leftmost peak represents the two electrons in the filled 1s subshell. The notation for carbon (C) is 1s2s2p as carbon has 2 electrons in the s orbital of the first shell, two electrons in the s orbital of shell 2, and 2 electrons in the p orbital of shell 2. And because of these repulsive forces among the likely charged electrons, the electrons scatter in different patterns around the nucleus of an atom. The chart offers all the information in little space which needs to be understood. 8. Electrons will fill orbitals in a specific order. An electron configuration chart gives information about the orbital structure of the elements and how those orbitals are filled with electrons. Well, atomic orbitals are nothing but the energy quantum states that tell the uncertain behavior and exact location of an electron in the electron cloud. Hence there is a slow but steady transition in properties from one transition element to another. Why is electronic configuration important? Each shell is separated by a full stop or a comma. That is, the number of electrons in cadmium is forty-eight. The atomic number tells you how many electrons to draw in total. { "5.01:_Prelude_to_Electronic_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.02:_Electrons_and_Valence" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.03:_Lewis_Diagrams" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.04:_The_Wave_Nature_of_the_Electron" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.05:_Wave_Mechanics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.06:_The_Uncertainty_Principle" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.07:_Electron_Waves_in_the_Hydrogen_Atom" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.08:_Orbitals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.09:_Quantum_Numbers_(Electronic)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.11:_Potential_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.12:_Electron_Density_and_Potential_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.13:_Atoms_Having_More_Than_One_Electron" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.14:_Hydrogen_Helium_Lithium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.15:_Beryllium_Boron_Carbon" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.16:_Electron_Configurations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.17:_Electron_Configurations_and_the_Periodic_Table" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Introduction_-_The_Ambit_of_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_Molecules_and_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Using_Chemical_Equations_in_Calculations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_The_Structure_of_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_The_Electronic_Structure_of_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Chemical_Bonding_-_Electron_Pairs_and_Octets" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Further_Aspects_of_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Properties_of_Organic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Solids_Liquids_and_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Reactions_in_Aqueous_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Chemistry_of_the_Representative_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Ionic_Equilibria_in_Aqueous_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Thermodynamics-_Atoms_Molecules_and_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Entropy_and_Spontaneous_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Electrochemical_Cells" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Chemical_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Nuclear_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Molecules_in_Living_Systems" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_Spectra_and_Structure_of_Atoms_and_Molecules" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "22:_Metals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 5.17: Electron Configurations and the Periodic Table, [ "article:topic", "periodic table", "representative element", "transition metal", "electron configuration", "valence electron", "Lewis diagram", "distinguishing electron", "transition element", "lanthanoid", "actinoid", "authorname:chemprime", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FBook%253A_ChemPRIME_(Moore_et_al.