the covalently bound D2d structure, both of which have electronic configurations consistent with electron attachment to the LUMO of the neutral van der Waals dimer. the electron configuration of a neutral calcium atom and then from that, we can take two of the highest energy electrons away. over here if you can see it. Determine the expected electron configuration of an element by its place on the periodic table. Why would an element need to be stable? Oxygen has the atomic number 8, which means the nuclei of its atoms have 8 protons. while isotopes are the same element with the same number of protons and different mass because of the neutrons is that right? Since 1s can only hold two electrons the next 2 electrons for sulfur go in the 2s orbital. so basing on my understanding of this so far, an atom is an element that has the same number of protons and neutrons, an ion is an element that has different numbers of protons and electrons, an ion is positive when it has more protons than electrons and negative when it has more electrons than ions . Direct link to abrokensha's post Just wondering if it's po, Posted 6 years ago. Its electron structure is 2, 8, 8, 1. Direct link to Adhithi Sriram's post so an element is only an , Posted 6 years ago. 2.7.1: Atomic Models of the Twentieth Century, status page at https://status.libretexts.org. They have the same number of electrons, but different electron structures. The maximum number of electrons in each shell, going from the middle to the outside, is 2, 8, 8, 18. This number defines the sulfur atom as a sulfur atom (i.e if there were 17 protons, the atom would be chlorine). Neutral boron would have five The acid with the least acidity will have the most basic conjugate base. And next we got to the 2p sub-shell. So then we go to 2s two. These two elements make up the first row of the periodic table (Figure 2.8. Its various salt forms and minerals play numerous roles as chemical reagents, industrial . Likewise, what would be the electron configuration of a sulfur ion S 2s 2? For the Cu+ ion we remove one electron from 4s1 leaving us with: 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10. This you would now call an ion because it has that net charge. Can atoms gain/lose electrons themselves? two electrons occupy the first shell eight electrons occupy the second shell one electron occupies the third shell This electronic structure can be written as 2,8,1 (each comma, or dot,. For the Cu+ ion we remove one electron from 4s1 leaving us with: 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10. For example: Sodium (2,8,1) loses its outer electron and forms a Na + ion (2,8). Carbon-13, which has an atomic mass number of 13, has 7 neutrons (13 nucleons - 6 protons = 7 neutrons). To write the electronic structure for Cl -: To write the electronic structure for O2-: To write the electronic structure for Na+: To write the electronic structure for Ca2+: Here you are faced with one of the most irritating facts in chemistry at this level! Oxygen has the atomic number 8, which means the nuclei of its atoms have 8 protons. Similar questions. The configuration notation provides an easy way for scientists to write and communicate how electrons are . It is going to have six electrons and that's what makes it neutral. But the big idea is, and we Alright, so let's think The fluorine has nabbed on our periodic table. To bond the four chloride ions as ligands, the empty 4s and 4p orbitals are used (in a hybridised form) to accept a lone pair of electrons from each chloride ion. Electrons that are closer to the nucleus slightly repel electrons that are farther out, offsetting the more dominant electron-nucleus attractions slightly (recall that all electrons have 1 charges, but nuclei have + Z charges). Now you could have a carbon ion, although they aren't that typical. of carbon has six protons. Atoms and atomic ions with sequences of completely filled electron shells exhibit enhanced stability. For ""^32S^(2-), there are 16 protons, 18 electrons, and 16 neutrons. An atom that has the maximum number of electrons in its outer shell will be stable. Well remember, protons define what element you're dealing with, so now if you look at what Fluoride ions are found in various minerals but are only present in trace amounts in water. The K + ion is isoelectronic with the Ca 2+ ion. A Mg 2+ ion has the same electron structure Glasses containing transition metal (TM) ion give the information of site symmetry around the Cu +2 ion of the host glass. neutral fluorine atom's electron configuration would be. Of these, 1.6.5 Metallic Bonding & Lattices. Administration (OVPR) Research output: Contribution to journal Article peer-review. 3. Negative ions called cations form as if an atom gains electrons it now has more electron than protons that means there is not a balanced number of . A Cl-ion has the same electron structure as . Solve any question of Structure of Atom with:-Patterns of problems > Was this answer helpful? when calculating for a positively charged atom does it gain protons or loose electrons, like does an ion depend on the number of electrons gained and lost in a neutral atom. So as we know that the Okay Plus iron and it's just a potassium atom and they eat his has won electron. VIEW SOLUTION . Magnesium ion | Mg+2 | CID 888 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety/hazards/toxicity information, supplier lists, and more. A Li + ion has the same electron structure as Helium. So we're dealing with platinum. Does that help? in ions number of electron is less or more but in an isotope it is the number neutrons that varies, http://www.popsci.com/sites/popsci.com/files/styles/large_1x_/public/periodic_table_large.jpg?itok\x3d0gYVEwsY\x26fc\x3d50,50, Creative Commons Attribution/Non-Commercial/Share-Alike. The electrons in the highest-numbered shell, plus any electrons in the last unfilled subshell, are called valence electrons; the highest-numbered shell is called the valence shell. The same concept applies to the other columns of the periodic table. to another. This means that it will not react with other atoms. n,-n /) is an atom or molecule with a net electrical charge.. An electron charge density in the region of an oxygen vacancy reduces, at the nearest-neighbour O 2 ions, the screening of the O 2 (1s) electrons from their nucleus thus raising the effective nuclear charge Z eff, i.e., the binding energy, of an O II 2 (1s) electron relative to that of an O I 2 1s electron. 0. And if it is neutral carbon it is going to have the Direct link to ysuzette's post I think adding a video on, Posted a year ago. We investigate theoretically the electronic structure of (CS2)2-. two electrons occupy the first shell eight electrons occupy the second shell one electron occupies the third shell This electronic structure can be written as 2,8,1 (each comma, or dot, separates. For a neutral atom, if there are 16 positive nuclear charges, there must . However, most of NASICON-type cathode materials exhibit redox reaction of no more than three electrons per formula, which strictly limits capacity and energy density. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1. Up there when we talked electrons or more protons, and this is true of an atom or a molecule, we will then call it an ion. Question 9. So we're still dealing with carbon, but now we have one more positive charge than we have a negative charge. What do we know about State (i) Valency of each element (ii) which one is a metal (iii) which is non-metal (iv) which is an inert gas . { "2.01:_Introduction_to_Atoms_and_Molecules" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.02:_Basic_Atomic_Theory" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.03:_Atomic_Theory" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.04:_Indivisible_-_The_Atomic_Theory" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.05:_Isotopes_and_Atomic_Mass" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.06:_Quantum_Numbers_for_Electrons" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.07:_Organization_of_Electrons_in_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.08:_Electronic_Structure_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_to_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms,_Molecules,_and_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Periodic_Table_of_the_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Introduction_to_acids_and_bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Solids_and_Liquids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Radioactivity" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Chemical_Bonds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Organic_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Biochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Solids,_Liquids,_and_Gases,_Solutions_and_energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_The_Chemical_Equation" : "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]()" }, 2.8: Electronic Structure and the Periodic Table, [ "article:topic", "periodic table", "subshell", "valence electrons", "s block", "p block", "f block", "d block", "showtoc:no", "electron configurations", "Electronic Structure", "chemical elements", "license:ccbyncsa", "transcluded:yes", "source[1]-chem-64055", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FBridgeValley_Community_and_Technical_College%2FConsumer_Chemistry%2F02%253A_Atoms%252C_Molecules%252C_and_Ions%2F2.08%253A_Electronic_Structure_and_the_Periodic_Table, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Food and Drink Application: Artificial Colors. to figure this out is first we could figure out Among the following series of transition metal ions, the one where all metal ion have the sae 3d electronic configuration is . Direct link to Ryan W's post Another atom or molecule , Posted 6 years ago. Theoretical explanation should start with the structure of ruby crystal. All these films were polycrystalline and exhibit a single-phase orthorhombic structure with space group pbnm.Atomic force microscopy (AFM) studies revealed that surface roughness and grains size decreases with . Answer (1 of 6): Element X will donate all the 3 electrons in its valence shell. of protons and electrons. questions on electronic structures of ions. However because electrons are transferred frequently we can have two particles with the same electron configuration, but from different elements. has nine electrons, and we could just use our Think the K plus and I minus signs have electronic structure debt are identical to which two interfaces. Lithium has an electronic structure of 1s 2 2s 1. For instance, if you combined Magnesium Ion, Mg 2+ and Phosphate Ion, PO 4 3-, to balance the charges you would need 3 magnesium ions and 2 phosphate ions: Mg 3 (PO 4) 2 The parenthesis are placed around the polyatomic ion to indicate that the subscript creates a multiple of the entire ion not just a single atom. All ions have electronic structure of a noble gas, and that was the reason why these atoms form ions-to be stable. So as we know that the Okay Plus iron and it's just a potassium atom and they eat his has won electron. Think the K plus and I minus signs have electronic structure debt are identical to which two interfaces. Five different low-lying forms of the anion are identified. Are there 18 electrons in the third shell or 8 and if there are 18 electrons in the third shell why do we only fill it up to 8. Cyanoimine derivatives of planar diquinones were synthesized and studied by electrochemical methods. 1.7 Covalent Bonding & Structure. Arthur H. Winter, Daniel E. Falvey, Christopher J. Cramer. An atom is stable if the outermost shell contains the maximum number of electrons. The ground state electron configuration of ground state gaseous neutral silver is [Kr].4d 10.5s 1 and the term symbol is 2 S 1 / 2. I'll say N for neutrons is equal to 195. little bit of practice, try to pause this video and think about what is since the postive charged Ca ion has the same configuration as Ar does that mean that the Ca ion is now considered Ar?? (b) How does the electronic configuration of the atom of an element relate to its position in the modern periodic table? These levels all have the same energy, and so the electrons go in singly at first. (d) Is it possible to have an element having atomic number 1.5 placed between hydrogen and helium? does this mean you can't differentiate between atoms just by their electron configuration? Glasses containing transition metal (TM) ion give the information of site symmetry around the Cu +2 ion of the host glass. Direct link to skippyjoe13's post Protons are just our name, Posted 6 years ago. electrons you no longer would call it an atom, you would Correct option is D) M n 2 + = [A r] 4 s 0 3 d 5 does not have noble gas configuration. has a negative charge. septum surgery yesterday. Lithium's electron goes into the 2s orbital because that has a lower energy than the 2p orbitals. For a neutral atom, if there are 16 positive nuclear charges, there must . (f) Z belongs to the noble gases group or the zero group of the periodic table. So when sodium fluoride is in water, the water molecules essentially separate the sodium cations and fluoride anions from each other and they exist as individual ions. The actual electron configuration for copper will move one electron from the 4s sublevel into the 3d sublevel resulting in The oxidation state of the metal is . Elements from group 3 across to the noble gases all have their outer electrons in p orbitals. A Mg 2+ ion has the same electron structure (For example, H 2 O has 2x1 + 6 = 8 valence electrons, CCl 4 has 4 + 4x7 = 32 valence electrons.) The elements are listed by atomic number (the number of protons in the nucleus), and elements with similar chemical properties are grouped together in columns. Well, we still have six protons. The nucleus of a sodium ion is the nucleus of a sodium atom and has 11 protons. Yes. Updated On: 21-6-2020. These are then described as p-block elements. In other words, there is an imbalance in the number of protons (positively charged particles) and electrons (negatively charged particles) in a chemical species. about electron configuration and now in this video we're going to extend that understanding by thinking about the electron And 195 looks pretty You could do this as a neutral calcium that has lost two electrons. Isoelectronic chemical species typically display similar chemical properties. Elements in groups 1 and 2 are described as s-block elements. STRUCTURE OF ATOM. And we are going to have, we're talking about a neutral fluorine, we are going to have one two Insert yet another electron, and we'd have 3px^1 3py^1 3pz^1. of argon and no 4s two. We add electrons to fill the outermost orbital that is occupied, and then add more electrons to the next higher orbital. Posted 6 years ago. So you could write this as There are two types of food colorings: natural and artificial. noble gas configuration. Therefore the compound formed will have the formula XY_3. Electron configurations for the second period. And so the electron configuration here for calcium with a positive two charge, this calcium cation, is going to be the electron configuration All ions have electronic structure of a noble gas, and that was the reason why these atoms form ions-to be stable. It can happen where an element loses a proton because it is unstable, that is what we call radioactive decay. So the fluoride anion is going to have an electron configuration H and He represent the filling of the 1s subshell. configuration of ions. But we're not done answering the question. Just wondering if it's possible to get access to this copy of the periodic table? is if you don't have an equal amount of protons and electrons. The parentheses are only used . So I will leave you there, The electron configuration of Li is, 1s2 2s1. Legal. Working out the electronic structures of ions. Many processed foods have food colorings added to them. . All ions have electronic structure of a noble gas, and that was the reason why these atoms form ions-to be stable. These include the representative elements of Groups I, II and III in the Periodic Table, which have respectively 1, 2 and 3 electrons more than a neighboring inert gas, and the representative elements of 30 Scopus citations. The room temperature electron paramagnetic resonance (EPR) and optical absorption studies of PbO-Li 2 O-As 2 O 3-B 2 O 3 glasses have been done by introducing a transition metal ion Cu +2 ion as a spin probe with fixed mole% in the given glass composition. The atomic number, Z, specifies the number of protons, positively charged, massive, fundamental particles present in the sulfur nucleus. So you can write it like this, one minus. These are then described as p-block elements. To bond the four chloride ions as ligands, the empty 4s and 4p orbitals are used (in a hybridised form) to accept a lone pair of electrons from each chloride ion. These include the ionmolecule complex and a covalently bonded dimer anion, both of which have electronic configurations consistent with electron attachment to the LUMO of the van der Waals dimer. Electrostatic attraction attraction between positively and negatively charged particles Ionic Bond electrostatic force of attraction between positively and negatively charged ions Covalent Bond the strong attraction between two non-metal atoms that share one or more pairs of electrons Delocalised Electrons electrons from an element's outer shell that is free to move through a structure . Many foods, such as tomatoes, are highly colored; in fact, the common statement "you eat with your eyes first" is an implicit recognition that the visual appeal of food is just as important as its taste. But if we have an element in the third row (or period) like sulfur or phosphorus, we're only going to fill up the 3s and 3p orbitals in their electron configurations because that's where their valance electrons are. Magnesium (2,8,2) loses its outer electrons and forms a Mg 2+ ion (2,8). Having a chemical formula of F, fluoride ion is the simplest inorganic, monatomic anion of fluorine with basic properties. Pause this video and try to figure it out. For the Cu2+ ion we remove a total of two electrons (one from the 4s1 and one form the 3d10) leaving us with. CH 3 COCH 3 and CH 3 N=NCH 3 are not isoelectronic. Colorless transparent single crystals and white polycrystalline powder samples of Pt2In14Ga3O8F15 were obtained by heating a mixture of stoichiometric amounts of Pt, In, InF3, and Ga2O3, in a Pt crucible under Ar at 600 C. Arthur H. Winter, Daniel E. Falvey, Christopher J. Cramer. Direct link to Icedlatte's post That is the basis of how , Posted 3 years ago. have two electrons in 1s. Since 1s can only hold two electrons the next 2 electrons for sulfur go in the 2s orbital. The two gained electrons (purple dots) means that this oxygen ion has 10 electrons (-10 charge) and only 8 protons (+8 charge), giving the ion a net charge of -2. The maximum number of electrons in each shell, going from the middle to the outside, is 2, 8, 8, 18. This means that its electron configuration should end in a p4 electron configuration. So you're going to have For transition metals, the last s orbital loses an electron before the d orbitals. Mass number (A) of helium = 4. An ion (/ a. Natural food colorings include caramelized sugar for brown; annatto, turmeric, and saffron for various shades of orange or yellow; betanin from beets for purple; and even carmine, a deep red dye that is extracted from the cochineal, a small insect that is a parasite on cacti in Central and South America. From the XRD diffraction patterns of (where ) one can observe the peaks of secondary cubic phase at , and .This phase, ZnFe 2 O 4, is a normal spinel with tetrahedral (A) sites occupied by Zn 2+ ions and octahedral (B) sites occupied by Fe 3+ and Fe 2+ ions [].In spinel structure Fe 3+ has ionic radius 0.55 (in octahedral coordination) matching that of Zn 2+ (0.6 in tetrahedral coordination . GoogleCookieCookie, How Much Does Sidney Crosby Make From Tim Hortons, keynesian beauty contest alice in borderland, e learning vs classroom learning informative speech. Consider Se, as shown in Figure \(\PageIndex{10}\). and Ions Ions When atoms lose or gain electrons, they become ions. Ions are atoms (or groups of atoms) which carry an electric charge because they have either gained or lost one or more electrons. Indeed, the electron configuration of Se is [Ar]4s23d104p4, as expected. To write the electronic structure for Zn2+: This time there is no need to use any of the 3d electrons. It belongs to a group called . Neon, Ne A neon atom (Ne) has the same electronic structure as a sodium ion. Isoelectronic refers to two atoms, ions, or molecules that have the same electronic structure and the same number of valence electrons.The term means "equal electric" or "equal charge". If it loses electrons, it becomes positively charged. Five different low-lying forms of the anion are identified. element has five protons we're dealing with boron. What is the. of 1s two, 2s two, 2p, now it's going to have an It's going to be equal to 195. We can use this method to predict the charges of ions in ionic compounds. everything around you wants to get as stable as possible because that means having potential energy as low as possible. Similarly, the p block is the right-most six columns of the periodic table, the d block is the middle 10 columns of the periodic table, while the f block is the 14-column section that is normally depicted as detached from the main body of the periodic table. So this is a boron ion right over here. A Mg 2+ ion has the same electron structure as a Na + ion and a O 2-ion. In order to categorize them according to their basic strength, we need to compare the acidity of the respective acids. The conformations of pure carbon cationic species have been previously reported as pure linear chains for n 6, mixed chains and . It could be part of the main body, but then the periodic table would be rather long and cumbersome. And I encourage you, In fact, if you want a It's odd because here in the high school chemistry section it's excluded (the extra material), but included in the AP chemistry section. has a mass number of 195 and contains 74 electrons. When these metals form ions, the 4s electrons are always lost first. Well, here you're now going A cation is an atom that has lost a valence electron and therefore has more positive protons than negative electrons, so it is positively charged. For anions, add one valence electron for each unit of negative charge; for cations, subtract one electron for each unit of positive charge. Posted 2 years ago. Once those 3s and 3p orbitals are filled, we'll have used 8 electrons. Valence electrons being the electrons that are important to chemical bonding. Atomic structure Electrical state. You have the six positive charges and the six negative charges. The corresponding structures of the valence isolectronic (CO2)2- ion are the only The photodissociation and theoretical results both indicate low-energy forms of that anion.13-16 that the most stable form of (CS2)2- contains a C2S2 ring and The remaining (CS2)2- structures, III-V, are cyclic. Electron configurations for the first period. 2p six. These species had electronic absorptions in the near infrared . For example, to find the configuration for the lithium ion (Li), start with neutral lithium (1s2s). D Protons 18 neutrons 22. That is a positive ion. Noble gas configuration. Write the distribution of electrons in carbon and sodium atoms. (That's rightyou may be eating bug juice!). Since 1 Y atom can only accept 1 electron therefore 2 more Y atoms will be required to take the remaining 2 electrons given by X. that one atom of carbon? The Electronic Structure of d-block Ions. Of these, 1.6.5 Metallic Bonding & Lattices. Explain with examples. Refer to the explanation. These include the ion-molecule complex and a covalently bonded dimer anion, both of which have electronic configurations consistent with electron attachment to the LUMO of the van der Waals dimer. Why are the apparently higher energy 3d electrons not the ones to get lost when the metal ionises? For example, take the elements in the first column of the periodic table: H, Li, Na, K, Rb, and Cs. Four more of the positive thing than you have of the negative things. (The inner electrons are called core electrons.) So this is going to be boron. Both the ions have the electronic configuration 2,8,8 S has electronic configuration 2,8,6 and when it forms S 2- ion it gains 2 electrons and so its electronic configuration will be 2,8,8. Direct link to Angelica Chen's post When dealing with chemist.
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