Full and abbreviated electron configuration of silver?
The correct e⁻ configuration for Ag is [Kr] 4d^10 5s^1 I'll let you do the long form. http://en.wikipedia.org/wiki/Silver Wikipedia has for some time had the e⁻ configurations correct, that is, 4d < 5s (see below). The reason that the 4d^10 is completely filled is because of a quantum mechanical effect know as spin exchange but for you there is extra stability associated with a completely filled d shell. Why is 4d < 5s? Go to SHRIVER and ATKINS, Inorganic Chemistry 4th ed (2006: note 4th ed and it has ten authors, so any mistakes at the fundamental level have probably been corrected). Fig 1.22 (p 20) shows that except for K and Ca the 4s AO is ALWAYS [my caps] higher in energy than the 3d AOs BUT (p 22): “the determination of actual ground states by spectroscopy and calculation shows that is advantageous to occupy orbitals predicted to be HIGHER in energy (the 4 s orbitals). The explanation for this order is that the occupation of orbitals of higher energy can result in a reduction in the repulsion between electrons that would occur if the lower energy 3d were occupied.” I have known about this since 1978: 4s is always above 3d! F. L. Pilar, J. Chem. Ed. 1978, 55, 2. For anyone who would like to delve into this perennial problem in more detail go to: "The Nature of the Bonding in Transition Metal Compounds," G. Frenking, N. Frohlich, Chem Rev 2000, 100, 717 (in particular 720-721). I am surprised that my learned colleague is not up with current theory as he is with hybridization.
Abbreviated electron configuration for Sb?
The full configuration is : 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3 This is too long so you have to look at the most previous noble gas (the first noble gas with an atomic number lower than Sb). This is Kr. So Kr's electron configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6. So you can write Sb's configuration as [Kr] 5s2 4d10 5p3 Hope I helped!!
Abbreviated electron configuration for cobalt?
I'm not really familiar with the terms unabbreviated and abbreviated. There are three common forms of electron configurations. The first is orbital notation, where you write the blanks for each orbital. The second is shorthand for the first and you just write the orbitals with superscripts with the numbers of electrons. Na - I can't draw arrows but there should be an up and down arrow above each number representing electrons except for 3s has only one. __...__... __..__..__.. __ 1s ... 2s......... 2p...... 3s Abbreviated would be 1s^2 2s^2 2p^6 3s^1
What's the difference between complete and abbreviated electron configuration?
The complete is starting at the first orbital 1S2 until you reach the right element. Abbreviated electron configuration starts at the noble gas just before the element. So Si instead of starting with 1S2 could be abbreviated by starting with the electron configuration of Ne (written "[Ne]" and then just start with the rest of the orbitals following Ne until you reach Si.
What is the complete electron configuration of rubidium?
For the best answers, search on this site https://shorturl.im/aD3C1 the complete ground state electron configurations for.... the order of filling orbitals in electron configurations goes like this: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6 Take the atomic number, (number of protons) this will equal the number of electrons in a neutral atom. Start with 1s2 and fill until you've depleted all of the electrons. There may not be enough electrons to complete the last orbital for example in Pb. lithium 1s2 2s1 (3 electrons) oxygen 1s2 2s2 2p4 (8 electrons) calcium 1s2 2s2 2p6 3s2 3p6 4s2 (20 electrons) titanium 1s2 2s2 2p6 3s2 3p6 4s2 3d2 (22 electrons) rubidium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 (37 electrons) lead 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2 (82 electrons) erbium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f12 (68 electrons) and the abbreviated ground state electron configurations for these.... helium same as ground state: 1s2 (no abbreviated ground state ec for this element) nitrogen [He] 2s2 2p3 chlorine [Ne] 3s2 3p5 iron [Ar] 4s2 3d6 zinc [Ar] 4s2 3d10 barium [Xe] 6s2 polonium [Xe] 6s2 4f14 5d10 6p4 to check: count the number of electrons each noble gas gives and add it to the superscripts in the rest of the electron configuration. For example, iron: [Ar] 4s2 3d6: 18 + 2 + 6 = 26 electrons
Can someone help me with these electron configurations...Please?
this periodic table gives electronic configurations. http://www.dayah.com/periodic/ click on the orbitals tab. Rb is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 since Kr, the next lower noble gas is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 we can abbreviate Rb as [Kr] 5s1 ******** Fe full... 1s2 2s2 2p6 3s2 3p6 4s2 3d6 Fe abbr...[Ar] 4s2 3d6 I full... 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5 I abbr..[Kr] 5s2 4d10 5p5 ************* now obviously you wont have this periodic table during a test. So you need to learn this material... so I suggest you do this... 1) spend some time clicking around the table and watch how orbitals fill 2) note that rows for s and p orbitals (the left two columns and right 6 columns) match up with the s and p electrons... 4s2 is 4th row..etc 3) note that d orbitals ( the center 10 columns) are shifted 1 row down. 4th row = 3d electrons. 4) note that f orbitals are shifted 2 rows 6th row = 4f electrons 5) note that as you go left to right across a particular type of electron (from Sc to Zn for example) electrons first fill each empty orbital then pair up. 6)... finally... note exceptions... all elements in the Cr and Cu columns borrow an s electron to either half fill or completely fill the d electrons.. this is always the case and it's due to energy.. half filled d orbitals are lower energy.. etc Pd.. borrows both s electrons. note what happens with elements 58 to 65 and 90 to 97
Write the complete electron configuration for germanium and the shorthand notation for the electron configurat?
This Site Might Help You. RE: Write the complete electron configuration for germanium and the shorthand notation for the electron configurat? configuration is the word that was cut off. PLEASE HELP!!!!