Q: Which of the following electron configurations is correct for nickel? O a. (Ar] 4s 3a8 O b. [Kr] 45'…
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A: O2+ ->Atomic number of O = 8 Number of electrons in O2 = 16 Number of electrons in O2+ = 15
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Write the full electron configuration of the ion oxide, O2-
You can indicate superscript through the ^ symbol (e.g. 3s2 could be written as 3s^2) or use the superscript text formatting tool above.
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- Write the full electron configuration of the ion oxide, O2- You can indicate superscript through the ^ symbol (e.g. 3s2 could be written as 3s^2) or use the superscript text formatting tool above.People Tab Window Help d Tap - Cengage Learning vo/index.html?deploymentld%3D55750828934189288909969212&elSBN=9781305657571&nbld%3D2199 NDTAP Use the References to access important values if needed for this question. Predict the larger ion in each of the following pairs. (a) Br or Rb+ (b) Co+ or Co2+ (c) Sor S2- (d) I or BrIf possible attempt to ionize Rb by pulling a valence electronfrom the electron shell. Describe what happened. (Were you successful? Was it “easy” to remove the electron? Did the atom seem to have a strong hold on the electron?)
- 17. a) How many valence electrons are there in an atom of each of these elements? neon; bromine; sulfur; strontium; sodium; chlorine; tin; magnesium; silicon. b) Draw the Lewis structure for the elements in a) above. c) Without consulting a periodic table, classify each element from a) above as metal, non-metal or metalloid.Indicate which choice is the best explanation for the following factual statement: the IE1 of lithium is lower than the IE1 of helium. A) The thrid electron in lithium goes into a new shell further away from the nucleus. This shell will be easier to remove an electron from, and therefore the IE1 is lower. B) The third proton pulls on the extra electron harder, thus lowering the IE1. C) Extra electrons always increase the electron-electron repulsion so the IE1 simply goes down. D) None of the abovea) Write the electronic configuration in s, p, d, f and K L M N, for the atom which belongs to period 5 and cannot form the ions? b) Mention the number of electrons and neutrons of the above atom. c) What is the volume (in ml) of a 0.2 M AgNO3 solution containing 8.5 grams of AgNO3?
- A districtims.seattleschools.org/common-assessment-delivery/start/4777996531?action3Donresume&submissionld%3D464527652 Below is a picture of the first three groups on the periodic table. 1. Draw a "circle" around the element with the strongest attractive force between the proton(s) and electron(s). 2. Draw an "X" over the element with the weakest attractive force between the proton(s) and electron(s). x Clear A Undo A Redo H. 37 Li 152 Ве 111 80 74 73 7. Na 186 Mg 160 Al Si 118 143 110 103 10 1. 3. エ11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).Use the periodic table to (i) predict electron configurations for the following species: Arsenic ion, As3– Magnesium ion, Mg2+ Vanadium(II) ion, V2+ (ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above. Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule. CS2 and H2S CF4 and SiH4 NH2Cl CO32– and BF3 PCl5 ClF3, XeF2, Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched) Give the electron-pair and molecular geometries for NF3 and XeF4.
- 1) give the electron configuration, (not condensed or orbital) for the imaginary ion Ge^-2 3) give the electron configuration, (not condensed or orbital) 7) what would the electron configuration of nickel look like if the quantum theory was the exact same as ours now except that each orbital was able to hold three electrons instead of two? What would the most stable ion of nickel look like and why would it be stable?What is the zeff, atomic radius, and ionization energy of Arsenic?Draw the Lewis Dot Structure for MeS2. Me is a ficticious element with 4 valence electrons.