The following Lewis diagram represents the valence electron configuration of a main-group element. The element in period 3 that has this valence electron congfiguration is 1A 8A H 2A 3A 4A 5A 6A 7A He Li Be B C NO F Ne Na Mg 3B 4B 5B 1B 28 A1 Si P S CI Ar 6B 7B 8B H K Ca sc Ti v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn Fr Ra Ac Rf Ha Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

The following Lewis diagram represents the valence electron configuration of a main-group element. The element in period 3 that has this valence electron congfiguration is 1A 8A H 2A 3A 4A 5A 6A 7A He Li Be B C NO F Ne Na Mg 3B 4B 5B 1B 28 A1 Si P S CI Ar 6B 7B 8B H K Ca sc Ti v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn Fr Ra Ac Rf Ha Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which of these ions is the largest? Ga3+ Li+ Mg2+ K+
Determine the systematic name for CaSO4 Atomic numbers: Ca = 20, S = 16, O = 8
Explain why it is possible to determine the charge of monoatomic ions from their position on the periodic table for s-block metals and p-block nonmetals.
Which of the following combination of elements is the most reactive? Cs and I Na and Br Cs and Br K and I
13. Below, the ionic radii of several ions are shown relative to the radius of neutral atoms of the same element. Na" 2+ Mg Na Mg F CI 154 pm 116 pm 130 pm 86 pm 71 pm 119 pm 99 pm 167 pm Explain why the ions in the diagram on the left are smaller than their neutral counterparts, while the ions in the diagram on the right are larger than their neutral counterparts.
Pls help on this question. Pls explain in detail and do it ASAP.
In the Periodic Table below, shade all the elements for which the neutral atom has a valence electron configuration of ns²np5, where n stands for an integer. H Li Be Na Mg K Ca Sc Rb Sr Y Cs Ba La Fr Ra Ac B C Al Si P Ge As Ti V Cr Mn Fe Co Ni Cu Zn Ga Zr Nb Mo Tc Ru Rh Pd Ag Cd In Hf Ta W Re Os Ir Rf Db Sg Bh Hs Mt He OF Ne S Cl Ar Se Br Kr Sn Sb Te I Xe Pt Au Hg Tl Pb Bi Po At Rn Ds Rg Cn H
In the Periodic Table below, shade all the elements for which the neutral atom has a valence electron configuration of ns“, where n stands for an integer. Не BCNOF Ne H Li Be Na Mg Al Si P S c1 Ar к Са Sc Ti V Cr Mn| Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Te Ru Rh Pd Ag Cd In Sn Sb Te I Xe Hf Ta W Re Os Ir Pt Au Hg T1 Pb Bi Po At Rn Rf Db Sg Bh Hs Mt Ds Rg Cn Cs Ba La Fr Ra Ac
How many electrons are in the most likely ion formed from an atom located in group 5A and period 3? O 12 O 16 18
The electron configuration of an element, X, is [Ne] 3s¹. The formula of the most probable ionic compound that this element will form with Br is Note: The compound Fe(CIO4)3 should be entered as "Fe(CIO4)3".
Given the following enthalpy values for Na and Cl, calculate the lattice energy of NaCl using the Born- Haber cycle. for Na = 107.5 kJ/mole for Na = 495.8 kJ/mole for Cl, = 242.6 kJ/mole AHO sublimation AH ionization energy AHO dissociation energy ΔΗΡ electron affinity TOr Cl, = -348.6 kJ/mole AH formation for NaCl(s) = -4l1.2 kJ/mole
Use the data table for the first eight ionization energies of a particular element shown below to predict and explain which element you would expect to show this trend in successive ionization energies. Ionization Number 1st 2nd 3rd 4th 5th 6th 7th 8th I.Fluorine 1. I and III 2. II and III 3. I and IV 4. II and IV 04 02 O 3 Ionization Energy (kJ/mol) 0 1 1,314 3,388 5,300 7,469 10,990 13,327 II.Oxygen Because III.core electrons are more strongly attracted to the nucleus than valence electrons. IV.valence electrons release more energy when they are removed from the atom. 71,330 84,078