Use the electron configurations of the alkali metals to explain why they tend to form 1+ ions.
All alkali metals have the electronic configuration of ns1 .Take for example the electronic configuration of sodium is 1s22s22p63s1 then the sodium atom loses an electron it achieves an electronic configuration nearest to the noble gas configuration hence it becomes exceptionally stable . The electronic configuration hence achieved of Na+ ion is is very stable and it is very difficult to remove an electron further hence it usually shows an oxidation state of +1.
Use the electron configurations of the alkali metals to explain why they tend to form 1+ ions.
Use the electron configurations of the alkali metals to explain why they tend to form 1+ ions.
Explain why only alkali metals form solid stable hydrogen carbonate (bicarbonate) salts.
Why do Group 2 alkaline earth metals have a large positive electron affinity, while Group 1 alkali metals have a negative electron affinity? Use their electron configurations and box diagrams to support your answer.
Thank you so much for your help :) Chapter 7 Homeworlk Introduction to the Alkali Metals Part A Learning Goal: Predict the product(s) of the following reaction: The equation is not necessarily balanced. Express your answer as a View Available Hint(s) To be able to predict the products of some alkali metal reactions The alkali metals are in the first group of the periodic table and nclude lithium, sodium, potassium, rubidium, cesium, and francium. They all have the ns valence...
Electron Configurations of Ions Choose from the list the correct electron configurations for the following ions. NK+ c In+ F Be2+ A. 1s22s22p63s23p63010 B. 1s22s22p63s23p645230104p64010552 c. 152 D. 1822s22p63s23p63d10452 E. 1s22s22p63s23p64523d104p64d105525p1 F. 1922s22p 3s 3p6 G. 1822s22p5 H. 151 I. 1522s22p63523p6451 J. none of the above
8. Write the condensed electron configurations for each of the following ions. (The condensed electron configurations use the prior noble gas symbol enclosed in square brackets to depict the core electrons.) a) Cr3+ b) 52 Co2+,
Use your knowledge of electron configuration to explain the following observations: a) Silver tends to form ions with a charge of 1+, but the element to the right of silver in the periodic table tends to form ions with 2+ charge. b) The heavier elements of group 14 (Sn, Pb) tend to form ions with charge of 2+ and 4+.
The reactivity of the alkali metals increase going down the group; however, the reactivities of the halogens decrease going down the group. Why do the reactivities of these two groups differ? Hints: think about the ionization energy and electron affinity trends, and think about how cations and anions form.
Do I have the correct answer for the question below? Thank you for your time. Alkali metals tend to form ions with what charge? O +1 O +2 0 -1 0-2
Part A What is the general valence-electron ground-state electron configuration for neutral alkali metals? 1922s22p3 Ons 152251 ns2 Submit Request Answer Provide Feedback