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+...
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.
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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...
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.
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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
Electron configurations are not always 'predictable' from the periodic table Briefly explain why Cr and Cu have experimental electron configurations that differ from what is expected from the periodic table. Then explain why so many f block elements have ‘unusual’ experimental electron configurations.
What are the ground state electron configurations of the d-metals from yttrium to cadmium.