Across a period I.E increases progressively from left to right
Explanation:
The trend of the first ionization energy is such that across a period I.E increases from left to right due to the decreasing atomic radii caused by the increasing nuclear charge. This not compensated for by successive electronic shells.
- Ionization energy is a measure of the readiness of an atom to lose an electron.
- The lower the value, the easier it is for an atom to lose an electron.
- Elements in group I tend to lose their electrons more readily whereas the halogens hold most tightly to them.
- The first ionization energy is the energy needed to remove the most loosely bonded electron of an atom in the gaseous phase.
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Ionization energy brainly.com/question/6324347
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this is a lot sorry i can't help
Answer:
<em>I</em><em> </em><em>think</em><em> option</em> ( b) <em>tea </em><em>is</em><em> right</em><em> answer</em>
I think the correct answer from the choices listed above is the second option. The other true statement would be that the solution contains more hydronium ions than hydroxide ions. Since <span>pH = -log[H3O+]. As pH decreases, the acidity increases. Hope this answers the question.</span>
