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Slav-nsk [51]
2 years ago
7

As you move down a group, you will recall that the radius increases. Why do you think an increase in atomic radius would result

in a lower ionization energy?
Chemistry
1 answer:
Assoli18 [71]2 years ago
8 0

Answer:

Because as we move down the group size/ radius of atom increases due to increase in shells and screening effect. The hold of nucleus on valence electrons decreases and effective nuclear charge decreases so it is easy to remove electron from greater sized atoms as compared to smaller sized aroms.

Energy required to remove electron is ionization energy so greater sized atoms have low ionization energy.

Explanation:

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3 years ago
Tin reacts with Fluorine to form two different compounds, A and B. Compounds A contains 77.0 g tin for each 24.6 g of fluorine.
Ratling [72]
A contains 38.5 g of tin for each 12.3 g of fluorine: 
<span>mole ratio: </span>
<span>(38.5 g)/(118.71 g/mol):(12.3 g)/(18.998 g/mol) = 0.324:0.647 = 1:2 ⇒ SnF₂ </span>

<span>B contains 56.5 g of tin for each 36.2 g of fluorine: </span>
<span>mole ratio: </span>
<span>(56.5 g)/(118.71 g/mol):(36.2 g)/(18.998 g/mol) = 0.476:1.905 = 1:4 ⇒ SnF₄

Thank you for posting your question here at brainly. I hope the answer will help you. Feel free to ask more questions.


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What graph would you use if you wanted to compare similar data for several individual items or events?
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Explanation:

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