Trends to Know

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DomMaiorca_1I
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Trends to Know

Postby DomMaiorca_1I » Sun May 06, 2018 6:08 pm

For the midterm, I know the important trends to know are atomic radii, ionic radii, and ionization energy. Are there any other trends I'm forgetting that we should definitely know? And if so, could you explain the trend?

MeghetyManoyan1A
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Re: Trends to Know

Postby MeghetyManoyan1A » Sun May 06, 2018 6:48 pm

There's the trend of electronegativity. As you move from left to right, electronegativity increases, and as you move from top to bottom, electronegativity decreases, with some exceptions.

Amanda 1A
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Re: Trends to Know

Postby Amanda 1A » Sun May 06, 2018 7:04 pm

what would the specific exceptions be or what trend do the exceptions follow? or are they not relevant to what we would need to know for the midterm?

Harmonie Ahuna-1C
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Re: Trends to Know

Postby Harmonie Ahuna-1C » Sun May 06, 2018 7:23 pm

Another trend is electron affinity. Electron affinity tells how how much energy must either be supplied (-) or is released(+) when an electron attaches to an atom. It generally increases as you move right and up along the periodic table. However, noble gases in group 18 have low ones because they're already stable. There may be some other exceptions shows on figure 2.28 on pg 56 of the textbook.

Shione Nakahara 1F
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Re: Trends to Know

Postby Shione Nakahara 1F » Sun May 06, 2018 9:30 pm

I think you should know how electron affinity increases from left to right within a period (caused by the decrease in atomic radius) and how electron affinity decreases from top to bottom within a group (caused by the increase in atomic radius).

hannahtweedy
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Re: Trends to Know

Postby hannahtweedy » Sun May 06, 2018 9:52 pm

All the ones listed so far are the only ones we went over in Step Up

Madeleine Farrington 1B
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Re: Trends to Know

Postby Madeleine Farrington 1B » Sun May 06, 2018 10:11 pm

Harmonie Ahuna-1C wrote:Another trend is electron affinity. Electron affinity tells how how much energy must either be supplied (-) or is released(+) when an electron attaches to an atom. It generally increases as you move right and up along the periodic table. However, noble gases in group 18 have low ones because they're already stable. There may be some other exceptions shows on figure 2.28 on pg 56 of the textbook.

Why does electron affinity increase as you move up along the table? I was under the impression that atoms further to the right had increased affinity because they are closer to achieving the stable state of a full valence shell, but how does this correspond to moving up the table?

Jennifer Tuell 1B
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Re: Trends to Know

Postby Jennifer Tuell 1B » Sun May 06, 2018 10:23 pm

I'm pretty sure this won't be on the midterm. The midterm covers Chapter 1 and 2 and the Fundamentals.

SammiOrsini_1B
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Re: Trends to Know

Postby SammiOrsini_1B » Sun May 06, 2018 10:25 pm

I thought electron affinity was apart of chapter 2, I am just not positive if we specifically covered that in class.

Rummel Requerme 1E
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Re: Trends to Know

Postby Rummel Requerme 1E » Sun May 06, 2018 11:05 pm

Professor Lavelle said to only worry about Chapter 1, 2, and the Fundamentals. Best to review Outline 1 & 2!

Maria Roman 1A
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Re: Trends to Know

Postby Maria Roman 1A » Mon May 07, 2018 12:11 am

Trends to know would be the atomic radius, cation and anion trends, ionization energy, and electronegativity

breannasung_1K
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Re: Trends to Know

Postby breannasung_1K » Mon May 07, 2018 12:14 pm

It might be best to know the trends for electron affinity. Electron affinity increases as ionization energy increases.

JooHyun Koh 1H
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Re: Trends to Know

Postby JooHyun Koh 1H » Mon May 07, 2018 11:42 pm

Yea, My TA said that Professor Lavelle didn't really cover electron affinity and said it would most likely not be on the exam.


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