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greatest shielding means greatest number of shells. the greater number of shells the more the outer electrons are shielded from the nucleus, thus aren't as held tightly.
Based on that reasoning, it's most likely going to be B.
Sorry for just now getting back to you! Thank you so much for helping me out.
No problem. Think about it like this: |dw:1446607767573:dw| The closer the electrons are to the nucleus the more tightly they will be pulled. remember in the nucleus is positively charged and electrons are located in shells outside the nucleus.
That makes more sense, the way you put it
If we keep adding shells, the electrons become farther from the nucleus |dw:1446608024473:dw|
and what happens is that, they aren't as tightly held A question to YOU Which electron would be easier to remove and why? I circled the electrons. |dw:1446608196466:dw| |dw:1446608170950:dw|
The one in blue right? because it is further out?
and this is what we mean by shielding
the farther the electrons are from the nucleus, they become shielded and are not as tightly held.
You have no idea how much you helped me better understand this. Thank you so much.
Absolutely, anytime. The ideas underlying this are very simple. if you noticed the number of shells also has to do with something called electronegativity too
If we go down a group this is what happens |dw:1446608554756:dw|
As we go down a period the vertical columns on the periodic table, the number of shells increases. ALSO the electronegativity goes down, because the number of shells increases and the electrons aren't as tightly held by the nucleus. The same thing we discussed earlier.
@KimberNicoleee question for you
What has a higher electronegativity and why rubidium or sodium?
FYI they are in the same group
Would it be Sodium because it's higher up than Rubidium?
Yes, but what can help to explain that based on our discussion?
Rubidium has more shells and the electrons aren't as tightly held by the nucleus while Sodium has less shells and the electrons are held tighter..?
You see why this helps right? just knowing that electronegativy increases as you go down a group won't help you out very much
okay last thing see the horizontal lines on the periodic table? those are called periods
if you look at a period something interesting happens. the number of shells stays the same , while the atomic number goes up. that means as we move across a period, the number of protons increases while the number of shells stays the same. how do you think this would affect electronegativty?
Wouldn't it have something to do with the nucleus since protons are inside of there? I know I probably sound really stupid but Chemistry isn't my best subject lol
Yes so if the number of protons goes UP and the number of shells stays the same. the nucleus has more protons and the electrons are held more tightly. Also the electronegativy goes up does that make sense?
That makes perfect sense. (:
look at period 3
which has a higher electronegativy and why> Sodium or Chlorine and why?
Chlorine It has 17 protons while Sodium has 11. The more the protons go up so does the electronegativity.
so that's part of the reasoning behind why as we go ACROSS a PERIOD that the electronegativity increases
that's why I don't like just blindly memorizing the as you go up this happens as you go down that happens lol
I totally see why now. This subject is pretty much the only one that homeschooling has been hard for me in. I just really appreciate you taking the time to explain it to me rather than simply tell me what the answer is.
Yeah, the best explanation is a simple one. This site has helped me a-lot too. once you understand the WHY the details will become easier to understand and remember. I've spoken to people on here who have had virtual labs. I think for a subject like chemistry you should take a lab class where you get to do the experiments physically. it makes this stuff come alive.
One more question.... Do you understand how to tell if an equation is balanced? I have 2 equations left and I am a bit confused.
@KimberNicoleee I made a tutorial on that
How do I look at it..?