a1234
  • a1234
How would I write the electron configuration for an element with 8 electrons?
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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chestercat
  • chestercat
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
Photon336
  • Photon336
@a1234 you can start by doing this we know that each orbital has 2 electrons in it right? and we fill orbitals from the lowest energy up. s orbital = 2 electrons p orbital = 6 electrons maximum so when we start off at the lowest energy level 1s and we would put 2 electrons in that orbital. then we would put another 2 in 2s. we're left with four. if we were to stop there we would have beryllium. this would be our configuration \[1s ^{2}2s ^{2}2p ^{4}\] say we start off |dw:1447046977330:dw|
a1234
  • a1234
I got it. Thanks!
Photon336
  • Photon336
do you see the pattern right?

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Photon336
  • Photon336
the periodic table is organized based on energy levels
a1234
  • a1234
Yes, we're arranging based on the maximum number of electrons in each shell.
Photon336
  • Photon336
take a look at this
Photon336
  • Photon336
Periodic table
1 Attachment
a1234
  • a1234
So why did we go to the p-orbital instead of the d-orbital?
Photon336
  • Photon336
we start from the top first from the lowest energy level 1s then we move down and across. so it would be 1s 2s then 2p
a1234
  • a1234
I see...there's no 2d.
Photon336
  • Photon336
also there's no 1P either
Photon336
  • Photon336
@a1234 you always start with the lowest energy levels first then work your way up when your putting electrons in orbitals and writing configurations.
a1234
  • a1234
Alright. The image is very helpful.
Photon336
  • Photon336
@a1234 can you tell me what the configuration of carbon is?
a1234
  • a1234
It's 1s^2 2s^2 2p^2. It's atomic number is 6, so the number of electrons is also 6.
Photon336
  • Photon336
yep how did you come to that conclusion?
Photon336
  • Photon336
BTW that's correct
a1234
  • a1234
Atoms are stable, so the positive and negative charges are balanced
a1234
  • a1234
neutral, not stable
Photon336
  • Photon336
yeah so one more using the periodic table I posted show me the configuration for fluorine
Photon336
  • Photon336
you can start by looking at how many electrons it has and then filling them from the lowest energy level up
a1234
  • a1234
1s^2 2s^2 2p^5...there are 9 electrons
Photon336
  • Photon336
let me ask you one more question: which one of these is not as reactive as the other and why? 1s^2-2s^2-2p^6 1s^2-2s^2-2p^5
a1234
  • a1234
The first one is less reactive because the second one lacks an electron
Photon336
  • Photon336
the first one is a noble gas
Photon336
  • Photon336
it's octet is filled
Photon336
  • Photon336
second one is fluorine
a1234
  • a1234
The shells of noble gases are already full
Photon336
  • Photon336
yes that's why they aren't as reactive inert is the correct term.
Photon336
  • Photon336
I think you got the hang of it
a1234
  • a1234
I think so

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