Question

The electronic configuration of an element is given below.

Element 1: 1s22s22p4

Which statement about the reactivity of the element is true?

It is reactive because it has to gain an electron to have a full outermost energy level.
It is unreactive because it has to lose an electron to have a full outermost energy level.
It is reactive because it has to gain two electrons to have a full outermost energy level.
It is unreactive because it has to gain two electrons to have a full outermost energy level.

Answer 1

Am i right wtih A? or is it D?

Answer 2

@tetsxpreme

Answer 3

@tranquility

Answer 4

@axie

Answer 5

What do you need help with?

Answer 6

this is literally the last difficult question

Answer 7

What element has the electron configuration of 1s2 2s2 2p4

Answer 8

isnt it oxygen

Answer 9

Yes, and how many electrons does it need to gain to get a valence shell

Answer 10

8

Answer 11

So remember that the electron configuration for the next noble gas which is Neon is 1s2 2s2 2p6

Oxygen has 2p4

How many more electrons would you need in the p orbital to go from 4 to 6?

Answer 12

two

Answer 13

And would oxygen be reactive or unreactive?

It wants to become stable and have the electron configuration of a noble gas

Answer 14

reactive

Answer 15

yep!

Answer 16

There you go!

Answer 17

like tranq taid 8 is needed for it to be nonreactive

Answer 18

yh thats why i was mainly going with A

Answer 19

so reactive is correct because oxygen doesnt have 8

Answer 20

Re-read answer choice A

Answer 21

and compare it with answer choice C

Answer 22

I would also say, re-read choice A

Answer 23

ohh mb its C because of the two electrons

Answer 24

yep!

Answer 25

Thanks man

Answer 26

No problem

Answer 27

np

Answer 28

if i helped any ._.