Question

Example of Lewis Dot Structure on an element

Answer 1

Is it the atomic number , is that how many dots there are supposed to be?

Answer 2

Like for Chlorine it would be 17?

Answer 3

hm, no, I think you're only supposed to show valence electrons

Answer 4

And how do you determine that again :S the number of valance electrons? :S

Answer 5

chlorine is kind of a weird example because chlorine is diatomic

Answer 6

valence electrons --> use its position on the ptable

Answer 7

chlorine is group 7a so each chlorine atom gets 7 electrons, but chlorine doesn't like to exist by itself, so it'll combine with another chlorine so they both have a full valence shell

Answer 8

Oh so the number group its in is the number of valance electrons?

Answer 9

SO 7?

Answer 10

sort of (for alkali metals, alkaline earth metals, nonmetals, and ~some~ transition metals yes, for most transition metals you can't predict based on group #)

Answer 11

so yeah, one chlorine atom would ~technically~ have 7 although chlorine atoms don't like to exist by themselves in nature

Answer 12

actually for Ars-enic, should be 5

Answer 13

it worked

Answer 14

FOr this I'm getting it wrong. I need to do single dots first?

Answer 15

huh. weird. as far as I know that should work.

Answer 16

Look again at As and Se. You need to maximize the number of unpaired electrons in each case. For example, selenium should have two single dots and two pairs of dots.

Answer 17

This is what it says ^^^

Answer 18

oh, yeah, you should separate pairs of electrons into single electrons, whenever possible.

Answer 19

SO basically do the 4 single ones and then double them up?

Answer 20

yeah, so you start by putting down 4 separate electrons, then pairing up the last 2

Answer 21

same concept with ars-enic