00:02
Hi there.
00:03
In this question, we are asked to draw the lewis dot structure for asbr5.
00:11
So to do this, we first need to determine how many valence electrons we have to work with, since the lewis dot structure shows valence electrons as dots.
00:20
So looking at the periodic table, arsenic is in group 5.
00:23
So it has five valence electrons.
00:25
And then there are five bromines.
00:28
Bromene is a halogen in group 7a.
00:31
All of the elements in group 7a have seven valence electrons.
00:35
So adding these together, 5 plus 35 gives us 40 valence electrons, which means our loose dot structure needs 40 dots.
00:47
Exactly 40 dots, no more, no less.
00:51
All right, we're going to start out with our single element in the center surrounded by the five bromines.
01:08
And we know that we have to have at least a single bond holding each of these bromines to the arsenic.
01:17
All right.
01:18
So that took up 24, 6, 8, 10 of our dots.
01:21
We have 30 remaining.
01:23
We need to start completing the octets on each of the bromine until we run out of dots.
01:30
Or until we've completed the octets.
01:31
We'll see where we are after we've completed these octets.
01:41
All right.
01:42
So we have all five bromines with eight dots around them.
01:45
Five times eight, that took all 40 of our dots.
01:49
Arsenic, as a result, has five bonds around it.
01:52
So this is our lewis dot structure...