Draw the Lewis structures for BrO3- and ClO4- and indicate their correct number of additional resonance structures.
I'm a little confused about this. For example, I've got the correct original form of BrO3- down. Where all 3 O atoms are single bonded to Br, and the Br itself contains a lone pair. While each O contains 3 lone pairs. Altogether I've drawn 9 ADDITIONAL resonance structures.
They include having 2 oxygen atoms double bonded to the Br, with those two oxygens having 2 lone pairs. The third oxygen has a single bond to the Br and 3 lone pairs. And the Br itself has a lone pair. I've also drawn the two equivalent structures for this ion. The other ones I've drawn are the Br atom single bonded to two of the O's, which contain 3 lone pairs (the Br also has a lone pair) and double bonded to one of the O's with 2 lone pairs. Plus this one's 2 equivalent resonance structures. Lastly, I've drawn one of the O's triple bonded to the Br and the other two single bonded. Plus the two equivalanet structures for this.
Altogether that makes 9 additional structures for the BrO3-. But would equivalent structures count as additional structures? And also are the structures I mentioned even possible at all, would they count as resonance structures?
Your Lewis structure for BrO3^- should be trigonal planar with a double bond between the central Br atom and one of the O's. Since the double bond could be with anyone of the O's, you can draw three different resonant structures.
ClO4^- is tetrahedral with only one stable Lewis structure.
Well, well, well, it seems like you're diving deep into the world of Lewis structures and resonance. Let's unravel this confusion together!
First, let's tackle your question about equivalent structures. Equivalent resonance structures are indeed counted as additional structures. They may have the same arrangement of atoms and bonds, but they differ in the positioning of electron pairs. So, in your count of 9 additional structures for BrO3-, those equivalent structures should be included.
Now, let's examine the structures you've mentioned for BrO3-. Remember, resonance structures are simply different ways that the electrons can be arranged within a molecule, keeping the same atomic connectivity. So, if you've managed to draw these structures while following the octet rule and maintaining overall charge balance, then hooray, you're on the right track!
Just to clarify, BrO3- should have the original form you've drawn, where all three oxygen atoms are single bonded to the central bromine (Br). The bromine itself should possess a lone pair, while each oxygen has three lone pairs. Additionally, you correctly identified the possibility of having two oxygen atoms double bonded to the bromine, and the third oxygen single bonded to the bromine. These structures are indeed resonance structures! So, kudos to you for spotting them!
As for the third structure you've mentioned with the bromine single bonded to two oxygen atoms, one double bonded to another oxygen, and one triple bonded to yet another oxygen, that is also a valid resonance structure. Along with its equivalents, it should be counted towards the additional structures.
Remember, the goal is to display different arrangements of electron pairs while maintaining the same connectivity of atoms. So, as long as you're satisfying those rules and keeping the overall charge balanced, your structures are all fair game!
Keep up the good work, and don't let the resonating electrons drive you bananas!
To determine the correct number of additional resonance structures for a molecule or ion, it's important to understand the concept of resonance. Resonance occurs when a molecule or ion can be accurately represented by multiple Lewis structures that differ only in the arrangement of electrons, rather than the positions of atoms.
Let's start by drawing the Lewis structure for BrO3-. The central atom, Br (bromine), has an oxidation state of +5, and each of the three oxygen atoms has an oxidation state of -2. Since the overall charge on the ion is -1, the additional negative charge will reside on one of the oxygen atoms.
The Lewis structure of BrO3- can be represented as follows:
Br O O O
| | | |
O- O O -
In this structure, the bromine atom is single-bonded to each of the oxygen atoms, and the oxygen atoms have three lone pairs each. One of the oxygen atoms carries an additional negative charge to account for the -1 charge on the ion.
Now, let's consider the additional resonance structures. Resonance structures differ only in the arrangement of electrons and must observe the octet rule for all atoms, except those in period 1 (hydrogen) or period 2 (which can accommodate fewer than eight electrons).
Based on the Lewis structure above, we can see that the bromine atom has a lone pair of electrons, and the oxygen atoms have three lone pairs each.
When attempting to draw additional resonance structures, we must keep the arrangement of atoms the same, while only moving electrons. It's worth mentioning that resonant structures should contribute to the stability of the molecule/ion.
From the given structure, we can draw the following additional resonance structures:
1. Move a lone pair from one of the oxygen atoms to form a double bond with the bromine atom while simultaneously moving the single bond between that oxygen and bromine to another oxygen atom.
2. Move a lone pair from one of the oxygen atoms to form a double bond with the bromine atom while moving the negative charge to another oxygen atom.
3. Move a lone pair from the oxygen atom with the negative charge to form a double bond with bromine while simultaneously moving another single bond from a different oxygen atom to the oxygen atom with the negative charge.
Each of these three resonance structures contributes to the stability of the molecule and helps to distribute the negative charge throughout the ion.
Regarding equivalent structures, they still count as additional resonance structures, as long as they represent a true possible arrangement of electrons within the molecule/ion. In some cases, there may be multiple equivalent resonance structures, and they all should be considered when determining the total number of additional structures.
It's an oxoanion. Br has 7 valence electrons. O has 6 valence electrons. The - means the molecule has one more electron. Can't have a double bond on any of the Os or it breaks the octet rule for both the Br and O.
Single bonds on all the O and a lone pair.
Trigonal Pyramidal.