Question

Give the Lewis structure of (a) the strongest oxoacid of bromine. (b) a hydrogen compound of nitrogen in which there is \(a n-N-N-\) bond. (c) an acid added to cola drinks.

Short answer

Question: Provide the Lewis structures for the following substances: (a) the strongest oxoacid of bromine, (b) a hydrogen compound of nitrogen with an N-N bond, and (c) an acid added to cola drinks. Answer: (a) The Lewis structure for the strongest oxoacid of bromine (HBrO4) is: ``` O " || O-H-Br-O | O ``` (b) The Lewis structure for a hydrogen-nitrogen compound with an N-N bond (HN3) is: ``` H-N=N≡N ``` (c) The Lewis structure for an acid added to cola drinks (H3PO4) is: ``` H | O=P<=>O / \ O-H H-O ```

Step-by-step solution

(a) Find the strongest oxoacid of bromine.

The strongest oxoacid of bromine is HBrO4, also known as perbromic acid.

(a) Assign valence electrons and choose the central atom.

For HBrO4, the total number of valence electrons is: H (1) + Br (7) + 4 * O (6) = 32 electrons. Bromine (Br) is the central atom as it has the lowest electronegativity.

(a) Connect the atoms with single bonds.

Connect the Br atom to each O atom with a single bond. Then, connect one O atom to the H atom. This will consume 4 + 1 = 5 bonds or 10 electrons.

(a) Distribute remaining electrons.

Distribute the remaining 22 electrons (32 - 10) to the surrounding oxygen atoms to complete their octets.

(a) Recheck the formal charges.

To have minimal formal charges, we need to add a double bond between Br and one of the O atoms. The final Lewis structure for HBrO4 is: ``` O " || O-H-Br-O | O ```

(b) Find a hydrogen-nitrogen compound with \(N-N\) bond.

The hydrogen-nitrogen compound with an \(N-N\) bond is HN3, also known as Hydrazoic acid.

(b) Assign valence electrons and choose the central atom.

For HN3, the total number of valence electrons is: H (1) + 3 * N (5) = 16 electrons. Nitrogen (N) is the central atom.

(b) Connect the atoms with single bonds.

Starting from H, connect it to the first N atom, and then connect the other two N atoms in a chain. This will consume 2 bonds or 4 electrons.

(b) Distribute remaining electrons.

Distribute the remaining 12 electrons (16 - 4) to the nitrogen atoms to complete their octets.

(b) Recheck the formal charges.

To have minimal formal charges, we need to add a triple bond between the last two N atoms. The final Lewis structure for HN3 is: ``` H-N=N≡N ```

(c) Find an acid added to cola drinks.

The acid commonly added to cola drinks is phosphoric acid (H3PO4).

(c) Assign valence electrons and choose the central atom.

For H3PO4, the total number of valence electrons is: 3 * H (1) + P (5) + 4 * O (6) = 32 electrons. Phosphorus (P) is the central atom.

(c) Connect the atoms with single bonds.

Connect the P atom to each O atom with a single bond. Then, connect three O atoms to an H atom. This will consume 6 bonds or 12 electrons.

(c) Distribute remaining electrons.

Distribute the remaining 20 electrons (32 - 12) to the surrounding oxygen atoms to complete their octets.

(c) Recheck the formal charges.

To have minimal formal charges, we need to add a double bond between P and one of the O atoms. The final Lewis structure for H3PO4 is: ``` H | O=P<=>O / \ O-H H-O ```

Key concepts

Oxoacid of Bromine

When discussing oxoacids of bromine, we refer to compounds where bromine is bonded to oxygen, and typically hydrogen is also present. These acids are part of a larger group of compounds known as halogen oxoacids.

An example of the strongest oxoacid of bromine is perbromic acid (HBrO4). Its strength is partly due to the high oxidation state of bromine in this acid. When learning to write the Lewis structure for such a compound, one must remember to account for all the valence electrons and distribute them in a way that fills the octets of the atoms involved while also ensuring minimal formal charges on the atoms. The Lewis structure is not just a diagram; it's a visual representation that shows how atoms are bonded in a molecule and how the valence electrons are distributed among them.

Lewis Structure Notation

Understanding Lewis structure notation is crucial for mastering the representation of molecules. Using Lewis dot structures, we can visualize the valence electrons of atoms and how they form chemical bonds.

The notation involves arranging dots around the chemical symbols to represent electrons and drawing lines to symbolize chemical bonds. For instance, in the provided solution for HBrO4, the connecting lines show bonding between bromine and oxygen, and the double lines indicate a double bond where two pairs of electrons are shared. Aspiring chemists should practice by drawing simple molecules before tackling more complex structures such as oxoacids.

Chemical Bond in Compounds

A chemical bond is the force of attraction that holds atoms together within a compound. There are several types of bonds - ionic, covalent, and metallic being the primary types.

Covalent bonds involve the sharing of electron pairs between atoms, which is the type of bonding present in the oxoacid of bromine (HBrO4). This kind of bond is directional and dictates the shape of the molecule, which is essential for the molecule's properties. When Lewis structures are drafted, the type and quantity of bonds have a significant impact on the final structure, demonstrating the nature of electron sharing within the compound.