Anthracene is a yellow, crystalline solid found in coal tar. Complete this structure for anthracene, C14H10, by adding bonds and hydrogen atoms as necessary.

What type of hybrid orbitals are utilized by carbon in anthracene?
>>sp3

How many σ bonds and π bonds are there in an anthracene molecule? How many valence electrons occupy σ-bond orbitals and how many occupy π -bond orbitals?
>>26 σ bonds
>>7 π bonds
>> I don't know how to figure out how many valence electrons occupy the bond orbitals

What type of hybrid orbitals are utilized by carbon in anthracene?

>>sp2

How many ó bonds and ð bonds are there in an anthracene molecule? How many valence electrons occupy ó-bond orbitals and how many occupy ð -bond orbitals?
>>26 ó bonds
>>7 ð bonds
How many valence electrons occupy ó-bond orbitals and how many occupy ð -bond orbitals?
>>2(26)=52 ó bonds
>>2(7)=14 ð bonds

Well, carbon in anthracene is quite the multitasker! It utilizes sp3 hybrid orbitals to form its bonds. As for the number of sigma (σ) and pi (π) bonds in anthracene, we have 26 sigma bonds (holy smokes!) and 7 pi bonds (that's pretty fly!).

Now, figuring out the number of valence electrons occupying the bond orbitals can be a bit trickier. It's like trying to count the number of clowns fitting into a tiny car - it can get a bit crowded in there! But fear not, my friend, for I have a joke to distract you from this dilemma:

Why did the electron bring a map to the party?

Because it didn't want to get lost in all those bond orbitals! Ha!

But on a serious note, determining the exact number of valence electrons occupying each type of bond orbital in anthracene can be a bit complex, as it involves molecular orbital theory. I recommend consulting a chemistry textbook or a knowledgeable expert to get a precise answer.

To determine how many valence electrons occupy σ-bond orbitals and how many occupy π-bond orbitals in anthracene, we need to know the bonding pattern and the hybridization of the carbon atoms in the molecule.

In anthracene, there are 10 carbon atoms, and they are all sp2 hybridized.

Each sp2 hybridized carbon atom forms three σ bonds and one π bond. Therefore, there are a total of 10 × 3 = 30 σ bonds and 10 × 1 = 10 π bonds in the anthracene molecule.

For each σ bond, there are two electrons occupying the bond orbitals. Therefore, the number of valence electrons occupying σ-bond orbitals is 30 × 2 = 60.

For each π bond, there are two electrons occupying the π -bond orbitals. Therefore, the number of valence electrons occupying π-bond orbitals is 10 × 2 = 20.

So, in the anthracene molecule, there are 60 valence electrons occupying σ-bond orbitals and 20 valence electrons occupying π-bond orbitals.

To determine how many valence electrons occupy σ-bond and π-bond orbitals in anthracene, we need to understand the concept of bonding in organic molecules.

In anthracene (C14H10), each carbon atom forms four sigma (σ) bonds to neighboring atoms. These σ bonds are formed by overlapping of hybrid orbitals. In anthracene, carbon atoms are sp3 hybridized, meaning that each carbon atom has four sp3 hybrid orbitals available for bonding. These four orbitals are directed towards the four corners of a tetrahedron.

To create the structure for anthracene, we can start by placing the carbon atoms in a linear chain. Each carbon atom is bonded to two adjacent carbon atoms, utilizing sp3 hybrid orbitals to form σ bonds. After placing the carbon atoms in a linear chain, we can connect them by adding alternating single and double bonds.

Now, let's analyze the σ bonds and π bonds in anthracene:

- For each carbon atom, one σ bond is formed with the adjacent carbon atom in the linear chain.
- The remaining three sp3 hybrid orbitals on each carbon atom form σ bonds with hydrogen atoms.

Therefore, each carbon atom contributes one σ bond to the linear chain and three σ bonds to hydrogen atoms. Since there are 14 carbon atoms, we have a total of 14 σ bonds in the molecule (14 carbon-carbon σ bonds and 42 carbon-hydrogen σ bonds).

Moving on to π bonds, we need to understand that π bonds result from the sideways overlap of p orbitals. Each carbon atom in anthracene has two remaining unhybridized p orbitals perpendicular to the plane of the molecule. These unhybridized p orbitals can form π bonds by overlapping with adjacent carbon atoms.

In anthracene, there are alternating single and double bonds between adjacent carbon atoms. This arrangement allows for the formation of π bonds. The double bonds in anthracene are formed by side-by-side overlap of p orbitals, resulting in the formation of π bonds.

Looking at the structure of anthracene, we can observe that there are three fused aromatic rings in the molecule. Each aromatic ring consists of alternating single and double bonds. By counting the number of double bonds in the rings, we can determine the number of π bonds in anthracene.

In anthracene, there are two double bonds in each aromatic ring, resulting in a total of 6 π bonds (2 π bonds in each of the three aromatic rings).

To summarize:
- Anthracene has 14 σ bonds (carbon-carbon) and 42 σ bonds (carbon-hydrogen).
- Anthracene has 6 π bonds.

Determining how many valence electrons occupy σ-bond and π-bond orbitals requires a more advanced analysis using molecular orbital theory. In this theory, electrons are distributed among molecular orbitals that span the entire molecule. However, it is beyond the scope of a simple explanation to calculate the exact number of electrons in each type of orbital.