To determine whether the molecule [tex]\( \text{CH}_2\text{O} \)[/tex] contains two single bonds and one double bond, let's break down its structure step by step.
1. Molecular Formula: [tex]\( \text{CH}_2\text{O} \)[/tex] describes a molecule consisting of one Carbon atom (C), two Hydrogen atoms (H), and one Oxygen atom (O).
2. Identify the central atom: In organic chemistry, the Carbon atom often serves as the central atom to which other atoms are bonded.
3. Determine the bonds:
- Hydrogen atoms form single bonds because they only need one additional electron to complete their valence shell.
- Oxygen typically forms two bonds: it prefers to form either two single bonds or one double bond to complete its valence shell.
4. Construct the molecule:
- Carbon has 4 valence electrons and forms 4 bonds to complete its octet.
- Attach the two Hydrogen atoms to the Carbon with single bonds. This uses up 2 of the Carbon's bonding sites (2 single bonds).
- Attach the Oxygen atom to the Carbon with a double bond. This uses up the remaining 2 bonding sites of the Carbon, and completes Oxygen's octet as well (1 double bond).
5. Review the structure:
- The Carbon atom is bonded to two Hydrogen atoms with single bonds.
- The Carbon atom is also bonded to one Oxygen atom with a double bond.
Thus, the molecule [tex]\( \text{CH}_2\text{O} \)[/tex] indeed contains two single bonds (between Carbon and each Hydrogen) and one double bond (between Carbon and Oxygen).
So, the statement "The molecule [tex]\( \text{CH}_2\text{O} \)[/tex] contains two single bonds and one double bond." is True.
