Which molecule is most likely to contain only single covalant bonds
A molecule that is most likely to contain only single covalent bonds is methane (CH4). In methane, carbon forms four single covalent bonds with four hydrogen atoms.
The molecule that is most likely to contain only single covalent bonds is methane (CH4). Methane consists of one carbon atom bonded to four hydrogen atoms. Each bond in methane is a single covalent bond, where the atoms share one pair of electrons.
To determine which molecule is most likely to contain only single covalent bonds, you need to consider the atoms that are involved and their valence electron configuration.
In general, covalent bonds result from the sharing of electrons between atoms. The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight electrons in their outermost shell.
Typically, atoms that are located in the left-hand side of the periodic table (also known as main group elements) are more likely to form single covalent bonds. These elements include hydrogen (H), carbon (C), nitrogen (N), oxygen (O), fluorine (F), and other elements in those respective groups (Group 1, Group 4, Group 5, Group 6, and Group 7).
For example, molecules like H2, N2, O2, F2 are formed by two atoms of the same element sharing a pair of electrons to form a single covalent bond. Similarly, molecules like H2O (water), CH4 (methane), and CO2 (carbon dioxide) contain only single covalent bonds.
In summary, molecules formed by combining atoms like hydrogen, carbon, nitrogen, oxygen, and fluorine are most likely to contain only single covalent bonds.