The bonds in methane (CH₄) are covalent, as the electronegativity difference between carbon (2.5) and hydrogen (2.1) is small, indicating that they share electrons rather than transferring them. Carbon has four valence electrons and needs four more to complete its octet, while each hydrogen atom has one valence electron and needs one more to achieve a full shell. By forming four covalent bonds with hydrogen atoms, carbon can share its electrons, allowing it to effectively bond and stabilize its electronic configuration. Thus, methane's molecular structure results from these shared electron pairs, leading to a stable compound.
Use the periodic table to complete the activity.
An illustration shows the periodic table of elements with elements arranged in increasing order of atomic number in 18 columns (groups) and 7 rows (periods). The electronegativity of elements increases from left to right, across a period. The hydrogen on the left is included in group with medium electronegativity. Also, fluorine is shown as element with highest electronegativity.
Methane ( CH4 ) is a gas that is found in small quantities in Earth’s atmosphere. Are the bonds in methane ionic or covalent according to their electronegativities, and how can one carbon atom bond with four hydrogen atoms based on their valence electrons? In three to five sentences, explain your answer.
(4 points)
1 answer