Final answer:
Option D is incorrect because CH4 has a tetrahedral geometry with bond angles of 109.5 degrees, not straight lines.
Step-by-step explanation:
When comparing the Lewis structures of N2, O2, H2O, and CH4, we can determine that each molecule has a specific arrangement and number of bonds. For N2 (nitrogen gas), the structure shows a triple bond between the nitrogen atoms, which is correct as it completes the octet rule for both atoms. The O2 (oxygen gas) molecule correctly has a double bond, displayed as :O=O:, which also satisfies the octet rule. The structure of H2O (water) involves two single covalent bonds between both hydrogen atoms and the oxygen atom, while oxygen also has four nonbonding electrons, satisfying the octet rule. The CH4 (methane) structure has four single bonds connecting the carbon atom to each hydrogen atom in a tetrahedral arrangement, with bond angles close to 109.5 degrees, which is the correct shape for a molecule with four equivalent bonding regions around a central atom.
The answer to the question would be that option D is incorrect because the bonds in CH4 are supposed to be bent at 109.5 degrees to reflect the tetrahedral geometry of the molecule, facilitated by the repulsion of electrons clouds in its valence shell.