Draw the Lewis structure for a hydrogen fluoride (HF) molecule.

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CramX · Accepted Answer

Step 1: : Recall the rules for drawing Lewis structures.. - Determine the total number of valence electrons in the molecule. For HF, hydrogen has 1 valence electron and fluorine has 7 valence electrons, giving a total of 8 valence electrons. - Place the atoms in a way that satisfies their octets (except for hydrogen, which only needs 2 electrons to complete its duplet). - Distribute the remaining electrons as lone pairs to achieve a stable octet for each atom. Step 2: : Draw the initial structure.. - Place the hydrogen atom on the left side and the fluorine atom on the right side with a single bond between them. \mathrm{H}-\mathrm{F} Step 3: : Add lone pairs to complete the octets.. - Add a lone pair of electrons to the hydrogen atom (not necessary as hydrogen only needs 2 electrons to complete its duplet). - Add another lone pair of electrons to the fluorine atom to complete its octet. \mathrm{H}:	oori: Step 4: : Check the formal charges.. - The formal charge on hydrogen is 0 (it has 1 valence electron and 1 electron in its single bond). - The formal charge on fluorine is 0 (it has 7 valence electrons, 6 electrons in its lone pairs, and 1 electron in its single bond). Final Answer:  \mathrm{H}:	oori:

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QuestionChemistry

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Full Solution Locked

Step 1:
: Recall the rules for drawing Lewis structures.

Step 2:
: Draw the initial structure.

Step 3:
: Add lone pairs to complete the octets.

Final Answer

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