Draw Lewis structures for N5+, ClO2+, SbF6-, XeF4, HCN, N2O, NH3, AlCl3, O3, and PH3.
The Correct Answer and Explanation is:
Here are the Lewis structures for each of the given molecules and ions along with a brief explanation of how to draw them:
- N5+: This is a positively charged ion with five nitrogen atoms. To form a stable structure, nitrogen atoms will be connected by double bonds, and the positive charge is distributed by removing one electron from one of the nitrogen atoms. The Lewis structure would have each nitrogen connected by a double bond, with formal charges balancing the overall +1 charge.
- ClO2+: The chlorine atom is bonded to two oxygen atoms with single bonds, and the ion carries a +1 charge. The chlorine atom would have a lone pair of electrons, and one of the oxygen atoms will also carry a lone pair. To balance the positive charge, chlorine will form a double bond with one oxygen.
- SbF6-: The antimony (Sb) atom is surrounded by six fluorine (F) atoms. Each fluorine is connected to the antimony by a single bond. The negative charge is placed on the fluorine atoms, and they each carry three lone pairs of electrons.
- XeF4: Xenon (Xe) is in the center of the structure, bonded to four fluorine (F) atoms. The xenon atom will have two lone pairs of electrons. Each fluorine is connected to the xenon by a single bond, with each fluorine also having three lone pairs of electrons.
- HCN: The hydrogen (H) is bonded to carbon (C), and the carbon atom is triple-bonded to the nitrogen (N) atom. The nitrogen atom carries a lone pair, and the carbon atom has a single bond to hydrogen and a triple bond to nitrogen.
- N2O: This molecule consists of two nitrogen (N) atoms and one oxygen (O) atom. The first nitrogen is triple-bonded to the second nitrogen, and the second nitrogen is single-bonded to the oxygen atom. The nitrogen atoms have lone pairs to satisfy the octet rule.
- NH3: Ammonia consists of one nitrogen atom bonded to three hydrogen atoms. The nitrogen atom has a lone pair, and each hydrogen atom is connected to nitrogen by a single bond.
- AlCl3: Aluminum (Al) is bonded to three chlorine (Cl) atoms. Each chlorine atom has three lone pairs, and aluminum has no lone pairs. This is an example of an electron-deficient molecule.
- O3: Ozone has a bent structure with two oxygen atoms bonded to a central oxygen atom. One of the bonds between the oxygens is a double bond, and the other is a single bond. There is a lone pair of electrons on the central oxygen atom.
- PH3: Phosphine consists of a phosphorus (P) atom bonded to three hydrogen atoms. The phosphorus atom has a lone pair, and each hydrogen atom is bonded to phosphorus by a single bond.
In each case, the goal is to follow the octet rule (for atoms like carbon, nitrogen, oxygen, and fluorine), account for formal charges, and ensure that the total number of valence electrons in the structure matches the number of electrons available from the atoms. For charged species, the formal charges must be taken into account to balance the molecule’s overall charge.
