Question

1. chemical name: sulfur pentachloride anion formula: scl₅⁻ lewis electron - dot structure: perspective drawing with bond angles: standard electron geometry: molecular geometry: hybridization of central atom: is the molecule polar, nonpolar, or ion?

Explanation:

Step1: Determine valence - electrons

Sulfur has 6 valence electrons and each chlorine has 7 valence electrons. The anion has a - 1 charge. So the total number of valence electrons is \(6 + 5\times7+1=42\).

Step2: Draw Lewis structure

Place sulfur in the center and 5 chlorine atoms around it. Distribute the electrons to complete the octets of all atoms. Sulfur can expand its octet.

Step3: Determine electron - geometry

The number of electron - groups around sulfur is 6 (5 bonding pairs and 1 lone pair). So the standard electron geometry is octahedral.

Step4: Determine molecular geometry

With 5 bonding pairs and 1 lone pair, the molecular geometry is square - pyramidal.

Step5: Determine hybridization

The hybridization of the central sulfur atom is \(sp^{3}d^{2}\) as it has 6 electron - groups.

Step6: Determine polarity

The molecule is polar due to the presence of the lone pair on sulfur which causes an uneven distribution of charge.

Answer:

Lewis electron - dot structure: Sulfur in the center with 5 single bonds to chlorine atoms and 1 lone pair on sulfur, and each chlorine has 3 lone pairs.
Perspective drawing with bond angles: Square - pyramidal shape with bond angles approximately \(90^{\circ}\) between axial and equatorial bonds.
Standard electron geometry: Octahedral
Molecular geometry: Square - pyramidal
Hybridization of central atom: \(sp^{3}d^{2}\)
Is the molecule polar, non - polar, or ion? Polar ion.