In thionyl chloride, cl2so (s is the central atom), the formal charge on sulfur and number of lone pairs on sulfur are, respecti
vely, (assume all the atoms obey the octet rule) g
2 answers:
Sulfur in the thionyl compound carries a formal charge of +1 and possesses two lone electrons, which constitutes one lone pair.
Additional Explanation
Lewis Structures
To ascertain the formal charge and count of lone pairs, it is crucial to first construct the Lewis structure. The steps to delineate lone pairs are as follows:
- Calculate the total valence electrons by adding the valence electrons of each atom in the compound.
- Identify the central atom.
- Position the remaining atoms around the central atom, connecting each with a single bond. Each bond corresponds to 2 of the total valence electrons shared.
- Distribute any leftover valence electrons to the terminal atoms, prioritizing one until it reaches an octet, then proceed to the next. If all terminal atoms satisfy the octet rule, remaining electrons go to the central atom.
For thionyl chloride, sulfur serves as the central atom, and the overall valence electron count is:
Cl = 7 × 2 = 14
S = 6
O = 6
Total Valence Electrons = 14 + 6 + 6 = 26 electrons. Following these steps generates the corresponding Lewis structure shown in the attachment.
Having established the Lewis structure, the number of lone pairs on the central atom can be determined. In thionyl chloride, sulfur possesses two unshared electrons, signifying one lone pair.
Formal Charge Assessment
The electron distribution in a molecule is defined through the formal charges on its atoms. A formal charge reflects the disparity between the electrons surrounding an atom in a molecule versus when it is isolated. For molecular stability, formal charges across all atoms need to be minimized.
The formula for formal charge calculation is:
Formal Charge = # valence electrons for isolated atom - (# bonds + non-bonding electrons)
For the thionyl compound, sulfur's formal charge is evaluated using this formula in conjunction with the Lewis Structure:
- Valence Electrons of a Sulfur atom = 6
- Number of bonds surrounding Sulfur = 3
- Number of non-bonding electrons on Sulfur = 2
Formal Charge of S = 6 - (3 + 2)
Formal Charge of S = +1
This indicates that sulfur possesses fewer electrons in the molecule than it would as an isolated atom.
Further Exploration
Key Terms: formal charge, lone pairs
In thionyl chloride, the formal charge on sulfur is while the number of lone pairs on sulfur is
. (For the structure, please refer to the attached image).
Additional Explanation:
Lewis structures are used to illustrate the bonding arrangements between atoms in covalent compounds. They are sometimes referred to as electron dot diagrams, Lewis dot structures, or Lewis dot formulas.
The Lewis structure of (see the attached image for reference):
The total valence electrons of can be calculated as follows:
Sulfur forms one double bond with an oxygen atom and two single bonds with chlorine atoms. From the total of 26 electrons, eight are used in creating one S-O double bond plus two S-Cl single bonds, leaving 18 electrons remaining. Each chlorine atom retains three lone pairs, the oxygen atom holds two lone pairs, and sulfur has one lone pair.
Formal charge on an atom considers equal sharing in chemical bonds irrespective of the atoms' electronegativities.
The formal charge calculation formula is:
...... (1)
Sulfur participates in three single bonds—one with an oxygen atom and two with distinct chlorine atoms—and has one lone pair.
The total number of valence electrons for a free sulfur atom is 6.
The total number of non-bonding electrons in the sulfur atom is 2.
The total binding electrons around sulfur sum up to 6.
With these values substituted into equation (1), we can find sulfur's formal charge.
Further Insights:
1. Molecular geometry surrounding the central atoms in glycine:
2. Constructing resonance structures for the azide ion:
Response Details:
Grade: Senior School
Subject: Chemistry
Chapter: Molecular structure and chemical bonding
Key Terms: Lewis structure, valence electrons, sulfur, S atom, formal charge, +1, 6, 2, lone pair.
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Explanation:
Initial moles of ethanoic acid = 0.020 mol
At equilibrium, half of the ethanoic acid molecules have reacted.
Thus, moles of ethanoic acid reacted = 0.020 mol * (50% / 100%)
= 0.010 mol
Moles of ethanoic acid remaining = 0.020 mol - 0.010 mol = 0.010 mol
The moles of product gas formed are determined as follows:
0.010 mol CH3COOH * (1 mol / 2 mol CH3COOH)
= 0.005 mol
Consequently, the total moles of gas present in the vessel at equilibrium are 0.010 mol CH3COOH and 0.005 mol
Total gas moles at equilibrium = 0.010 mol + 0.005 mol = 0.015 mol
Next, let’s determine the pressure:
0.020 mol of gas has a pressure of 0.74 atm; so under the same conditions, we find the pressure exerted by 0.015 mol of gas:
P1/n1 = P2/n2
P2 = P1*(n2 / n1)
= 0.74 atm * (0.015 mol / 0.020 mol)
= 0.555 atm
Answer:
La masa molar del compuesto es: 168.82 g/mol
La masa molar del gas es: 16.38 g/mol
Explanation:
(a)
Utilizando la ecuación de gases ideales:
donde,
P es la presión
V es el volumen
n es el número de moles
T es la temperatura
R es la constante de los gases, cuyo valor es = 0.0821 L.atm/K.mol
Además,
Moles = masa (m) / Masa molar (M)
La densidad (d) = Masa (m) / Volumen (V)
Así, la ecuación de gases ideales se puede expresar como:
Dado que:-
Presión = 20 kPa = 20000 Pa
La expresión para la conversión de presión en Pascal a presión en atm se muestra a continuación:
P (Pa) = P (atm)
20000 Pa = atm
Presión = 0.1974 atm
Temperatura = 330 K
d = 1.23 kg/m³ = 1.23 g/L
Masa molar =?
Aplica la fórmula:
0.1974 atm × M = 1.23 g/L × 0.0821 L.atm/K.mol × 330 K
⇒M = 168.82 g/mol
La masa molar del compuesto es: 168.82 g/mol
(b)
Dado que:
Presión = 152 Torr
Temperatura = 298 K
Volumen = 250 cm³ = 0.25 L
Utilizando la ecuación de gases ideales:
R =
Aplicando la fórmula:
152 Torr × 0.25 L = n × 62.3637 L.torr/K.mol × 298 K
⇒n = 0.002045 moles
Dado que:
Masa del gas = 33.5 mg = 0.0335 g
Masa molar =?
La fórmula para calcular los moles se muestra a continuación:
Así,
La masa molar del gas es: 16.38 g/mol