Answer : The formal charge on central Cl atom is -1.
Explanation :
The given molecule is, ![Cl^-_3](https://tex.z-dn.net/?f=Cl%5E-_3)
First we have to determine the total number of valence electrons in, ![Cl^-_3](https://tex.z-dn.net/?f=Cl%5E-_3)
As we know, chlorine has 7 valence electrons.
Total number of valence electrons in
= 3(7) + 1 = 22 electrons
Electrons used in bonding pair = 4
Electrons used as lone pair = 22 - 4 = 18
Now we have to calculate the formal charge on central Cl atom.
- Formal charge = Number of valence electrons of a central atom - (2 × Number of lone pairs) - Number of bond pairs
Formal charge on central Cl atom = 7 - (2 × 3) -2 = -1
Therefore, the formal charge on central Cl atom is -1.
The lewis-dot structure of
is shown below.
Answer:
[Cl⁻] = 1,5x10⁻⁴M
Explanation:
First of all, let's determinate the mole of each salt.
Molarity . volume = Mole
Volume must be in L, cause molarity is mol/L
NaCl → Na⁺ + Cl⁻
Ratio is 1:1
0.15 mol/L . 0.025L = 3.75x10⁻³ mole
As ratio is 1:1, from 3.75x10⁻³ mole of salt, I have 3.75x10⁻³ mole of chloride
CaCl₂ → Ca²⁺ + 2Cl⁻
Ratio is 1:2 so, from 1 mol of salt I'll get the double of mole of chloride
0.075 mol/L . 0.010 L = 7.5x10⁻⁴ mol
7.5x10⁻⁴ mol . 2 = 1.5x10⁻³ mole
Total mole of Cl⁻: 3.75x10⁻³ + 1.5x10⁻³ = 5.25x10⁻³
This 5.25x10⁻³ mole are present in a total volume of 35 mL.
Let's convert 35 mL in L → 0.035L (35/1000)
Molarity is mol/L → 5.25x10⁻³ mol / 0.035L = 1,5x10⁻⁴M