Okay so I kinda understand where to put the numbers into the formula but i'm not sure how to calculate the distance so could someone kindly walk me through the problem so i can understand it. Thank you so much.
Calculate the amount of energy required for the formation of one mole of BeS bonds (not lattice energy). The radius of the beryllium ion is 0.31 A (has a squiggle on the top), and the radius of the sulfide ion is 1.84 A (has a squiggle on top also). Note that 1A (has a squiggle) = 10^-10m.
I'm suppose to use the formula E=(kq1q2)/d
k is the constant 2.31 * 10^-28 J*m
E in joules = kq1q2/d
k you have in the problem
q1 = 2
q2 = 2
d = radius anion + radius cation = 1.84+0.31 = ? and convert to meters.
Substitute and solve.
Calculate the amount of energy released in the formation of one mole of BaSe bonds (not lattice energy). The radius of the barium ion is 1.35 Å, and the radius of the selenide ion is 1.98 Å. Note that 1Å=10−10m. needs to be using the dimensions of enthalpy for the answer
falds
Calculate the amount of energy released in the formation of one mole of BaSe bonds (not lattice energy). The radius of the barium ion is 1.35 Å, and the radius of the selenide ion is 1.98 Å. Note that 1Å=10−10m. needs to be using the dimensions of enthalpy for the answer
fda
Ah, calculating the energy required for bond formation, huh? Let me see if I can help you with a touch of humor.
Well, it seems like you already have the formula E = (kq1q2) / d, so that's a great start! Now, let's break it down step by step, or should I say, "joke by joke."
First, let's replace those squiggly A's with their proper values. One angstrom (Å) is equal to 10^-10 meters. So, the radius of the beryllium ion (0.31 Å) becomes 0.31 * 10^-10 meters, and the radius of the sulfide ion (1.84 Å) becomes 1.84 * 10^-10 meters. These ions must be having quite the mini dance party!
Now comes the fun part - assigning some values to our charges. Since we're dealing with ions, they'll have some charge attached to them. And since it's one mole of BeS bonds we're talking about, we'll consider the charges of a mole of beryllium and a mole of sulfur.
Be careful, though! Beryllium has a charge of +2 because it loses two electrons to become stable, while sulfur has a charge of -2 because it gains two electrons. Quite the charge difference, huh? It's like a shocking love story!
Now, we need to find the distance between these two ions (d), which helps determine the strength of their bond. In this case, the distance is simply the sum of the ionic radii of beryllium and sulfur, now converted into meters. I imagine it's like measuring the length of a dance move!
Finally, plug in all the values into the formula: E = (2.31 * 10^-28 J*m) * (+2) * (-2) / (sum of the ionic radii in meters).
Calculate that, and you've got the amount of energy required for the formation of one mole of BeS bonds. Quite an energetic dance move, I must say!
I hope that helps you understand the problem a bit better with a bit of humor. If you have any more questions, feel free to ask!
To calculate the amount of energy required for the formation of one mole of BeS bonds, you can use Coulomb's law, which relates the energy of interaction between two charged particles to their charges and distance. The formula you mentioned, E = (k * q1 * q2) / d, is the mathematical representation of Coulomb's law.
Here's how you can solve this problem step by step:
Step 1: Convert the given ionic radii from angstroms (Å) to meters (m).
- The radius of the beryllium ion (Be²⁺) is 0.31 Å = 0.31 * 10^-10 m.
- The radius of the sulfide ion (S²⁻) is 1.84 Å = 1.84 * 10^-10 m.
Step 2: Calculate the distance between the centers of the two ions.
- In this case, since the ions are not touching but forming a bond, the distance (d) is the sum of their radii.
- Therefore, d = (0.31 + 1.84) * 10^-10 m.
Step 3: Calculate the amount of energy required using Coulomb's law.
- Substitute the values into the formula: E = (k * q1 * q2) / d.
- The charge (q) for both Be²⁺ and S²⁻ ions is the elementary charge, which is 1.6 * 10^-19C.
- The constant (k) is given as 2.31 * 10^-28 J*m.
- So, E = (2.31 * 10^-28 J*m) * ((1.6 * 10^-19 C) * (1.6 * 10^-19 C)) / ((0.31 + 1.84) * 10^-10 m).
Step 4: Calculate the final result.
- Perform the calculations, making sure to handle the units properly.
- After evaluating the expression, you will obtain the energy required in joules (J).
Remember to be cautious with the unit conversions and calculations to ensure accurate results.