Solution 2 Compound Experimental distance Theoretical distance Prediction accura

Question

Solution 2

Compound

Experimental distance

Theoretical distance   

Prediction accurate?

LiF

2.01

2.09

No

NaCl

2.82

2.83

Yes

KBr

3.30

3.34

Yes

RbI  

3.67

3.72

No

Solution 3

Compound

Theoretical distance (Using bonding atomic radii)

Theoretical distance (Using ionic radii)

Difference

LiF

1.34+0.71 = 2.05

2.09

0.04

NaCl

1.54+0.99 = 2.53

2.83

0.30

KBr

1.96+1.14 = 3.10

3.34

0.24

RbI

2.11+1.33 = 3.44

3.72

0.28

Comparing the two methods

Compound

Difference (Bonding radii)

Difference (ionic radii)

More accurate?

LiF

0.04

0.08

Bonding radii

NaCl

0.29

0.01

Ionic radii

KBr

0.20

0.04

Ionic radii

RbI

0.23

0.05

Ionic radii

From the data, we can see that the atomic bonding radii method is more accurate for smaller compounds. This is because the ionic character of a small compound like LiF is dominated by its covalent character. Hence, bond length calculations involving ionic radii for LiF are less accurate.

Compound

Experimental distance

Theoretical distance   

Prediction accurate?

LiF

2.01

2.09

No

NaCl

2.82

2.83

Yes

KBr

3.30

3.34

Yes

RbI  

3.67

3.72

No

Explanation / Answer

I need help with question 2 and 3 please.

The answer to number 1 is

here's the question if you need to see it also.

And table used in book is

12. 13 14 each applicable question. t worth 20 points. Please nvert this melting point to ury used to fill the cylinder re 13 ic centimeter ts of each. color Denity is 1s. Unit V Problem Solving In the ionic compounds LiF, NaCI, KBr, and Rbl, the measured cation-anion distances are 2.01 A (Li-F), 2.82 (Na-CI), 3.30 A (K-Br), and 3.67 A (Rb-l), respectively Predict the cation-anion distance of each ionic compo und above using the values of ionic radii given in Figure 1. w how you predicted the distance for each lution for each molecule is worth 8 2

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