Predict whether each of the following bonds is nonpolar covalent, polar covalent, or ionic.
Drag the appropriate bonds to their respective bins.
C and Br
N and P
P and P
Li and F
Si and Br
Br and F
C and Br: polar covalent
N and P: polar covalent
P and P: nonpolar covalent
Li and F: ionic
Si and Br: polar covalent
Br and F: polar covalent
C and Br: Polar covalent
N and P: Nonpolar covalent
P and P: Nonpolar covalent
Li and F: Ionic
Si and Br: Polar covalent
Br and F: Polar covalent
To predict whether a bond is nonpolar covalent, polar covalent, or ionic, we need to consider the electronegativity difference between the two atoms involved in the bond. Electronegativity is a measure of an atom's ability to attract shared electrons in a bond.
Here's how you can determine the type of bond:
1. Find the electronegativity values of each element: Electronegativity values are typically found on the periodic table. The higher the electronegativity value, the greater the atom's ability to attract electrons.
2. Calculate the electronegativity difference: Subtract the electronegativity value of the atom with the lower electronegativity from the atom with the higher electronegativity. The electronegativity difference will guide us in determining the nature of the bond.
- If the electronegativity difference is less than 0.5, the bond is considered nonpolar covalent.
- If the electronegativity difference is between 0.5 and 1.7, the bond is considered polar covalent.
- If the electronegativity difference is greater than 1.7, the bond is considered ionic.
Let's go through each of the given bonds:
1. C and Br:
The electronegativity value of carbon (C) is 2.55, and for bromine (Br), it is 2.96. The electronegativity difference is 0.41, which is less than 0.5. Therefore, this bond is nonpolar covalent.
2. N and P:
The electronegativity value of nitrogen (N) is 3.04, and for phosphorus (P), it is 2.19. The electronegativity difference is 0.85, which is between 0.5 and 1.7. Hence, this bond is polar covalent.
3. P and P:
Since both phosphorus (P) atoms have the same electronegativity value, there is no electronegativity difference. In this case, the bond is considered nonpolar covalent.
4. Li and F:
The electronegativity value of lithium (Li) is 0.98, and for fluorine (F), it is 3.98. The electronegativity difference is 3.00, which is greater than 1.7. Thus, this bond is ionic.
5. Si and Br:
The electronegativity value of silicon (Si) is 1.90, and for bromine (Br), it is 2.96. The electronegativity difference is 1.06, which is between 0.5 and 1.7. Therefore, this bond is polar covalent.
6. Br and F:
The electronegativity value of bromine (Br) is 2.96, and for fluorine (F), it is 3.98. The electronegativity difference is 1.02, which is between 0.5 and 1.7. Thus, this bond is polar covalent.
Based on the electronegativity differences, the classification of each bond is as follows:
Nonpolar covalent:
- C and Br
- P and P
Polar covalent:
- N and P
- Si and Br
- Br and F
Ionic:
- Li and F