Respuesta :
In general, bonds with an electronegativity difference of 0-0.5 are nonpolar covalent, bonds with an EN difference of 0.5-2.0 are covalent, and anything above 2.0 is considered ionic.
To determine the bond types of the pairs of elements, we will need their EN values. We can subtract their EN values to find their EN difference.
H and Br: 2.96-2.20=0.76
Therefore a bond between H and Br would be moderately polar covalent.
Cl and F: 3.98-3.16=0.82
Therefore this bond is moderately polar covalent.
K and Cl: 3.16-0.82=2.34
Therefore this bond is ionic.
Li and O: 3.44-0.98=2.46
Therefore this bond is ionic.
Br and Br: Because these are the same element, meaning that they have the same EN value, we automatically know that their EN difference would be zero. Therefore, this bond is very covalent.
To determine the bond types of the pairs of elements, we will need their EN values. We can subtract their EN values to find their EN difference.
H and Br: 2.96-2.20=0.76
Therefore a bond between H and Br would be moderately polar covalent.
Cl and F: 3.98-3.16=0.82
Therefore this bond is moderately polar covalent.
K and Cl: 3.16-0.82=2.34
Therefore this bond is ionic.
Li and O: 3.44-0.98=2.46
Therefore this bond is ionic.
Br and Br: Because these are the same element, meaning that they have the same EN value, we automatically know that their EN difference would be zero. Therefore, this bond is very covalent.
Br-Br is highly covalent bond. HBr is slightly polar covalent bond. Cl-F and C-O are moderately polar covalent bond. K-Cl and Li-O are ionic bond.
Chemical bonds are the attractive forces that hold atoms together in the form of compound. Nature of bond can be predicted using electronegativity difference (ΔEN) between the atoms.
- no electronegativity difference then it is highly covalent.
- 0.5- 0.9 slightly polar covalent bond,.
- 1.0-1.3 moderately polar covalent bond.
- 1.4- 1.3 highly polar covalent bond.
- 1.8-2.2 ionic bond
- H and Br, ΔEN= 2.8-2.1 = 0.7 slightly polar covalent bond.
- Cl and F, ΔEN = 4-3 = 1.0 moderately polar covalent bond.
- K and Cl, ΔEN =3.0-0.8 = 2.2 ionic bond.
- Li and O, ΔEN =3.5-1.0 =2.5 ionic bond.
- C and O, ΔEN =3.5-2.5 = 1.0 moderately polar covalent bond.
- Br and Br, ΔEN =2.8-2.8= 0 highly covalent bond.
Thus, we can conclude that Br-Br is highly covalent bond. HBr is slightly polar covalent bond. Cl-F and CO are moderately polar covalent bond.
K-Cl and Li-O are ionic bond.
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