Questions: Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the following pairs of elements. a. Cs and Cl b. N and N c. C and F d. Rb and Br e. H and H f. Si and Cl

Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the following pairs of elements.
a. Cs and Cl
b. N and N
c. C and F
d. Rb and Br
e. H and H
f. Si and Cl
Transcript text: Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the following pairs of elements. a. Cs and Cl b. N and N c. C and F d. Rb and Br e. H and H f. Si and Cl
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Solution

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Solution Steps

Step 1: Understanding Bond Types

To predict the type of bond between two elements, we need to consider the difference in electronegativity between them. The general guidelines are:

  • Ionic Bonds: Formed when the electronegativity difference is greater than 2.0. Typically occurs between metals and non-metals.
  • Covalent Bonds: Formed when the electronegativity difference is 0.0, indicating equal sharing of electrons. Typically occurs between two identical non-metals.
  • Polar Covalent Bonds: Formed when the electronegativity difference is between 0.5 and 2.0, indicating unequal sharing of electrons.
Step 2: Analyze Each Pair

Let's analyze each pair of elements based on their electronegativity values:

a. Cs and Cl:

  • Cesium (Cs) is a metal with low electronegativity.
  • Chlorine (Cl) is a non-metal with high electronegativity.
  • The electronegativity difference is large, suggesting an ionic bond.

b. N and N:

  • Both are nitrogen atoms with identical electronegativity.
  • The electronegativity difference is 0, indicating a covalent bond.

c. C and F:

  • Carbon (C) and fluorine (F) are both non-metals.
  • The electronegativity difference is significant but not enough for an ionic bond, suggesting a polar covalent bond.

d. Rb and Br:

  • Rubidium (Rb) is a metal with low electronegativity.
  • Bromine (Br) is a non-metal with higher electronegativity.
  • The electronegativity difference is large, suggesting an ionic bond.

e. H and H:

  • Both are hydrogen atoms with identical electronegativity.
  • The electronegativity difference is 0, indicating a covalent bond.

f. Si and Cl:

  • Silicon (Si) and chlorine (Cl) are both non-metals.
  • The electronegativity difference is moderate, suggesting a polar covalent bond.

Final Answer

a. Cs and Cl: \(\boxed{\text{Ionic}}\)

b. N and N: \(\boxed{\text{Covalent}}\)

c. C and F: \(\boxed{\text{Polar Covalent}}\)

d. Rb and Br: \(\boxed{\text{Ionic}}\)

e. H and H: \(\boxed{\text{Covalent}}\)

f. Si and Cl: \(\boxed{\text{Polar Covalent}}\)

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