VSEPR - Bonding and Molecular Geometry

Therefore, it is nonpolar. In summary, the electron pair geometry of SCN− and BeCl2 is linear, while O3 is trigonal planar. NO2+ and ClO2− are ionic structures, while XeF2 is nonpolar due to its linear and symmetric structure. The bond angles at the central atoms of ClF2+, HCN, and SO2 are 109, 180, and 120 degrees, respectively. Additionally, O3 is linear and nonpolar due to its symmetric structure. XeF2 is nonpolar due to its linear and symmetric structure, which does not allow for a dipole moment.
  • #1
WK95
139
1

Homework Statement


What is the electron pair geometry of the following?
SCN−
BeCl2
O3

The Attempt at a Solution


SCN− Linear
BeCl2 Linear
O3 Trigonal Planar


Homework Statement


Would the following structures be polar or nonpolar? (Not applicable if the structure is an ion. Pick "ionic" in that case).
NO2+
XeF2
ClO2−

The Attempt at a Solution


NO2+ ionic
XeF2 nonpolar
ClO2− ionic


Homework Statement


What is the bond angle at the central atom of the following?
ClF2+
HCN
SO2

The Attempt at a Solution


ClF2+ 109
HCN 180
SO2 120
 
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  • #2
O3 is linear
 
  • #3
Can you explain? Isn't there a lone pair in the center Oxygen atom?

IMG00007.GIF
 
  • #4
Of course you are right, sorry. Was thinking in another question.
 
  • #6
dextercioby said:
How's XeF2 nonpolar ?

It is linear and symmetric, so can't have a dipole moment.
 

1. What is VSEPR theory and how does it explain bonding and molecular geometry?

VSEPR (Valence Shell Electron Pair Repulsion) theory is a model used to predict the shapes of molecules based on the repulsion between valence electron pairs. It states that electron pairs will arrange themselves in a way that minimizes repulsion and maximizes distance between them, resulting in specific molecular geometries. This theory explains how the number and arrangement of bonding and non-bonding electron pairs around a central atom determine the shape of a molecule.

2. What are the main factors that affect molecular geometry according to VSEPR theory?

The main factors that affect molecular geometry are the number of bonding and non-bonding electron pairs around the central atom, as well as the types of bonds (single, double, or triple) present in the molecule. These factors influence the overall shape and bond angles of the molecule.

3. How does VSEPR theory account for the differences in bond angles observed in molecules?

VSEPR theory predicts that electron pairs will arrange themselves in a way that minimizes repulsion. This means that the presence of non-bonding electron pairs will cause bonding pairs to be pushed closer together, resulting in a smaller bond angle. Double and triple bonds also create more electron density and can affect bond angles. For example, a molecule with a double bond will have a smaller bond angle compared to a molecule with only single bonds.

4. Can VSEPR theory accurately predict the shapes of all molecules?

No, VSEPR theory has limitations and cannot accurately predict the shapes of all molecules. It is most accurate for molecules with central atoms that have no lone pairs of electrons, such as carbon in methane (CH4). Molecules with multiple central atoms or with lone pairs of electrons may have more complex shapes that cannot be predicted solely by VSEPR theory.

5. How does VSEPR theory relate to the properties of molecules?

The shape of a molecule, determined by VSEPR theory, can greatly influence its physical and chemical properties. For example, molecules with polar bonds may have different overall dipole moments depending on their molecular geometry, which can affect their reactivity and solubility. Additionally, the shape of a molecule can also affect its intermolecular forces and boiling point.

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