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Zorluk: KolayMolecular Shapes, VSEPR Theory, and Hybridization

Pair each of the given chemical molecules with its corresponding molecular geometry as predicted by Valence Shell Electron Pair Repulsion (VSEPR) theory.

  • BF3BF_3Trigonal planar
  • CH4CH_4Tetrahedral
  • BeCl2BeCl_2Linear
  • H2OH_2OBent (V-shaped)

Cevap

BF3BF_3 matches Trigonal planar, CH4CH_4 matches Tetrahedral, BeCl2BeCl_2 matches Linear, and H2OH_2O matches Bent (V-shaped).
According to VSEPR theory, molecular shape depends on the total number of bonding pairs and lone pairs surrounding the central atom. BeCl2BeCl_2 has 2 bonding pairs with no lone pairs, yielding a linear geometry. BF3BF_3 has 3 bonding pairs with no lone pairs, producing a trigonal planar geometry. CH4CH_4 has 4 bonding pairs with no lone pairs, resulting in a tetrahedral geometry. H2OH_2O has 2 bonding pairs and 2 non-bonding lone pairs, creating a bent (V-shaped) geometry.

Adım Adım Çözüm

1
Determine the number of valence electron pairs (bonding pairs and lone pairs) surrounding the central atom for each chemical species.
BF3BF_3 has 3 bonding pairs and 0 lone pairs; CH4CH_4 has 4 bonding pairs and 0 lone pairs; BeCl2BeCl_2 has 2 bonding pairs and 0 lone pairs; H2OH_2O has 2 bonding pairs and 2 lone pairs.
VSEPR theory states that electron pairs around a central atom arrange themselves to minimize electrostatic repulsion.
2
Deduce the resulting molecular geometry for each molecule based on the arrangement of bonding and lone pairs.
3 bond pairs (0 lone pairs) = Trigonal planar; 4 bond pairs (0 lone pairs) = Tetrahedral; 2 bond pairs (0 lone pairs) = Linear; 2 bond pairs + 2 lone pairs = Bent.
Lone pairs exert greater repulsive force than bonding pairs, bending the molecular framework accordingly.

Anahtar Kavram

VSEPR Theory and Molecular Geometries
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Konular

Molecular Shapes, VSEPR Theory, and Hybridization

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