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The molecular geometry of a molecule with 2 bonded atoms and 3 lone pairs is bent or angular. This arrangement is derived from the VSEPR (Valence Shell Electron Pair Repulsion) theory, which states that lone pairs occupy more space than bonding pairs, causing the bonded atoms to be pushed closer together. The bond angle in this case is typically less than 120 degrees due to the influence of the lone pairs.
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What factors affect the shape of the molecule?
The factors affecting the shape of the molecules are the bonded e and the lone pairs of electrons
What shape is a 2 bonded and 2 lone pair?
A molecule with 2 bonded pairs and 2 lone pairs adopts a bent or angular shape due to the repulsion between the lone pairs. This arrangement is commonly seen in molecules like water (H₂O). The lone pairs occupy more space than the bonded pairs, causing the bonded atoms to be pushed closer together, resulting in a bond angle of approximately 104.5 degrees.
How can becl2 have a different shape that h2o when they both have central atom and 2 non-metals?
BeCl2 and H2O have different shapes due to their differing electron geometries and the presence of lone pairs. BeCl2 has a central beryllium atom with two bonded chlorine atoms and no lone pairs, resulting in a linear shape. In contrast, H2O has a central oxygen atom bonded to two hydrogen atoms and two lone pairs, leading to a bent shape due to the repulsion between the lone pairs. The differing arrangements of bonding and non-bonding electrons dictate their distinct molecular geometries.
According to the VSEPR theory what is the shape of a molecule that has a central atom bound to three other atoms with no lone pairs of electrons?
According to VSEPR theory, a molecule with a central atom bonded to three other atoms and no lone pairs of electrons adopts a trigonal planar shape. The bond angles in this configuration are approximately 120 degrees. This arrangement minimizes repulsion between the bonded electron pairs, leading to a stable molecular geometry.
IS IF4 a tetrahedral shape?
IF4 (iodine tetrafluoride) does not have a tetrahedral shape; instead, it has a square planar geometry. This is due to the presence of four fluorine atoms bonded to the iodine atom and two lone pairs of electrons that occupy equatorial positions in a trigonal bipyramidal arrangement. The lone pairs push the fluorine atoms into a square planar configuration.
If two atoms are bonded to a central atom with no lone pairs how will they be arranged?
linear
Molecular geometry of XeO2F2?
see-saw shaped. Note that the MOLECULAR structure is only concerned about the BONDED atoms, not the lone pairs. Although we take the lone pairs repulsive effects into consideration, we do not include them when DESCRIBING the shape of the bonded atoms
What factors affect the shape of the molecule?
The factors affecting the shape of the molecules are the bonded e and the lone pairs of electrons
What shape is a 2 bonded and 2 lone pair?
A molecule with 2 bonded pairs and 2 lone pairs adopts a bent or angular shape due to the repulsion between the lone pairs. This arrangement is commonly seen in molecules like water (H₂O). The lone pairs occupy more space than the bonded pairs, causing the bonded atoms to be pushed closer together, resulting in a bond angle of approximately 104.5 degrees.
What would cause the shape of a molecule to be tetrahedral?
A molecule with four bonded atoms and no lone pairs on the central atom will have a tetrahedral shape. This occurs when the central atom is bonded to four other atoms, resulting in equal distances between the atoms, leading to a tetrahedral shape due to the arrangement of electron pairs around the central atom.
Which shape would represent a molecule with two bonded atoms and three lone pairs on only one of them?
This molecule would have a linear shape, with a bond angle of 180 degrees between the two bonded atoms. The lone pairs would be situated on the same atom, causing repulsion that pushes the bonded atoms closer together.
What shape would a molecule with two bound groups and two lone pairs have?
The correct answer is: Bent.
Whuch of the following are classified as an electron group?
Lone-pair electrons, Bonded pairs of electrons
What is the bond of AB2E2?
An AB2E2 molecule has two atoms and two lone pairs surrounding the central atom. This is the situation is water. The molecule will have a bent shape and the bond angle will probably as in water (105 0) be less than tetrahedral 109.5 0 )- due to lone pair - bond repulsion.
If two atoms are bonded to central atom with no lone pairs how will they be arranged?
linear
Does a diatomic atom contain two lone pairs?
No. There is no such thing as a diatomic atom. A diatomic molecule is a molecule that contains two atoms. The number of lone pairs depends on what atoms are bonded.
How can becl2 have a different shape that h2o when they both have central atom and 2 non-metals?
BeCl2 and H2O have different shapes due to their differing electron geometries and the presence of lone pairs. BeCl2 has a central beryllium atom with two bonded chlorine atoms and no lone pairs, resulting in a linear shape. In contrast, H2O has a central oxygen atom bonded to two hydrogen atoms and two lone pairs, leading to a bent shape due to the repulsion between the lone pairs. The differing arrangements of bonding and non-bonding electrons dictate their distinct molecular geometries.
