VSEPR and Bond Hybridization - AP Chemistry
Card 0 of 644
What is the molecular shape of 
?
What is the molecular shape of
NH3 is trigonal pyramidal because it has 4 electron domains, one of them being a lone pair of electrons and the other three being H atoms. When this is arranged in a three-dimensional space, it is trigonal pyramidal in shape.
NH3 is trigonal pyramidal because it has 4 electron domains, one of them being a lone pair of electrons and the other three being H atoms. When this is arranged in a three-dimensional space, it is trigonal pyramidal in shape.
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What is the bond angle in the following structure?
COH2
What is the bond angle in the following structure?
COH2
CO2H is trigonal planar, so the bond angles will be 120 only.
CO2H is trigonal planar, so the bond angles will be 120 only.
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What is the hybridization on the sulfur molecule in the following molecule?
H2S
What is the hybridization on the sulfur molecule in the following molecule?
H2S
the sulfur has 2 atoms bonded (the H) and 2 pairs of electrons, which is a total of 4 electron domains. The hybridization of the sulfur therefore is sp3
the sulfur has 2 atoms bonded (the H) and 2 pairs of electrons, which is a total of 4 electron domains. The hybridization of the sulfur therefore is sp3
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What is the molecular shape of the following molecule?
SF6
What is the molecular shape of the following molecule?
SF6
when a central atom of a molecule has 6 electron domains coming off of it (none of which are lone pairs of electrons), it is considered octahedral
when a central atom of a molecule has 6 electron domains coming off of it (none of which are lone pairs of electrons), it is considered octahedral
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is an example of what type of molecular geometry?
SF4 has 6 electron domains coming off of it- 4 F molecules and 2 lone pairs of e–. This is an example of see-saw shape.
SF4 has 6 electron domains coming off of it- 4 F molecules and 2 lone pairs of e–. This is an example of see-saw shape.
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What is/are the approximate bond angle(s) in the following molecule?
COH2
What is/are the approximate bond angle(s) in the following molecule?
COH2
COH2:
:O:
||
H—C—H
This is a trigonal planar molecule, which only has bond angles of 120o
COH2:
:O:
||
H—C—H
This is a trigonal planar molecule, which only has bond angles of 120o
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What are the shapes of the following compounds:
- (a) SF6
- (b) XeF4
- (c) NH3
- (d) CH4
- (e) PCl5
What are the shapes of the following compounds:
- (a) SF6
- (b) XeF4
- (c) NH3
- (d) CH4
- (e) PCl5
(a) Octahedral: six charge clouds and six atoms (b) Square planar: six charge clouds and four atoms (c) Trigonal pyramidal: four charge clouds and three atoms (d) Tetrahedral: four charge clouds and four atoms (e) Trigonal bipyramidal: five charge clouds and five atoms
(a) Octahedral: six charge clouds and six atoms (b) Square planar: six charge clouds and four atoms (c) Trigonal pyramidal: four charge clouds and three atoms (d) Tetrahedral: four charge clouds and four atoms (e) Trigonal bipyramidal: five charge clouds and five atoms
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What is the shape of the SO2 molecule?
What is the shape of the SO2 molecule?
The answer to this question can be determined by drawing a Lewis structure of the molecule. The S atom is central, with an O atom on each side. Adding in double bonds to each O atom and placing lone pairs on the O atoms give them each an octet, which leaves 2 more lone pairs of electrons to go on the S atom, creating a bent shape.
The answer to this question can be determined by drawing a Lewis structure of the molecule. The S atom is central, with an O atom on each side. Adding in double bonds to each O atom and placing lone pairs on the O atoms give them each an octet, which leaves 2 more lone pairs of electrons to go on the S atom, creating a bent shape.
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VSEPR theory predicts that a BF3 molecule will be which of the following shapes?
VSEPR theory predicts that a BF3 molecule will be which of the following shapes?
Molecules with three atoms around a central atom such as BF3 are trigonal planar because electron repulsion is minimized by positioning the three attachments toward the corners of an equilateral triangle.
Molecules with three atoms around a central atom such as BF3 are trigonal planar because electron repulsion is minimized by positioning the three attachments toward the corners of an equilateral triangle.
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Which of the following is not a characteristic of a preferred Lewis structure?
Which of the following is not a characteristic of a preferred Lewis structure?
Multiple bonds, although they may be stronger, are not necessarily favored in a Lewis structure. It is dependent on the atoms involved. Thus, this is not a criterion used in determining a preferred Lewis structure.
Multiple bonds, although they may be stronger, are not necessarily favored in a Lewis structure. It is dependent on the atoms involved. Thus, this is not a criterion used in determining a preferred Lewis structure.
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What is the molecular geometry of the 
molecule?
What is the molecular geometry of the
There are three bonding electron pairs around the 
central atom and one non-bonding pair, for a total of 4 electron groups. They arrange spontaneously to be furthest apart according to VSEPR theory, which corresponds to when they form a trigonal pyramidal shape.
There are three bonding electron pairs around the
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The most similar electronic geometry will be observed between which pair of compounds?
The most similar electronic geometry will be observed between which pair of compounds?
It is important to note that electronic geometry includes the orientation fo lone pairs, while molecular geometry considers only the geometry of the atoms present in the compound.
Methane, or CH4, has four hydrogen atoms bound to a central carbon, resulting in a tetrahedral geometry.
BF3 has three fluorine atoms bound to a central boron, resulting in a trigonal planar geometry.
Be(Cl)2 has two chlorine atoms bound to a central beryllium, resulting in a linear geometry.
Water, or H2O, has two hydrogen atoms bound to a central oxygen atom with two lone pairs. The molecular geometry is bent, but the electronic geometry is tetrahedral.
Ammonia, or NH3, has three hydrogens bound to a central nitrogen atom with one lone pair. The moelcular geometry is trigonal pyramidal, but the electronic geometry is tetrahedral.
Ammonia, water, and metahne all have the same electronic geometries (tetrahedral), giving us our final answer.
It is important to note that electronic geometry includes the orientation fo lone pairs, while molecular geometry considers only the geometry of the atoms present in the compound.
Methane, or CH4, has four hydrogen atoms bound to a central carbon, resulting in a tetrahedral geometry.
BF3 has three fluorine atoms bound to a central boron, resulting in a trigonal planar geometry.
Be(Cl)2 has two chlorine atoms bound to a central beryllium, resulting in a linear geometry.
Water, or H2O, has two hydrogen atoms bound to a central oxygen atom with two lone pairs. The molecular geometry is bent, but the electronic geometry is tetrahedral.
Ammonia, or NH3, has three hydrogens bound to a central nitrogen atom with one lone pair. The moelcular geometry is trigonal pyramidal, but the electronic geometry is tetrahedral.
Ammonia, water, and metahne all have the same electronic geometries (tetrahedral), giving us our final answer.
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Rank the following compounds in order of increasing bond angle:
, 
, 
, 
, 
If there are multiple bond angles in a single molecule, only consider the smaller bond angle
Rank the following compounds in order of increasing bond angle:
If there are multiple bond angles in a single molecule, only consider the smaller bond angle
has two bonding regions and no lone pairs around the central atom, so it has a linear geometry, so its bond angle is 
.
has four bonding regions and no lone pairs around the central atom, so it has a tetrahedral geometry with bond angles of 
.
has six bonding regions and no lone pairs around the central atom, so it has an octahedral geometry with bond angles of 
and 
. For the sake of ranking, we will only consider the smaller angle.
has three bonding regions and one lone pair around the central atom, so it has a trigonal pyramidal geometry with bond angles of 
.
has three bonding regions and no lone pairs around the central atom, so it has a trigonal planar geometry with bond angles of 
.
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Molecule 
has a trigonal bipyramidal shape. What type of hybridization describes its bonds?
Molecule
Trigonal bipyramidal geometries arise from the hybridization of one s orbital, three p orbitals, and one d orbital, hence the name 
.
Trigonal bipyramidal geometries arise from the hybridization of one s orbital, three p orbitals, and one d orbital, hence the name
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Consider the following reaction, called the Sabatier reaction:
What are the molecular geometries of the products?
Consider the following reaction, called the Sabatier reaction:
What are the molecular geometries of the products?
has four bonding regions and no lone pairs, so it has a tetrahedral geometry. 
has two bonding regions, but it also has two lone pairs, so it has a bent geometry.
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What is the hybridization of the molecular bonds and molecular geometry of 
?
What is the hybridization of the molecular bonds and molecular geometry of
Nitrogen is a Group 5 element, so when it is bound to three hydrogen atoms, it will have a lone pair.
has four areas of electron density (three bonds and one lone pair), so its bonds are 
hybridized.
Because of the lone pair, 
has a trigonal pyramidal geometry.
Nitrogen is a Group 5 element, so when it is bound to three hydrogen atoms, it will have a lone pair.
Because of the lone pair,
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Consider the following reactions that lead to the production of dichloromethane, 
:
What is the Cl-Cl bond angle of the product, dichloromethane?
Consider the following reactions that lead to the production of dichloromethane,
What is the Cl-Cl bond angle of the product, dichloromethane?
has four bonding regions and no lone pairs, so it has a tetrahedral geometry. The bond angles between all of the bonded atoms is 
.
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Consider the following reaction, which occurs at high temperatures with a silver catalyst:
What is the change in the geometry of the carbon atom between the reactant and the product?
Consider the following reaction, which occurs at high temperatures with a silver catalyst:
What is the change in the geometry of the carbon atom between the reactant and the product?
In the reactant, 
, the carbon is bound to three hydrogens and one oxygen, and it has no lone pairs, so it has a tetrahedral geometry. In the product, 
, the carbon is bound to two hydrogens and one oxygen, so it must be double bonded to the oxygen in order to have a complete octet. Therefore, it has a trigonal planar geometry.
In the reactant,
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Figure 1: Ammonia gas formation and equilibrium
What type of geometry does ammonia exhibit?
Figure 1: Ammonia gas formation and equilibrium
What type of geometry does ammonia exhibit?
Ammonia exhibits a tetrahedral electron pair geometry. It has three bonded pairs (between nitrogen and each hydrogen), and one lone pair (on nitrogen). This combination forms a trigonal pyramidal molecular geometry.
Ammonia exhibits a tetrahedral electron pair geometry. It has three bonded pairs (between nitrogen and each hydrogen), and one lone pair (on nitrogen). This combination forms a trigonal pyramidal molecular geometry.
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For which of the following molecules are the molecular and electronic geometries NOT the same?
For which of the following molecules are the molecular and electronic geometries NOT the same?
The molecular geometry refers to the shape of the molecule's atoms, while the electronic geometry refers to the shape of the molecule's atoms and lone pair electrons. PCl3 has a trigonal pyramidal molecular geometry and a tetrahedral electronic geometry. All other answers have no lone pairs, and therefore have the same molecular and electronic geometries.
The molecular geometry refers to the shape of the molecule's atoms, while the electronic geometry refers to the shape of the molecule's atoms and lone pair electrons. PCl3 has a trigonal pyramidal molecular geometry and a tetrahedral electronic geometry. All other answers have no lone pairs, and therefore have the same molecular and electronic geometries.
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