I've already attempted this question a few times and haven't gotten the correct answers yet... Can you explain to me how you get the answers so I can understand it better for the final exam? Thanks!
What is the shape of each molecule below? Select the correct answer. Answers can be used more than once.
XeF2
SeF4
ClF5
XeF4
SF6
AsCl5
IF3
What is the shape of each molecule below? Select the correct answer. Answers can be used more than once.
XeF2
SeF4
ClF5
XeF4
SF6
AsCl5
IF3
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XeF2:
Notice that normally Xe has 8 electrons (4 pairs) around it. When 2 fluorides bond, it takes an electron from Xe contribute to each bond. Thus, there are still 6 electrons (3 pairs) of electrons and 2 Xe-F bonds. This makes 5 structures around the central atom (Xe). Since only 2 of them are actual bonds, these bonds will line up at 180 degrees to each other. The structure of the molecule is then linear.
SeF4:
Se has 6 electrons around it in its neutral state. With 4 fluorides bonded, that leaves a single lone pair of electrons and 4 bonds. This also has 5 structures around the central atom. Since 4 are bonds, this leaves a see-saw molecular structure.
ClF5:
Cl normally has 7 electrons around it. With 5 fluorides bonded, that leaves a single lone pair of electrons and 5 bonds. This has 6 structures around the central atom. With 5 actual bonds, this molecule is square pyrimidal.
XeF4:
Xe normally has 8 electrons around it. With 4 fluorides bonded, that leaves two lone pairs of electrons and 4 bonds. This has 6 structures around the central atom. With 4 actual bonds, this molecule is square planar.
SF6:
S has 6 electrons around it normally. All 6 are used to make the six bonds to the fluorides. This is thus an octahedral molecule.
AsCl5:
As normally has 5 electrons around it. All 5 are used to bond to the chlorides. This is thus a trigonal bipyramidal molecule.
IF3:
I normally has 7 electrons around it. 3 are used to bond to the fluorides leaving 2 lone pairs and 3 bonds. The central atom, thus, has 5 structures around it. Since only 3 are actual bonds, this is a T-shaped molecule.
Notice that normally Xe has 8 electrons (4 pairs) around it. When 2 fluorides bond, it takes an electron from Xe contribute to each bond. Thus, there are still 6 electrons (3 pairs) of electrons and 2 Xe-F bonds. This makes 5 structures around the central atom (Xe). Since only 2 of them are actual bonds, these bonds will line up at 180 degrees to each other. The structure of the molecule is then linear.
SeF4:
Se has 6 electrons around it in its neutral state. With 4 fluorides bonded, that leaves a single lone pair of electrons and 4 bonds. This also has 5 structures around the central atom. Since 4 are bonds, this leaves a see-saw molecular structure.
ClF5:
Cl normally has 7 electrons around it. With 5 fluorides bonded, that leaves a single lone pair of electrons and 5 bonds. This has 6 structures around the central atom. With 5 actual bonds, this molecule is square pyrimidal.
XeF4:
Xe normally has 8 electrons around it. With 4 fluorides bonded, that leaves two lone pairs of electrons and 4 bonds. This has 6 structures around the central atom. With 4 actual bonds, this molecule is square planar.
SF6:
S has 6 electrons around it normally. All 6 are used to make the six bonds to the fluorides. This is thus an octahedral molecule.
AsCl5:
As normally has 5 electrons around it. All 5 are used to bond to the chlorides. This is thus a trigonal bipyramidal molecule.
IF3:
I normally has 7 electrons around it. 3 are used to bond to the fluorides leaving 2 lone pairs and 3 bonds. The central atom, thus, has 5 structures around it. Since only 3 are actual bonds, this is a T-shaped molecule.