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WorksheetsHybridization and Molecular Geometry
Total questions: 20
Worksheet time: 13mins
Hybrid orbitals in (a) molecules like methane are the combination of the 2s and three 2p orbitals on the central atom so that atoms can be as far apart as possible.
Which of the following are true about the molecule ammonia?
The electron domain geometry is trigonal planar.
The molecular geometry is trigonal planar.
The electron domain geometry is tetrahedral.
The molecular geometry is trigonal pyramidal.
There is a lone pair on the central atom.
Which is true about the molecule benzene?
There are 3 pi bonds.
The pi bond electrons are delocalized.
It is a zigzag ring shape.
It is a planar ring shape.
The sigma bonds are delocalized.
What takes up the most space around a central atom?
Pi bonds
Lone Pairs
Sigma Bonds
sp3 hybrid orbitals
The central atom with octahedral geometry has six bonding orbitals which include (check all that are added together):
one s orbital
three p orbitals
one p orbital
one d orbital
two d orbitals
The sulfate ion (SO4)-2 has what molecular geometry?
linear
trigonal planar
trigonal pyramidal
tetrahedral
square planar
In the fake compound ZX3, Z has a lone pair. What is the geometry around Z?
trigonal planar
trigonal pyramidal
tetrahedral
In the compound MX5, there are no lone pairs on the central atom, M. What is the molecular geometry?
trigonal planar
trigonal pyramidal
octahedral
tetrahedral
trigonal bipyramidal
The fake compound LX3 has 2 lone pairs. What is its molecular geometry?
Trigonal planar
Trigonal bipyramidal
T shaped
See-Saw
Which are true about the compound water?
Electron domain geometry is bent.
Molecular geometry is bent.
Since water has two similar bonds, it is nonpolar.
Since water has a net partial positive and partial negative side, it is polar.
Molecular geometry is linear because there are only 2 atoms.
The hybridization of C in the CO2 molecule is
sp
sp2
sp3
sp3d
What is true about lone pairs?
Lone pairs take up more space than bonding pairs.
They are electron domains, like bonding pairs.
They take up less space than bonding pairs.
Lone pairs affect the molecular geometry.
What is true about sigma bond orbitals?
They always have electron density between 2 nuclei in a bond.
They are the same energy as the atomic orbitals on single atoms.
They have an antibonding orbital too.
They are formed from atomic orbitals between atoms.
They can form between hybrid orbitals.
Why do hybrid orbitals form?
Electrons repel each other and try to get as far apart as possible.
Chemistry needs to be as hard as possible.
The presence of bonding atoms changes the atomic orbitals.
Core electrons remain unchanged.
The geometry of carbon atoms depends on
the number of protons
the number of bonds
the number and type of bonds
the number of valence electrons
In this molecule, what is the geometry of the carbon at the bottom of the image?
sp2
sp3
trigonal planar
tetrahedral
Planar structures containing C and H always have _______________ geometry C atoms.
tetrahedral
trigonal bipyramidal
trigonal pyramidal
trigonal planar
How are hybrid orbitals like atomic orbitals?
Have definite energies
Contain 2 electrons maximum
Electrons in an orbital have the same spin
Have same nucleus
There are only a few possible geometries for each type of central atom.
True
False
Which kind of molecular bond has electron density above and below the nuclei in the bond?
Pi
Sigma
sp
sp2
