Inorganic Chemistry Exam 1

Units 1-4

Name the molecular geometry for:

3 electron pairs and no lone pairs

Trigonal Planar

Name the molecular geometry for:

4 electron pairs and no lone pairs

tetrahedral

Name the molecular geometry for:

5 electron pairs no lone pairs

trigonal bipyramidal

Name the molecular geometry for:

6 electron pairs and no lone pairs

octahedral

Name the molecular geometry for:

2 electron pairs and 1 lone pair

Bent

Name the molecular geometry for:

3 electron pairs and one lone pair

trigonal bipyramidal

Name the molecular geometry for:

4 electron pairs and one lone pair

seesaw

Name the molecular geometry for:

5 electron pairs and one lone pair

square pyramidal

Name the molecular geometry for:

2 electron pairs and 2 lone pairs

T-shaped

Name the molecular geometry for:

3 electron pairs 2 lone pairs

T-shaped

Name the molecular geometry for:

4 electron pairs 2 lone pairs

square planar

Name the molecular geometry for:

2 electron pairs and 3 lone pairs

Linear

Linear bond angle

180

Trigonal planar bond angle

120

Tetrahedral bond angle

109.5

Trigonal bipyramidal bond angle

120 and 90

Octahedral bond angle

90

As the number of lone pairs increase, the angle between other bonds ____________

decreases

True or False: Double and Triple bonds are MORE repulsive than single bonds.

True

Rule for L quantum number

n - 1

n represents

principal quantum number

L quantum number represents 

angular distribution or shape of the orbital

The quantum number m_L represents

magnetic quantum number or orientation of orbitals within a subshell

Rules for m_L quantum number

-L to +L

Quantum number m_s represents

Electron spin

Principal shell with n = 1 has  __ subshell L=

one s,  L=0

Principal shell with n = 2 has __ subshell. L=

one s and one p, L=0,1

Principal shell with n = 3 has __ subshell

one s subshell, one p subshell, and one d, L= 0, 1, 2

Number of orbitals in an S subshell

1

Number of orbitals in a P subshell

3

Number of orbitals in a D subshell

5

What does Pauli’s Exclusion Principle say?

A set of quantum numbers is specific to a certain electron, so no two electrons can have the same values for n, l, ml, and ms

What does Hund’s Rule say?

Orbitals may have identical energy levels when they are of the same principal shell. These orbitals are called degenerate, or "equal energy.”
So electrons fill orbitals one at a time (half fill all in that subshell before full filling).

What does the Heisenberg Uncertainty Principal say?

we cannot precisely measure the momentum and position of an electron at the same time

Where do nodes occur?

occurs at points where the wave function is zero and changes signs