Inorganic Chemistry Exam 1

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36 Terms

1
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Name the molecular geometry for:

3 electron pairs and no lone pairs

Trigonal Planar

<p>Trigonal Planar</p>
2
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Name the molecular geometry for:

4 electron pairs and no lone pairs

tetrahedral

<p>tetrahedral </p>
3
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Name the molecular geometry for:

5 electron pairs no lone pairs

trigonal bipyramidal

<p>trigonal bipyramidal </p>
4
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Name the molecular geometry for:

6 electron pairs and no lone pairs

octahedral

<p>octahedral </p>
5
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Name the molecular geometry for:

2 electron pairs and 1 lone pair

Bent

<p>Bent</p>
6
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Name the molecular geometry for:

3 electron pairs and one lone pair

trigonal bipyramidal

<p>trigonal bipyramidal</p>
7
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Name the molecular geometry for:

4 electron pairs and one lone pair

seesaw

<p>seesaw</p>
8
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Name the molecular geometry for:

5 electron pairs and one lone pair

square pyramidal

<p>square pyramidal</p>
9
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Name the molecular geometry for:

2 electron pairs and 2 lone pairs

T-shaped

<p>T-shaped</p>
10
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Name the molecular geometry for:

3 electron pairs 2 lone pairs

T-shaped

<p>T-shaped</p>
11
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Name the molecular geometry for:

4 electron pairs 2 lone pairs

square planar

<p>square planar</p>
12
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Name the molecular geometry for:

2 electron pairs and 3 lone pairs

Linear

<p>Linear</p>
13
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Linear bond angle

180

14
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Trigonal planar bond angle

120

15
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Tetrahedral bond angle

109.5

16
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Trigonal bipyramidal bond angle

120 and 90

<p>120 and 90</p>
17
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Octahedral bond angle

90

18
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As the number of lone pairs increase, the angle between other bonds ____________

decreases

19
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True or False: Double and Triple bonds are MORE repulsive than single bonds.

True

20
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Rule for L quantum number

n - 1

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n represents

principal quantum number

22
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L quantum number represents 

angular distribution or shape of the orbital

23
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The quantum number mL represents

magnetic quantum number or orientation of orbitals within a subshell

24
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Rules for mL quantum number

-L to +L

25
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Quantum number ms represents

Electron spin

26
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Principal shell with n = 1 has  __ subshell L=

one s,  L=0

27
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Principal shell with n = 2 has __ subshell. L=

one s and one p, L=0,1

28
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Principal shell with n = 3 has __ subshell

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

29
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Number of orbitals in an S subshell

1

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Number of orbitals in a P subshell

3

31
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Number of orbitals in a D subshell

5

32
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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

33
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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).

34
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What does the Heisenberg Uncertainty Principal say?

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

35
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Where do nodes occur?

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

36
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