PQ - Orbital and bonding Flashcards
1
Q
Name the blocks on the periodic table
A
2
Q
Full electronic configuration
A
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2
they usually put 3d10 first and then 4p6
3
Q
A
4
Q
A
5
Q
A
6
Q
A
7
Q
A
8
Q
A
9
Q
Define orbitals, shells and sub-shells
A
10
Q
Blurt everything you know about 2 electron pairs.
A
11
Q
Blurt everything you know about 3 electron pairs.
A
12
Q
Blurt everything you know about 4 electron pairs.
A
13
Q
Blurt everything you know about 5 electron pairs.
A
14
Q
Blurt everything you know about 6 electron pairs.
A
15
Q
electronegativity trend
A
16
Q
How do we calculate number of orbitals in shells
A
17
Q
Polarity, non-polar,polar and ionic
A
18
Q
dipoles
A
19
Q
A
20
Q
How do we calculate the number of electrons in shells
A
21
Q
A
22
Q
A
23
Q
A
24
Q
intermolecular forces table
A
25
26
We treat the double bond as one bonding area. even though its a double bond
27
28
The alkyl group is the first 2 carbon and the carbocylic acid is the last carbon.
104.5
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37
what does the strength of vdw forces depend on ?
vdWaals depends on atomic radius, and number of shells and electrons. Br2 has more electrons and more shells, therefore its vdWaals is greater than NH3.
In general, H-bonds are much stronger than vdWaals. However, there if the molecuele is large enough, and therefore the vdWaals strong enough, BP of something with H-bonds can be lower than that of vdWaals.
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