PQ - Orbital and bonding

Question 1

Name the blocks on the periodic table

Answer 1

Question 2

Full electronic configuration

Answer 2

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2

they usually put 3d10 first and then 4p6

Question 3

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Question 4

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Question 5

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Question 6

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Question 7

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Question 8

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Question 9

Define orbitals, shells and sub-shells

Answer 9

Question 10

Blurt everything you know about 2 electron pairs.

Answer 10

Question 11

Blurt everything you know about 3 electron pairs.

Answer 11

Question 12

Blurt everything you know about 4 electron pairs.

Answer 12

Question 13

Blurt everything you know about 5 electron pairs.

Answer 13

Question 14

Blurt everything you know about 6 electron pairs.

Answer 14

Question 15

electronegativity trend

Answer 15

Question 16

How do we calculate number of orbitals in shells

Answer 16

Question 17

Polarity, non-polar,polar and ionic

Answer 17

Question 18

dipoles

Answer 18

Question 19

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Question 20

How do we calculate the number of electrons in shells

Answer 20

Question 21

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Question 22

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Question 23

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Question 24

intermolecular forces table

Answer 24

Question 25

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Question 26

Answer 26

We treat the double bond as one bonding area. even though its a double bond

Question 27

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Question 28

Answer 28

The alkyl group is the first 2 carbon and the carbocylic acid is the last carbon.

104.5

Question 29

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Question 30

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Question 31

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Question 32

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Question 33

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Question 34

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Question 35

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Question 36

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Question 37

what does the strength of vdw forces depend on ?

Answer 37

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.

Question 38

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Question 39

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Question 40

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