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CHEM1110 > FINAL - SECTION 4 > Flashcards

FINAL - SECTION 4 Flashcards

1
Q

5 basic electron groups (egg)

A
  • Count the number of electron groups around central atom (bonded atoms + LPo central)
  • 2 electron groups = linear (sp)
  • 3 electron groups = trigonal planar (sp2)
  • 4 electron groups = tetrahedral (sp3)
  • 5 electron groups = trigonal bypyramidal (sp3d)
  • 6 electron groups = octahedral (sp3d2)
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2
Q

Dashed lines

A

Behind plane

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3
Q

Solid line

A

Infront of plane

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4
Q

7 molecular geometry shapes (mg)

A
  • Only count ATOMS bonded to central atom
  • Bent
  • Linear
  • Trigonal pyramidal
  • T shape
  • Seesaw
  • Square planar
  • Square pyramidal
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5
Q

egg = mg when

A

All electron groups are atoms

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6
Q

egg ≠ atoms when

A

LP are present

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7
Q

BLT sandwich

A

BP LP
2 1 Bent
2 2
2 3 Linear
3 1 Trigonal pyramidal
3 2 T shape
4 1 Seesaw
4 2 Square planar
5 1 Square pyramidal

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8
Q

In diatomic molecules..

A

Only 1 bond so the bond dipole determines polarity

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9
Q

In polyatomic molecules…

A

The total polarity is determined by bond polarity and bond angle

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10
Q

Valence bond theory

A

Defines covalent bond as an electron density between 2 atoms and the ideal distance occurs with overlap from partially filled atomic orbitals of each atom

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11
Q

Sigma bond

A

Formed head to head by overlap of orbitals (single bonds always)

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12
Q

Pi bond

A

Formed by lateral overlap of 2 lobes of orbital

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13
Q

Sigma and pi bond in bonds

A
  • Single bond = 1 sigma bond
  • Double bond = 1 sigma bond + 1 pi
  • Triple bond = 1 sigma bond + 2 pi
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14
Q

Hybridization clues

A
  • Attached to 2 atoms: sp
  • Attached to 3 atoms: sp2
  • Attached to 4 atoms: sp3
  • Attached to 5 atoms: sp3d
  • Attached to 6 atoms: sp3d2
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15
Q

Molecular orbital theory

A

Typically used for diatomic molecules or at lease treat it like that (only on valence electrons

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16
Q

Bonding molecular orbital

A

High electron density

17
Q

Antibonding molecular orbital

A

0 electron density

18
Q

*

A

High energy antibonding orbital

19
Q

Bond order formula

A

Bonded electrons - anti bonded electrons/2

20
Q

Bond order 1

A

Single bond

21
Q

Bond order 2

A

Double bond

22
Q

Bond order 3

A

Triple bond

23
Q

Bond order 1/2

A

Rare usually on H2

24
Q

What does high bond order mean

A

Strong bond

25
Q

HOMO

A

Highest energy orbital (has electrons)

26
Q

LUMO

A

Lowest energy orbital (no electrons)

27
Q

There are 2 versions of molecular orbitals. Why

A

One of them is for atomic numbers less than 8, the other is atomic numbers 8 or more

28
Q

MO is usually for diatomic molecules so how would you know which versions of diagram to use in an occasion like OF?

A

Calculate the average and the less electronegative one goes on the left and more electronegative goes on the right

29
Q

Draw both MO

A

ok

30
Q

Relationship between bonding MO and anti bonding BO energy

A

Antibonding MO is stronger. so sigma 2p<sigma 2p, and pi2p < pi2p

31
Q

Condensed phase

A

Solid and liquids are considered condensed phase because they are packed close together but still vibrate

32
Q

Intramolecular force

A

Force that binds atoms making up molecules

33
Q

Intermolecular force

A

Force between a molecule

34
Q

3 types of intermolecular force

A
  • Dispersion
  • Dipole-dipole
  • H bond
35
Q

Dispersion

A

Every molecule has it and is the weakest (exhibits small partial charges)

36
Q

Dipole-dipole

A

Has a partial positive and partial negative. The more polar it is, the stronger dipole it has = high boiling point (harder to pull apart)

37
Q

H bond

A

Strongest and occurs when a partially positive H is covalently bonded to small electronegative N, O, F

38
Q

Order of increasing strength intermolecular force

A

London dispersion –> dipole-dipole –> H-bond

CHEM1110 (18 decks)

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