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1101 > Molecular Bonding > Flashcards

Molecular Bonding Flashcards

1
Q

Describe aspects of Lewis Theory

  • IONIC
  • COVALENT
A

BONDING uses VALENCE e-s
VSPER
FORMAL CHARGES

Ionic: valence e- transfer from metal to non-metal to achieve OCTET.

Covalent: valence e- pairs shared between atoms to achieve OCTET.
BONDING & LONE PAIRS.

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2
Q

Define electronegativity

A

tendency of an atom to attract a bonding pair of electrons

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3
Q

What is formal charge?

A

Formal charge = valence e-s - (lone pair e-s + 1/2 bonding e-s)

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4
Q

What is a polar covalent bond?

A

Unequal sharing of e-s due to difference in EN.

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5
Q

What is an ATOMIC ORBITAL?

A

Area around a nucleus where e-s are likely found.

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6
Q

State the shape of an s AO.

A

SPHERICAL

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7
Q

State the shape of a p orbital

A

DUMBELL

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8
Q

What is a NODE?

A

Region of ZERO probability of finding an e-

Where waves of opposite phases DESTRUCTIVELY overlap & cancel.

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9
Q

Compare the energy of a p & s orbital

A

p orbital HIGHER ENERGY than s

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10
Q

Describe the shape of a p orbital

A

DUMBELL split by a NODAL PLANE into 2 lobes.

3 DEGENERATE p AOs w symmetry about x, y, z axes.

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11
Q

Why do AOs combine to form MOs?

A

To achieve a MORE STABLE, LOWER ENERGY state.

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12
Q

Describe the MO theory

A

AOs combine to MOs.

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13
Q

Aufbau principle states…

A

e-s fill lowest energy orbitals first.

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14
Q

Pauli exclusion principle states

A

max. 2 e-s occupy an orbital, of opposite spins

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15
Q

Hund’s rule states

A

for degenerate AOs, e-s occupy empty orbitals first

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16
Q

antibonding orbitals:

A

e-s NOT located between 2 distinct nuclei

HIGHER ENERGY

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17
Q

bonding orbitals:

A

HIGH e- DENSITY between nuclei.

LOWER ENERGY

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18
Q

Compare energy states of bonding & anti-bonding orbitals

A

AB > B

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19
Q

END ON OVERLAP forms __ bonds

A

σ bonds

20
Q

SIDE-TO-SIDE OVERLAP forms __ bonds

A

∏ bonds

21
Q

Compare strength of σ & ∏ bonds

A

σ > ∏

22
Q

HOMO =

A

Highest Occupied Molecular Orbital - filled MO highest in energy

23
Q

LUMO =

A

Lowest Unoccupied Molecular Orbital - empty orbital above HOMO.

24
Q

DESTRUCTIVE CANCELLATION ->

A

No e- density between 2 nuclei

ANTIBONDING

25
Q

CONSTRUCTIVE

A

e- density between 2 nuclei

BONDING

26
Q

Hybridisation of: C-C bond

A

sp3-sp3

27
Q

Hybridisation of: C=C bond

A

sp2-sp2

28
Q

Compare C-C and C=C bond length & strength

A

C=C shorter & stronger

29
Q

Hybridisation of: C≡C

A

sp-sp

30
Q

Hybridisation of: AMMONIA

A

sp3-s N-H overlap

31
Q

sp3 bonds are

A

σ ONLY

32
Q

sp2 bonds are

A

σ & ∏

33
Q

sp bonds are

A

σ & ∏

34
Q

Describe INDUCTIVE EFFECT

A

Atoms ability to polarise a bond

35
Q

DIPOLE MOMENT

A

NET POLARITY of a molecule

D = e x d

36
Q

Hydrogen Bond Donor

A

ELECTRON DEFICIENT H

37
Q

Hydrogen Bond Acceptor

A

ELECTRON RICH HETEROATOM

38
Q

State 2 possible ethane conformations

A

STAGGERED or ECLIPSED

39
Q

What is TORSIONAL STRAIN

A

Repulsion between bonding e-s of adjacent substituents

40
Q

Which conformation is more stable: staggered ir eclipsed

A

STAGGERED

41
Q

Expand on ‘molecules are not static’

A

MANY INTERCONVERTING CONFORMERS can exist mutually at a time.

42
Q

ANGLE STRAIN

A

Deviation from ideal geometrical bond angle

43
Q

TORSIONAL STRAIN

A

repulsion of proximate bonding e-s

44
Q

STERIC STRAIN

A

atoms/groups approach too closely

45
Q

State the NEAR STRAINLESS CONFORMATION

A

CHAIR

- no angular/torsional strain

46
Q

Compare boat & chair strain

A

Boat more strained

47
Q

What is a ‘ring flip’

A

Chair conformational can interconvert for cycloalkanes - exchange of axial/equatorial positions.

1101 (8 decks)

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