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Chem - Gr11 > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

q

Electrovalent Bond

A

The bond formed, as a result of the electrostatic attraction between the positive and negative ions

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2
Q

How to write Lewis Dot structure

A
  1. Add up the total number of electrons (valence)
  2. Add / Subtract the charges as well
  3. Knowing chemical symbols, distirbute total number of electrons
  4. Least electronegative occupies central position
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3
Q

Formal charges

A

Total number of valence electrons - Total number of non bonding electrons - 1/2 (total number of bonding electrons)

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4
Q

Lowest energy structure has _ formal charges

A

Smallest

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5
Q

Examples of incomplete octet

A

LiCl, BCl3, HBeH

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6
Q

Odd electron molecules

A

N = O or O = N - O

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7
Q

Expanded octets

A

PF5, SF6, H2SO4 etc.

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8
Q

Electron Gain Enthalpy

A

Enthalpy change when a gas phase atom in its ground state gains an electron

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9
Q

Is ionization endo or exo

A

Always endo (+)

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10
Q

Ease of formation of ionic bonds

A
  • Elements with low ionization enthalpies
  • Elements with high electron gain enthalpy
  • Higher lattice enthalpy = stronger bonds
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11
Q

Lattice enthalpy

A

Energy required to completely separate one mole of a solid ionic compound into gaseous constituent ions

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12
Q

Bond length

A

Equilibrium distance between nuclei of two bonded atoms in a molecule

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13
Q

Covalent Radius

A

Radius of an atom’s core which is in contact with the core of an adjacent atom in a bonded situation

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14
Q

van Der Waals radius

A

Represents the overall size of the atom which includes its valence shell in a nonbonded situation

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15
Q

Bond Angle

A

Angle between the orbitals containing bond electron pairs around the central atom in a molecule

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16
Q

Bond order

A

Number of bonds between two atoms in a molecule

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17
Q

Bond order in isoelectronic species

A

Identical

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18
Q

Relation between bond order bond enthalpy and bond length

A

Bond order increases = Bond enthalpy increases = Bond length decreases

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19
Q

Dipole Moment

A
  • Product of magnitude of charge and distance of separation
  • Basically tells how polar it is
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20
Q

Why is dipole more in NH3 compared to NF3

A
  1. In NH3 the lone pair has the upward direction
  2. In NF3, the lone pair faces the bonds of F, and hence has cancelling of dipoles
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21
Q

Factors affecting covalent character in ionic bonds

A
  1. Smaller cation & Larger anion = Greater covalent character
  2. Greater charge on cation = Greater covalent character of ionic bond
  3. Transition metals generally more polarising than noble gases
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22
Q

Higher ionic character characterized by

A
  • Larger difference in electronegativity
  • Higher polarizing power
  • Higher polarizability
23
Q

VSEPR of central atom with no lone pair of electrons

A
  1. Linear (180 degrees) (BeCl2, HgCl2)
  2. Trigonal Planar (120 degrees) (BF3)
  3. Tetrahedral (109.5 degrees) (CH4, NH4+)
  4. Trigonal Bipyramidal (120 and 90) (PCl5)
  5. Octahedral (90 degrees) (SF6)
24
Q

Repulsive interaction of electron pairs decrease in order of

A

lp - lp > lp - bp > bp - bp

25
Q

Bond electrons for with lone pair

A

-

26
Q

Why is there a lone pair at equatorial position?

A
  • Minimize repulsion
  • Equatorial has 120 degree bond angle with each other
  • Better for it to have because only two 90 degree repulsions
27
Q

Explain VBT

A

Find the minimum bond enthalpy

28
Q

Sigma Bonds

A
  • End - to - end (head on) overlap of bonding orbitals
  • Axial overlap
  • Formed by s-s overlap, s-p overlap, p-p overlap head on
29
Q

Pi bonding

A
  • Axes remain parallel to each other and perpendicular to internuclear axis
  • Saucer type formation
30
Q

Sigma vs Pi bond strength

A
  • Sigma - Overlapping of orbitals to a larger extent (stronger)
  • Pi bond - Overlapping to a smaller extent (weaker)
31
Q

What is hybridization?

A

Process of intermixing of the orbitals of slightly different energies so as to redistribute their energies, resulting in the formation of new set of orbitals of equivalent energies and shape

32
Q

sp hybridization example

A
  • 50 - 50 s and p character
  • Linear geometry
  • Diagonal hybridization
33
Q

sp2 hybridization example

A
  • 33 - 66 s and p character
  • BCl3
  • Trigonal Planar arrangement
  • Bond angle 120 degrees
34
Q

sp3 hybridization example

A
  • 25 - 75 s and p character
  • Tetrahedron and bond angle is 109.5
  • NH3 and H2O
35
Q

Explain NH3 and H2O

A
  • NH3 - 3 unpaired electrons in the sp3 hybrid and lone pair of electrons present in fourth. Bond angle now 107
  • H2O - Tetrahedral shape (two lone pairs and two electron pairs) - reduced from 109.5 to 104.5
36
Q

sp3 hybridization in C2H6 molecule

A
  • One of four orbitals overlaps axially with similar orbitals of other atom to form sp3 - sp3 sigma bond
37
Q

sp hybridization in C2H2

A
  • Both carbon atoms undergo sp - hybridization having two unhybridised orbital
38
Q

sp2 hybridization in C2H4

A
  • One of the orbitals overlaps axially
  • Other two are used for sp2 - s sigma bond with two hydrogen atoms
  • Unhybridized overlaps sideways
39
Q

Name the shapes and orbitals for undergoing sp and d orbital hybridization

A

-

40
Q

Bonding vs Antibonding molecular orbital

A
  • Bonding - Bond electrons paired with each other, forming a covalent bond. Have a lower energy and greater stability
  • Antibonding - Do not participate in bonding; have a higher energy than component atomic orbitals
41
Q

MOT for oxygen, flourine

A

sigma 1s < sigma * 1s < sigma 2s < sigma * 2s < sigma (2pz) < (pi 2px == pi 2py) < (pi * 2px = pi * 2py) < sigma * 2pz

42
Q

MOT for below oxygen

A

sigma 1s < sigma * 1s < sigma 2s < sigma * 2s < (pi 2px = pi 2py) < sigma 2pz < (pi * 2px = pi * 2py) < sigma * 2pz

43
Q

Bond order

A

One half the difference between the number of electrons present in bonding and antibonding orbitals
= 1/2 (Nb - Na)

44
Q

Stability through bond order

A
  1. Positive bond order means stable molecule
  2. Negative bond order / zero means an unstable bond order
45
Q

Relation between bond order and bond length

A

Inversely proportional

46
Q

Diamagnetic vs Paramagnetic

A

Diamagnetic - Molecular orbitals are doubly occupied
Paramagnetic - Molecular orbitals are singly occupied

47
Q

Hydrogen bond

A

Attractive force which binds hydrogen atom of one molecule with the electronegative atom of another molecule

48
Q

Atoms which can go through hydrogen bonding

A

F , O , N

49
Q

Intermolecular hydrogen bond

A

Between two different molecules of the same or different compounds. Eg: HF, alcohol, water, etc.

50
Q

Intramolecular hydrogen bond

A

Hydrogen atom is in between two highly electronegative atoms (F , O , N)
Eg: o-nitrophenol molecule

51
Q

Electronegativity order

A

F > O > Cl > N > Br > S > C

52
Q

Which has higher electronegativity difference: ClF3 or SO2

A

ClF3

53
Q
A

Chem - Gr11 (8 decks)

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