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H2 JC1 Chem > Chem bonding > Flashcards

Chem bonding Flashcards

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1
Q

what are the four types of interactions bond and their structures

A

Metallic, Covalent, and Ionic
Giant Metallic, Giant molecular and Simple Molecular, Giant ionic

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2
Q

What is a metallic bond and what determines its strength

A

electrostatic force of attraction between a lattice of cations and sea of delocalised electrons

No. of valence electrons available for delocalisation per atom / size of metal cation

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3
Q

What is a ionic bond and what is lattice energy

A

electrostatic force of attraction between oppositely-charged ions

lattice energy: energy released when one mole of solid ionic compound is formed from a its constituent gaseous ions

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4
Q

What is a covalent bond

A

electrostatic force of attraction between shared pair of electrons and positively charged nuclei of two atoms

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5
Q

what is a sigma and pi bond

A

sigma: a head on overlap of orbitals with one overlapping region

pi: a side-on overlap of orbitals with two overlapping regions

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6
Q

What is a Coordinate bond

A

Electrostatic forces of attraction between shared pair of electrons and nuclei of donor and acceptor atoms

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7
Q

what is a donor atom and acceptor atom

A

electron rich: has a pair of non-bonding valence electrons (lone pair) available to form dative bond

electron- deficient: has a vacant low-lying orbital to accept the pair of electrons from donor atim

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8
Q

Types of coordinate bond

A

Cation, Adduct, Dimer, Complex ion

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9
Q

What is electronegativity

A

ability of an atom to attract the shared pair of electrons towards itself

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10
Q

what happens when one atom is more electronegative

A

The EFOA between the more electronegative atom and shared pair of electron will be stronger, resulting in a permanent dipole to form

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11
Q

How is the strength of covalent bond indicated

A

Bond Dissociation Energy:
B.D.E is the energy required to break one mole of a particular covalent bond in a specific molecule in gaseous state to form gaseous atoms

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12
Q

Factors affecting strength of covalent bond

A

Bond order, Effectiveness of bond overlap (a covalent bond between two large atoms involves overlap of valence orbitals which are more diffused hence less effective ), bond length, bond polarity

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13
Q

Exceptions of octet rule and explanations

A

Electron deficient central atom, Ability to expand octet structure (in period 3 and above due to availability of low-lying vacant d orbital to accommodate electron for bonding)
unpaired electrons

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14
Q

two principles of vsepr theory

A

1) electron pairs are arranged around the central atom in a molecule as far apart as possible to minimise repulsion between them

2) lone pair-lone pair repulsion > lone pair - bond pair repulsion > bond-pair bond-pair repulsion

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15
Q

What causes bond angle

A

Lone pairs are closer to central atom, repulsion between lone pairs of electrons will be stronger than between bond pairs, Difference in repulsion will influence the angle between bonds of molecule)

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16
Q

2 bond pair 0 lone pair

A

Linear 180degree

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17
Q

3 bond pair 0 lone pair

A

Trigonal planar 120degree

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18
Q

2 bond pair 1 lone pair

A

Bent less than 120 degree

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19
Q

4 bond pair 0 lone pair

A

tetrahedral 109.5 degree

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20
Q

3 bond pair 1 lone pair

A

trigonal pyramidal 107 degree

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21
Q

2 bond pair 2 lone pair

A

bent 104.5 degree

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22
Q

5 bond pair 0 lone pair

A

trigonal bipyramidal 90 and 120 degree

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23
Q

4 bond pair 1 lone pair

A

see saw distorted tetrahedral

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24
Q

3 bond pair 2 lone pair

A

T shaped 90 degree

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25
2 bond pair 3 lone pair
linear 180 degree
26
6 bond pair 0 lone pair
Octahedral 90 degree
27
5 bond pair 1 lone pair
square pyramidal 90 degree
28
4 bond pair 2 lone pair
square planar 90 degree
29
What influences bond angle
electronegativity of central atom or atoms around it size of surroundings atoms bonded to central atom number of lone pairs
30
Why are polar bond stronger
due to the additional electrostatic attraction between oppositely charged dipoles
31
How does covalent character arise
Polarisation of anion electron cloud by neighbouring cations in ionic compound. The electron density between oppositely charged ions increases
32
Factors affecting extent of covalent character
Polarising power: charge density Polarisability: how easily can the electron cloud of the anion be distorted, proportional to size of anion
33
What are intermolecular forces of attraction
Electrostatic forces of attraction which arise from interactions of net dipole of simple molecules, weaker than inter atomic bonds
34
Types of intermolecular forces of attraction and where they are present
instantaneous dipole- induced dipole interactions in simple molecules permanent dipole-permanent dipole interaction in polar molecules hydrogen bonding in molecules with H-F. O-H and N-H honds
35
What are instantaneous dipole-induced dipole interactions
EFOA between oppositely-charged poles of temporary dipoles as molecules are in constant random motion, electron cloud is distorted and unsymmetrically distributed at any instant. electron cloud can be described as momentary polarised, forming instantaneous dipoles which induce a temporary dipole on neighbouring molecules upon close approach
36
Factors affecting id-id interactions
Total number of electrons: greater number of electrons present, the larger size of electron cloud, leading to greater momentary polarisation of electron cloud, stronger id-id interactions Shape of molecule: linear molecule has greater surface area than branched
37
What are permanent dipole-permanent dipole interactions
EFOA between oppositely-charged permanent dipoles of polar molecules.
38
What are hydrogen bonds
EFOA between H atom already covalently bonded to a small, highly electronegative atom and lone pair of electrons on a second small, highly electronegative atom
39
Factors affecting hydrogen bonding
number of lone pairs of electron available on highly electronegative atom number of hydrogen atoms covalently bonded to highly electronegative atom
40
What happen to acid in gas or in non-polar organic solvent
hydrogen bonding between two organic acid molecules lead to dimerization which does not occur in water as the hydrogen bonds are formed between acid and more abundant water molecules instead of
41
42
What is a lattice
Crystalline solid. Molecules are regularly arranged in 3d space, represented by a repeating array of points known as lattice
43
How to determine solubility
Energy released from formation of solute-solvent interactions is sufficient to overcome the solute-solute and solvent-solvent interactions
44
What is a giant metallic lattice
lattice of metal cations in a sea of delocalised electrons held by strong electrostatic forces of attractions
45
Melting point and boiling point of metal
High. Large amount of energy needed to overcome strong electrostatic forces of attraction between cations and sea of delocalised electrons (metallic bonds)
46
Metal Conductivity of electricity
When p.d is applied, delocalised electrons act which are free and mobile act as charge carriers to move in direction of positive potential
47
Malleability and ductility
As force is applied to metal, metal ions are pushed and rearrange in a different order to give desired shape without breaking metallic bonds
48
Thermal conductivity of metal
When heated at one end, electrons and metallic cations take in thermal energy. Electrons move faster and more randomly colliding with other electrons and passing energy to them. Metallic cations also vibrate faster, passing energy to adjacent cations when colliding with them.
49
What is Giant Ionic Lattice
Lattice of oppositely-charged ions held by strong electrostatic forces of attraction between cations
50
Melting point of ionic
Large amount of energy needed to overcome strong ionic bond ( EFOA between oppositely charged ions)
51
electrical conductivity of ionic
in solid, ions can only vibrate about fixed positions and not mobile in molten or aqueous, the ions are free and mobile to function as charge carriers
52
Hard and Brittle ionic
The regular arrangement of ion in in the lattice resist any applied force as ions of the same charge becomes closer and repels one another. If the applied the force is sufficiently strong to slide one layer of ions over another, the resultant be positive forces will shatter the lattice
53
solubility of ionic structure
The formation of ion dipole interactions between the ions and water molecules releases sufficient energy to overcome the strong ionic bonds and allow detachment of the ions from the ionic lattice for hydration (polar solvent also) ionic compound with very exothermic lattice energies are not soluble in water these compounds that energy released from ion dipole interactions is insufficient to overcome the strong ionic bonds to allow detachment of ions from the ionic lattice
54
What is Giant molecular Lattice structure
lattice of atoms held together by strong covalent bonds in an extensive network
55
Melting point of giant molecular
High, large amount of energy is needed to overcome the strong covalent bonds between atoms (electrostatic forces of attraction between the nuclei of atoms, and the shared pair of electrons) in a giant extensive network
56
Electrical Conductivity of giant molecular
absence of free, Mobile ions or localised electrons to conduct electricity All valence electrons are used for covalent bonding.
57
Solubility of Giant molecular
insoluble the energy released in the formation of the solute solvent interactions is insufficient to overcome the strong covalent bonds in the giant molecular structure
58
Why are Giant molecular hard
atoms are helped together by strong covalent bonds in a giant extensive network
59
What is Giant Molecular Layered
Atoms help together by strong covalent bonds in a giant, extensive flat, parallel layers with the adjacent layers held together by instantaneous, dipole induced dipole interactions
60
Melting point of giant molecular layered
large more energy is needed to overcome the strong covalent bonds between atoms in the giant, extensive, flat, parallel layers during melting
61
Electrical Conductivity of giant molecular layered
Good conductor of electricity parallel to layers: Non-bonding valence electrons of the carbon atoms are delocalised over each plane of layers and function as charged carriers to conduct electricity Non-conductor of electricity perpendicular to the layers: Absence of free, mobile ions, ions or delocalised electrons to conduct electricity
62
Solubility of Giant molecular layered
insoluble, weak interactions from between graphite and water, release, insufficient energy to overcome the strong covalent bonds in the giant molecular structure
63
Why is Giant Molecular Layered Soft and Slippery
As adjacent layers of carbon have together by weak, instantaneous, dipole induced dipole interactions, the layers can easily slide over one another
64
What is Simple Molecular
Discrete molecules held together by weak intermolecular forces of attraction (instantaneous -dipole induced dipole, permanent, dipole, permanent, dipole interactions, or hydrogen bonds
65
Melting Point of Simple Molecular
Low, little energy is needed to overcome the weak into molecular instantaneous, diaper induced typo, or permanent, dipole, permanent dipole or hydrogen bonding
66
Electrical conductivity of simple molecular
Absence of free, mobile ions, or localised electrons as charged carriers
67
Solubility of Simple molecular in non polar
Soluble in non-polar but insoluble in water when added to nonpolar solvent, the energy release from the formation of instantaneous, dipole induced dipole interactions between the solute molecules and the nonpolar solvent molecules is sufficient to overcome the similar intermolecular instantaneous dipole induced dipole interactions in the solute, and in the solvent
68
Solubility of simple molecular in water
The instantaneous dipole induced dipole or permanent dipole, permanent dipole, interact form between the solid molecules and the water, molecules release, insufficient energy to overcome the stronger hydrogen bonds present in the water
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H2 JC1 Chem (3 decks)

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