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Chemical Bonding Flashcards

1
Q

Valency and ionisation energy rule

A

In order to remove electrons that are closer to the nucleus than the valence electrons, a lot more energy is needed, so if there is a big jump in IE in between the 3rd and 4th for example, it means the element has 3 valence electrons and is in group 3

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2
Q

Types of chemical bonding (3)

A

Ionic
Metallic
Covalent (pure and polar)

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3
Q

Electronegativity

A

The power of an atom to attract electrons to itself

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4
Q

Pure covalent bond electronegativity value

A

0 - 0.4

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5
Q

Polar covalent bond electronegativity value

A

0.5-1.9

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6
Q

Ionic bond electronegativity value

A

> 1.9

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7
Q

Factors that affect electronegativity (2)

A

Across the period
Down the group

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8
Q

How moving across the group affects electronegativity

A

As you move across the period, there in an increase in the number of protons which results in a greater nuclear charge and a larger electronegativity value

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9
Q

How moving down the group affects electronegativity

A

As we move down the group, the atomic radius increases along with the shielding effect resulting in a lower electronegativity value

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10
Q

Ionic bonding

A

The electrostatic attraction between oppositely charges ions (positively charged cations and negatively charged anions

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11
Q

Ionic bond properties (4)

A

High MP+BP - strong electrostatic forces between oppositely charged ions
Conducts if molten/aqueous - If solid the ions are in a fixed crystal lattice = can’t carry charge
Brittle
Soluble in polar solvents

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12
Q

Metallic bonding

A

Electrostatic attraction between positive cations and delocalised electrons

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13
Q

Properties of metallic bonds (3)

A

Malleable and ductile (due to non-directional bonds)
High conductivity (due to delocalised electrons)
High melting and boiling point(strong electrostatic force between cations and anions(the high the P number the more))

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14
Q

Covalent bonding

A

The electrostatic attraction between the nuclei of 2 atoms and shared pair of electrons

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15
Q

Polar covalent

A

When there is an unequal distribution of charge

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16
Q

Single bond (3)

A

(Single sigma (σ) bond)
Overlap of s-orbitals
Overlap of s and p-orbitals
Head to toe overlap of p-orbitals

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17
Q

Pi bond

A

Forms from the sideways overlap of p-orbitals

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18
Q

Double bond

A

1 σ (sigma) bond and 1 π (pi) bond
CAN ONLY FORM IF YOU HAVE A P VALENCE ELECTRON

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19
Q

Dative covalent bond

A

(Coordinate bond)
When a substance shares its lone pair of electrons with another substance, only occurs when an atom has an incomplete octet

20
Q

Molecular shapes

A

Based on valence shell electron pair repulsion theory (VSEPR), electrons pairs need to be as far from each other as possible
Based on :
-no. of areas of negative charge
-lone pairs

21
Q

Ions rule

A

Gained/lost by the central atom only

22
Q

Pure covalent bond

A

No unequal distribution of charge

23
Q

Dipole moment

A

Unequal distribution of charge

24
Q

What determines if a molecule is polar (2)

A

Whether bond is polar or not
Molecule shape (symmetrical :i ndividual dipoles cancel each other out)

25
Polar and non-polar solubility rule
Like dissolves like
26
IMF vs bonds
IMF is between molecules, bonds is within molecules
27
Van Der Waals forces (3)
Hydrogen bonding Pd-pd Id -id
28
Hydrogen bonding
Strongest VDW force, when H is directly bonded to N O F Hydrogen bonding is a special case of permanent dipole - permanent dipole force between molecules where hydrogen is bonded to a highly electronegative atom
29
Pd-pd
Permanent dipole-permanent dipole 2nd strongest VDW that occurs between polar molecules Carbon to N, O, halogens, Hydrogen to Cl and Br
30
Id-id
Instantaneous dipole - induced dipole/ London dispersion Non-polar molecules Weakest VDW, thenmore electrons the stronger
31
Anomalous properties of water (3)
Due to high no of hydrogen bonds: -relatively high MP+BP -relatively high surface tension Low density of the solid ice compared with water
32
Surface tension
The tendency of molecules of a liquid to be attracted more towards one another at the surface of the liquid than to the air above it
33
Buckminsterfullerene
C60, buckyballs Carbon molecule made up of 60 atoms arranged like the faces of a soccer ball (pentagon and hexagons). Simplest of a family of similar nanoparticles known as fullerenes
34
Covalent radius of a carbon atom
0,077 nm
35
Nanoparticles
Usually have sizes in the range of 1-100nm (1nm is 10-9 metres)
36
Properties/characteristics of buckminsterfullerene (4)
Due to van der Waals dispersion IMF forces, it has a lower Mp than diamond/graphite Sublimes at 800k (527*C) vs Diamond and graphite at 4000K Insoluble in water but slightly soluble in organic solvents (benzene/methylbenzene) More slippery than Teflon (PTFE -poly(tetrafluoroethene))
37
Solubility of C60
(Buckminsterfullerene) Insoluble in water since it can’t for hydrogen bonds with it Slightly soluble in organic solvents eg. Benzene since it forms van der Waals attractions with them
38
Carbon nanotube
Single sheet of carbon atoms which make up graphite (graphene) rolled up
39
Characteristics of nanotubes (5)
-Have a diameter of about 1nm, can be very long. Individual tubes are very strong and stiff due to strong covalent bonds between atoms making up the tubes -Van Der Waals forces between individual tubes is weak so bulk material isn’t so strong -May be open ended or capped one side/both by half a Bucky ball -Delocalised electron suggests they should be good conductors of electricity (can achieve by changing the way they are made) -Delocalised electrons also shows that they are good conductors of heat (transferred via electron movement. Conductivity is good along the tube, not across.
40
Structure of graphene
Single sheet from a graphite structure, 2D Extends indefinitely in both dimensions Stacking them would give you graphite
41
Giant metallic bond properties(3)
Malleable/ductile due to non-directional bonds High MP+BP due to strong electrostatic forces Good conductor of electricity due to delocalised electrons
42
Giant ionic bonds
43
Giant ionic bond properties (3)
Brittle Conducts electricity when molten/aqueous High MP+BP due to strong electrostatic forces
44
Giant covalent bond properties (
45
Giant covalent bond properties (

AS Chemistry (3 decks)

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