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BONDING Flashcards

(50 cards)

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1
Q

Define ionic bonding

A

The electrostatic force of attraction

between oppositely charged ions

formed by electron transfer

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2
Q

Metal atoms ___ electron to form _ve ions

Non-metal atoms ___ electron to form _ve ions

A

Metal lose to form +ve

Non-metal gain to form -ve

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3
Q

How do smaller ions impact melting points

A

High melting points

In smaller ions

Because ionic bonding is stronger

Or a higher charge

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4
Q

Define covalent bonding

A

A shared pair of electrons

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5
Q

Define dative covalent bonding / Coordinate bindi g

A

A shared pair of electrons

Donated from only one of the bonding atoms

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6
Q

Give the 3 common dative covalent molecules

A

NH4 +

H3O +

NH3BF3

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7
Q

How is a dative covalent bond represented

A

An arrow

From the atom providing the lone pair

To the deficient atom

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8
Q

Define metallic bonding

A

Electron static force of attraction

Between positive metal ions

And delocalised electrons

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9
Q

List the 3 factors effecting the strength of a metallic bond

A

Proton number

Delocalised electron number (per atom)

Size of ion

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10
Q

How does proton number affect the strength of metallic bonding

A

More protons

Stronger bond

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11
Q

How does delocalised electron number affect the strength of metallic bonding

A

More delocalised electrons

Stronger bond

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12
Q

How does ion size affect the strength of metallic bonding

A

Smaller ion

Stronger bond

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13
Q

Give an example of a giant ionic lattice molecule

A

Sodium chloride

Magnesium oxide

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14
Q

Give an example of a simple molecular molecule

A

Iodine

Ice

Carbon dioxide

Water

Methane

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15
Q

Give an example of a macromolecular molecule

A

Diamond

Graphite

Silicon dioxide

Silicon

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16
Q

Give an example of a giant metallic lattice molecule

A

Magnesium

Sodium

All metals

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17
Q

Outline the properties of giant ionic lattices

A

High melting and boiling point

Soluble in water

Poor conductor when solid

Good conductor when molten/dissolved

Crystalline solid

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18
Q

Outline the properties of a simple molecular molecule

A

Low melting and boiling point

Poor solubility in water

Poor conductor when solid and molten

Mostly gas or liquid

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19
Q

Outline the properties of a macromolecule

A

High melting and boiling point

Insoluble in water

Diamond/Sand are poor conductors when solid but graphite is good

Poor conductors when molten

Solids

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20
Q

Describe the properties of a metallic molecule

A

High melting and boiling point

Insoluble in water

Good conductors when solid and molten

Shiny

Malleable

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21
Q

Outline a linear molecule. Give an example.

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A

2 bonding pairs

No lone pairs

180 bond angle

CO2, CS2, HCN, BeF2

22
Q

Outline a trigonal planar molecule. Give an example.

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A

3 bonding pairs

No lone pairs

120 bond angle

BF3, AlCl3, SO3, NO3 -, CO3 2-

23
Q

Outline a tetrahedral molecule. Give an example.

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A

4 bonding pairs

No lone pairs

109.5 bond angle

SiCl4, SO4 2-, ClO4 -, NH4 -

24
Q

Outline a trigonal pyramidal molecule. Give an example.

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A

3 bonding pairs

1 lone pair

107 bond angle

NCl3, PF3, ClO3, H3O +

25
Outline a bent molecule. Give an example.
2 bonding pairs 2 lone pairs 104.5 bond angle OCl2, H2S, OF2, SCl2
26
Outline a trigonal bipyramidal molecule. Give an example.
5 bonding pairs No lone pairs 120 and 90 bond angles PCl5
27
Outline a octrahedral molecule. Give an example.
6 bonding pairs No lone pairs 90 bonding angle SF6
28
Outline the structure for explaining the shape of a molecule
1. state number of bonding pairs and lone pairs 2. State electron pairs repel to a position of minimum repulsion (3. State lone pairs repel more than bonding pairs) 3. State actual shape and bonding angle/s
29
How much do lone pairs reduce bond angles
2.5
30
Outline a square planar molecule. Give an example.
4 bonding pairs 2 lone pairs Bond angle 90 XeF4
31
Outline the shape of BrF5
Bond angle 89 4 bond pairs 2 lone pairs
32
Outline the shape of I3 -
Bond angle 180 2 bonding pairs 3 lone pairs
33
Outline the shape of ClF3
Bond angle 89 3 bonding pairs 2 lone pairs
34
Outline the shape of SF4 of IF4 +
Bond angles of 119 and 89 3 bonding pairs 1 lone pair
35
Define electronegativity
The relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself
36
List the 4 most electronegative elements
Fluorine Oxygen Nitrogen Chlorine
37
What factors affect electronegativity
Proton number Atomic radius Shielding
38
Outline how electronegativity changes across the period
Increases Larger proton numbers Smaller atomic radius Electrons closer to nucleus
39
Outline how electronegativity changes down a group
Decreases More shells More shielding Electrons further from the nucleus
40
How does electronegativity effect the type of bonding in a compound
Similar electronegativity Covalent bond Large difference in electronegativity Ionic bond
41
Outline how a permanent dipole (polar covalent) bond forms
Elements in the bond have different electronegativity Difference of around 0.3 to 1.7 Causing an unequal distribution in electrons And thus a charge separation (Delta) + and (delta) -
42
Outline the effects of symmetry in molecules
All bonds are identical With no lone pairs Cannot be a polar molecule As the any dipoles cancel out Due to symmetry
43
When does van der waals occur
Between all molecular substances And Nobel gases Not in ionic substances
44
Describe how van der waals (induced dipole) occurs
Electron density fluctuates Parts of the molecule become more/less negative Induces neighbouring molecules to do the same (induced dipole) The induced dipole is the opposite to the original one
45
Outline the factors effecting van der waals
More electrons More likely to form Increased van der waals Higher boiling points Long chain alkanes more likely More surface area Eg halogens increase down group due to more van der waals
46
When does permanent dipole-dipole occur
Between polar molecules
47
Outline permanent dipole dipole forces
Stronger than van der waals Further increase boiling point Molecules are asymmetrical and have significant electronegativity difference between atoms
48
When does hydrogen bonding occur?
Between hydrogen atoms and either: Oxygen Nitrogen fluorine With a lone pair available
49
Outline hydrogen bonding
Strongest intermolecular bond Causes very high boiling points (eg water is a liquid not gas) Alcohols, carboxylic acids, proteins, amides all form hydrogen bonds
50
Order the intermolecular forces from strongest to weakest
Hydrogen bonding Permanent dipole dipole Van der waals

AS CHEMISTRY (17 decks)

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