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Physical Chem (AS) > 1.3 Bonding > Flashcards

1.3 Bonding Flashcards

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1
Q

Where does ionic bonding occur

A

non-metal and metal

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2
Q

Describe how ionic bonding works

A

Electrons transferred from the metal to the non metal, to achieve full outer shells

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3
Q

How is a giant ionic lattice formed through ionic bonding

A

electrons are transferred, creating charged particles called ions,
oppositely charged ions attract through electrostatic forces of attraction,
forming giant ionic lattices

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4
Q

Give an example of an ionic lattice

A

Sodium Chloride

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5
Q

State the formulas for:
1) Sulfate ion
2) Hydroxide ion
3) Nitrate ion
4) Carbonate ion
5) Ammonium Ion

A
  1. SO4(2-)g
  2. OH(-)
  3. NO3(-)
  4. CO3(2-)
  5. NH4(+)
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6
Q

Where does covalent bonding occur

A

Between non-metal and non-metal

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7
Q

How does covalent bonding occur

A

Electrons are shared betwen the two outer shells in order to achieve a full outer shell of electrons.

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8
Q

What is a dative/ coordinate covalent bond

A

When both of the electrons in the shared pair are supplied from a single atom

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9
Q

Give an example of a dative bond

A

NH4(+)

NH3 has a lone pair, forms a dative bond with H+

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10
Q

How does metallic bonding occur

A

Lattice of positively charged ions, surrounded by a sea of delocalised electrons, forming strong electrostatic force of attraction between oppositely charged particles

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11
Q

How does charge on the positive ion affect the attractive force

A

Greater charge on positive ions, stronger attraction as more electrons are released into the sea

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12
Q

How does size affect attraction

A

Larger size, weaker attraction because of greater atomic radius

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13
Q

Name the four main types of
crystal structures

A
  1. Ionic
  2. metallic
  3. simple molecular
  4. macromolecular
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14
Q

Explain melting and boiling point in ionic crystal structures

A
  • High Melting / Boiling point
  • strong electrostatic forces of attraction
  • holding the ionic lattice together
  • require alot of energy to overcome
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15
Q

Explain electrical conductivity in ionic substances

A
  • Can conduct in molten / solution
  • ions are separated and no longer held in lattice
  • free to move carry a flow of charge
  • and therefore electrical current
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16
Q

Why are ionic substances brittle

(Hard but liable to break easily)

A

Layers of alternating charges distorted, like charges repel, breaking the lattice into fragments

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17
Q

Explain conductivity in metallic structures

A
  • Good conductors
  • sea of delocalised electrons
  • carries charge flow
  • allowing current to pass through
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18
Q

Why are metals malleable

A
  • Layers of positive ions can slide over each other
  • delocalised electrons prevent fragmentation
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19
Q

What is the only metal that is liquid at room temperature

A

Mercury

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20
Q

Explain melting points of metallic structures

A
  • High melting points
  • strong electrostatic forces between positive ions and delocalised electrons
  • require alot of energy to overcome
21
Q

Describe a simple molecular structure

A

Consisting of covalently bonded molecules
Held together by weak Van Der Waals forces

22
Q

Give an example of a simple molecular structure

A

Iodine

23
Q

Explain the melting / boiling point of simple mplecular structures

A
  • Low melting / boiling point
  • weak van der waals forces
  • easy to overcome
24
Q

Why are simple molecular substances poor conductors

A

Their structure contains no charged particles to carry charge flow

25
Q

Describe macromolecular substances

A

Macromolecular structure is covalently bonded into a giant lattice structure

26
Q

Give 2 examples of macromolecular substances made from carbon

A

Diamond and Carbon

27
Q

Why is diamond one of the strongest materials known

A

Each of the carbon atoms is bonded to further four carbon attoms

28
Q

Why can graphite conduct electricity

A
  • Each carbon is bonded to three other carbons in falt sheets
  • Free electrons can move between layers
  • Conducting electricity
29
Q

How much distortion does one lone pair of electrons cause

A

2.5(degrees)

30
Q

Give Name and bond angle

  • 2 bonding pairs
  • 0 lone pairs
A

Linear shape
Bond angle 180°

31
Q

Give Name and bond angle

  • 2 Bonding pairs
  • 2 Lone pairs
A

V - Shaped
Bond angle 104.5°

32
Q

Give name and bond angle

  • 3 Bonding pairs
  • 0 Lone pairs
A

Trigonal Planar
Bond angle 120°

33
Q

Give name and bond angle

  • 3 bonding pairs
  • 1 Lone pair
A

Triangular Pyramid
107°

34
Q

Give name and bond angle

  • 4 Bonding pairs
  • 0 Lone pairs
A

Tetrahedral
109.5°

35
Q

Give name and bond angle

  • 5 Bonding pairs
  • 0 Lone pairs
A

Trigonal Bipyramid
90° and 120°

36
Q

Give name and bond angle

  • 6 Bonding pairs
  • 0 Lone pairs
A

Octahedral
90°

37
Q

Define electronegativity

A

The ability of an atom to attractive a pair of electrons with negative charge

38
Q

Explain how electronegativity changes across a period

A
  • Elecgronegativity increases along a period
  • Atomic radius decreases
39
Q

Explain how electronegativity changes down a group

A
  • Electronegativity decreases down a group
  • Shielding increases
40
Q

When does a polar bond form

A

When two atoms have different electrongetaivities, and one atom draws electrons closer to itself, and away from the other producing partial charges

41
Q

Give an example of a polar molecule

A
  • Water
  • Hydrogen Fluoride
42
Q

What can polar molecules with permenant dipoles form

A

Lattice of molecules

Similar to an ionic lattice

43
Q

Name the three types of intermolecular forces

A
  1. Van Der Waals
  2. Permenant Dipoles
  3. Hydrogen Bonding
44
Q

What does the strength of Van der Waals depend on

A

Mr of the molecule and its shape

45
Q

Explain the link between size of molecule and Van der waals

A

The larger the Mr
Stronger Intermolecular forces
More opportunity for Van der Waals

46
Q

Where do Hydrogen Bonds form

A
  • Hydrogen and Nitrogen
  • Hydrogen and Oxygen
  • Hydrogen and Fluorine

(between the most electronegative elements)

47
Q

How do hydrogen bonds form

A

The Lone pair on the atom forms a bond with the hydrogen, shown with a dotted line

48
Q

What are the melting points like with hydrogen bonding

A

High melting / boilings
strongest intramolecular force
alot of energy to overcome

Physical Chem (AS) (8 decks)

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