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chemistry ol igcse > Ch.2: Bonding > Flashcards

Ch.2: Bonding Flashcards

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1
Q

What are the properties of Physical Reactions?

A

-The product has same properties as the substances in the beginning

-Easily reversible ⇌

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2
Q

What are examples of physical reactions?

A

Examples:
Melting, Evaporation, Sublimation, Condensation, Dissolving

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3
Q

What are properties of Chemical Reactions?

A

-New substances formed with different characteristics

-Irreversible or cannot easily be reversed

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4
Q

What are examples of chemical reactions?

A

Examples:
Photosynthesis, Combustion (burning), Rusting, Respiration, Neutralization

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5
Q

Define ionic bonding:

A

Electrostatic attraction force between positive and negative ions

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6
Q

How does ionic bonding happen?

A

By the total transfer of electrons from metals to non-metals

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7
Q

Remember that →

A

Metals → loose electrons → Positive ions → Cations
Non-metals → gain electrons → Negative ions → Anions

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8
Q

Define lattice:

A

3D regular arrangement between alternating positive & negative ions

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9
Q

Properties of Ionic Compounds:

A
  • Hard/Strong
  • High b.p & m.p
  • Soluble in water
  • Can conduct electricity only when molten or aqueous
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10
Q

Why do ionic compounds have high melting & boiling points?

A

Due to presence of strong electrostatic attraction force between ions that need high energy to break up the lattice

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11
Q

Why can ionic compounds conduct electricity/heat only when molten or aqueous?

A

As there are free moving ions in molten/aqueous while ions are fixed in lattice when solid and thus are not free moving.

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12
Q

What is simple covalent bonding?

A

Involves the sharing of electrons between non-metals and each-other OR non-metals & hydrogen

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13
Q

Properties of simple covalent compounds:

A
  • Liquids/Gases
  • Insoluble in water
  • Can’t conduct electricity → No free moving electrons
  • Low b.p & m.p (Volatile)
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14
Q

Why are simple covalent compounds simple?

A

Due to weak intermolecular forces that need low energy to break

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15
Q

Remember that →

A

There are no weak covalent bonds. All covalent bonds are strong!

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16
Q

What is the bonding in graphite?

A

Each carbon bonded to 3 carbon atoms by strong covalent bonds forming
layers of hexagons

17
Q

Properties of Graphite:

A
  • Soft & Slippery
  • High m.p & b.p
  • Can conduct electricity
18
Q

Uses of Graphite:

A

Pencils & lubricants → as it is soft & slippery
Electrodes → As they conduct electricity

19
Q

Why can graphite conduct electricity?

A

Have free moving electrons

20
Q

Why is graphite soft & slippery?

A

Layers slide over each-other due to weak wander waal forces

21
Q

What is the bonding in diamond?

A

Each carbon bonded to 4 carbon atoms in tetrahedral structure by
strong covalent bonds

22
Q

Properties of diamond:

A
  • Hard & Strong
  • High m.p & b.p
  • Can not conduct electricity
23
Q

Uses of Diamond:

A

Jewelry → Shiny appearance
Cutting & Drilling → Hard & Strong

24
Q

Why is diamond used in drilling & cutting? (Hard & Strong)

A

Each carbon bonded to 4 carbon atoms in tetrahedral structure by strong covalent bonds

25
Q

What is the bonding in SiO2?

A

Each silicon atom is bonded to 4 oxygen atoms while each oxygen atom is bonded to 2 silicon atoms.

26
Q

Properties of SiO2:

A
  • Hard & Strong
  • High m.p & b.p
  • Can not conduct electricity
27
Q

Uses of SiO2:

A
  • Glass
  • Sandpaper
28
Q

Why is the silicon oxide formula SiO2 not SiO4?

A

Each silicon atom is bonded to 4 oxygen atoms while each oxygen atom is bonded to 2 silicon atoms.

29
Q

Define Metallic Bonding

A

Electrostatic attraction force between layers of positive ions and a sea of free moving electrons

30
Q

Properties of metals:

A
  • Solids at r.t.p
    -Malleable (can be shaped)
    -Ductile (drawn into wires)
    -Conduct heat & electricity
31
Q

Why are metals malleable?

A

Layers of ions slide over each other without breaking metallic bond

chemistry ol igcse (3 decks)

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