Bonding and Structures Flashcards

1
Q

Name the three types of chemical bond

A

Ionic, covalent, metallic

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2
Q

When does ionic bonding occur?

A

When a metallic element reacts with a non-metallic element

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3
Q

How does an ionic bond form?

A

Metal atoms lose electrons to form positive ions, they transfer these to the atoms of non-metallic elements, which form negative ions

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4
Q

What is an ionic bond?

A

An electrostatic force of attraction between oppositely charged ions

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5
Q

When does metallic bonding occur?

A

In a metallic element or alloy, between the metal ions

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6
Q

How does a metallic bond form?

A

Each ion contributes its outer electrons to a ‘sea’ of delocalised electrons, leaving behind positive ions in a lattice structure

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7
Q

What is a metallic bond?

A

An electrostatic force of attraction between the positive ions in the lattice and the negative delocalised electrons

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8
Q

When does covalent bonding occur?

A

When non-metallic atoms bond together. This can be during a reaction, or in the case of diatomic molecules, occur naturally

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9
Q

How does a covalent bond form?

A

When the outer shells of two non-metallic elements overlap each other, causing a pair outer electrons to be shared between the bonding atoms

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10
Q

What is a covalent bond?

A

The electrostatic force of attraction between the positively charged nuclei of the bonded atoms and the shared pair of electrons

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11
Q

Why do atoms form bonds?

A

To achieve a full outer shell of electrons

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12
Q

Describe and explain the melting and boiling properties of ionic compounds

A

High mp and bp because of the large amounts of energy required to break many strong bonds

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13
Q

Describe and explain the electrical conductivity of ionic compounds

A

When melted or dissolved, they conduct electricity because the ions are free to move and a charge can flow

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14
Q

Describe and explain the melting and boiling properties of small molecules

A

They only have weak forces of attraction BETWEEN the molecules, it is these that are overcome NOT the covalent bonds when the substance mealts or boils

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15
Q

Describe and explain the melting and boiling properties of giant covalent structures

A

These are solids with high melting and boiling points. All the atoms are linked by strong covalent bonds. These many bonds must be overcome to melt or boil the substance.

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16
Q

Explain why pure metals can be bent and shaped

A

The atoms are arranged in layers, which can slide over each other

17
Q

Explain why alloys are much harder than pure metals

A

The layers are distorted because the atoms are different sizes, preventing the layers sliding over each other

18
Q

Explain why metals are conductors of electricity

A

The delocalised electrons carry electrical charge through the metal

19
Q

Explain why metals are good heat conductors

A

Thermal energy is tranbferred by the delocalised electrons

20
Q

Describe the similarities and differences in the structures of diamond and graphite

A

Both made of carbon atoms
Both contain many strong covalent bonds
Diamond atoms each bond to 4 other atoms
Graphite each atoms bonds to 3 others with a sea of delocalised electrons between layers, there are no covalent bonds between the layers