3.1.3.3 Metallic Bonding Flashcards

1
Q

What is the structure of a metal?

A

A lattice of positive ions in a sea of delocalised electrons

Ions sit within the dimples of the recent layer, called a close structure

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2
Q

What does the strength of a metallic bond depend on?

A

Charge of ion: greater the ion, the stronger the electrostatic attraction
Size of ion: smaller the ion, closer the electrons are to the nucleus so the stronger the bond

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3
Q

In a metallic bond, how many electrons are lost?

A

It depends on how many are lost by each atom

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4
Q

What are the properties of metals? (No explanation)

A
Conduct electricity
Have high thermal conductivity
Malleable
High melting/boiling points
Ductile
Mostly insoluble
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5
Q

Why do metals conduct electricity?

A

Delocalised electrons can move through the structure so they’re good conductors of electricity

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6
Q

Why do metals have high thermal conductivity?

A

Because energy is spread via the ions vibrating

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7
Q

Why are metals malleable and ductile?

A

Because the lattice can shift along the layers

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8
Q

Why do metals have high melting/boiling points?

A

Because of the giant structure and the strong attractive force

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9
Q

Why are alloys stronger than pure metals?

A

The particles are different sizes which disrupts the layes and stops them from sliding over eachother

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10
Q

What causes an electrostatic force of attraction?

A

Opposing charges

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11
Q

Is a metal held together by chemical bonds?

A

No

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12
Q

Why is solid carbon strong?

A

Because of the macromolecular structure

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