C3.9 and C3.10 - Bonding In Metals and propeties(Finished) Flashcards

1
Q

Why are metals malleable?

A

The layers of atoms can slide over eachother

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2
Q

Why are alloys harder than pure metals?

A

Different elements have different sized atoms so when another element is mixed with the metal, the layers will become distorted making it harder for them to slide over each other

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3
Q

What does it mean that electrons are delocalised in a metal?

A

The electrons in the outer shell of the metal atoms are delocalised (free to move around)

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4
Q

What is metallic bonding and what causes it?

A

Metalic bonding is the strong forces of electrostatic attraction between positive metal ions and negative delocalised electrons holding atoms together

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5
Q

Why can metals conduct electricity and heat well?

A

The delocalised electrons can carry current and thermal energy through the structure and quickly

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6
Q

Why can metal layers slide over each other despite large attraction electrostatic forces?

A

Because the delocalised electrons can move and hold ions together at the same time

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7
Q

Why do metals have high boiling and melting points?

A

The electrostatic forces of attraction between metal atoms and delocalised electrons is very strong so lots of energy is needed to break them

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