The metallic model - properties of metals & their uses Flashcards

1
Q

What is metallic bonding?

A

Metal atoms are tightly packed together in lattice structures

In metallic bonding, the electrons in their outer shells are free to move throughout the structure.

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2
Q

What are delocalised electrons?

A

Electrons that are not bound to their atom and can move freely throughout the metallic structure

Delocalised electrons contribute to metallic bonding and conductivity.

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3
Q

What happens to metal atoms when electrons are delocalised?

A

The metal atoms become positively charged

The positive charges repel each other, maintaining the lattice structure.

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4
Q

What are the properties of metals?

A

Malleability, strength, electrical conductivity, thermal conductivity, high melting and boiling points

These properties result from metallic bonding and the structure of metals.

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5
Q

What is malleability in metals?

A

The ability of metallic compounds to be shaped without breaking

When a force is applied, metal layers can slide and reform metallic bonds.

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6
Q

What contributes to the strength of metallic compounds?

A

The strong attractive forces between metal ions and delocalised electrons

This strong attraction makes metals hard and durable.

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7
Q

How do metals conduct electricity?

A

Through the movement of mobile electrons in solid or liquid states

Delocalised electrons repel from the negative terminal and move towards the positive terminal when a potential difference is applied.

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8
Q

As the number of outer electrons increases across a Period, what happens to electrical conductivity?

A

The ability to conduct electricity increases

For example, sodium has 1 outer electron, while aluminium has 3 outer electrons.

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9
Q

What is thermal conductivity in metals?

A

The ability of metals to conduct heat effectively

This is due to the vibration of cations and the movement of delocalised electrons.

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10
Q

What causes high melting and boiling points in metals?

A

Strong electrostatic forces of attraction between cations and delocalised electrons

Large amounts of energy are required to overcome these forces.

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11
Q

What factors are considered when choosing a metal for a particular use?

A

Malleability, electrical conductivity, thermal conductivity, melting/boiling point, strength, strength-to-weight ratio, density, toxicity, corrosion resistance, reactivity, lustre, sonority

Each property influences the suitability of a metal for specific applications.

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12
Q

Why is aluminium used in food cans?

A

It is non-toxic and resistant to corrosion and acidic foodstuffs

Aluminium’s properties make it ideal for food packaging.

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13
Q

Why is copper used in electrical wiring?

A

It is a good electrical conductor and is malleable/ductile

Copper’s properties allow for effective and flexible wiring solutions.

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14
Q

What is the use of stainless steel?

A

It is used for cutlery due to its strength and corrosion resistance

Stainless steel’s properties make it suitable for kitchenware.

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