C3 Ionic bonding, metallic bonding and structure Flashcards

1
Q

What is an ion?

A

atom that has either lost or gained electrons

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2
Q

What type of elements form ionic bonds?

A

metals and non-metals

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3
Q

What charge ion does group two form?

A

2+

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4
Q

What charge ion does group six form?

A

2-

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5
Q

What force holds oppositely charged ions together?

A

electrostatic force of attraction

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6
Q

Describe the structure of a giant ionic lattice.

A

alternating positive and negative ions held together by electrostatic force of attraction

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7
Q

Why do ionic substances have a high melting point?

A

lots of energy needed to break the electrostatic force of attraction

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8
Q

Can ionic substances conduct electricity when solid?

A

No

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9
Q

Why don’t ionic substances conduct electricity when solid?

A

ions are in a fixed position and there are no delocalised electrons

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10
Q

Under what circumstances can ionic compound conduct electricity?

A

when molten or dissolved

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11
Q

Describe metallic bonding

A

electrostatic attraction between positive metal ions and delocalised electrons

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12
Q

Properties of pure metals

A

malleable

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13
Q

Why are pure metals malleable?

A

Because each layer of the metal can slide over each other

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14
Q

Why are metals good conductors?

A

Due to the delocalised electrons being able to move throughout the whole structure

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15
Q

Why do metals have a high melting and boilong point?

A

electrostatic force of attraction between the metal ions is strong

so lots of energy is needed to break them

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16
Q

What is an alloy?

A

Mixture of a metal with atoms of another element

17
Q

Why are alloys harder than pure metals?

A

Different sized atoms disturb the layers preventing them from sliding over eachother