metallic bonding and metals Flashcards

1
Q

how are the atoms within a molecule held together

A

very strong covelent bond

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2
Q

what makes a boiling point/melting point low

A

when the molecules are easilly seperated

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3
Q

why do covenalnt structures have hight boiling points

A

beacuse the covalent bonds are so strong it takes alot of energy to break the forces between the atoms

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4
Q

what cuases a material to conduct electricty

A

when electrons or ions move

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5
Q

what are ionic compounds made of

A

a lattice of negativly and posativly charded ions

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6
Q

why dont solid ionic coumpounds not conduct electricity

A

because the ions arent able to move

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7
Q

how are metals held together

A

metallic bonding

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8
Q

what is the stucture of metals

A

a giant structure of posotive ions surrounded by a sea of de localised electrons

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9
Q

what is metalic bonding

A

the elctrostatic attractions between the nuclei of the posotive ions and the electrons

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10
Q

why are metals good conductors of electricity and heat

A

because the de localaises electrons are able to move through the strcture.

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11
Q

how metals and non metals bond

A

ionic bonding

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12
Q

how to non metals and non metals bond

A

covalent bonding

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13
Q

how to metals bond to other matals

A

metallic bonding

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14
Q

explain metallic bonding

A

when atoms are together in a metal they all give up there outer shell electrons to shair them with the other atoms in the metal. This means that the atoms will all become postaive ions as they have lost negative electrons. The electrons are now free to move about and we call that de localised electrons. There is now electrostatic attractions between the posative ions and the negative electrons.

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