C4e Flashcards

1
Q

What is a metals structure?

A
  • metals have crystal structures
  • held together by metallic bonding (giving all metals the same basic properties)
  • this allows the outer electron(s) of each atom to move freely
  • creating a sea of delocalised (free) electrons throughout metal which gives rise to many of metals properties
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2
Q

What are the properties of most metals?

A
  • high melting and boiling point and density
  • strong, bendy and malleable
  • good conductors of electricity and heat
  • hard, dense and lustrous
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3
Q

Why do metals have high melting and boiling points?

A
  • strong attraction between delocalised electron and the closely packed positive ions causes very strong metallic bonding
  • metals have high melting and boiling points because of this, you need lots of energy to break them apart
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4
Q

Why are metals strong and flexible and malleable?

A
  • metals have a high tensile strength (strong and hard to break)
  • but can be hammered into different shapes (malleable)
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5
Q

Why are metals good conductors of heat and electricity?

A

-sea of delocalised electrons move freely through metal, carrying electrical current and heat energy

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6
Q

What transition metals and their compounds?

A

-mainly everyday metals

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7
Q

Why are transition metal compounds colourful?

A

-due to the transition metal ion they contain

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8
Q

What are transitional metals used for and where are they on the periodic table?

A
  • catalysts

- middle of periodic table

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9
Q

How does the strength of metallic bonding decrease?

A

-as atomic radius increases

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10
Q

What are some examples of transition metal compounds and their colours?

A
  • iron(II) compounds=light green
  • iron(III) compounds=orange/brown
  • copper compounds=blue
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