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Flashcards in Metallic Structures Deck (11):
1

What do metallic bonds involve?

Metallic bonds involve free electrons. These delocalised electrons come from the outer shell of every metal atom in the structure

2

Why are metals God conductors of heat and electricity?

They have free electrons which are free to move through the whole structure

3

What are the forces of attraction like in metals?

There are strong forces of electrostatic attraction between the positive metal ions and the negative electrons

4

What is an alloy?

A mix of two or more metals

5

Describe the structure of an alloy ...

Different elements have different sized atoms. This will distort the layers making it more difficult for them to slider which other so alloys are harder

6

Name the four types of substance structures

Giant ionic
Simple molecular
Giant covalent
Giant metallic

7

How is covalent bonding different from ionic bonding?

In a covalent bond the atoms share electrons . in an ionic bond one of the atoms donates electrons to the other Atom

8

Describe the differences in the physical properties of diamond and graphite

Diamond is very hard and graphite is very soft. Graphite conducts electricity and diamond doesn't.

9

Give an example of a substance that has a giant covalent structure...

Silicone dioxide
Graphite
Diamond

10

Why does chlorine have a very low boiling point?

Because the intermolecular forces between the chlorine molecules are very weak

11

What structure do metals have?

Giant structure