Covalent Bonding Flashcards

0
Q

Are these bonds strong?

A

Yes the attractions between the bonding pair of electrons are strong.

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1
Q

What is a covalent bond?

A

A covalent bond is formed when two atoms (usually non-metals) share a pair of electrons to form a stable electron arrangement.

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2
Q

Do small molecules have simple molecular structures?

A

Yes

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3
Q

What are the forces like between the molecules in small molecules? And what does this result in?

A

The forces between molecules are weak and therefore their melting points and boiling points are low; they are gases liquids or solids with low melting points.

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4
Q

Do simple molecular structures conduct electricity and why?

A

They don’t conduct electricity because there aren’t any free electrons or ions.

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5
Q

Do simple SMS dissolve in anything?

A

Insoluble in water and dissolve in organic solvents.

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6
Q

Give two examples of giant covalent structures.

A

Diamond and graphite.

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7
Q

Describe the structure of atoms in a diamond structure

A

All of covalent bonds are strong and each carbon atom is bonded to 4 others.

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8
Q

Why does diamond have a high melting and boiling point and why is it hard? And does it dissolve in water?

A

Because a lot of energy is needed to break these strong covalent bonds.
No it doesn’t dissolve in water

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9
Q

Why don’t diamonds conduct electricity?

A

Because they’re aren’t any free electrons.

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10
Q

What are graphite and diamond examples of ?

A

Giant covalent structures

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11
Q

Describe the structure of the atoms in a graphite molecule.

A

Graphite consists of many flat layers of hexagons. Each carbon atom is joined to three other carbon atoms. These layers are held together by strong forces of attraction. And the spare electron from each carbon atom is delocalised between the layers and these electrons can move through the structure allowing graphite to conduct electricity.

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