Bonding, Structure, and Properties of Matter Flashcards

1
Q

What is ionic bonding?

A

Metals combined with non-metals, particles are oppositely charged ions.

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2
Q

What is covalent bonding?

A

Non-metals and non-metals sharing pairs of electrons.

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3
Q

What is metallic bonding?

A

Metallic elements and alloys, particles are atoms which share delocalised electrons.

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4
Q

Explain ionic bonding.

A

*Electrons in the outer shell of the metal atom are transferred.
*Metal atoms lose electrons to become positively charged ions.
* Non-metal atoms gain electrons to become negatively charged ions.

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5
Q

Describe the structure of ionic compounds.

A

*Giant structure of ions held together by strong electrostatic forces of attraction between oppositely charged ions.
*Regular structures
*The forces act in all directions in the lattice.
*High melting and boiling points
*Due to large amounts of energy needed to break strong bonds
*Conduct electricity when melted or dissolved in water as free to carry charge

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6
Q

What ions do group 1 elements form?

A

1+ ions

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7
Q

What ions do group 2 elements form?

A

2+ ions

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8
Q

What ions do group 6 elements form?

A

2- ions

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9
Q

What ions do group 7 elements form?

A

1- ions

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10
Q

What does the amount of energy needed to change state depend on?

A

The strength of the intermolecular forces

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11
Q

When would boiling and melting points be higher?

A

When the intermolecular forces are stronger

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12
Q

What is the state symbol for solids?

A

s

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13
Q

What is the state symbol for liquids?

A

l

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14
Q

What is the state symbol for gases?

A

g

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15
Q

What is the state symbol for aqueous

A

aq

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16
Q

Describe properties of small molecules

A

*usually gases or liquids
*low melting and boiling points
*weak intermolecular forces
*Don’t conduct electricity

17
Q

What are the forces like between polymers?

A

*Very large molecules so string covalent bonds
*Relatively strong intermolecular forces
*So solids at room temperatures

18
Q

Describe giant covalent structures

A

*Solids with very high melting points
*Linked with strong covalent bonds
*Diamond and graphite and silicon dioxide are examples

19
Q

Describe properties of metals

A

*Giant structures of atoms with strong metalic bonds
*High melting and boiling points

20
Q

Describe properties of metals

A

*Giant structures of atoms with strong metalic bonds
*High melting and boiling points

21
Q

What are pure metals and why are they alloyed?

A

*Arranged in layers
*Metals can be bent and shaped
*Alloyed as they are too strong
*Alloys distrupt layers and make metals harder

22
Q

Why are metals good conductors?

A

They have a delocalised electron that is free to move and carry charge

23
Q

Describe the structure and bonding or diamond

A

*Each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure
*Diamond is very hard
*HIgh melting and boiling points
*Does not conduct electricity

24
Q

Describe structure and bonding of graphite.

A

*Each carbon atom forms 3 covalent bonds
*Forming layers of hexagonal rings
*No covalent bonds between layers
*One electron from each carbon atom is delocalised
*So can conduct electricity

25
Q

Describe structure and bonding of Graphene

A

*One layer of Graphite
*One atom thick
*Covalent bonds make it very strong
*Contains delocalised electrons
*So can conduct electricity

26
Q

describe structure and bonding of fullerenes.

A

*molecules of carbon atoms with hollow shapes
*First fullerene was buckminsterfullerene C60

27
Q

Describe carbon nanotubes

A

*Fullerenes can form nanotubes
*Conduct electricity and thermal energy
*Can be used in electronics, drug delivery or to strengthen materials without adding much weight