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Chemistry > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

1
Q

What are the three types of bonding?

A

Ionic Bonding, Covalent Bonding and Metallic Bonding.

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2
Q

What is Ionic Bonding?

A

The bonding of metals and non-metals. Involves the transfer of electrons.

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3
Q

What happens to the metal atoms in an ionic bond?

A

The metal atoms lose electrons to form positively charged ions.

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4
Q

What happens to the non-metal atoms in an ionic bond?

A

The non-metal atoms gain the electrons lost by the metal atoms to form negatively charged ions.

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5
Q

How does the group a metal is in effect how it bonds?

A

The group of a metal tells us how many electrons it will gain or lose. eg. Mg (Group 2), becomes +2 ions.

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6
Q

What are some properties of Ionic Compounds?

A

high melting & boiling points and can conduct electricity in a solution or when melted.

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7
Q

What is Covalent Bonding?

A

Bonding between two non-metals.

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8
Q

What do dot and cross Diagrams show us?

A

Show how electrons rearranged in an atom or ion. Each electron is represented by a dot or a cross.

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9
Q

What is covalent bonding?

A

The bonding of non-metals and non-metals. Atoms share electrons to form two full outer shells.

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10
Q

What is a molecular formula?

A

A molecular formula describes the atoms present in a molecule, eg. H2O (2xH) (1XO)

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11
Q

What are two examples of giant covalent structures?

A

Diamond: each carbon atom is bonded to 4 other carbon atoms (tetrahedral structure).
Graphite: each carbon atom is bonded to 3 other carbon atoms (layers of hexagonal rings)

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12
Q

What are some properties of Graphite structures?

A
  • Has some delocalised electrons
  • Forces between layers are weak. (lubricant)
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13
Q

What is Metallic Bonding?

A

The bonding of metals and metals. The electrons are delocalised and are free to move.

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14
Q

Why can Metallic Bonds conduct electricity?

A

Because the electrons are delocalised and free to move.

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15
Q

What are Alloys?

A

Mixtures of different metals.

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15
Q

What are the three states of matter?

A

Solid, liquid and gas

16
Q

Describe the particles in each of the states of matter?

A

Solid: particles all touching, neat rows, can vibrate to move.
Liquid: particles touching each other and their container, not in rows, particles can move past each other.
Gas: particles moving freely, not touching each other but can collide.

17
Q

Name for the change of matter in:
liquid -> solid
solid -> liquid
liquid -> gas
gas -> liquid

A

freeze
melt
evaporate
condense

18
Q

What are some properties of Diamond structures?

A

Very Hard, high melting points

19
Q

What is the structure of Ionic Compounds? Describe what this means.

A

Giant ionic lattice structures where ions are packed in a regular structure with strong electrostatic forces between oppositely charged ions.

20
Q

Why do small covalent molecules have low melting/boiling points?

A

Weak intermolecular forces.

21
Q

Why do small covalent molecules not conduct electricity?

A

They do not have an overall electric charge.

22
Q

What are the seven diatomic molecules?

A

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine and iodine.

23
Q

What are the three main examples of Giant Covalent Structures?

A

Diamond, Graphite and Silicon Dioxide.

24
Q

Why do Giant Covalent Structures have high melting/boiling points?

A

Strong intermolecular forces.

25
Q

What element is Diamond formed from?

A

Carbon

26
Q

Do Diamond Structures conduct electricity? Explain your answer.

A

No, because all of the outer electrons are in covalent bonds and so there are no free electrons to carry an electrical charge.

27
Q

What are some of the key properties of Graphite? (3)

A

Soft and slippery.
High melting and boiling point.
Conductor of electricity and heat.

28
Q

What element is Graphite formed from?

A

Carbon

29
Q

Why is Graphite soft and slippery?

A

Carbon atoms bond with three other carbon atoms, forming layers of hexagonal shapes. These layers have no covalent bonds between them, so they can slide over each other.

30
Q

Why does Graphite conduct heat and electricity?

A

Carbon atoms have four electrons in their outer shell. In graphite, each carbon atom bonds with three other carbon atoms, leaving one electron. These electrons are delocalised and so can move and conduct electricity.

31
Q

What is Graphene?

A

A single layer of graphite (one atom thick)

32
Q

What are the properties of Graphene? (3)

A
  • Conducts electricity (delocalised electrons)
  • Strong
  • High Melting/Boiling Points
33
Q

What are Fullerenes?

A

Molecules of Carbon forming spheres or tubes.

34
Q

What is Buckminsterfullerene?

A

The first fullerene to be discovered.

35
Q

What are Allotropes?

A

Structures made of the same element but arranged differently.

Chemistry (14 decks)

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