Structure and Bonding Flashcards

1
Q

What type of bonding occurs between metals and non-metals?

A

Ionic

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2
Q

What type of bonding occurs between non-metals?

A

Covalent

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3
Q

What type of bonding occurs between metals?

A

Metallic

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4
Q

What type of bonding occurs in sodium chloride?

A

Ionic

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5
Q

What type of bonding occurs in carbon dioxide?

A

Covalent

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6
Q

What type of bonding occurs in sodium?

A

Metallic

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7
Q

What is an ionic bond?

A

Electrostatic attraction between positive metal ions and negative non-metal ions

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8
Q

What is a covalent bond?

A

The sharing of electrons between non-metals

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9
Q

What is a metallic bond?

A

Electrostatic attraction between positive metal ions and negative electrons

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10
Q

What structure are ionic compounds?

A

Ionic lattice

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11
Q

Describe three properties of ionic compounds

A

High melting and boiling points, do not conduct electricity, solid at room temperature

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12
Q

Why do ionic compounds have high melting and boiling points?

A

Ions are held together by very strong bonds, which need a lot of energy to break

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13
Q

Why do ionic compounds not conduct electricity?

A

Ions are held in fixed positions and cannot move

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14
Q

When do ionic compounds conduct electricity?

A

When dissolved or molten

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15
Q

What are the properties of small covalent substances?

A

Usually gas or liquid at room temperature, low melting and boiling points

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16
Q

Why do small covalent substances have low melting or boiling points?

A

Weak intermolecular forces between molecules, which do not need much energy to overcome

17
Q

What are the properties of giant covalent substances?

A

High melting and boiling points, do not conduct electricity

18
Q

Why do giant covalent substances have high melting and boiling points?

A

Atoms are held together by very strong bonds, which need a lot of energy to break

19
Q

Which giant covalent substance is the only one to conduct electricity?

20
Q

Why do covalent substances not conduct electricity?

A

There are no free electrons to carry the charge

21
Q

What is a polymer?

A

A large molecule containing a repeating unit called a monomer

22
Q

Why do polymers have high melting and boiling points?

A

Atoms are held together by very strong bonds, which need a lot of energy to break

23
Q

What is a delocalised electron?

A

An electron which is not held in an atomic shell, is free to move around

24
Q

What are three properties of metals?

A

High melting and boiling points, conducts electricity, malleable

25
Why are metals malleable?
Layers of atoms are able to slide over each other
26
Why do metals have high melting and boiling points?
Strong attraction between positive metal ions and negative electrons requrie a lot of energy to overcome
27
Why do metals conduct electricity?
Delocalised electrons can move and carry the charge
28
What is an alloy?
A mixture of two or more substances, one of which must be a metal
29
Why are alloys stronger than pure metals?
The layers of atoms are distorted by the different sized atoms, these layers do not slide over each other easily
30
Describe what happens to a metal atom and a non-metal atom when an ionic bond forms
Metal atoms lose electrons to become a positive ion. Non-metals gains electrons to become a negative ion.
31
Describe what happens when one chlorine atom forms a bond with another chlorine atom
An electron from each atom is shared so that each atom has a complete outer shell of electrons
32
Explain why most polymers are solid at room temperature
The atoms within polymer molecules are held together by strong covalent bonds. The intermolecular forces between the large polymer molecules are also quite strong