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11E > Structure and Bonding > Flashcards

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?

A

Graphite

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
Q

Why are metals malleable?

A

Layers of atoms are able to slide over each other

26
Q

Why do metals have high melting and boiling points?

A

Strong attraction between positive metal ions and negative electrons requrie a lot of energy to overcome

27
Q

Why do metals conduct electricity?

A

Delocalised electrons can move and carry the charge

28
Q

What is an alloy?

A

A mixture of two or more substances, one of which must be a metal

29
Q

Why are alloys stronger than pure metals?

A

The layers of atoms are distorted by the different sized atoms, these layers do not slide over each other easily

30
Q

Describe what happens to a metal atom and a non-metal atom when an ionic bond forms

A

Metal atoms lose electrons to become a positive ion. Non-metals gains electrons to become a negative ion.

31
Q

Describe what happens when one chlorine atom forms a bond with another chlorine atom

A

An electron from each atom is shared so that each atom has a complete outer shell of electrons

32
Q

Explain why most polymers are solid at room temperature

A

The atoms within polymer molecules are held together by strong covalent bonds. The intermolecular forces between the large polymer molecules are also quite strong

11E (24 decks)

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