C3 Structure and Bonding

Question 1

What are the three main types of chemical bonding?

Answer 1

Ionic bonding, covalent bonding, and metallic bonding.

Question 2

What happens in ionic bonding?

Answer 2

Atoms transfer electrons, forming oppositely charged ions that attract each other.

Question 3

What happens in covalent bonding?

Answer 3

Atoms share electrons to achieve a full outer shell of electrons.

Question 4

What happens in metallic bonding?

Answer 4

Electrons are delocalized and free to move between metal ions, creating a “sea of electrons.”

Question 5

What is the structure of an ionic compound?

Answer 5

Ionic compounds form a regular lattice structure of oppositely charged ions.

Question 6

What is the structure of a covalent compound?

Answer 6

Covalent compounds may have simple molecular structures or giant covalent structures.

Question 7

What are the properties of metals?

Answer 7

Metals are malleable, ductile, good conductors of electricity and heat, and have high melting points.

Question 8

What is a giant covalent structure?

Answer 8

A structure where atoms are bonded by strong covalent bonds in a large, repeating network.

Question 9

What is an example of a material with a giant covalent structure?

Answer 9

Diamond and graphite are examples of giant covalent structures.

Question 10

How do the properties of ionic compounds differ from those of covalent compounds?

Answer 10

Ionic compounds have high melting points and conduct electricity when molten, while covalent compounds generally have low melting points and do not conduct electricity.

Question 11

What type of bonding is present in sodium chloride (NaCl)?

Answer 11

Sodium chloride has ionic bonding between sodium and chlorine ions.

Question 12

What is the melting point of ionic compounds like?

Answer 12

Ionic compounds typically have high melting and boiling points due to strong electrostatic forces between ions.

Question 13

Why do metals conduct electricity?

Answer 13

Metals conduct electricity because of the free-moving delocalized electrons in metallic bonding.

Question 14

Why do ionic compounds conduct electricity when molten?

Answer 14

In molten form, the ions are free to move, allowing electrical current to pass through.

Question 15

What is the general structure of a polymer?

Answer 15

Polymers have long chains of repeating monomers linked by covalent bonds.

Question 16

What is a polymer?

Answer 16

A polymer is a long chain of repeating monomer units linked by covalent bonds.

Question 17

How does the structure of diamond affect its properties?

Answer 17

Diamond has a strong, rigid structure, making it extremely hard and an excellent heat conductor.

Question 18

How does the structure of graphite affect its properties?

Answer 18

Graphite has layers of carbon atoms with weak forces between layers, making it slippery and a good conductor of electricity.

Question 19

What is the main difference between metallic and ionic bonding?

Answer 19

Metallic bonding involves a sea of delocalized electrons, while ionic bonding involves transfer of electrons between ions.

Question 20

What happens to the electrons in an ionic bond?

Answer 20

Electrons are transferred from one atom to another, forming positively and negatively charged ions.

Question 21

How does the bond strength of covalent compounds compare to ionic compounds?

Answer 21

Covalent bonds are generally weaker than ionic bonds, but they can form large structures (e.g., diamond) that are very strong.

Question 22

What is an example of a covalent bond?

Answer 22

The bond between two hydrogen atoms in H₂ (hydrogen molecule) is an example of a covalent bond.

Question 23

What is a simple molecular structure?

Answer 23

A simple molecular structure consists of individual molecules held together by weak intermolecular forces.

Question 24

What is a metallic structure like?

Answer 24

A metallic structure consists of metal atoms arranged in a regular lattice, surrounded by a sea of delocalized electrons.

Question 25

Why are metals good conductors of electricity?

Answer 25

Metals conduct electricity due to the presence of free-moving, delocalized electrons.

Question 26

What is an example of a material with metallic bonding?

Answer 26

Copper (Cu) is an example of a material with metallic bonding.

Question 27

What is the difference between a conductor and an insulator?

Answer 27

A conductor allows electricity to flow through it easily, while an insulator does not.

Question 28

Why does ionic bonding occur?

Answer 28

Ionic bonding occurs because atoms transfer electrons to achieve a stable electron configuration.

Question 29

What is the structure of silicon dioxide (SiO₂)?

Answer 29

Silicon dioxide has a giant covalent structure, with each silicon atom bonded to four oxygen atoms.

Question 30

How does covalent bonding differ in different substances?

Answer 30

In some substances, covalent bonds form simple molecules (e.g., H₂O), while others form giant structures (e.g., diamond).

Question 31

Why are ionic compounds usually solid at room temperature?

Answer 31

Ionic compounds have strong electrostatic forces between ions, which require a lot of energy to break.

Question 32

What type of bond is present in chlorine gas (Cl₂)?

Answer 32

Chlorine gas has a covalent bond between two chlorine atoms.

Question 33

What is a giant ionic structure?

Answer 33

A giant ionic structure is a large lattice of ions bonded by strong ionic bonds, as seen in sodium chloride (NaCl).

Question 34

How do covalent bonds form between atoms?

Answer 34

Covalent bonds form when atoms share electrons to fill their outer electron shell.

Question 35

Why do ionic compounds have high melting and boiling points?

Answer 35

Ionic compounds have strong electrostatic forces between oppositely charged ions, requiring high energy to break.

Question 36

What is the relationship between bond length and bond strength in covalent bonding?

Answer 36

Shorter bonds tend to be stronger because the atoms are held together more tightly.

Question 37

What is the significance of delocalized electrons in metals?

Answer 37

Delocalized electrons allow metals to conduct electricity and heat and make them malleable.

Question 38

How does the size of an ion affect the strength of ionic bonds?

Answer 38

Smaller ions create stronger ionic bonds because they can get closer together, increasing the electrostatic attraction.

Question 39

What is the relationship between structure and properties in materials?

Answer 39

The structure of a material determines its properties, such as strength, flexibility, and conductivity.