Chemical bonding and structure

Question 1

What are ions?

Answer 1

Ions are charged particles formed when atoms gain or lose electrons.

Question 2

How do metals form ions?

Answer 2

Metals lose electrons to form positive ions (cations).

Question 3

How do non-metals form ions?

Answer 3

Non-metals gain electrons to form negative ions (anions).

Question 4

What is the charge on Group 1 ions?

Answer 4

+1

Question 5

What is the charge on Group 2 ions?

Answer 5

+2

Question 6

What is the charge on Group 3 ions?

Answer 6

+3

Question 7

What is the charge on Group 5 ions?

Answer 7

–3

Question 8

What is the charge on Group 6 ions?

Answer 8

–2

Question 9

What is the charge on Group 7 ions?

Answer 9

–1

Question 10

What is ionic bonding?

Answer 10

Ionic bonding is the electrostatic attraction between oppositely charged ions.

Question 11

What happens during ionic bonding?

Answer 11

A metal transfers electrons to a non-metal, forming positive and negative ions.

Question 12

What is the structure of an ionic compound?

Answer 12

A giant ionic lattice—a regular 3D pattern of ions held together by strong forces.

Question 13

Why do ionic compounds have high melting points?

Answer 13

Because of strong electrostatic forces between ions that require a lot of energy to break.

Question 14

What are the properties of ionic compounds?

Answer 14

High melting and boiling points

Conduct electricity when molten or dissolved in water

Usually soluble in water

Question 15

Why can ionic compounds conduct electricity when molten or in solution?

Answer 15

Because the ions are free to move and carry charge.

Question 16

What is covalent bonding?

Answer 16

Covalent bonding is when two or more non-metal atoms share electrons to form a molecule.

Question 17

What are simple covalent molecules?

Answer 17

Molecules with a few atoms bonded covalently, like H₂O or CO₂

Question 18

What is a molecule?

Answer 18

A group of atoms held together by covalent bonds.

Question 19

What are the properties of simple covalent molecules?

Answer 19

Low melting and boiling points

Do not conduct electricity

Often gases or liquids at room temperature

Question 20

Why do simple covalent molecules have low boiling points?

Answer 20

They have weak intermolecular forces, which are easy to break.

Question 21

Why don’t simple covalent substances conduct electricity?

Answer 21

They have no free electrons or ions to carry charge.

Question 22

hat is a giant covalent structure?

Answer 22

A very large structure where all atoms are bonded together by strong covalent bonds (e.g., diamond, graphite).

Question 23

What are the properties of giant covalent structures?

Answer 23

Very high melting and boiling points

Hard

Usually don’t conduct electricity (except graphite)

Question 24

Describe the structure of diamond

Answer 24

each carbon atom forms 4 covalent bonds in a 3D structure. Very hard and strong.

Question 25

Why is diamond hard and has a high melting point?

Answer 25

Because of the many strong covalent bonds throughout the structure.

Question 26

Why doesn’t diamond conduct electricity?

Answer 26

All electrons are used in bonding, so there are no free electrons.

Question 27

Describe the structure of graphite.

Answer 27

Each carbon atom forms 3 covalent bonds, creating layers of hexagons with free (delocalized) electrons between layers.

Question 28

Why does graphite conduct electricity?

Answer 28

It has delocalized electrons that can move and carry charge.

Question 29

Why is graphite soft and slippery?

Answer 29

The layers are held by weak forces and can slide over each other easily.

Question 30

What is metallic bonding?

Answer 30

Metallic bonding is the electrostatic attraction between positive metal ions and delocalized electrons.

Question 31

Why do metals conduct electricity?

Answer 31

They have free-moving delocalized electrons that carry current.

Question 32

Why are metals malleable and ductile?

Answer 32

The layers of atoms can slide over each other without breaking bonds.

Question 33

What are the properties of metals?

Answer 33

Conduct heat and electricity Malleable and ductile Shiny (lustrous) High melting and boiling points

Question 34

What is the structure of metals like?

Answer 34

A giant structure with positive ions in a lattice surrounded by a sea of delocalized electrons.