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Chemistry Module 2 - Own Flashcards > Chapter 5.2 - Electrons and Bonding (Ionic Bonding) > Flashcards

Chapter 5.2 - Electrons and Bonding (Ionic Bonding) Flashcards

1
Q

What is ionic bonding?

A

Ionic bonding is the electrostatic attraction between positive (cations) and negative (anions) ions, which holds them together in ionic compounds.

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2
Q

What are examples of common cations?

A

Metal Ions: Na+, Ca2+, Al3+
Ammonium ions: NH4+

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3
Q

What are examples of common anions?

A

Non-metal ions: Cl-, O2-
Polyatomic ions: NO3-, SO4(2-)

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4
Q

What is the basic structure of the simplest ionic compounds?

A

They contain metal ions and non-metal ions.

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5
Q

How does ionic bonding occur through electron transfer?

A
  1. Outer-shell electrons from a metal atom are transferred to the outer shell of a non-metal atom.
  2. This forms positive and negative ions.
  3. The ions achieve outer shells with the same electron configuration as the nearest noble gas.
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6
Q

What do dot-and-cross diagrams show in ionic compounds?

A

Dot-and-cross diagrams represent:
1. Electrons in the original atoms as dots or crosses.
2. The charge on each ion.
3. A way to account for all electrons in the structure.

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7
Q

What is the structural feature of all ionic compounds?

A

Ionic compounds form giant ionic lattice structures, where:

  1. Each ion is surrounded by oppositely charged ions.
  2. Billions of ions are arranged in a repeating pattern, determined by the size of the crystal.
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8
Q

Why do ionic compounds generally have high melting and boiling points?

A
  1. Strong electrostatic forces of attraction exist between oppositely charged ions in the giant ionic lattice.
  2. A large amount of energy is required to overcome these forces.
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9
Q

How does ionic charge affect melting points?

A

Higher ionic charges result in stronger ionic attractions, leading to higher melting points.

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10
Q

What is the melting point of: NaF?

A

993°C

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11
Q

What is the melting point of: CaF2?

A

1423°C

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12
Q

What is the melting point of: Na2O?

A

1275°C

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13
Q

What is the melting point of: CaO?

A

2614°C

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14
Q

What types of solvents dissolve many ionic compounds?

A

Polar solvents, such as water.

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15
Q

How does water dissolve ionic compounds?

A

Polar water molecules:

  1. Interact with the ions
  2. Break down the ionic lattice.
  3. Surround the individual ions in solution.
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16
Q

Why might some ionic compounds not dissolve well?

A

In compounds with large ionic charges, the attraction within the lattice may be too strong for water to break down the structure, resulting in low solubility.

17
Q

What two processes are necessary for solubility?

A
  1. Breaking down the ionic lattice.
  2. Attraction of water molecules to surround the ions.
18
Q

How does ionic charge affect solubility?

A

Higher ionic charges lead to stronger lattice attractions, which reduce solubility.

19
Q

Do solid ionic compounds conduct electricity? Why or why not?

A

No, because:

  1. The ions are fixed in position in the giant ionic lattice.
  2. There are no mobile charge carriers.
20
Q

Why are ionic compounds solids at room temperature?

A

At room temperature, there is insufficient energy to overcome the strong electrostatic forces of attraction between the ions in the giant lattice.

21
Q

Why do ionic compounds require high temperatures to melt?

A

High temperatures provide the large amount of energy needed to overcome the strong electrostatic forces between the oppositely charged ions.

22
Q

When do ionic compounds conduct electricity?

A

When they are:

  1. Melted: The lattice breaks down, allowing ions to move freely as mobile charge carriers.
  2. Dissolved in water: The ions become mobile in the solution.
23
Q

What are the main properties of ionic compounds?

A
  1. High melting and boiling points.
  2. Tend to dissolve in polar solvents (e.g., water).
  3. Conduct electricity in the liquid state or aqueous solution, but not in the solid state.
24
Q

Why are dot-and-cross diagrams used in ionic bonding?

A

Dot-and-cross diagrams:

  1. Show the transfer of electrons between atoms.
  2. Indicate the resulting charge on each ion.
  3. Help visualize how the outer-shell electrons are arranged after bonding.
25
Q

What do the outer shells of ions in ionic compounds resemble?

A

The outer shells of ions in ionic compounds usually have the same electron configuration as the nearest noble gas.

26
Q

How are electrons represented in dot-and-cross diagrams?

A

Electrons are shown as:

  1. Dots for one atom.
  2. Crosses for the other atom.
27
Q

What part of the electron structure is typically omitted in dot-and-cross diagrams?

A

The inner (core) electrons are not shown because they do not participate in bonding.

28
Q

What happens to the ionic bonding in a giant ionic lattice?

A

Each ion attracts oppositely charged ions in all directions, resulting in a large, repeating three-dimensional structure.

29
Q

What determines the size of the giant ionic lattice?

A

The size of the lattice depends on the size of the crystal.

30
Q

What is the key feature of a giant ionic lattice?

A

The arrangement of ions ensures that every positive ion is surrounded by negative ions and vice versa.

31
Q

How does the size of ions affect the melting point of an ionic compound?

A

Smaller ions form stronger attractions, leading to higher melting points.

32
Q

What determines the solubility of ionic compounds in water?

A

The solubility depends on:

  1. The strength of attraction within the giant ionic lattice.
  2. The strength of attraction between the ions and water molecules.
33
Q

What happens if the ionic attraction is too strong in a compound?

A

If the ionic lattice attraction is too strong, water cannot break it down, and the compound will have low solubility.

34
Q

Why should predictions of solubility be treated with caution?

A

The relative strengths of lattice attraction and water-ion attraction can vary, making solubility predictions complex.

Chemistry Module 2 - Own Flashcards (10 decks)

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