question 1. complete the following table:
| characteristic | ionic compound |
| --- | --- |
| representative unit | |
| types of elements | |
| bond formation | |
| physical state | |
| melting point | |
| boiling point | |
| solubility in water | |
| electrical conductivity in aqueous solution | |
question 2. most ionic compounds are ____________ at room temperature.
question 3. is the following statement true or false? explain your reasoning.
statement: ionic compounds generally have low melting points.
question 4. list three properties and provide two examples of ionic compounds.

Question

question 1. complete the following table:
| characteristic | ionic compound |
| --- | --- |
| representative unit |  |
| types of elements |  |
| bond formation |  |
| physical state |  |
| melting point |  |
| boiling point |  |
| solubility in water |  |
| electrical conductivity in aqueous solution |  |
question 2. most ionic compounds are ____________ at room temperature.
question 3. is the following statement true or false? explain your reasoning.
statement: ionic compounds generally have low melting points.
question 4. list three properties and provide two examples of ionic compounds.

Accepted Answer

### Question 1
# Explanation:
## Step1: Representative unit
Ionic compounds are made of ions, so the representative unit is a formula unit (e.g., $ \text{NaCl} $ for sodium chloride, representing the ratio of $ \text{Na}^+ $ and $ \text{Cl}^- $ ions).
## Step2: Types of elements
Ionic compounds form between a metal (which loses electrons to form a cation) and a non - metal (which gains electrons to form an anion). Some can also form between a metal and a polyatomic ion (e.g., $ \text{Na}_2\text{CO}_3 $, where $ \text{Na} $ is metal and $ \text{CO}_3^{2 - } $ is a polyatomic ion).
## Step3: Bond formation
Ionic bonds are formed by the transfer of electrons from a metal to a non - metal (or polyatomic ion). The metal atom loses electrons to become a cation, and the non - metal (or polyatomic ion) gains electrons to become an anion. The electrostatic attraction between the oppositely charged ions forms the ionic bond.
## Step4: Physical state
At room temperature, most ionic compounds are solids. This is because the strong electrostatic forces between the ions hold them in a rigid, ordered lattice structure.
## Step5: Melting point
Ionic compounds have high melting points. The strong electrostatic forces between the ions require a large amount of energy to break the lattice structure and convert the solid into a liquid. For example, sodium chloride ($ \text{NaCl} $) has a melting point of around $ 801^\circ\text{C} $.
## Step6: Boiling point
Ionic compounds also have high boiling points. Similar to the melting point, a large amount of energy is needed to overcome the strong ionic attractions and convert the liquid into a gas. For $ \text{NaCl} $, the boiling point is around $ 1413^\circ\text{C} $.
## Step7: Solubility in water
Many ionic compounds are soluble in water. Water is a polar molecule, and the polar water molecules can surround the ions (hydration) and separate them from the lattice. However, some ionic compounds like silver chloride ($ \text{AgCl} $) are insoluble due to the relatively low energy of hydration compared to the lattice energy.
## Step8: Electrical conductivity in aqueous solution
When ionic compounds dissolve in water, they dissociate into ions. These mobile ions can carry an electric current, so ionic compounds in aqueous solution are good electrical conductors.

The completed table is as follows:

| Characteristic | Ionic Compound |
|--|--|
| Representative unit | Formula unit (e.g., $ \text{NaCl} $ represents the ratio of $ \text{Na}^+ $ and $ \text{Cl}^- $ ions) |
| Types of elements | Metal and non - metal (or metal and polyatomic ion) |
| Bond formation | Transfer of electrons from metal to non - metal (or polyatomic ion) to form oppositely charged ions, held together by electrostatic attraction |
| Physical state | Solid (at room temperature, most) |
| Melting point | High (e.g., $ \text{NaCl} $: $ 801^\circ\text{C} $) |
| Boiling point | High (e.g., $ \text{NaCl} $: $ 1413^\circ\text{C} $) |
| Solubility in water | Many are soluble (e.g., $ \text{NaCl} $), some insoluble (e.g., $ \text{AgCl} $) |
| Electrical conductivity in aqueous solution | Good (ions are mobile and can carry charge) |

### Question 2
# Explanation:
Ionic compounds have a rigid, ordered lattice structure held together by strong electrostatic forces between ions. At room temperature (around $ 25^\circ\text{C} $), the thermal energy is not sufficient to break this lattice structure. So, most ionic compounds are solids at room temperature.
# Answer:
solid

### Question 3
# Explanation:
Ionic compounds have a lattice structure where ions are held together by strong electrostatic forces of attraction. To melt an ionic compound, we need to supply enough energy to overcome these strong forces. Since the electrostatic forces are very strong, a large amount of energy (in the form of heat) is required, which corresponds to a high melting point. For example, $ \text{NaCl} $ has a melting point of about $ 801^\circ\text{C} $, which is relatively high. So the statement "Ionic compounds generally have low melting points" is false.
# Answer:
False. Ionic compounds have a lattice structure with ions held by strong electrostatic forces. A large amount of energy is needed to break this lattice, so they generally have high melting points (e.g., $ \text{NaCl} $ melts at $ 801^\circ\text{C} $).

### Question 4
# Explanation:
## Step1: Properties of ionic compounds
- Property 1: High melting and boiling points. As explained earlier, the strong electrostatic forces between ions require a large amount of energy to break the lattice structure for melting and further energy for boiling.
- Property 2: Solubility in polar solvents (like water). Polar solvents can hydrate the ions and separate them from the lattice. For example, $ \text{NaCl} $ dissolves in water as $ \text{Na}^+ $ and $ \text{Cl}^- $ ions are hydrated by water molecules.
- Property 3: Good electrical conductivity in aqueous solution or molten state. In aqueous solution, the ions are mobile and can carry an electric current. In the molten state, the ions are also free to move.

## Step2: Examples of ionic compounds
- Example 1: Sodium chloride ($ \text{NaCl} $). It is formed from $ \text{Na}^+ $ (sodium ion) and $ \text{Cl}^- $ (chloride ion) by ionic bonding.
- Example 2: Calcium carbonate ($ \text{CaCO}_3 $). It is formed from $ \text{Ca}^{2+} $ (calcium ion) and $ \text{CO}_3^{2 - } $ (carbonate ion).

# Answer:
Properties: 1. High melting and boiling points; 2. Soluble in polar solvents (e.g., water) (many); 3. Good electrical conductivity in aqueous solution or molten state.

Examples: 1. Sodium chloride ($ \text{NaCl} $); 2. Calcium carbonate ($ \text{CaCO}_3 $).

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Question 1

Step1: Representative unit

Step2: Types of elements

Step3: Bond formation

Step4: Physical state

Step5: Melting point

Step6: Boiling point

Step7: Solubility in water

Step8: Electrical conductivity in aqueous solution

Question 2

Answer:

Question 3

characteristic	ionic compound
types of elements
bond formation
physical state
melting point
boiling point
solubility in water
electrical conductivity in aqueous solution

Characteristic	Ionic Compound
Types of elements	Metal and non - metal (or metal and polyatomic ion)
Bond formation	Transfer of electrons from metal to non - metal (or polyatomic ion) to form oppositely charged ions, held together by electrostatic attraction
Physical state	Solid (at room temperature, most)
Melting point	High (e.g., \( \text{NaCl} \): \( 801^\circ\text{C} \))
Boiling point	High (e.g., \( \text{NaCl} \): \( 1413^\circ\text{C} \))
Solubility in water	Many are soluble (e.g., \( \text{NaCl} \)), some insoluble (e.g., \( \text{AgCl} \))
Electrical conductivity in aqueous solution	Good (ions are mobile and can carry charge)