11. define ionic bond.
12. what is the charge on an ionic compound?
13. ionic bonds occur between a _____________ and a _____________.
14. metals always __________ electrons.
15. nonmetals always __________ electrons.
16. write out the rules for writing ionic formulas when you have the name of the ionic compound.
17. what is the super easy way to write ionic formulas?
18. what are the rules for writing the names of ionic compounds when you have the formula?
19. write all of the nonmetals and their -ide name

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Accepted Answer

### Question 11: Define ionic bond.
# Brief Explanations:
An ionic bond is a type of chemical bond formed through the electrostatic attraction between oppositely charged ions. These ions are created when atoms (usually a metal and a non - metal) transfer electrons: the metal atom loses one or more electrons to become a positively charged cation, and the non - metal atom gains those electrons to become a negatively charged anion. The electrostatic force of attraction between these cations and anions holds the ionic compound together.
# Answer:
An ionic bond is the electrostatic attraction between positively - charged cations and negatively - charged anions, formed by electron transfer between a metal and a non - metal atom.

### Question 12: What is the charge on an ionic compound?
# Brief Explanations:
In an ionic compound, the total positive charge from the cations is equal to the total negative charge from the anions. This is because the electrons lost by the metal atoms (to form cations) are gained by the non - metal atoms (to form anions). So, the overall charge of an ionic compound is zero (neutral). For example, in NaCl, Na⁺ has a + 1 charge and Cl⁻ has a - 1 charge, and (+1)+(- 1)=0.
# Answer:
The charge on an ionic compound is zero (neutral), as the total positive charge of cations equals the total negative charge of anions.

### Question 13: Ionic bonds occur between a _ and a _.
# Brief Explanations:
Ionic bonds are formed when there is a transfer of electrons. Metals have a tendency to lose electrons (due to their low ionization energy) and form positive ions (cations). Non - metals have a tendency to gain electrons (due to their high electron affinity) and form negative ions (anions). The electrostatic attraction between these cations (from metals) and anions (from non - metals) results in an ionic bond.
# Answer:
Ionic bonds occur between a metal and a non - metal.

### Question 14: Metals always _ electrons.
# Brief Explanations:
Metals are located on the left - hand side of the periodic table. They have relatively few valence electrons (usually 1 - 3) and a low ionization energy. This means it is relatively easy for them to lose these valence electrons. When they lose electrons, they form positively charged ions (cations). For example, sodium (Na) loses one electron to form Na⁺, and magnesium (Mg) loses two electrons to form Mg²⁺.
# Answer:
Metals always lose electrons.

### Question 15: Nonmetals always _ electrons.
# Brief Explanations:
Non - metals are located on the right - hand side of the periodic table (except for hydrogen). They have a relatively high number of valence electrons (usually 4 - 7) and a high electron affinity. This means they have a strong tendency to gain electrons to achieve a stable electron configuration (usually a full octet). For example, chlorine (Cl) gains one electron to form Cl⁻, and oxygen (O) gains two electrons to form O²⁻.
# Answer:
Nonmetals always gain electrons.

### Question 16: Write out the rules for writing ionic formulas when you have the name of the ionic compound.
# Brief Explanations:
1. **Identify the ions**: Determine the cation (from the metal or polyatomic cation) and the anion (from the non - metal or polyatomic anion) from the name. For example, in "sodium chloride", the cation is Na⁺ (from sodium) and the anion is Cl⁻ (from chloride, which comes from chlorine).
2. **Determine the charges**: Know the common charges of the ions. For main - group metals, the charge is usually equal to their group number (e.g., Group 1 metals have + 1 charge, Group 2 metals have + 2 charge). For non - metals, the charge is usually equal to (group number - 8) (e.g., Group 17 non - metals have - 1 charge). For polyatomic ions, use the known charge of the polyatomic ion (e.g., OH⁻ has a - 1 charge, SO₄²⁻ has a - 2 charge).
3. **Balance the charges**: The total positive charge of the cations must equal the total negative charge of the anions. To do this, use subscripts. The subscript of a cation is equal to the magnitude of the anion's charge, and the subscript of an anion is equal to the magnitude of the cation's charge. For example, for aluminum oxide: Al has a + 3 charge, O has a - 2 charge. The subscript for Al is 2 (magnitude of O's charge) and the subscript for O is 3 (magnitude of Al's charge), so the formula is Al₂O₃. If the charges are equal (e.g., Na⁺ and Cl⁻), the subscripts are 1 (and usually not written), so NaCl.
4. **Write the formula**: Write the symbol of the cation first, followed by the symbol of the anion. Include the subscripts to show the ratio of ions needed to balance the charges.
# Answer:
1. Identify the cation (from metal/polyatomic cation) and anion (from non - metal/polyatomic anion) from the name.
2. Determine the charges of the ions (using group number for main - group elements, known charges for polyatomic ions).
3. Balance the total positive and negative charges by using subscripts (subscript of cation = magnitude of anion's charge, subscript of anion = magnitude of cation's charge).
4. Write the cation symbol first, then the anion symbol, with subscripts as needed.

### Question 17: What is the SUPER EASY WAY to write ionic formulas?
# Brief Explanations:
The "criss - cross" method is a simple way.
1. **Step 1: Write the ions with their charges**: Write the symbol of the cation with its charge and the symbol of the anion with its charge. For example, for calcium nitride, Ca has a + 2 charge (Ca²⁺) and N has a - 3 charge (N³⁻).
2. **Step 2: Criss - cross the charges**: Take the magnitude of the charge of the cation and use it as the subscript for the anion, and take the magnitude of the charge of the anion and use it as the subscript for the cation. So for Ca²⁺ and N³⁻, we get Ca₃N₂.
3. **Step 3: Simplify (if needed)**: If the subscripts have a common factor, divide them by that factor. For example, for Mg²⁺ and O²⁻, we would initially get Mg₂O₂, but we can simplify by dividing by 2 to get MgO.
# Answer:
The "criss - cross" method: 1. Write ions with charges (cation first, anion second). 2. Swap (criss - cross) the magnitude of each ion's charge to be the subscript of the other ion. 3. Simplify subscripts if they have a common factor.

### Question 18: What are the rules for writing the names of ionic compounds when you have the formula?
# Brief Explanations:
1. **For binary ionic compounds (containing a metal and a non - metal)**:
    - Name the cation first: If the metal is a main - group metal with only one common charge, use the element's name. For example, Na⁺ is sodium, Mg²⁺ is magnesium. If the metal is a transition metal (or a main - group metal with more than one common charge), use the element's name followed by a Roman numeral in parentheses to indicate the charge of the cation. For example, Fe²⁺ is iron(II), Fe³⁺ is iron(III).
    - Name the anion second: For a non - metal anion, change the ending of the non - metal's name to - ide. For example, Cl⁻ is chloride, O²⁻ is oxide, S²⁻ is sulfide.
2. **For ionic compounds with polyatomic ions**:
    - Name the cation first (following the same rules as for binary compounds: element name or element name with Roman numeral for charge).
    - Name the polyatomic ion second. Use the name of the polyatomic ion as it is (e.g., OH⁻ is hydroxide, SO₄²⁻ is sulfate, NH₄⁺ is ammonium). For example, NaOH is sodium hydroxide, (NH₄)₂SO₄ is ammonium sulfate, Fe(NO₃)₃ (Fe has + 3 charge) is iron(III) nitrate.
# Answer:
1. Binary (metal - non - metal):
    - Cation: Main - group (1 charge) - element name; Transition/main - group (multiple charges) - element name + Roman numeral (charge).
    - Anion: Non - metal name → - ide.
2. With polyatomic ions:
    - Cation: As above.
    - Anion: Use polyatomic ion name.

### Question 19: Write all of the nonmetals and their - IDE name
# Brief Explanations:
First, we list some common non - metals and their corresponding - ide names:
- Hydrogen: Hydride (H⁻)
- Fluorine: Fluoride (F⁻)
- Chlorine: Chloride (Cl⁻)
- Bromine: Bromide (Br⁻)
- Iodine: Iodide (I⁻)
- Oxygen: Oxide (O²⁻)
- Sulfur: Sulfide (S²⁻)
- Nitrogen: Nitride (N³⁻)
- Phosphorus: Phosphide (P³⁻)
- Carbon: Carbide (C⁴⁻, though carbon can also form other anions, carbide is a common - ide anion for carbon)

These non - metals gain electrons to form anions, and the - ide suffix is used in their anion names.
# Answer:
| Non - metal | - IDE name (anion) |
| ---- | ---- |
| Hydrogen | Hydride (H⁻) |
| Fluorine | Fluoride (F⁻) |
| Chlorine | Chloride (Cl⁻) |
| Bromine | Bromide (Br⁻) |
| Iodine | Iodide (I⁻) |
| Oxygen | Oxide (O²⁻) |
| Sulfur | Sulfide (S²⁻) |
| Nitrogen | Nitride (N³⁻) |
| Phosphorus | Phosphide (P³⁻) |
| Carbon | Carbide (C⁴⁻) |

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Question 11: Define ionic bond.

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Question 12: What is the charge on an ionic compound?