quiz 5 review ionic compounds & crystal lattices
name:
period:
date:
1. what is an ionic bond?
an ionic bond forms when electrons are transferred from a metal atom to a nonmetal atom, creating oppositely charged ions that attract each other.

in your own words:
explain how ionic bonds form:
2. writing ionic compound formulas
follow these steps:
1. write the symbol and charge for each ion.
2. balance the charges so the overall compound is neutral.
3. write the formula (cation first, anion second).
examples:
• ( ext{na}^+ ) and ( ext{cl}^- o ext{nacl} )
• ( ext{mg}^{2+} ) and ( ext{cl}^- o ext{mgcl}_2 )
• ( ext{al}^{3+} ) and ( ext{o}^{2-} o ext{al}_2 ext{o}_3 )
practice:

Question

quiz 5 review ionic compounds & crystal lattices
name:
period:
date:
1. what is an ionic bond?
an ionic bond forms when electrons are transferred from a metal atom to a nonmetal atom, creating oppositely charged ions that attract each other.

in your own words:
explain how ionic bonds form:
2. writing ionic compound formulas
follow these steps:
1. write the symbol and charge for each ion.
2. balance the charges so the overall compound is neutral.
3. write the formula (cation first, anion second).
examples:
• ( 	ext{na}^+ ) and ( 	ext{cl}^- 	o 	ext{nacl} )
• ( 	ext{mg}^{2+} ) and ( 	ext{cl}^- 	o 	ext{mgcl}_2 )
• ( 	ext{al}^{3+} ) and ( 	ext{o}^{2-} 	o 	ext{al}_2	ext{o}_3 )
practice:

Accepted Answer

# Explanation:
## Step1: Balance charges for $Ca^{2+}$ and $F^{-}$
Calcium has a charge of $+ 2$, fluorine has a charge of $-1$. To balance, we need $2$ $F^{-}$ ions.
## Step2: Write formula for $Ca^{2+}$ and $F^{-}$
Cation ($Ca^{2+}$) first, anion ($F^{-}$) second. So formula is $CaF_{2}$, name is calcium fluoride.
## Step3: Balance charges for $K^{+}$ and $O^{2 -}$
Potassium has a charge of $+1$, oxygen has a charge of $-2$. To balance, we need $2$ $K^{+}$ ions.
## Step4: Write formula for $K^{+}$ and $O^{2 -}$
Cation ($K^{+}$) first, anion ($O^{2 -}$) second. So formula is $K_{2}O$, name is potassium oxide.
## Step5: Balance charges for $Na^{+}$ and $S^{2 -}$
Sodium has a charge of $+1$, sulfur has a charge of $-2$. To balance, we need $2$ $Na^{+}$ ions.
## Step6: Write formula for $Na^{+}$ and $S^{2 -}$
Cation ($Na^{+}$) first, anion ($S^{2 -}$) second. So formula is $Na_{2}S$, name is sodium sulfide.
## Step7: Balance charges for $Mg^{2+}$ and $N^{3 -}$
Magnesium has a charge of $+2$, nitrogen has a charge of $-3$. LCM of $2$ and $3$ is $6$. So we need $3$ $Mg^{2+}$ ($3\times2 = 6$) and $2$ $N^{3 -}$ ($2\times3=6$)
## Step8: Write formula for $Mg^{2+}$ and $N^{3 -}$
Cation ($Mg^{2+}$) first, anion ($N^{3 -}$) second. So formula is $Mg_{3}N_{2}$, name is magnesium nitride.

# Answer:
| Ions | Final Formula | Name of Compound |
|---|---|---|
| $Ca^{2+}$ and $F^{-}$ | $CaF_{2}$ | calcium fluoride |
| $K^{+}$ and $O^{2 -}$ | $K_{2}O$ | potassium oxide |
| $Na^{+}$ and $S^{2 -}$ | $Na_{2}S$ | sodium sulfide |
| $Mg^{2+}$ and $N^{3 -}$ | $Mg_{3}N_{2}$ | magnesium nitride |

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QUESTION IMAGE

Question

Explanation:

Step1: Balance charges for \(Ca^{2+}\) and \(F^{-}\)

Step2: Write formula for \(Ca^{2+}\) and \(F^{-}\)

Step3: Balance charges for \(K^{+}\) and \(O^{2 -}\)

Step4: Write formula for \(K^{+}\) and \(O^{2 -}\)

Step5: Balance charges for \(Na^{+}\) and \(S^{2 -}\)

Step6: Write formula for \(Na^{+}\) and \(S^{2 -}\)

Step7: Balance charges for \(Mg^{2+}\) and \(N^{3 -}\)

Step8: Write formula for \(Mg^{2+}\) and \(N^{3 -}\)

Answer:

Ions	Final Formula	Name of Compound
\(K^{+}\) and \(O^{2 -}\)	\(K_{2}O\)	potassium oxide
\(Na^{+}\) and \(S^{2 -}\)	\(Na_{2}S\)	sodium sulfide
\(Mg^{2+}\) and \(N^{3 -}\)	\(Mg_{3}N_{2}\)	magnesium nitride