write the chemical formula for each of the following compounds. identify each as ionic (i) or covalent (c).
__ i __ 11. nickel (ii) chloride
______ 12. copper (ii) nitrate
______ 13. sulfur dioxide
______ 14. magnesium nitride
______ 15. mercury (i) sulfide
______ 16. carbon monoxide
______ 17. iron (ii) oxide
______ 18. diphosphorus pentoxide
______ 19. dihydrogen monoxide
______ 20. ammonium carbonate

Question

Accepted Answer

### 11. nickel (II) chloride
# Explanation:
## Step1: Identify ions and charges
Nickel (II) has a charge of $+2$ ($Ni^{2+}$), chloride ion is $Cl^-$ (charge $ - 1$).
## Step2: Balance charges
To balance the charges, we need 2 chloride ions for 1 nickel (II) ion. So the formula is $NiCl_2$. It is ionic (I) as it has a metal (nickel) and non - metal (chlorine) ion.
# Answer:
I, $NiCl_2$

### 12. copper (II) nitrate
# Explanation:
## Step1: Identify ions and charges
Copper (II) has a charge of $+2$ ($Cu^{2+}$), nitrate ion is $NO_3^-$ (charge $ - 1$).
## Step2: Balance charges
We need 2 nitrate ions to balance the $+2$ charge of copper (II). So the formula is $Cu(NO_3)_2$. It is ionic (I) as it has a metal (copper) and polyatomic non - metal ion.
# Answer:
I, $Cu(NO_3)_2$

### 13. sulfur dioxide
# Explanation:
## Step1: Identify atoms and prefixes
Sulfur (S) and oxygen (O). The prefix "di - " for oxygen means 2 oxygen atoms.
## Step2: Write the formula
So the formula is $SO_2$. It is covalent (C) as it is formed by non - metals (sulfur and oxygen) sharing electrons.
# Answer:
C, $SO_2$

### 14. magnesium nitride
# Explanation:
## Step1: Identify ions and charges
Magnesium has a charge of $+2$ ($Mg^{2+}$), nitride ion is $N^{3 - }$.
## Step2: Balance charges
Using the criss - cross method: the charge of magnesium becomes the subscript of nitrogen and vice - versa. So we have $Mg_3N_2$. It is ionic (I) as it has a metal (magnesium) and non - metal (nitrogen) ion.
# Answer:
I, $Mg_3N_2$

### 15. mercury (I) sulfide
# Explanation:
## Step1: Identify ions and charges
Mercury (I) exists as $Hg_2^{2+}$ (charge $+2$ for the dimer), sulfide ion is $S^{2 - }$.
## Step2: Balance charges
The charges are equal in magnitude ($+2$ and $- 2$), so the formula is $Hg_2S$. It is ionic (I) as it has a metal (mercury) and non - metal (sulfur) ion.
# Answer:
I, $Hg_2S$

### 16. carbon monoxide
# Explanation:
## Step1: Identify atoms and prefixes
Carbon (C) and oxygen (O). The prefix "mono - " for oxygen means 1 oxygen atom.
## Step2: Write the formula
So the formula is $CO$. It is covalent (C) as it is formed by non - metals (carbon and oxygen) sharing electrons.
# Answer:
C, $CO$

### 17. iron (II) oxide
# Explanation:
## Step1: Identify ions and charges
Iron (II) has a charge of $+2$ ($Fe^{2+}$), oxide ion is $O^{2 - }$.
## Step2: Balance charges
The charges are equal in magnitude ($+2$ and $- 2$), so the formula is $FeO$. It is ionic (I) as it has a metal (iron) and non - metal (oxygen) ion.
# Answer:
I, $FeO$

### 18. diphosphorus pentoxide
# Explanation:
## Step1: Identify atoms and prefixes
Phosphorus (P) with prefix "di - " means 2 phosphorus atoms, oxygen (O) with prefix "pento - " means 5 oxygen atoms.
## Step2: Write the formula
So the formula is $P_2O_5$. It is covalent (C) as it is formed by non - metals (phosphorus and oxygen) sharing electrons.
# Answer:
C, $P_2O_5$

### 19. dihydrogen monoxide
# Explanation:
## Step1: Identify atoms and prefixes
Hydrogen (H) with prefix "di - " means 2 hydrogen atoms, oxygen (O) with prefix "mono - " means 1 oxygen atom.
## Step2: Write the formula
This is the covalent compound water, formula $H_2O$. It is covalent (C) as it is formed by non - metals (hydrogen and oxygen) sharing electrons.
# Answer:
C, $H_2O$

### 20. ammonium carbonate
# Explanation:
## Step1: Identify ions and charges
Ammonium ion is $NH_4^+$ (charge $+1$), carbonate ion is $CO_3^{2 - }$ (charge $- 2$).
## Step2: Balance charges
We need 2 ammonium ions to balance the $- 2$ charge of carbonate. So the formula is $(NH_4)_2CO_3$. It is ionic (I) as it has a polyatomic metal - like ion (ammonium) and polyatomic non - metal ion (carbonate).
# Answer:
I, $(NH_4)_2CO_3$

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QUESTION IMAGE

Question

Explanation:

11. nickel (II) chloride

Step1: Identify ions and charges

Step2: Balance charges

Step1: Identify ions and charges

Step2: Balance charges

Step1: Identify atoms and prefixes

Step2: Write the formula

Answer:

12. copper (II) nitrate