chemistry: ionic (binary, polyatomic, transition metals) and covalent formulas
write the formula for each of the following compounds. find the molar mass
1 sodium hydroxide
1.
2 tetraphosphorus decoxide
2.
3. lead (ii) phosphate
3.
4. ammonium sulfide
4.
5. dicarbon dihydride
5.
6. copper (i) carbonate
6.
7. silicon tetrahydride
7.
8. manganese (ii) sulfate
8.
9. iron (iii) oxide
9.
10. magnesium nitrate
10.
11. calcium sulfide
11.
12. potassium oxide
12.
13. magnesium chloride
13.
14. tricarbon octachloride
14
15. gold (iii) bromide
15.
16. iodine heptafluoride
16.
17. sulfur hexachloride
17
18. iron (ii) phosphide
18.
19. aluminum nitrate
19.
20. diphosphorus pentoxide
20

Question

Accepted Answer

### Problem 1: Sodium Hydroxide
# Explanation:
## Step 1: Determine ions and charges
Sodium ($Na$) has a charge of $+1$, hydroxide ($OH^-$) has a charge of $-1$.
## Step 2: Write formula
To balance charges, the formula is $NaOH$.
## Step 3: Calculate molar mass
Molar mass of $Na$: $22.99$ g/mol, $O$: $16.00$ g/mol, $H$: $1.01$ g/mol.
Molar mass = $22.99 + 16.00 + 1.01 = 40.00$ g/mol.
# Answer: Formula: $NaOH$, Molar Mass: $40.00$ g/mol

### Problem 2: Tetraphosphorus Decoxide
# Explanation:
## Step 1: Use prefixes for subscripts
"Tetra-" means 4 (for P), "deca-" means 10 (for O). So formula is $P_4O_{10}$.
## Step 2: Calculate molar mass
Molar mass of $P$: $30.97$ g/mol (4 atoms: $4\times30.97 = 123.88$ g/mol), $O$: $16.00$ g/mol (10 atoms: $10\times16.00 = 160.00$ g/mol).
Total = $123.88 + 160.00 = 283.88$ g/mol.
# Answer: Formula: $P_4O_{10}$, Molar Mass: $283.88$ g/mol

### Problem 3: Lead (II) Phosphate
# Explanation:
## Step 1: Identify ions and charges
Lead (II): $Pb^{2+}$, Phosphate: $PO_4^{3-}$.
## Step 2: Balance charges
Find least common multiple of 2 and 3, which is 6. So 3 $Pb^{2+}$ and 2 $PO_4^{3-}$. Formula: $Pb_3(PO_4)_2$.
## Step 3: Calculate molar mass
$Pb$: $207.2$ g/mol (3 atoms: $3\times207.2 = 621.6$ g/mol), $P$: $30.97$ g/mol (2 atoms: $2\times30.97 = 61.94$ g/mol), $O$: $16.00$ g/mol (8 atoms: $8\times16.00 = 128.00$ g/mol).
Total = $621.6 + 61.94 + 128.00 = 811.54$ g/mol.
# Answer: Formula: $Pb_3(PO_4)_2$, Molar Mass: $811.54$ g/mol

### Problem 4: Ammonium Sulfide
# Explanation:
## Step 1: Identify ions and charges
Ammonium: $NH_4^+$ (charge +1), Sulfide: $S^{2-}$ (charge -2).
## Step 2: Balance charges
2 $NH_4^+$ and 1 $S^{2-}$. Formula: $(NH_4)_2S$.
## Step 3: Calculate molar mass
$N$: $14.01$ g/mol (2 atoms: $2\times14.01 = 28.02$ g/mol), $H$: $1.01$ g/mol (8 atoms: $8\times1.01 = 8.08$ g/mol), $S$: $32.07$ g/mol (1 atom: $32.07$ g/mol).
Total = $28.02 + 8.08 + 32.07 = 68.17$ g/mol.
# Answer: Formula: $(NH_4)_2S$, Molar Mass: $68.17$ g/mol

### Problem 5: Dicarbon Dihydride
# Explanation:
## Step 1: Use prefixes for subscripts
"Di-" means 2 for C and 2 for H. Formula: $C_2H_2$ (also known as ethyne).
## Step 2: Calculate molar mass
$C$: $12.01$ g/mol (2 atoms: $2\times12.01 = 24.02$ g/mol), $H$: $1.01$ g/mol (2 atoms: $2\times1.01 = 2.02$ g/mol).
Total = $24.02 + 2.02 = 26.04$ g/mol.
# Answer: Formula: $C_2H_2$, Molar Mass: $26.04$ g/mol

### Problem 6: Copper (I) Carbonate
# Explanation:
## Step 1: Identify ions and charges
Copper (I): $Cu^+$, Carbonate: $CO_3^{2-}$.
## Step 2: Balance charges
2 $Cu^+$ and 1 $CO_3^{2-}$. Formula: $Cu_2CO_3$.
## Step 3: Calculate molar mass
$Cu$: $63.55$ g/mol (2 atoms: $2\times63.55 = 127.10$ g/mol), $C$: $12.01$ g/mol (1 atom: $12.01$ g/mol), $O$: $16.00$ g/mol (3 atoms: $3\times16.00 = 48.00$ g/mol).
Total = $127.10 + 12.01 + 48.00 = 187.11$ g/mol.
# Answer: Formula: $Cu_2CO_3$, Molar Mass: $187.11$ g/mol

### Problem 7: Silicon Tetrahydride
# Explanation:
## Step 1: Use prefixes for subscripts
"Tetra-" means 4 for H. Formula: $SiH_4$ (also known as silane).
## Step 2: Calculate molar mass
$Si$: $28.09$ g/mol (1 atom: $28.09$ g/mol), $H$: $1.01$ g/mol (4 atoms: $4\times1.01 = 4.04$ g/mol).
Total = $28.09 + 4.04 = 32.13$ g/mol.
# Answer: Formula: $SiH_4$, Molar Mass: $32.13$ g/mol

### Problem 8: Manganese (II) Sulfate
# Explanation:
## Step 1: Identify ions and charges
Manganese (II): $Mn^{2+}$, Sulfate: $SO_4^{2-}$.
## Step 2: Balance charges
1 $Mn^{2+}$ and 1 $SO_4^{2-}$. Formula: $MnSO_4$.
## Step 3: Calculate molar mass
$Mn$: $54.94$ g/mol (1 atom: $54.94$ g/mol), $S$: $32.07$ g/mol (1 atom: $32.07$ g/mol), $O$: $16.00$ g/mol (4 atoms: $4\times16.00 = 64.00$ g/mol).
Total = $54.94 + 32.07 + 64.00 = 151.01$ g/mol.
# Answer: Formula: $MnSO_4$, Molar Mass: $151.01$ g/mol

### Problem 9: Iron (III) Oxide
# Explanation:
## Step 1: Identify ions and charges
Iron (III): $Fe^{3+}$, Oxide: $O^{2-}$.
## Step 2: Balance charges
Find least common multiple of 3 and 2, which is 6. So 2 $Fe^{3+}$ and 3 $O^{2-}$. Formula: $Fe_2O_3$.
## Step 3: Calculate molar mass
$Fe$: $55.85$ g/mol (2 atoms: $2\times55.85 = 111.70$ g/mol), $O$: $16.00$ g/mol (3 atoms: $3\times16.00 = 48.00$ g/mol).
Total = $111.70 + 48.00 = 159.70$ g/mol.
# Answer: Formula: $Fe_2O_3$, Molar Mass: $159.70$ g/mol

### Problem 10: Magnesium Nitrate
# Explanation:
## Step 1: Identify ions and charges
Magnesium: $Mg^{2+}$, Nitrate: $NO_3^-$ (charge -1).
## Step 2: Balance charges
1 $Mg^{2+}$ and 2 $NO_3^-$. Formula: $Mg(NO_3)_2$.
## Step 3: Calculate molar mass
$Mg$: $24.31$ g/mol (1 atom: $24.31$ g/mol), $N$: $14.01$ g/mol (2 atoms: $2\times14.01 = 28.02$ g/mol), $O$: $16.00$ g/mol (6 atoms: $6\times16.00 = 96.00$ g/mol).
Total = $24.31 + 28.02 + 96.00 = 148.33$ g/mol.
# Answer: Formula: $Mg(NO_3)_2$, Molar Mass: $148.33$ g/mol

### Problem 11: Calcium Sulfide
# Explanation:
## Step 1: Identify ions and charges
Calcium: $Ca^{2+}$, Sulfide: $S^{2-}$.
## Step 2: Balance charges
1 $Ca^{2+}$ and 1 $S^{2-}$. Formula: $CaS$.
## Step 3: Calculate molar mass
$Ca$: $40.08$ g/mol (1 atom: $40.08$ g/mol), $S$: $32.07$ g/mol (1 atom: $32.07$ g/mol).
Total = $40.08 + 32.07 = 72.15$ g/mol.
# Answer: Formula: $CaS$, Molar Mass: $72.15$ g/mol

### Problem 12: Potassium Oxide
# Explanation:
## Step 1: Identify ions and charges
Potassium: $K^+$ (charge +1), Oxide: $O^{2-}$ (charge -2).
## Step 2: Balance charges
2 $K^+$ and 1 $O^{2-}$. Formula: $K_2O$.
## Step 3: Calculate molar mass
$K$: $39.10$ g/mol (2 atoms: $2\times39.10 = 78.20$ g/mol), $O$: $16.00$ g/mol (1 atom: $16.00$ g/mol).
Total = $78.20 + 16.00 = 94.20$ g/mol.
# Answer: Formula: $K_2O$, Molar Mass: $94.20$ g/mol

### Problem 13: Magnesium Chloride
# Explanation:
## Step 1: Identify ions and charges
Magnesium: $Mg^{2+}$, Chloride: $Cl^-$ (charge -1).
## Step 2: Balance charges
1 $Mg^{2+}$ and 2 $Cl^-$. Formula: $MgCl_2$.
## Step 3: Calculate molar mass
$Mg$: $24.31$ g/mol (1 atom: $24.31$ g/mol), $Cl$: $35.45$ g/mol (2 atoms: $2\times35.45 = 70.90$ g/mol).
Total = $24.31 + 70.90 = 95.21$ g/mol.
# Answer: Formula: $MgCl_2$, Molar Mass: $95.21$ g/mol

### Problem 14: Tricarbon Octachloride
# Explanation:
## Step 1: Use prefixes for subscripts
"Tri-" means 3 for C, "octa-" means 8 for Cl. Formula: $C_3Cl_8$.
## Step 2: Calculate molar mass
$C$: $12.01$ g/mol (3 atoms: $3\times12.01 = 36.03$ g/mol), $Cl$: $35.45$ g/mol (8 atoms: $8\times35.45 = 283.60$ g/mol).
Total = $36.03 + 283.60 = 319.63$ g/mol.
# Answer: Formula: $C_3Cl_8$, Molar Mass: $319.63$ g/mol

### Problem 15: Gold (III) Bromide
# Explanation:
## Step 1: Identify ions and charges
Gold (III): $Au^{3+}$, Bromide: $Br^-$ (charge -1).
## Step 2: Balance charges
1 $Au^{3+}$ and 3 $Br^-$. Formula: $AuBr_3$.
## Step 3: Calculate molar mass
$Au$: $197.0$ g/mol (1 atom: $197.0$ g/mol), $Br$: $79.90$ g/mol (3 atoms: $3\times79.90 = 239.70$ g/mol).
Total = $197.0 + 239.70 = 436.70$ g/mol.
# Answer: Formula: $AuBr_3$, Molar Mass: $436.70$ g/mol

### Problem 16: Iodine Heptafluoride
# Explanation:
## Step 1: Use prefixes for subscripts
"Hepta-" means 7 for F. Formula: $IF_7$.
## Step 2: Calculate molar mass
$I$: $126.90$ g/mol (1 atom: $126.90$ g/mol), $F$: $19.00$ g/mol (7 atoms: $7\times19.00 = 133.00$ g/mol).
Total = $126.90 + 133.00 = 259.90$ g/mol.
# Answer: Formula: $IF_7$, Molar Mass: $259.90$ g/mol

### Problem 17: Sulfur Hexachloride
# Explanation:
## Step 1: Use prefixes for subscripts
"Hexa-" means 6 for Cl. Formula: $SCl_6$.
## Step 2: Calculate molar mass
$S$: $32.07$ g/mol (1 atom: $32.07$ g/mol), $Cl$: $35.45$ g/mol (6 atoms: $6\times35.45 = 212.70$ g/mol).
Total = $32.07 + 212.70 = 244.77$ g/mol.
# Answer: Formula: $SCl_6$, Molar Mass: $244.77$ g/mol

### Problem 18: Iron (II) Phosphide
# Explanation:
## Step 1: Identify ions and charges
Iron (II): $Fe^{2+}$, Phosphide: $P^{3-}$.
## Step 2: Balance charges
Find least common multiple of 2 and 3, which is 6. So 3 $Fe^{2+}$ and 2 $P^{3-}$. Formula: $Fe_3P_2$.
## Step 3: Calculate molar mass
$Fe$: $55.85$ g/mol (3 atoms: $3\times55.85 = 167.55$ g/mol), $P$: $30.97$ g/mol (2 atoms: $2\times30.97 = 61.94$ g/mol).
Total

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QUESTION IMAGE

Question

Explanation:

Problem 1: Sodium Hydroxide

Step 1: Determine ions and charges

Step 2: Write formula

Step 3: Calculate molar mass

Step 1: Use prefixes for subscripts

Step 2: Calculate molar mass

Step 1: Identify ions and charges

Step 2: Balance charges

Step 3: Calculate molar mass

Answer:

Problem 2: Tetraphosphorus Decoxide