Question

mixed naming practice
when given the name, give the formula, when given the formula, give the name.
acid naming

1. chromic acid
2. hydrobromic acid
3. nitrous acid
4. sulfuric acid
5. hf
6. h₃po₄
7. h₂co₃
8. h₂s
9. acetic acid
10. sulfurous acid

covalent naming

1. cf₄
2. n₂o₅
3. cs₂
4. so₃
5. p₄o₈
6. iodine tribromide
7. chlorine dioxide
8. sulfur hexafluoride
9. difluorine octachloride
10. tribromine nonatelluride
11. h₂o
12. p₂s₄
13. n₂o₄
14. xef₄
15. si₄

ionic naming

1. rubidium and iodine
2. barium and chlorine
3. lithium and selenium
4. magnesium and nitrogen
5. cs₂s
6. bao
7. ali₃
8. mno₂
9. cdbr₂
10. nacl
11. rubidium sulfide

more prefixes covalent
7 hepta
8 octa
9 nona
10 deca

Explanation:

Let's solve the first problem in Acid naming: Chromic acid. Chromic acid has the formula $H_2CrO_4$ (or sometimes $H_2Cr_2O_7$ but the common chromic acid is $H_2CrO_4$ for the purpose of naming - formula conversion here, we use the standard chromic acid formula which is $H_2CrO_4$ (or the other form is dichromic acid). Wait, actually, chromic acid is $H_2CrO_4$ (the oxyacid of chromium(VI)).

Step 1: Identify the acid type

Chromic acid is an oxyacid (contains oxygen). The name "chromic" comes from the chromium ion with a +6 oxidation state (since chromic is the higher oxidation state for chromium in oxyacids, chromous would be +2 or +3, but chromic is +6).

Step 2: Determine the formula

For oxyacids, the general rule is: the -ic acid suffix corresponds to the anion with the -ate suffix. Chromate ion is $CrO_4^{2 - }$. So to form the acid, we add $H^+$ ions to neutralize the charge. The chromate ion has a charge of -2, so we need 2 $H^+$ ions. So the formula is $H_2CrO_4$.

Let's do another one, Hydrobromic acid. Hydrobromic acid is a binary acid (contains hydrogen and a non - metal). Binary acids have the formula $HX$ where $X$ is the non - metal. For hydrobromic acid, the non - metal is bromine, so the formula is $HBr$.

For Nitrous acid: Nitrous acid is an oxyacid. The -ous suffix in the acid name corresponds to the -ite suffix in the anion. Nitrite ion is $NO_2^ -$. To form the acid, we add $H^+$ to neutralize the -1 charge of $NO_2^ -$, so the formula is $HNO_2$.

Sulfuric acid: Oxyacid, -ic suffix corresponds to -ate anion. Sulfate ion is $SO_4^{2 - }$. So we need 2 $H^+$ ions to neutralize the -2 charge, formula is $H_2SO_4$.

For HF: This is a binary acid. The formula $HF$ corresponds to hydrofluoric acid (since binary acids are named hydro - + non - metal root + -ic acid).

$H_3PO_4$: This is phosphoric acid. The anion is phosphate ($PO_4^{3 - }$), and with 3 $H^+$ ions to neutralize the -3 charge, the name is phosphoric acid (since -ic suffix for -ate anion, phosphate is $PO_4^{3 - }$).

$H_2CO_3$: Carbonic acid. The anion is carbonate ($CO_3^{2 - }$), 2 $H^+$ ions, so name is carbonic acid ( -ic for -ate, carbonate is $CO_3^{2 - }$).

$H_2S$: Binary acid, named hydrosulfuric acid (hydro - + sulfur root + -ic acid).

Acetic acid: The formula for acetic acid is $CH_3COOH$ (or $C_2H_4O_2$), but the common formula used for naming - formula conversion is $CH_3COOH$ (ethanoic acid in IUPAC, but acetic acid is common name).

Sulfurous acid: Oxyacid, -ous suffix corresponds to -ite anion. Sulfite ion is $SO_3^{2 - }$, so we need 2 $H^+$ ions, formula is $H_2SO_3$.

Now for Covalent naming:

1. $CF_4$: Covalent compound, named using prefixes. Carbon is first, no prefix (1 atom), fluorine is tetra (4 atoms), so carbon tetrafluoride.

2. $N_2O_5$: Dinitrogen pentoxide (di for 2 N, penta for 5 O).

3. $CS_2$: Carbon disulfide (di for 2 S).

4. $SO_3$: Sulfur trioxide (tri for 3 O).

5. $P_4O_8$: Tetraphosphorus octoxide (tetra for 4 P, octa for 8 O).

6. Iodine tribromide: Formula is $IBr_3$ (iodine is 1, tribromide means 3 Br).

7. Chlorine dioxide: Formula is $ClO_2$ (chlorine 1, dioxide means 2 O).

8. Sulfur hexafluoride: Formula is $SF_6$ (sulfur 1, hexafluoride means 6 F).

9. Difluorine octachloride: Formula is $F_2Cl_8$ (di for 2 F, octa for 8 Cl).

10. Tribromine nonatelluride: Formula is $Br_3Te_9$ (tri for 3 Br, nona for 9 Te).

11. $H_2O$: Dihydrogen monoxide (or water, but covalent naming: dihydrogen monoxide).

12. $P_2S_4$: Diphosphorus tetrasulfide (di for 2 P, tetra for 4 S).

13. $N_2O_4$: Dinitrogen tetroxide (di for 2 N, tetra for 4 O).

14. $XeF_4$: Xenon tetrafluoride (xenon 1, tetrafluoride means 4 F).

15. $SI_4$: Sulfur tetraiodide (sulfur 1, tetraiodide means 4 I).

For Ionic Naming:

1. Rubidium and iodine: Rubidium is $Rb^+$, iodine is $I^ -$. So the formula is $RbI$ (since +1 and -1 charges balance).

2. Barium and chlorine: Barium is $Ba^{2 + }$, chlorine is $Cl^ -$. To balance the charge (2+ and -1), we need 2 $Cl^ -$ ions. So formula is $BaCl_2$.

3. Lithium and selenium: Lithium is $Li^+$, selenium is $Se^{2 - }$. To balance the charge (+1 and -2), we need 2 $Li^+$ ions. So formula is $Li_2Se$.

4. Magnesium and nitrogen: Magnesium is $Mg^{2 + }$, nitrogen is $N^{3 - }$. To balance the charges (2+ and 3 - ), we use the criss - cross method: $Mg_3N_2$ (3 $Mg^{2 + }$ ions for 2 $N^{3 - }$ ions, since 3*2 = 2*3 = 6).

5. $Cs_2S$: Cesium sulfide. Cesium is $Cs^+$, sulfide is $S^{2 - }$. 2 $Cs^+$ ions balance the -2 charge of $S^{2 - }$.

6. $BaO$: Barium oxide. Barium is $Ba^{2 + }$, oxide is $O^{2 - }$, charges balance (2+ and 2 - ).

7. $AlI_3$: Aluminum iodide. Aluminum is $Al^{3 + }$, iodide is $I^ -$. 3 $I^ -$ ions balance the +3 charge of $Al^{3 + }$.

8. $MnO_2$: Manganese(IV) oxide. Manganese has a +4 oxidation state (since $O$ is -2, 2*(-2)= - 4, so Mn is +4), and oxide is $O^{2 - }$.

9. $CdBr_2$: Cadmium bromide. Cadmium is $Cd^{2 + }$, bromide is $Br^ -$. 2 $Br^ -$ ions balance the +2 charge of $Cd^{2 + }$.

10. $NaCl$: Sodium chloride. Sodium is $Na^+$, chloride is $Cl^ -$, charges balance (+1 and -1).

11. Rubidium sulfide: Rubidium is $Rb^+$, sulfide is $S^{2 - }$. So formula is $Rb_2S$ (2 $Rb^+$ ions to balance -2 charge of $S^{2 - }$).

Answer:

(Here are the answers for each sub - problem as per the above explanations. For example, for Chromic acid (Acid naming 1), formula is $H_2CrO_4$; Hydrobromic acid (Acid naming 2) formula is $HBr$; Nitrous acid (Acid naming 3) formula is $HNO_2$; Sulfuric acid (Acid naming 4) formula is $H_2SO_4$; HF (Acid naming 5) name is Hydrofluoric acid; $H_3PO_4$ (Acid naming 6) name is Phosphoric acid; $H_2CO_3$ (Acid naming 7) name is Carbonic acid; $H_2S$ (Acid naming 8) name is Hydrosulfuric acid; Acetic acid (Acid naming 9) formula is $CH_3COOH$; Sulfurous acid (Acid naming 10) formula is $H_2SO_3$.

For Covalent naming 1: $CF_4$ name is Carbon tetrafluoride; Covalent naming 2: $N_2O_5$ name is Dinitrogen pentoxide; Covalent naming 3: $CS_2$ name is Carbon disulfide; Covalent naming 4: $SO_3$ name is Sulfur trioxide; Covalent naming 5: $P_4O_8$ name is Tetraphosphorus octoxide; Covalent naming 6: Iodine tribromide formula is $IBr_3$; Covalent naming 7: Chlorine dioxide formula is $ClO_2$; Covalent naming 8: Sulfur hexafluoride formula is $SF_6$; Covalent naming 9: Difluorine octachloride formula is $F_2Cl_8$; Covalent naming 10: Tribromine nonatelluride formula is $Br_3Te_9$; Covalent naming 11: $H_2O$ name is Dihydrogen monoxide; Covalent naming 12: $P_2S_4$ name is Diphosphorus tetrasulfide; Covalent naming 13: $N_2O_4$ name is Dinitrogen tetroxide; Covalent naming 14: $XeF_4$ name is Xenon tetrafluoride; Covalent naming 15: $SI_4$ name is Sulfur tetraiodide.

For Ionic Naming 1: Rubidium and iodine formula is $RbI$; Ionic Naming 2: Barium and chlorine formula is $BaCl_2$; Ionic Naming 3: Lithium and selenium formula is $Li_2Se$; Ionic Naming 4: Magnesium and nitrogen formula is $Mg_3N_2$; Ionic Naming 5: $Cs_2S$ name is Cesium sulfide; Ionic Naming 6: $BaO$ name is Barium oxide; Ionic Naming 7: $AlI_3$ name is Aluminum iodide; Ionic Naming 8: $MnO_2$ name is Manganese(IV) oxide; Ionic Naming 9: $CdBr_2$ name is Cadmium bromide; Ionic Naming 10: $NaCl$ name is Sodium chloride; Ionic Naming 11: Rubidium sulfide formula is $Rb_2S$.)