Question

m. cobalt (iii) oxide co₂o₃
q. nickel (iii) sulfide ni₂s₃
o. titanium (ii) acetate ti
r. manganese (ii) phosphate mn
p. silicon dioxide sio₂
directions: complete the chart below.

	name	chemical formula
1	silicon disulfide	sis₂
2	gold (iii) chloride	aucl₃
3	xenon trioxide	xeo₃
4	diphosphorous pentoxide	p₂o₅
5		zro₂
6	platinum (ii) cyanide
7		sri₂
8	chlorine monofluoride
9		sno
10		mo(so₄)₃
11	carbon tetrabromide
12		pbs₂
13		so₂
14		bf₃
15	scandium (iii) bicarbonate
16	titanium (iv) biphosphate
17		alpo₄
18		ni(c₂h₃o₂)₃
19		kio₂
20	iodine pentafluoride

Answer:

To solve this, we'll go through each row, determining the name from the formula or vice versa using chemical naming rules (ionic, covalent, polyatomic ions, oxidation states).

Row 1: Formula = $\ce{SiS2}$

• Type: Covalent (non - metal + non - metal). Prefixes: Si = silicon, S = sulfur. Subscript 2 for S → disulfide.
• Name: Silicon disulfide

Row 2: Formula = $\ce{AuCl3}$

• Type: Ionic (metal + non - metal). Au is gold, Cl is chloride. Oxidation state of Au: Cl is - 1, 3 Cl⁻ → Au³⁺ (gold(III)).
• Name: Gold(III) chloride

Row 3: Name = Xenon trioxide

• Type: Covalent (xenon is a noble gas, O is non - metal). Prefixes: xenon (no prefix), tri - for 3 O. Formula: Xe + 3 O → $\ce{XeO3}$

Row 4: Formula = $\ce{P2O5}$

• Type: Covalent. P = phosphorus, O = oxide. Subscripts: 2 P (di -), 5 O (penta -).
• Name: Diphosphorus pentoxide

Row 5: Formula = $\ce{ZrO2}$

• Type: Ionic. Zr = zirconium, O = oxide. Oxidation state: O is - 2, 2 O²⁻ → Zr⁴⁺ (zirconium(IV)).
• Name: Zirconium(IV) oxide

Row 6: Name = Platinum(II) cyanide

• Type: Ionic. Pt²⁺ (platinum(II)), $\ce{CN^-}$ (cyanide, charge - 1). To balance: 1 Pt²⁺ + 2 $\ce{CN^-}$ → $\ce{Pt(CN)2}$

Row 7: Formula = $\ce{SrI2}$

• Type: Ionic. Sr = strontium (group 2, + 2), I = iodide (- 1). 1 Sr²⁺ + 2 I⁻ → formula $\ce{SrI2}$.
• Name: Strontium iodide

Row 8: Name = Chlorine monofluoride

• Type: Covalent (both non - metals). Cl = chlorine, F = fluorine. Prefixes: mono - for 1 F. Formula: Cl + 1 F → $\ce{ClF}$

Row 9: Formula = $\ce{SnO}$

• Type: Ionic. Sn = tin, O = oxide. Oxidation state: O is - 2, so Sn²⁺ (tin(II)).
• Name: Tin(II) oxide

Row 10: Formula = $\ce{Mo(SO4)3}$

• Type: Ionic (metal + polyatomic ion). $\ce{SO4^{2 -}}$ (sulfate, - 2). 3 $\ce{SO4^{2 -}}$ → total - 6, so Mo⁶⁺ (molybdenum(VI)).
• Name: Molybdenum(VI) sulfate

Row 11: Name = Carbon tetrabromide

• Type: Covalent. C = carbon, Br = bromide. Prefix tetra - for 4 Br. Formula: C + 4 Br → $\ce{CBr4}$

Row 12: Formula = $\ce{PbS2}$

• Type: Ionic. Pb = lead, S = sulfide. Oxidation state: S₂²⁻ (disulfide, - 2), so Pb²⁺ (lead(II)).
• Name: Lead(II) disulfide

Row 13: Formula = $\ce{SO2}$

• Type: Covalent. S = sulfur, O = oxide. Subscript 2 for O → dioxide.
• Name: Sulfur dioxide

Row 14: Formula = $\ce{BF3}$

• Type: Covalent. B = boron, F = fluoride. Prefix tri - for 3 F.
• Name: Boron trifluoride

Row 15: Name = Scandium(III) bicarbonate

• Type: Ionic. Sc³⁺ (scandium(III)), $\ce{HCO3^-}$ (bicarbonate, - 1). To balance: 1 Sc³⁺ + 3 $\ce{HCO3^-}$ → $\ce{Sc(HCO3)3}$

Row 16: Name = Titanium(IV) biphosphate

• Type: Ionic. Ti⁴⁺ (titanium(IV)), $\ce{HPO4^{2 -}}$ (biphosphate, - 2). To balance: 1 Ti⁴⁺ + 2 $\ce{HPO4^{2 -}}$ → $\ce{Ti(HPO4)2}$

Row 17: Formula = $\ce{AlPO4}$

• Type: Ionic (metal + polyatomic ion). Al³⁺ (aluminum), $\ce{PO4^{3 -}}$ (phosphate, - 3). 1 Al³⁺ + 1 $\ce{PO4^{3 -}}$ → formula.
• Name: Aluminum phosphate

Row 18: Formula = $\ce{Ni(C2H3O2)3}$

• Type: Ionic. $\ce{C2H3O2^-}$ is acetate (- 1). 3 acetate⁻ → Ni³⁺? Wait, no: Ni + 3 $\ce{C2H3O2^-}$ → Ni³⁺? Wait, $\ce{C2H3O2^-}$ is - 1, 3 of them → - 3, so Ni³⁺? Wait, no, $\ce{Ni(C2H3O2)3}$: Ni has oxidation state + 3? Wait, no, acetate is $\ce{CH3COO^-}$ (same as $\ce{C2H3O2^-}$). Wait, actually, $\ce{Ni(C2H3O2)3}$: Ni is nickel, acetate is - 1. 3 acetates → Ni³⁺? No, wait, $\ce{Ni(C2H3O2)3}$: let's check. $\ce{C2H3O2^-}$ is - 1, 3 of them → total - 3, so Ni is + 3? But nickel can have + 2 or + 3. Wait, the formula is given, so name: nickel(III) acetate? Wait, no, maybe I made a mistake. Wait, $\ce{Ni(C2H3O2)3}$: Ni + 3 $\ce{C2H3O2^-}$ → Ni³⁺? Wait, no, $\ce{C2H3O2^-}$ is acetate, so the name is Nickel(III) acetate? Wait, no, actually, $\ce{Ni(C2H3O2)3}$: let's re - check. Oxidation state of Ni: 3 * (- 1) + x = 0 → x = + 3. So name: Nickel(III) acetate. Wait, but maybe it's nickel(III) acetate. Wait, no, maybe I messed up. Wait, the formula is $\ce{Ni(C2H3O2)3}$, so name: Nickel(III) acetate.

Row 19: Formula = $\ce{KIO2}$

• Type: Ionic. K⁺ (potassium), $\ce{IO2^-}$ (iodite, - 1).
• Name: Potassium iodite

Row 20: Name = Iodine pentafluoride

• Type: Covalent. I = iodine, F = fluoride. Prefix penta - for 5 F. Formula: I + 5 F → $\ce{IF5}$

Final Chart (Key Rows Filled)

#	Name	Chemical Formula
2	Gold(III) chloride	$\ce{AuCl3}$
3	Xenon trioxide	$\ce{XeO3}$
4	Diphosphorus pentoxide	$\ce{P2O5}$
5	Zirconium(IV) oxide	$\ce{ZrO2}$
6	Platinum(II) cyanide	$\ce{Pt(CN)2}$
7	Strontium iodide	$\ce{SrI2}$
8	Chlorine monofluoride	$\ce{ClF}$
9	Tin(II) oxide	$\ce{SnO}$
10	Molybdenum(VI) sulfate	$\ce{Mo(SO4)3}$
11	Carbon tetrabromide	$\ce{CBr4}$
12	Lead(II) disulfide	$\ce{PbS2}$
13	Sulfur dioxide	$\ce{SO2}$
14	Boron trifluoride	$\ce{BF3}$
15	Scandium(III) bicarbonate	$\ce{Sc(HCO3)3}$
16	Titanium(IV) biphosphate	$\ce{Ti(HPO4)2}$
17	Aluminum phosphate	$\ce{AlPO4}$
18	Nickel(III) acetate	$\ce{Ni(C2H3O2)3}$
19	Potassium iodite	$\ce{KIO2}$
20	Iodine pentafluoride	$\ce{IF5}$

(Note: For row 18, if Ni is + 2, then 3 $\ce{C2H3O2^-}$ would need Ni²⁺, but 3*(- 1) + 2 = - 1 ≠ 0. So Ni must be + 3. However, nickel(II) acetate is more common, but based on the formula $\ce{Ni(C2H3O2)3}$, oxidation state is + 3.)