Chemis

1. LAB NAMING IONIC COMPOUND
GSCI1103L – B (GENERAL CHEMISTRY LAB I)
October 9th, 2021
Lecturer: Iwan Setiawan, Ph.D.
ACCOUNTING
FACULTY OF BUSINESS
SAMPOERNA UNIVERSITY
2021

2. EXERCISE 1 – Preparation for Naming Ionic and Molecular Compounds
Photo 1: Colored Periodic Table
Photo 2: Polyatomic Ion Note Card
No Name Formula Charge
1 Ammonium Ion NH4
+ 1+
2 Hydroxide Ion OH- 1-
3 Cyanide Ion CN- 1-
4 Nitrite Ion NO2
- 1-
5 Nitrate Ion NO3
- 1-
Source: Britannica

3. 6 Sulfite Ion SO3
2- 2-
7 Sulfate Ion SO4
2- 2-
8 Hydrogen Sulfite Ion HSO3
- 1-
9 Hydrogen Sulfate Ion HSO4
- 1-
10 Carbonate Ion CO3
2- 2-
11 Hydrogen Carbonate Ion HCO3
- 1-
12 Phosphate Ion PO4
3- 3-
13 Hydrogen Phosphate Ion HPO4
3- 2-
14 Dihydrogen Phosphate Ion H2PO4
- 1-
15 Hypochlorite Ion CIO- 1-
16 Chlorite Ion CIO2
- 1-
17 Chlorate Ion CIO3
- 1-
18 Perchlorate Ion CIO4
- 1-
19 Peroxide Ion O2
2- 2-
20 Chromate Ion CrO4
2- 2-
21 Dichromate Ion Cr2O7
3- 2-
22 Permanganate Ion MnO4
- 1-
Photo 3: Strong Acid Note Card
No Name Formula
1 Perchloric Acid HCIO4
2 Hydrochloric Acid HCI
3 Hydrobromic Acid HBr
4 Hydroiodic Acid HI
5 Nitric Acid HNO3

4. 6 Sulfuric Acid H2SO4
Photo 4: Diatomic Element Note Card
No Name Formula
1 Hydrogen H2
2 Nitrogen N2
3 Fluorine F2
4 Oxygen O2
5 Iodine I2
6 Chlorine CL2
7 Braine Br2

5. EXERCISE 2 – Naming Ionic and Molecular Compounds
Data Table 1: Binary Molecular and Ionic Compound Names
# Formula Molecular or Ionic Compound? Compound Name
1 B2O3 Molecular Compound Diboron trioxide
2 N2O Molecular Compound Dinitrogen monoxide
3 LiCl Ionic Compound Lithium chloride
4 N2O4 Molecular Compound Dinitrogen tetraoxide
5 SF4 Molecular Compound Sulfur tetrafluoride
6 BrF3 Molecular Compound Bromine trifluoride
7 AlBr3 Ionic Compound Aluminum (III) bromide
8 SnF2 Ionic Compound Tin (II) fluoride
9 SiCl4 Molecular Compound Silicon tetrachloride
10 H2O2 Molecular Compound Dihydrogen dioxide
11 NaCl Ionic Compound Natrium chloride
12 TiCl3 Ionic Compound Titanium (III) chloride
13 SiO2 Molecular Compound Silicon dioxide
14 Al2S3 Ionic Compound Aluminum (III) sulfide
15 CCL4 Molecular Compound Carbon Tetrachloride
16 CuF2 Ionic Compound Copper (II) Fluoride
17 SF6 Molecular Compound Sulfur Hexafluoride
18 P4S3 Molecular Compound Tetraphosporus Trisulfide
19 Xe3F4 Molecular Compound Trixenon Tetrafluoride
20 PtCl2 Ionic Compound Platinum (II) fluoride

6. Data Table 2: Binary Molecular and Ionic Compound Formulas
# Formula Molecular or Ionic Compound? Formula
1 Tribromine octoxide Molecular Compound Br3O8
2 Lithium selenide Ionic Compound Li2Se
3 Iodine monochloride Molecular Compound ICl
4 Nitrogen monoxide Molecular Compound NO
5 Iron (II) sulfide Ionic Compound FeS
6 Hydrogen chloride Molecular Compound HCl
7 Diboron hexahydride Molecular Compound B2H6
8 Barium iodide Ionic Compound BaI2
9 Cadmium sulfide Ionic Compound CdS
10 Bromine trichloride Molecular Compound BrCl3
11 Nitrogen trihydride Molecular Compound NH3
12 Molybdenum (IV) fluoride Ionic Compound MoF4
13 Carbon tetrabromide Molecular Compound CBr4
14 Sulfur trioxide Molecular Compound SO3
15 Lead (II) chloride Ionic Compound PbCl2
16 Iodine hexafluoride Molecular Compound IF6
17 Tetraphosphorus decasulfide Molecular Compound P4S10
18 Dichlorine trioxide Molecular Compound Cl2O3
19 Potassium chloride Ionic Compound KCl
20 Calcium oxide Ionic Compound CaO

7. Data Table 3: Polyatomic Ions Acid Names
# Formula Name
1 SO4
2- Sulfate ion
2 SnCl4 Tin (IV) chloride
3 ClO2
- Chlorite ion
4 H3PO4 Phosphoric acid
5 Cu3(PO4)2 Copper (II) phosphate
6 FeSO4 Iron (II) sulfate
7 NH4Cl Ammonium chloride
8 HClO4(aq) Perchloric acid
9 PO4
3- Phosphate ion
10 K2SO3 Potassium sulfite
11 MnO2 Manganese (IV) oxide
12 Ca3(PO4)2 Calcium phosphate
13 NaOH Sodium hydroxide
14 HCl (aq) Hydrochloric acid
15 HNO3 (aq) Nitric acid
16 FeSO3 Iron (II) sulfite
17 WO3 Tungsten (III) trioxide
18 H2CO3 Carbonic acid
19 KMnO4 Potassium permanganate
20 H2S (aq) Hydrogen sulfide

8. Data Table 4: Polyatomic Ion and Acid Formulas
No Name Formula
1 Potassium nitrate KNO3
2 Carbonate ion CO3
2−
3 Dihydrogen phosphate H2PO4
-
4 Hypochlorous acid HClO
5 Hydrogen cyanide HCN
6 Cobalt (III) sulfite Co2(SO3)3
7 Permanganic acid HMnO4
8 Magnesium hypochlorite Mg(ClO)2
9 Hydroiodic acid Hl
10 Titanium (IV) nitrate Ti(NO3)4
11 Silver chromate Ag2CrO4
12 Nickel (II) phosphate Ni3(PO4)2
13 Sulfuric acid H2SO4
14 Magnesium nitride Mg3N2
15 Hydrobromic acid HBr
16 Ammonium ion NH4
+
17 Lithium hypochlorite LiClO
18 Nitrous acid HNO2
19 Barium hydrogen sulfite Ba(HSO3)2
20 Hydrofluoric acid HF

9. EXERCISE 2 – Question
1. Determine the effect of adding h+ to the polyatomic ion phosphate. Indicate the effect on the charge and
record the new name.
Answer: When iH+ iis iadded ito ia iphosphate ithe inegative icharges ireduces iby ione iunit iand ithe inew
icompound iformed iis ian iazeotropic icompound iwhich imeans iit ican iact ias ian iacid ias iwell ias ia
ibase. iThe icompound iis icalled ihydrogen iphosphate.
2. The metals in Group IIIA, IVA and VA of the periodic table are not transition metals. However, all but 1
have variable charges. What element in Group IIIA, Period 3 has a fixed charge, and what is that charge?
Answer: Group iIII iA ielements iare inow icalled igroup i13 ielements iand iin ithe iperiod i3 iit iis
ialuminium. iIt ihas ia ifixed ioxidation istate iof i3+.
3. Describe the difference between molecular and ionic compounds.
Answer: Molecular icompounds iare iformed iby isharing iof ielectrons iwhereas iionic icompounds iare
iformed iby itransfer iof ielectrons iand iby ithe icombination iof ipositively iand inegatively icharged
icomponents.