### Chemical Formulas List For Class 10 PDF Download

As a student, it is your duty to have all the knowledge about the various subjects that you are studying. This is why we have come up with this list of chemical formulas for class 10 students. These are some of the most important and commonly used formulas in the world. So, without further ado, let us begin!

### What is a chemical formula?

A chemical formula is a set of letters that tells you the makeup of a molecule. It is similar to the recipe for a cake, except that the chemical formula is specific to each type of molecule.

For example, the chemical formula for water is H2O. This tells you that water contains two hydrogen atoms and one oxygen atom. You can also use chemical formulas to find out the properties of molecules. For example, water has a boiling point and an freezing point.

### What are the chemical formulas for common elements?

There are many different chemical formulas for common elements. The most common chemical formulas are shown below.

The chemical formula for oxygen is O2. The chemical formula for silicon is Si. The chemical formula for carbon is C. The chemical formula for nitrogen is N2.

### What are the chemical formulas for common compounds?

There are a vast number of chemical compounds, and knowing their formulas is essential for learning about them. The chemical formulas are the unique names that scientists give to compounds.

Most compounds have a basic structure, which is a group of atoms joined together in a specific way. This basic structure is usually expressed in terms of molecules. A molecule is a group of two or more atoms that are joined together by covalent bonds. Covalent bonds are strong links between atoms, and they can hold together very large molecules.

Some common chemical compounds have very simple molecular structures, while others have more complex structures. The molecular structure of a compound can be determined using quantum mechanics. Quantum mechanics is a branch of physics that studies the behavior of subatomic particles. It is used to predict the behavior of very complex molecules.

The chemical formulas for common compounds can be found in many textbooks and online sources.

### How to create a chemical formula in equation form

To create a chemical formula in equation form, you first need to identify the elements that are present in the compound. You do this by using the brackets that are usually used in equations. The brackets indicate that you are listing all of the elements that are present in the compound.

After you have identified all of the elements that are present in the compound, you need to add them together and solve for the unknown element. This is done by using basic algebraic operations. You can use parentheses to help organize your equations, and you can also use variables to represent different elements.

For example, let’s take a look at the chemical formula for acetic acid. Acetic acid has one molecule of carbon dioxide and two molecules of acetate (CO2 + H2O -> CH3COOH). To solve for the missing element, we would need to use algebraic operations to combine these two equations:

CH3COOH (1 + 2) = 5

We can also use variables to represent different elements when we are solving equations. In this example, we would use x to represent the number of molecules of acetate present in acetic acid. So, our final equation would be:

CH3

### How to simplify a chemical formula

Chemical formulas can be a bit complicated, especially if you’re trying to remember them for class. To make things a little easier, here is a list of chemical formulas with their simplified equivalents.

H2O = Water

H2S = Sulphur dioxide

C6H3O6 = Hexane

C12H6O12 = Methane

### How to find the equivalent weight of a compound

To find the equivalent weight of a compound, you need to know the molecular weight and the molarity. The molecular weight is the number of atoms in a molecule. The molarity is simply the number of molecules per unit of volume.

For example, let’s say you want to find the equivalent weight of potassium dichromate. Potassium dichromate has a molecular weight of 128 grams per mole (g/mol). So, its equivalent weight would be 128/1000 or 0.128 grams per mole.

### Chemical Formulas List for Class 10 PDF

Sl.No |
Name of the Chemical Compound |
Formula |

1 | Acetic acid formula | CH_{3}COOH |

2 | Aluminium hydroxide formula | Al(OH)_{3} |

3 | Acetate formula | CH_{3}COO- |

4 | Acetone formula | C_{3}H_{6}O |

5 | Aluminium acetate formula | Al_{2}O(C_{2}H_{3}O_{2})_{4} |

6 | Aluminum bromide formula | AlBr_{3} |

7 | Aluminum carbonate formula | Al_{2}(CO_{3})_{3} |

8 | Aluminum chloride formula | AlCl_{3} |

9 | Aluminum fluoride formula | AlF_{3} |

10 | Aluminum formula | Al |

11 | Aluminum iodide formula | AlI_{3} |

12 | Aluminum oxide formula | Al_{2}O_{3} |

13 | Aluminum phosphate formula | AlPO_{4} |

14 | Amino acid formula | R(NH_{2})-COOH |

15 | Ammonia formula | NH_{4} |

16 | Ammonium dichromate formula | Cr_{2}H_{8}N_{2}O_{7} |

17 | Ammonium acetate formula | C_{2}H_{3}O_{2}NH_{4} |

18 | Ammonium bicarbonate formula | NH_{4}HCO_{3} |

19 | Ammonium bromide formula | NH_{4}Br |

20 | Ammonium carbonate formula | (NH_{4})_{2}CO_{3} |

21 | Ammonium chloride formula | NH_{4}Cl |

22 | Ammonium hydroxide formula | NH_{4}OH |

23 | Ammonium iodide formula | NH_{4}I |

24 | Ammonium nitrate formula | NH_{4}NO_{3} |

25 | Aluminium sulfide formula | Al_{2}S_{3} |

26 | Ammonium nitrite formula | NH_{4}NO_{2} |

27 | Ammonium oxide formula | (NH_{4})_{2}O |

28 | Ammonium phosphate formula | (NH_{4})_{3}PO_{4} |

29 | Ammonium sulfate formula | (NH_{4})_{2}SO_{4} |

30 | Ammonium sulfide formula | (NH_{4})_{2}S |

31 | Argon gas formula | Ar |

32 | Ascorbic acid formula | C_{6}H_{8}O_{6} |

33 | Barium acetate formula | Ba(C_{2}H_{3}O_{2})_{2} |

34 | Barium bromide formula | BaBr2 |

35 | Barium chloride formula | BaCl2 |

36 | Barium fluoride formula | BaF2 |

37 | Barium hydroxide formula | Ba(OH)_{2} |

38 | Barium iodide formula | BaI2 |

39 | Barium nitrate formula | Ba(NO_{3})_{2} |

40 | Barium oxide formula | BaO |

41 | Barium phosphate formula | Ba_{3}O_{8}P_{2} |

42 | Barium sulfate formula | BaSO_{4} |

43 | Benzene formula | C_{6}H_{6} |

44 | Benzoic acid formula | C_{7}H_{6}O_{2} |

45 | Bicarbonate formula | CHO_{3}^{–} |

46 | Bleach formula | NaClO |

47 | Boric acid formula | H_{3}BO_{3} |

48 | Potassium Bromate formula | KBrO_{3} |

49 | Bromic acid formula | HBrO_{3} |

50 | Bromine formula | Br |

51 | Butane formula | C_{4}H_{10} |

52 | Butanoic acid formula | C_{4}H_{8}O_{2} |

53 | Calcium acetate formula | Ca(COO^{–})_{2} |

54 | Calcium bromide formula | CaBr_{2} |

55 | Calcium carbonate formula | CaCO_{3} |

56 | Calcium hydride formula | CaH_{2} |

57 | Calcium hydroxide formula | Ca(OH)_{2} |

58 | Calcium iodide formula | CaI_{2} |

59 | Calcium nitrate formula | Ca(NO_{3})_{2} |

60 | Calcium oxide formula | CaO |

61 | Carbon monoxide formula | CO |

62 | Carbon tetrachloride formula | CCl_{4} |

63 | Carbonic acid formula | H2CO_{3} |

64 | Calcium phosphate formula | Ca_{3}(PO_{4})_{2} |

65 | Carbonic acid formula | H_{2}CO_{3} |

66 | Citric acid formula | C_{6}H_{8}O_{7} |

67 | Chlorate formula | ClO^{–}_{3} |

68 | Chlorine formula | Cl_{2} |

69 | Chlorine gas formula | Cl_{2} |

70 | Chlorous acid formula | HClO_{2} |

71 | Chromate formula | CrO_{4}^{2-} |

72 | Chromic acid formula | H_{2}CrO_{4} |

73 | Citric acid formula | C_{6}H_{8}O_{7} |

74 | Copper ii carbonate formula | CuCO3 |

75 | Copper ii nitrate formula | Cu(NO3)2 |

76 | Cyanide formula | CN- |

77 | Dichromate formula | K_{2}Cr_{2}O_{7} |

78 | Dihydrogen monoxide formula | H_{2}O |

79 | Dinitrogen monoxide formula | N_{2}O |

80 | Dinitrogen pentoxide formula | N_{2}O_{5} |

81 | Dinitrogen trioxide formula | N_{2}O_{3} |

82 | Ethanol formula | C_{2}H_{5}OH |

83 | Iron oxide formula | Fe_{2}O_{3} |

84 | Ethylene glycol formula | C_{2}H_{6}O_{2} |

85 | Fluorine gas formula | F_{2} |

86 | Aluminum bromide formula | AlBr_{3} |

87 | Aluminum sulfide formula | Al2S_{3} |

88 | Ammonium carbonate formula | (NH_{4})_{2}CO_{3} |

89 | Ammonium nitrate formula | (NH_{4})(NO_{3}) |

90 | Ammonium phosphate formula | (NH_{4})_{3}PO_{4} |

91 | Barium chloride formula | BaCl_{2} |

92 | Barium sulfate formula | BaSO_{4} |

93 | Calcium nitrate formula | Ca(NO_{3})_{2} |

94 | Carbon monoxide formula | CO |

95 | Carbon tetrachloride formula | CCl_{4} |

96 | Carbonic acid formula | H_{2}CO_{3} |

97 | Hydrofluoric acid formula | HF |

98 | Hydroiodic acid formula | HI |

99 | Hypochlorous acid formula | HClO |

100 | Lithium phosphate formula | Li_{3}PO_{4} |

101 | Magnesium nitrate formula | MgNO_{3} |

102 | Magnesium phosphate formula | Mg_{3}(PO_{4})_{2} |

103 | Nitrogen monoxide formula | NO |

104 | Nitrous acid formula | HNO_{2} |

105 | Potassium carbonate formula | K_{2}CO_{3} |

106 | Potassium iodide formula | KI |

107 | Potassium nitrate formula | KNO_{3} |

108 | Potassium phosphate formula | KH_{2}PO_{4} |

109 | Sodium carbonate formula | Na_{2}CO_{3} |

110 | Sodium oxide formula | Na_{2}O |

111 | Fructose chemical formula | C_{6}H_{12}O_{6} |

112 | Glycerol formula | C_{3}H_{8}O_{3} |

113 | Helium gas formula | He |

114 | Hexane formula | C_{6}H_{14} |

115 | Hydrobromic acid formula | HBr |

116 | Hydrochloric acid formula | HCl |

117 | Hydrocyanic acid formula | HCN |

118 | Hydrofluoric acid formula | HF |

119 | Hydrogen carbonate formula | CHO_{3}^{–} |

120 | Hydrogen gas formula | H_{2} |

121 | Hydrogen peroxide formula | H_{2}O_{2} |

122 | Hydrogen phosphate formula | H_{3}PO_{4} |

123 | Hydrogen sulfate formula | HSO_{4}^{–} |

124 | Hydroiodic acid formula | HI |

125 | Hydrosulfuric acid formula | H_{2}SO_{4} |

126 | Hydroxide formula | OH^{–} |

127 | Hypobromous acid formula | HBrO |

128 | Hypochlorite formula | NaClO |

129 | Hypochlorous acid formula | HClO |

130 | Hypoiodous acid formula | HIO |

131 | Iodic acid formula | HIO_{3} |

132 | Iodide formula | I_{2} |

133 | Iodine formula | I_{2} |

134 | Iron iii nitrate formula | Fe(NO_{3})_{3} |

135 | Iron ii oxide formula | FeO |

136 | Iron iii carbonate formula | Fe_{2}(CO_{3})_{3} |

137 | Iron iii hydroxide formula | Fe(OH)_{3} |

138 | Iron iii oxide formula | Fe_{2}O_{3} |

139 | Iron iii chloride formula | FeCl_{3} |

140 | Lactic acid formula | C_{3}H_{6}O_{3} |

141 | Lead acetate formula | Pb(C_{2}H_{3}O_{2})_{2} |

142 | Lead ii acetate formula | Pb(C_{2}H_{3}O_{2})_{2} |

143 | Lead iodide formula | PbI_{2} |

144 | Lead iv oxide formula | PbO_{2} |

145 | Lead nitrate formula | Pb(NO_{3})_{2} |

146 | Lithium bromide formula | LiBr |

147 | Lithium chloride formula | LiCl_{2} |

148 | Lithium hydroxide formula | LiOH |

149 | Lithium iodide formula | LiI_{2} |

150 | Lithium oxide formula | Li_{2}O |

151 | Lithium phosphate formula | Li_{3}PO_{4} |

152 | Magnesium acetate formula | Mg(CH_{3}COO)_{2} |

153 | Magnesium bicarbonate formula | MgCO_{3} |

154 | Magnesium carbonate formula | MgCO_{3} |

155 | Magnesium chloride formula | MgCl_{2} |

156 | Magnesium hydroxide formula | Mg(OH)_{3} |

157 | Magnesium iodide formula | MgI_{2} |

158 | Magnesium nitrate formula | Mg(NO_{3})_{2} |

159 | Magnesium nitride formula | Mg_{3}N_{2} |

160 | Magnesium carbonate formula | MgCO_{3} |

161 | Magnesium bromide formula | MgBr_{2} |

162 | Magnesium oxide formula | MgO |

163 | Magnesium phosphate formula | Mg_{3}(PO_{4})_{2} |

164 | Magnesium sulfate formula | MgSO_{4} |

165 | Magnesium sulfide formula | MgS |

166 | Methane formula | CH_{4} |

167 | Methanol formula | CH_{3}OH |

168 | Nickel acetate formula | Ni(C_{2}H_{3}O_{2})_{2} |

169 | Nickel nitrate formula | Ni(NO_{3})_{2} |

170 | Nitric acid formula | HNO_{3} |

171 | Nitride formula | N_{3} |

172 | Nitrite formula | NO_{2}^{−} |

173 | Nitrogen dioxide formula | NO_{2} |

174 | Nitrogen monoxide formula | NO |

175 | Nitrous acid formula | HNO_{2} |

176 | Oxalate formula | C_{2}O_{4}^{2−} |

177 | Oxalic acid formula | H_{2}C_{2}O_{4} |

178 | Oxygen formula | O_{2} |

179 | Ozone formula | O_{3} |

180 | Perbromic acid formula | HBrO_{4} |

181 | Potassium Permanganate formula | KMnO_{4} |

182 | Permanganate ion formula | MnO_{4}^{–} |

183 | Phosphate formula | PO_{4}^{3-} |

184 | Sodium hydrogen phosphate formula | Na_{2}HPO_{4} |

185 | Sodium formate formula | CHNaO_{2} |

186 | Phosphoric acid formula | H_{3}PO_{4} |

187 | Phosphorus pentachloride formula | PCl_{5} |

188 | Phosphorus trichloride formula | PCl_{3} |

189 | Potassium acetate formula | CH_{3}CO_{2}K |

190 | Potassium bicarbonate formula | KHCO_{3} |

191 | Potassium carbonate formula | K_{2}CO_{3} |

192 | Potassium chlorate formula | KClO_{3} |

193 | Potassium hydrogen phosphate formula | K_{2}HPO_{4} |

194 | Potassium chloride formula | KCl |

195 | Potassium chromate formula | CrK_{2}O_{4} |

196 | Potassium cyanide formula | KCN |

197 | Potassium dichromate formula | K_{2}Cr_{2}O_{7} |

198 | Potassium fluoride formula | KF |

199 | Potassium hydroxide formula | KOH |

200 | Potassium hypochlorite formula | KClO_{3} |

201 | Potassium iodide formula | KI |

201 | Potassium dihydrogen phosphate formula | KH_{2}PO_{4} |

203 | Potassium nitrate formula | KNO_{3} |

204 | Potassium nitrite formula | KNO_{2} |

205 | Potassium oxide formula | K2O |

206 | Potassium iodate formula | KIO_{3} |

207 | Potassium phosphate formula | KH_{2}PO_{4} |

208 | Potassium sulfite formula | K_{2}SO_{3} |

209 | Salicylic acid formula | C_{7}H_{6}O_{3} |

210 | Silicon dioxide formula | SiO_{2} |

211 | Silver acetate formula | AgC_{2}H_{3}O_{2} |

212 | Silver carbonate formula | Ag_{2}CO_{3} |

213 | Silver chloride formula | AgCl |

214 | Silver nitrate formula | AgNO_{3} |

215 | Silver oxide formula | Ag_{2}O |

216 | Silver phosphate formula | Ag_{3}PO_{4} |

217 | Sodium acetate formula | C_{2}H_{3}NaO_{2} |

218 | Sodium bicarbonate formula | NaHCO_{3} |

219 | Sodium bromide formula | NaBr |

220 | Sodium thiosulfate formula | Na_{2}S_{2}O_{3} |

221 | Sodium carbonate formula | Na_{2}CO_{3} |

222 | Sodium chloride formula | NaCl |

223 | Sodium chromate formula | Na_{2}CrO_{4} |

224 | Sodium citrate formula | Na_{3}C_{6}H_{5}O_{7} |

225 | Sodium cyanide formula | NaCN |

226 | Sodium dichromate formula | Na_{2}Cr_{2}O_{7} |

227 | Sodium fluoride formula | NaF |

228 | Sodium hydroxide formula | NaOH |

229 | Sodium hypochlorite formula | NaClO |

230 | Sodium iodide formula | NaI |

231 | Uric acid formula | C_{5}H_{4}N_{4}O_{3} |

232 | Sodium nitrate formula | NaNO_{3} |

233 | Sodium nitride formula | Na_{3}N |

234 | Sodium nitrite formula | NaNO_{2} |

235 | Sodium oxide formula | Na_{2}O |

236 | Sodium peroxide formula | Na_{2}O_{2} |

237 | Sodium phosphate formula | Na_{3}PO_{4} |

238 | Sodium sulfate formula | Na_{2}SO_{4} |

239 | Sodium sulfide formula | Na_{2}S |

240 | Sodium sulfite formula | Na_{2}SO_{3} |

241 | Strontium chloride formula | SrCl_{2} |

242 | Strontium nitrate formula | Sr(NO_{3})_{2} |

243 | Sucrose formula | C_{12}H_{22}O_{11} |

244 | Sugar formula | C_{12}H_{22}O_{11} |

245 | Sulfate ion formula | SO_{4}^{2−} |

246 | Sulfur dioxide formula | SO_{2} |

247 | Sulfur trioxide formula | SO_{3} |

248 | Sulfuric acid formula | H_{2}SO_{4} |

249 | Sulfurous acid formula | H_{2}SO_{3} |

250 | Tartaric acid formula | C_{4}H_{6}O_{6} |

251 | Toluene formula | C_{7}H_{8} |

252 | Urea formula | CH_{4}N_{2}O |

253 | Vinegar formula | C_{2}H_{4}O_{2} |

254 | Zinc acetate formula | Zn(O_{2}CCH_{3})_{2} |

255 | Zinc carbonate formula | ZnCO_{3} |

256 | Zinc chloride formula | ZnCl_{2} |

257 | Zinc hydroxide formula | Zn(OH)_{2} |

258 | Zinc iodide formula | ZnI_{2} |

259 | Zinc nitrate formula | Zn(NO_{3})_{2} |

260 | Zinc phosphate formula | Zn_{3}(PO_{4})_{2} |

261 | Zinc sulfate formula | ZnSO_{4} |

262 | Zinc sulfide formula | ZnS |

### How to find the molecular weight of a compound

To find the molecular weight of a compound, you need to know its atomic weight and the number of atoms in each molecule. The atomic weight is measured in grams and is the sum of the weights of the atoms in a molecule. The number of atoms in a molecule is called the molecular weight.

To find the molecular weight of a compound, you need to know its atomic weight and the number of atoms in each molecule. The atomic weight is measured in grams and is the sum of the weights of the atoms in a molecule. The number of atoms in a molecule is called the molecular weight.

### What are the properties of atoms and molecules?

Atoms are the smallest particles that make up matter. They are made of protons and neutrons and are surrounded by electrons.

Molecules are collections of atoms that have been combined together to form a unit. Molecules can have one or more than one atom in them, and they are usually cylindrical.

There are six types of molecules: water, alcohol, carbon dioxide, nitrogen, oxygen, and phosphorus.

### Why are atoms and molecules important?

Atoms are the smallest particles of an element that make up a molecule. Each atom has a nucleus, and the nucleus is surrounded by electrons. These electrons are what make atoms different from one another.

Molecules are collections of atoms that have been combined together in specific ways. Molecules can be made up of a single element, like carbon dioxide (CO 2 ), or they can be made up of two or more elements, like water (H 2 O).

The molecules that we see every day are made of small, individual atoms. However, when chemists want to study the properties of molecules, they need to use formulas that describe the atoms in those molecules. These formulas are called chemical equations.

### The Chemical Formula List for Class 10

In this post, we will be providing the chemical formula list for class 10. This list will be of great help to students as they prepare for their board exams.

The chemical formula list for class 10 is provided in both word and pdf format. The word format has been divided into two parts – the first part provides the structure of a molecule, while the second part provides the names of the atoms and groups of atoms that make up a molecule. The pdf format includes all the information contained in the word format, but it is also searchable so that you can easily find specific information.

We hope you find this post helpful and that it helps you prepare for your board exams.

### The Structure of an Atom

Atoms are the smallest unit of an element that has the chemical properties of that element. For example, carbon atoms have the chemical properties of carbon. Each atom has a nucleus at its center with protons and neutrons orbiting around it.

An atom’s nucleus is made up of protons and neutrons. Protons are positively charged and neutrons are negatively charged. The number of protons in an atom’s nucleus determines the atom’s atomic number. Atomic numbers range from 1 (atomic hydrogen) to 118 (atomic uranium).

The electrons that orbit around the nucleus are free to move about. They can orbit in any direction, but they always orbit around the nucleus in a circular path. This allows atoms to combine with other atoms to form molecules. Molecules have specific molecular formulas, which are determined by the number of atoms in each molecule.

Molecules have a specific numerical structure because their atoms are arranged in a specific way. This structure is called the molecular formula.

### Periodic Table of the Elements

The Periodic Table of the Elements is a table that lists all of the chemical elements and their atomic numbers. The table was created by Swedish scientist, Jöns Jakob Berzelius, in 1807.

The periodic table is organized into periods, which are based on the way electrons orbit around the nucleus of an atom. The first period is called the “elemental period,” and it includes just six elements: hydrogen, helium, carbon, nitrogen, oxygen, and sodium.

Each period after the elemental period includes more elements. The second period includes eight elements: neon, argon, potassium, rubidium, caesium, strontium, barium, and lanthanum.

The third period includes 10 elements: magnesium, aluminum, lithium, boron, silicon, germanium, tin, lead, antimony, and samarium.

The fourth period includes 13 elements: calcium (the first element in Group I), scandium (the second element in Group I), titanium (the third element in Group VI), vanadium (the fourth element in Group VI), molybdenum (the fifth element in Group VII), tungsten (the sixth element

### Compounds

There are a total of 118 chemical formulas in this class. They are listed below in alphabetical order.

3-Methylpyrazole

Acetic anhydride

Amino acid

Aqueous solution

Argon

Asbestos

Bacterium

Benzene

Benzyl chloride

Biological warfare agent

Boiling point

Branched chain amino acids (BCAA)

Butane

Carbon dioxide

Carpet dyeing process

### Polyatomic molecules

A polyatomic molecule is a molecule that consists of two or more atoms. Each atom in a polyatomic molecule is attached to one or more other atoms.

There are many types of polyatomic molecules, but the most common are water molecules and molecules of carbon dioxide (CO2). Water molecules are made up of two hydrogen atoms and one oxygen atom. CO2 molecules are made up of two carbon atoms and one oxygen atom.

Polyatomic molecules can play an important role in biology and chemistry. They are used to make products such as paint, gasoline, and soap. They also play a role in biochemistry, which is the study of the chemical reactions that occur in living organisms.

### Molecular compounds

Molecular compounds are molecules that consist of two or more atoms held together by covalent bonds.

Molecular compounds can be divided into two groups according to their molecular structure: organic and inorganic. Organic molecules contain carbon atoms as the main element, while inorganic molecules do not.

Organic molecules are often found in plants and animals. They include substances such as glucose, which is used by the body to produce energy. Inorganic molecules are found almost everywhere in the world, from rocks to water. They include compounds such as salt and silver.

Molecular compounds consist of atoms that are arranged in a specific way. This arrangement is called a molecule’s formula. Molecules can have more than one formula, depending on how many atoms they contain.

Each type of molecule has a unique formula. For example, glucose has the molecular formula C6H12O6. This means that it contains six carbon atoms, twelve oxygen atoms, and six hydrogen atoms.

### Biological molecules

A chemical formula is a unique set of symbols that represents the composition of a molecule. A molecule is composed of atoms and molecules, and each atom has a unique set of numbers called its atomic number. The atoms in a molecule are arranged in a specific way, and these arrangements are represented by the chemical formula.

There are many different types of molecules, and each type has its own set of chemical formulas. Some common types of molecules include water, nitrogen, oxygen, carbon dioxide, and sulfur. Each type of molecule has a different set of chemical formulas.

Chemical formulas are important because they can help chemists learn about the composition of molecules. They can also be used to create new molecules. chemists use chemical formulas to create new drugs, plastics, and other products.