CHEMICAL FORMULA POWERPOINT PRESENTATION.pptx

CHEMICAL FORMULA

1. CHEMICAL FORMULA MOISES G. PASING Grade 12

2. LEARNING OBJECTIVE: Give the similarities and differences between the empirical formula and molecular formula of a compound; Represent compounds, using chemical formulas and models; Name compounds, give their formulas; and Write a formula, and give the names of the compounds.

3. 03 IONIC COMPOUNDS, and MOLECULAR COMPOUND 02 01 Table of Contents MOLECULAR FORMULA and EMPIRICAL FORMULA CHEMICAL FORMULA NAMING COMPOUNDS

4. C 10 H 8 What is my name? NAPHTHALENE

5. C 6 H 6 What is my name? BENZENE

6. NH 3 What is my name? AMMONIA

7. CH 4 What is my name? METHANE

8. NaNO 3 What is my name? SODIUM NITRATE

9. CaCO 3 What is my name? CALCIUM CARBONATE

10. Na 2 O What is my name? SODIUM OXIDE

11. CHEMICAL FORMULA 01 MOLECULAR FORMULA and EMPIRICAL FORMULA

12. CHEMICAL FORMULA Written structure of a compound. I t is made up of the elements and the corresponding number of each in a compound

13. CHEMICAL FORMULA Indicates the actual number of each element in a compound. Simplest chemical formula It only shows the simplest ratio of atoms of the different elements present in a compound. Molecular formula E mpirical formula

14. 1. C 2 H 2 2. N 2 O 4. P 4 O 20 PH 3 3. C 8 H 10 5. 6. C 2 H 4 2 Write the empirical formula of the following compounds.

15. 1. CH 2. N 2 O 4. PO 5 PH 3 3. C 4 H 5 5. 6. CH 2 Write the empirical formula of the following compounds.

16. CHEMICAL FORMULA Most compounds have the same molecular and empirical formula. EXAMPLE: W ater – H 2 O A mmonia – NH 3 Methane – CH 4 E thanol – C 2 H 6 O C arbon tetrachloride – CCl 4

17. NAMING COMPOUNDS 02 IONIC COMPOUND, MOLECULAR COMPOUND

18. WRITING CHEMICAL FORMULA In writing the chemical formula of a compound, oxidation number or oxidation state is used. The oxidation number of an element is a positive or negative integer that is related to the electronic structure of the atoms to keep track of the number of valence electrons lost or gained .

19. WRITING CHEMICAL FORMULA A. IONIC COMPOUND The oxidation number of an ion is the same as the charge of the ion. The atom that loses electrons has a positive oxidation number and the atom that gains electrons has a negative oxidation number.

20. WRITING CHEMICAL FORMULA B. COVALENT COMPOUND The oxidation number of an atom does not necessarily correspond with the number of covalent bonds joining the atom to another atom. The atom that is more electropositive has the positive oxidation number and the atom that is more electronegative has the negative oxidation number .

21. NAMING COMPOUNDS TRANSFER OF ELECTRONS (metals lost electrons, nonmetals gained electrons) Ionic compounds are made of cations and anions. COVALENT COMPOUNDS (sharing of electrons of two nonmetallic elements) IONIC COMPOUND MOLECULAR COMPOUND

22. 1. For binary compounds (2 distinct elements), the metal cation is named first using the name of the element; then, the anion is named by taking the first part of the elemental name and adding the suffix –IDE at the end. A. IONIC COMPOUND

23. 2. For ternary compounds (composed of 3 distinct elements), the elemental name of the cation goes first before the name of the polyatomic anion which usually ends in ITE or ATE. A. IONIC COMPOUND CATION POLYATOMIC ANION COMPOUND NAME Na + NO 3 -1 NaNO 3 SODIUM NITRATE Na + NO 2 -1 NaNO 2 SODIUM NITRITE Ca +2 CO 3 -2 CaCO 3 CALCIUM CARBONATE

24. 3. Two naming methods can be used for compounds containing a metallic ion with variable charge . CLASSICAL METHOD – named using the suffix –OUS (lower charge) or –IC (higher charge). Latin names STOCK METHOD – metal is named first, immediately followed by the value of the charge written in Roman numeral enclosed in parentheses. A. IONIC COMPOUND

25. ION OXIDATION # STOCK SYSTEM CLASSIC SYSTEM Sn +2 TIN (II) STANNOUS +4 TIN (IV) STANNIC Hg +1 MERCURY (I) MERCUROUS +2 MERCURY (II) MERCURIC Cu +1 COPPER (I) CUPROUS +2 COPPER (II) CUPRIC Fe +2 IRON (II) FERROUS +3 IRON (III) FERRIC Cr +2 CHROMIUM (II) CHROMOUS +3 CHROMIUM (III) CHROMIC Mn +2 MANGANESE (II) MANGANOUS +3 MANGANESE (III) MANGANIC Co +2 COBALT (II) COBALTOUS +3 COBALT (III) COBALTIC Au +1 GOLD (I) AUROUS +3 GOLD (III) AURIC

26. CATION ANION COMPOUND CLASSICAL NAME STOCK NAME Fe +2 Cl -1 FeCl 2 Ferrous chloride Iron (II) chloride Fe +3 Cl -1 FeCl 3 Ferric chloride Iron (III) chloride Sn +2 OH -1 Sn(OH) 2 Stannous hydroxide Tin (II) hydroxide Sn +4 OH -1 Sn(OH) 4 Stannic hydroxide Tin (IV) hydroxide Cu +2 ClSO -2 FeCl 3 Ferric chloride Iron (III) chloride

27. For one pair of elements that forms several different compounds, Greek prefixes are used to determine the number of each element in the compound. For the first elements, the prefix “mono is omitted. EXAMPLE: CO – carbon monoxide NO 2 – nitrogen dioxide B. COVALENT COMPOUND/ MOLECULAR COMPOUND MONO – 1 HEXA – 6 DI – 2 HEPTA – 7 TRI – 3 OCTA – 8 TETRA – 4 NONA – 9 PENTA – 5 DECA - 10

28. 2. For binary compounds, the name of the first element is used first, followed by the second element with –IDE added to its root. EXAMPLE: HCl – hydrogen chloride HBr – hydrogen bromide HI – hydrogen iodide SiC – Silicon carbide B. COVALENT COMPOUND/ MOLECULAR COMPOUND

29. 3. For binary compounds considered as acids, the prefix –HYDRO is added to the stem name of the anion with its suffix change to –IC . EXAMPLE: HCl – hydrochloric acid HBr – hydrobromic acid HI – hydroiodic acid HF – hydrofluoric acid B. COVALENT COMPOUND/ MOLECULAR COMPOUND

30. 4. Oxyacids (acids that contain hydrogen, oxygen, and other elements) are named in two ways. For ions ending with –ATE, with suffix of the anion, is changed from –ATE to -IC followed by the word acid. B. COVALENT COMPOUND/ MOLECULAR COMPOUND ANION NAME OF ANION FORMULA NAME OF ACID SO 4 2 SULFATE H 2 SO 4 SULFURIC ACID ClO 4 - PERCHLORATE HClO 4 PERCHLORIC ACID BrO 3 - BROMATE HBrO 3 BROMIC ACID

31. b. For anions ending with –ITE, the suffix of the anion is changed from –ITE to –OUS followed by the word “acid”. B. COVALENT COMPOUND/ MOLECULAR COMPOUND ANION NAME OF ANION FORMULA NAME OF ACID Cl 2 - CHLORITE HClO 2 CHLOROUS ACID NO 2 - NITRITE HNO 2 NITROUS ACID SO 3 2- SULFITE H 2 SO 3 SULFUROUS ACID

32. H 3 PO 4 PHOSPHORIC ACID H 3 PO 3 PHOSPHOROUS ACID HNO 3 NITRIC ACID HNO 2 NITROUS ACID H 2 C 2 O 4 OXALIC ACID HC 2 H 3 O 2 ACETIC ACID

33. INSTRUCTION: Write the formula of each of the following compounds. LITHIUM CARBONATE POTASSIUM CHROMATE SODIUM CYANIDE ALUMINUM CHLORIDE SULFUR DIOXIDE TRY THIS!

34. INSTRUCTION: Write the formula of each of the following compounds. Li 2 CO 3 K 2 CrO 4 NaCn AlCl 3 SO 2 TRY THIS!

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