chemical naming unit

8/18/2019 Chemical Naming Unit

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Chemical Naming

Chemical Naming:Chemical nomenclature is a set of rules to

generate systematic names for chemical compounds. Thenomenclature rules used most frequently worldwide are

these created and developed by the International Union ofPure and Applied Chemistry (IUPAC). For our purposes,we will simply say it is a system of naming chemicalcompounds.

There are two primary forms of compounds that willrequire naming in the world of chemistry. There areorganic compounds, compounds that contain the elementcarbon, and there are inorganic compounds, all remainingcompounds that do not include the element carbon.

In this course we are going to focus our attention onnaming the inorganic compounds, and writing theformulas of these compounds.

You should have already memorized the twenty fivecommon polyatomic ions that are listed on the back ofyour periodic table. If you haven’t memorized these yet,it is of utmost importance to accomplish this task as soonas possible. This is because these polyatomic ions play asignificant role in naming compounds and writingformulas.

The following are some examples of namingcompounds and writing formulas.

Chemical Name: Ions present: Formula:

Sodium chloride Na+1 Cl-1 NaClMagnesium nitride Mg+2 N-3 Mg3N2 Zinc oxalate Zn+2 C2O4

-2 ZnC2O4

Nickel (II) nitrate Ni+2 NO3-1 Ni(NO3)2

Iron (II) sulfate Fe+2 SO4-2 FeSO4

Iron (III) sulfate Fe+3 SO4-2 Fe2(SO4)3

Lead (IV) carbonate Pb+4 CO3-2 Pb(CO3)2

Ammonium phosphite NH4+1 PO3

-3 (NH4)3PO3

All the videos will be posted on YouTube and can beaccessed using multiple sources. The videos have beenformatted to work on iPhones, iPads, Android phonesKindles, and Nooks. The titles of the videos are listed below so that you can search them, and the creator of the

videos should be NRHSChemistry.

Lesson Target(s) for Each Video: Video 1 – Naming Overview

I can classify a chemical compound as either amolecular or ionic compound.

I can compare ionic and molecular compounds. Video 2 – Binary Compounds

I can identify and name a binary compound. Video 3 – Naming Ionic Compounds

I can determine the chemical name of an ioniccompound.

Video 4 –

Writing Ionic Formulas I can produce a correct ionic chemical formula.

I can distinguish between metals and their multipleoxidation numbers.

Video 5 – Naming Molecular Compounds I can differentiate between binary compounds and

other types of compounds

I can determine the chemical name of a molecularcompound.

Video 6 – Writing Molecular Formulas I can produce a correct molecular chemical formula.

Video 7 – Writing and Naming Acids

I can develop names and formulas of acids. I can recognize compounds that are acids.

Essential Learning Outcomes:1. The classification and nomenclature of compounds are

based upon which elements and the number of theseelements that a compound contains.

2. Chemical formulas will give clues to the type of chemicalreaction that will occur and the ways a chemical will react.

http://en.wikipedia.org/wiki/Systematic_namehttp://en.wikipedia.org/wiki/Chemical_compoundhttp://en.wikipedia.org/wiki/International_Union_of_Pure_and_Applied_Chemistryhttp://en.wikipedia.org/wiki/International_Union_of_Pure_and_Applied_Chemistryhttp://en.wikipedia.org/wiki/International_Union_of_Pure_and_Applied_Chemistryhttp://en.wikipedia.org/wiki/International_Union_of_Pure_and_Applied_Chemistryhttp://en.wikipedia.org/wiki/Chemical_compoundhttp://en.wikipedia.org/wiki/Systematic_name


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Required activities: Due dates are in parentheses

□ Chemical Naming P.S. 1-7 (12/4)o Video 1 – Naming Overview (11/30)o Video 2 – Binary Compounds (11/30)

□ Chemical Naming P.S. 8-13 (12/8)o Video 3 – Naming Ionic Cmpds (12/1)o Video 4 – Writing Ionic Formulas (12/2)

□ Chemical Naming P.S. 14-17 (12/10)o Video 5

–

Naming Molecular Cmpds (12/3)o Video 6 – Writing Molecular Cmpds (12/4)

□ Chemical Naming P.S. 18-20 (12/14)o Video 7 – Writing & Naming Acids (12/8)

□ Naming Worksheet 1 (12/11)□ Naming Worksheet 2 (12/11)□ Programmed Learning Packet (12/16)□ Sheet of 40 and 100 (12/17)□ Nomenclature and Household items (12/14)

o Data and Questions (12/17)

□ Chemistry NAME-O (Played as a class) (12/9)□ Naming Quiz 1 (12/15)□ Naming Quiz 2 (12/15)□ Chemical Naming Unit Quest (12/18)

Important Vocabulary Cation Polyatomic ion

Anion Molecular compound

Monoatomic ion Binary compound

Acid Base

Law of Definite

Proportions

Ionic compound

Additional Resources:1. http://www.quia.com/shared/science/2. http://www.sporcle.com/games/RyanWitchey/Chem_Ionic

iPhone and iPad Apps:1. Chemistry Formula Practice by Carolina Biological

Supplya. There is a FREE version but the better

version is $1.992. Chemistry Formulas by 99MediaLab LLC $0.99

http://www.quia.com/shared/science/http://www.quia.com/shared/science/http://www.sporcle.com/games/RyanWitchey/Chem_Ionichttp://www.sporcle.com/games/RyanWitchey/Chem_Ionichttp://www.sporcle.com/games/RyanWitchey/Chem_Ionichttp://www.sporcle.com/games/RyanWitchey/Chem_Ionichttp://www.quia.com/shared/science/


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Chemistry Name:

Problems and Questions Chemical Naming Hour:

Directions: Answer the following questions using complete sentences when necessary. On numerical problems, show all workcircle your answers, and follow all rules of significant figures for full credit.

1. Classify each of the following elements as a metal, nonmetal, or metalloid. Use complete sentences.a) Aluminumb) Silver

c) Silicond) Heliume) Zinc

2. What is an ion? Describe the formation of a cation and of an anion.

3. State the number of electrons either lost or gained in forming each ion. (ex: Sc+3 has lost three electrons.)a) S-2 b) K + c) Cl- d) Ba+2 e) Li+ f) H-

4. Name each of the ions in #3 and state whether they are cations or anions.

5. Using only the periodic table, name and write the formulas of the ions of these representative elements.a) Lithium b) Oxygen c) Barium d) Nitrogen

e) Fluorine f) Potassium g) Neon h) Beryllium

6. Would you expect the following compounds to be ionic or molecular?a) CO b) KBr c) Li2O d) C3H8 e) SO3 f) AlCl3

7. How are one of Dalton's theories and the law of definite proportions similar?

8. List three characteristics of ionic compounds and three characteristics of molecular compounds.

9. Name the following ions.a) NO3-1 b) H+ c) CN- d) Cr+3 e) Cr2O7-2

f) HPO4-2 g) Sn+4 h) MnO4- i) SO3-2 j) Se-2

10. Write the formula and charge of each of the following ions.a) Magnesium ionb) Lead (IV) ionc) Chromate iond) Tin (II) ione) Nitrite ionf) Iodide iong) Chlorate ionh) Hydroxide ioni) Iron (II) ionj) Ammonium ionk) Copper (I) ion

11. Write the formulas for the compounds formed from these pairs of ions.a) Sr+2, Se-2 b) K +, O-2 c) Ca+2, N-3 d) Co+3, I-

12. Write the formulas for these compounds.a) Silver sulfide b) Tin (IV) chloride c) Sodium nitrided) Strontium iodide e) Silver sulfate f) Potassium chlorateg) Mercury (II) bromide h) Ammonium dichromate i) Lithium hydrogen sulfatej) Chromium (III) nitrite


4/18

13. Rewrite this table in your notebook and write the correct formulas for the compounds formed by combining positive and negative ions. Then name each compound.

SO4-2 OH- PO4-3 S-2

Ca+2 _______ ________ _________ _________NH4+ _______ ________ _________ _________ Al+3 _______ ________ _________ _________Pb+4 _______ ________ _________ _________

14. Name each of the following substances.a) CaO b) Ba3(PO4 )2 c) I2 d) BaSO4 e) Mg(OH)2

f) NO2 g) CuC2H3O2 h) HClO4 i) Cl2O j) HgF2 k) (NH4 )2C2O4 l) NO2-1

15. Write the formulas of these compounds.a) Calcium carbonate b) Sodium bromide c) Iron (III) sulfated) Magnesium sulfide e) Sulfuric acid f) Sulfur trioxideg) Nitrogen gas h) Barium hydroxide i) Sulfite ionj) Copper (II) iodide k) Zinc oxalate l) Manganese (IV) oxide

16. Name each compound.a) NH4OH b) HF c) PI3 d) Be(NO3 )2 e) KMnO4

f) CO g) K 2CO3 h) N2H4 i) ZnO j) Mg(MnO4 )2 k) Li2HPO4 l)Li2CO3

17. Write the formulas of these compoundsa) Silver chlorideb) Aluminum carbidec) Lithium hydrided) Sodium acetatee) Iron (III) carbonatef) Copper (II) chlorateg) Sodium silicateh) Calcium oxidei) Potassium cyanidej) Tin (II) cyanide

k) Hydrogen bromidel) Potassium phosphide

18. Name these compounds.a) Na2Cr2O7 b) AlI3 c) SnO2 d) Fe(C2H3O2 )3 e) KHSO4 f) Co(NO2 )3 g) CaH2 h) HClO3 i) HgBr2 j) AlPk) FeCO3 l) H2CrO4

19. Write the formulas of these compounds.a) Phosphorus pentabromide g) Ammonium nitrateb) Carbon tetrachloride h) Dichlorine heptoxidec) Potassium permanganate i) Trisilicon tetranitrided) Ammonium perchlorate j) Sodium silicatee) Calcium hydrogen carbonatef) Copper (II) hydroxide

20. Write the formulas or names of the following acids.a) Sulfuric acid e) H2CO3 i) HNO3

b) HCl f) Nitrous acid j) Phosphorous acidc) H3PO4 g) H2SO3 d) Hydrofluoric acid h) Hydrosulfuric acid


5/18

Formula Writing Practice

WRITE THE CORRECT FORMULA FOR THE FOLLOWING COMPOUNDS:1. Iron (I) carbonate 51. Calcium sulfate 2. Lead (IV) phosphate 52. Calcium sulfite 3. Phosphorus pentoxide 53. Ammonium nitrite 4. Zinc sulfide 54. Sodium hydroxide 5. Sodium phosphate 55. Zinc chloride

6. Magnesium carbonate 56. Zinc nitrate 7. Ammonium nitrite 57. Zinc hydroxide 8. Iron (III) nitrate 58. Zinc hydrogen sulfite 9. Copper (II) hydroxide 59. Aluminum hydroxide 10. Calcium fluoride 60. Aluminum oxide 11. Bismuth (III) nitrate 61. Copper (III) permanganate 12. Iron (III) oxide 62. Sodium sulfite 13. Ammonium sulfite 63. Chromium (III) sulfide14. Calcium chloride 64. Ammonium acetate 15. Sodium nitrate 65. Ammonium bromide 16. Copper (II) bromide 66. Barium chloride 17. Aluminum sulfate 67. Calcium bromide

18. Potassium Nitrite 68. Calcium carbonate 19. Zinc Sulfate 69. Copper (III) chloride 20. Antimony (III) chloride 70. Lead (II) acetate 21. Silver sulfide 71. Magnesium sulfate 22. Iron (II) cyanide 72. Iron (III) oxide 23. Ammonium phosphate 73. Iron (II) sulfate 24. Sulfur dioxide 74. Iron (II) hydroxide 25. Silver bromide 75. Iron (III) cyanide 26. Tin (II) chloride 76. Thallium (II) chlorate 27. Tungsten (VI) oxide 77. Magnesium perchlorate 28. Chromium (III) nitrate 78. Manganese (II) nitrate 29. Magnesium hydroxide 79. Lead (IV) dichromate

30. Lead (II) carbonate 80. Mercury (II) sulfate 31. Mercury (II) nitrate 81. Sodium phosphate 32. Mercury (I) silicate 82. Sodium dichromate 33. Nickel (II) sulfate 83. Sodium acetate 34. Potassium chlorate 84. Iron (III) chloride 35. Magnesium nitride 85. Barium hydrogen carbonate 36. Sodium sulfite 86. Iron (III) hydroxide 37. Iron (III) chloride 87. Sodium silicate 38. Manganese (IV) oxide 88. Potassium carbonate 39. Platinum (IV) chlorite 89. Potassium nitrite 40. Ammonium nitrate 90. Potassium sulfate 41. Nickel (II) carbonate 91. Potassium oxalate 42. Cobalt (II) chloride 92. Silver nitrate43. Barium carbonate 93. Silver acetate 44. Radium bromide 94. Mercury (II) chloride 45. Carbon dioxide 95. Calcium hydrogen phosphate 46. Barium sulfate 96. Lead (II) chromate 47. Potassium permanganate 97. Sodium oxalate 48. Potassium hydroxide 98. Mercury (II) oxide 49. Calcium hydroxide 99. Mercury (I) chloride 50. Carbon tetrachloride 100. Sodium sulfide


6/18

Compound Names

GIVE THE CORRECT NAMES FOR THE FOLLOWING CHEMICAL FORMULAS:

1. KI 21. NH4Cl

2. CaF2 22. SnI4

3. Ba(ClO4)2 23. ZnO

4. ZnSO3 24. CuCN

5. AgNO3 25. Fe(OH)3

6. HF 26 PbCO3

7. MgO 27. Li2SO3

8. CaCO3 28. BaCr 2O7

9. Mn3(PO3)2 29. NaC2H3O2

10. AsCl3 30. Mg3(PO4)2

11. HgCl2 31. Na2O

12. PtCl 32. CCl4

13. Rb2S 33. K 2S

14. Al(NO2)3 34. Ni(NO2)2

15. K 2S 35. Mn2(Cr 2O7)3

16. Fe2O3 36. CaSO3

17. HI 37. K 2C2O4

18. SnCl2 38. Ca2C

19. SO3 39. CO

20. AlN 40. KCN


7/18

Nomenclature and ousehold Items

Background:Many household items contain chemicals that are commonly used in everyday life. Some chemicals are edible while

others would be poisonous to consume. Many non-edible household chemicals are used as cleaners. Soaps, detergents

drain-openers, countertop sprays, oven sprays, furniture polish, air fresheners and floor cleaners are examples of

chemical substances that are commonly used inside the home. Other chemicals are edible and can be used for cooking

or in medication. Baking soda, sugar, salt, and baking powder are all edible substances commonly used in cooking.

Antacids, aspirin, and vitamin C are edible substances that are used as medicines.

Household items can be classified as acids (pH7), or neutral (ph=7). Soaps, detergents, drain-openers,

antacids, and ammonia can be classified as bases. Antacids contain carbonates, bicarbonates, and hydroxides to

neutralize the hydrochloric acid in the stomach. Aspirin (acetyl salicylic acid), Vitamin C (ascorbic acid), and vinegar

(solution of acetic acid) can be classified as acidic.

Product containers list valuable information such as ingredients, warnings, customer service numbers, and expiration

dates. The chemical name listed first on the ingredient list is the main component of that substance. The warning label

will vary with the chemical hazard of the main ingredient. In this lab many household items will be viewed to obtain thechemical name. The chemical name will then be used to write the formula of the compound.

Procedure:1. Visit each of the twelve lab stations and copy down the name of the substance.2. While at the lab stations, decide the main use for the substance (cooking, cleaning, or medicine) and record this

in the usage column.

3. Look on the ingredient list to find the main component on the substance. Write the name of the maincomponent in the appropriate column of the data table.

4. Looking at the name of the main ingredient/component, write the formula of the substance.5. Look to see if the substance has a warning or hazard listed. Write “Yes” if the substance has a hazard or a

warning. Write “No” if the substance does not list a hazard or warning. Analysis:

1. Identify how many items you have in each usage category. Explain why you grouped particular items with eachother and not in a different group.

2. On what types of products did most of the warning/hazard labels appear? Explain why products that serve asimilar purpose might have similar warnings.

3. Make a general statement explaining a consistent pattern for each type of chemical (cooking, cleaning, andmedicine). Make a statement for all three types of products. Ex: All cleaning products….. All cooking products…

4. Create a fourth category you could have used to classify the products. What would that category have been

called? Which products would you have put into this new category? Why move these products to the newcategory.

5. What smell do you associate with a swimming pool? Is this smell also present in any of the products you lookedat? Hypothesize why swimming pools do not contain warning labels regarding the chemicals being used and

support your answer.


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Data Table:

Substance Usage Name of main componentFormula of main

component

Hazard or

Warning

1

2

3

4

5

6

7

8

9

10

11

12


9/18

Program Learning: Writing and Naming Chemical Formulas

There are a few inorganic compounds which are identified by their common or trivial names. The most

common of these are H20, named water, and NH3, named ammonia. All other inorganic compounds are named

according to the systematic rules of nomenclature. Two or more systems may be used in naming a compound.

Generally, no one system is used exclusively, and it is necessary to become familiar with the systems in

common use.

This program involves the nomenclature of compounds containing two different elements. Such compounds are

called binary compounds. The general rule for naming binary compounds is that the less electronegative (more

electropositive or more metallic) element is named first, followed by the name of the more electronegative

(more nonmetallic) element, with the name of the latter having its normal ending replaced by the suffix – ide.

KBr is classed as a (1) __________________ compound because it contains (2) ___________________

different elements. In this compound, the name of the metallic element is (3) _____________________

and the name of the nonmetallic element is (4) ________________. In naming this compound, the name

of the (5) ____________________ element is written first. The normal ending of the name of the

nonmetallic element is removed, forming a stem, and to this stem is added the suffix (6) ____________.

Following this procedure, the name of the compound KBr is written as (7) _______________________.

In forming a stem, the last syllable in the name of the element is generally dropped. The stem neverends in a vowel. Thus, the stem for chlorine is chlor . The stem for iodine is (8) __________________.

The stem for arsenic is (9) _____________________, for selenium (10) _________________________,

for carbon (11) _______________. Should the stem end in a vowel or a vowel sound, the vowel is also

dropped to make the stem. In making a stem from nitrogen, dropping the last syllable gives nitro. Since

o is a vowel, it also is dropped, giving nitr . A binary compound in which nitrogen is the more

electronegative element is called a nitride. The stem for oxygen is (12) ____________________ since

oxy ends in a vowel sound. The stem for phosphorus is (13)______________. There are exceptions to

these rules.

Consider the compound MgI2. The name of the metallic element is (14) ___________________ and the

name of the nonmetallic element is (15) _____________________. The (16) _____________________

element is named first. A stem is formed from the name of the (17) ___________________ element and

to this stem is added the suffix (18) _______________. Following this procedure, the name of the

compound MgI2 is written as (19) ______________________________.


10/18

To write the correct chemical name of the compound NH3, commonly known as

(20)__________________, it is necessary to know that nitrogen is more electronegative (nonmetallic)

than hydrogen. The element (21) ____________ is named first, and a stem is formed from the name of

the element (22)____________________. Thus, the correct chemical name for NH3 is

(23)__________________________. Usually, formulas of compounds are written with the symbol of

the more metallic element listed first.

Write the names of the following compounds, assuming that the more metallic element is listed first.

H20 (24) ___________________________________

AlF3 (25) ___________________________________

Ca2C (26) ___________________________________

K 2S (27) ___________________________________

Mg3 N2 (28) ___________________________________

Ca3P2 (29) ___________________________________

BaH2 (30) ___________________________________

HCl (31) ___________________________________

The binary and hydrogen-containing compounds of Group VII A elements and Group VI A elements other than

oxygen produce acids when dissolved in water. Such acids are named by adding the prefix hydro- and the

suffix – ic to the stem of the name of the nonmetal. This word is then followed by the word acid to complete the

name of the substance. Consider the name of the acid which results when the gas hydrogen chloride, HCl, is

dissolved in water.

The stem of the nonmetallic element is (32) _______________________. Adding to this stem the prefix

(33) _______________ and the suffix (34) ________________________ gives the word

(35) ____________________. Thus, a water solution of HCl is named (36) _____________________

acid. A water solution of HF is named (37) _________________________. A water solution of HBr is

named (38) ___________________________. (In naming sulfur compounds, the suffixes – ic and – ous

are added to the word sulfur rather than to the stem sulf .)


11/18

There are several polyatomic ions which are treated as single atoms when naming compounds. The names and

formulas of the most common of these ions are:

NH4+ - ammonium ion

OH- - hydroxide ion

CN- - cyanide ion

(Note the difference between NH3, ammonia, which is a neutral molecule, and NH4+, the ammonium

ion, which carries a charge of +1.) Compounds containing the above ions are named according to the

general rule for naming binary compounds. Thus, the name for NaOH is sodium hydroxide. The name

for NH4Cl is (39) __________________________________________. The name for KCN is

(40)_____________________________. The name for NH4OH is (41) ________________________.

The same elements can sometimes combine to form more than one compound. For example, the elements

sulfur and oxygen can combine to form the compounds SO2 and SO

3. Since SO

2 and SO

3 are two distinct

compounds, both cannot be named sulfur oxide. Several methods may be used to distinguish between such

compounds.

For binary compounds of nonmetals, the general rule is modified to include prefixes with the names of

the elements. The prefix mono- means one, but is generally not used. The other prefixes up to 10 are di-

, two; tri-, three; tetra-, four; penta-, five; hexa-, six; hepta-, seven; octa-, eight; ennea- or nona-, nine;

and deca-, ten. Thus N2O5 is named dinitrogen pentoxide, NO2 is named nitrogen dioxide, and N2O4 is

named dinitrogen tetroxide. For P4O10, the prefix (42) _____________________ is used with

phosphorus and the prefix (43)__________________ is used with oxide to give the name

(44)________________________________________________. When a prefix ending in a is added to

a word beginning with o or a, the a in the prefix is dropped.

Name the following compounds according to the above rule.

SF4 (45) _____________________________________

SF6 (46) _____________________________________

SO2 (47) _____________________________________

SO3 (48) _____________________________________

N2O3 (49) _____________________________________

N2O (50) _____________________________________

P4O6 (51) _____________________________________

P4S10 (52) _____________________________________


12/18

Write formulas for the following compounds.

Phosphorus trichloride (53) _______________________________

Phosphorus pentachloride (54) _______________________________

Dichlorine heptoxide (55) _______________________________

Chlorine dioxide (56) _______________________________

The preferred system for naming compounds of metals with variable oxidation states is the IUPAC

(International Union of Pure and Applied Chemistry) system, often known as the Stock system. According to

this system, the oxidation state of the metal is indicated by writing it in Roman numerals enclosed in

parentheses after the name of the metal. For binary compounds, the suffix – ide is added to the stem of the name

of the nonmetal as before. Consider the compounds SnO and SnO2. Since the usual oxidation number of

oxygen in compounds is – 2, the oxidation numbers of Sn in SnO and SnO2 are +2 and +4 respectively. Thus,

the compound SnO is named tin(II) oxide. In compounds of metals with chlorine, the oxidation number of

chlorine is –

1. Thus, in the compounds FeCl2 and FeCl3 the oxidation numbers of Fe are +2 and +3,

respectively. According to the IUPAC system, FeCl2 is named iron (II) chloride and FeCl3 is named

(57) _________________________________. Name the following compounds according to the IUPAC

system.

HgS (58) ___________________________________

Hg2S (59) ___________________________________

Sn(OH)2 (60) ___________________________________

Sn(OH)4 (61) ___________________________________

MnO (62) ___________________________________

Mn2O3 (63) ___________________________________

MnO2 (64) ___________________________________

CuCN (65) ___________________________________

Cu(CN)2 (66) ___________________________________

Fe2O3 (67) ___________________________________

FeO (68) ___________________________________

FeF2 (69) ___________________________________

PbO2 (70) ___________________________________

PbO (71) ___________________________________


13/18

Chemical Formula Writing Worksheet: Naming Worksheet 1

Write chemical formulas for the compounds in each box. The names are found by finding the

intersection between the cations and anions. Example: the first box is the intersection between

eh “zinc” cation and the “chloride” anion, so you should write “ZnCl 2”, as shown.

Zinc Sodium Magnesium Gallium Silver Lead (IV)

Chloride

Phosphite

Nitrate

Oxide

Nitride

Sulfate

Write the formulas for the following compounds:

1. Copper (II) chloride __________________________

2. Lithium acetate __________________________

3. Vanadium (III) selenide __________________________

4. Manganese (IV) nitride __________________________

5. Beryllium oxide __________________________

6. Sodium sulfate __________________________

7. Aluminum arsenide __________________________

8. Potassium permanganate __________________________

9. Chromium (VI) cyanide __________________________

10. Tin (II) sulfite __________________________

11. Vanadium (V) fluoride __________________________

12. Ammonium nitrate __________________________


14/18

Naming Covalent Compounds Worksheet: Naming Worksheet 1

Write the formulas for the following covalent compounds:

1. Antimony tribromide ____________________________

2. Hexaboron monosilicide ____________________________

3. Chlorine dioxide ____________________________

4. Hydrogen monoiodide ____________________________

5. Iodine pentafluoride ____________________________

6. Dinitrogen trioxide ____________________________

7. Ammonia ____________________________

8. Phosphorous triiodide ____________________________

Write the names for the following covalent compounds:

1. P4S5 ________________________________________

2. O2 ________________________________________

3. SeF6 ________________________________________

4. Si2Br6 ________________________________________

5. SCl4 ________________________________________

6. CH4 ________________________________________

7. B2Si ________________________________________

8. NF3 ________________________________________


15/18

P O

4 - 3

P h o s p h a t e

C O

3 - 2

C a r b o n a t e

S

O 4

- 2

S u

l f a t e

C N - 1

C y a n i d e

N O

3 - 1

N i t r a t e

O

H - 1

H y d

r o x i d e

C u O H

C o p p e r ( I ) h y d r o x i d e

C u ( O H ) 2

C o p p e r ( I I ) h y d r o x i d e

N a m i n g W o r k s h e e t

2 C u

+ 1

C o p p e r I

C u

+ 2

C o p p e r I I

F e

+ 2

I r o n I I

F e

+ 3

I r o n I I I

C r +

2

C h r o m i u m I

I

C r +

3

C h r o m i u m I

I I

P b + 2

L e a d I I

S n

+ 2

T i n I I

S n

+ 4

T i n I V


16/18

N - 3

N i t r i d e

P - 3

P h o s p h i d e

S - 2

S u

l f i d e

O - 2

O x i d e

B r -

1

B r o m i d e

C l - 1

C h l o r i d e

C

u C l

C o p p e r

( I ) c h l o r i d e

C u C l 2

C o p p e r ( I I ) c h l o r i d e

N a m i n g W o r k s h e e t

2 C u

+ 1

C o p p e r I

C u

+ 2

C o p p e r I I

F e

+ 2

I r o n I I

F e

+ 3

I r o n I I I

C r +

2

C h r o m i u m I

I

C r +

3

C h r o m i u m I

I I

P b + 2

L e a d I I

S n

+ 2

T i n I I

S n

+ 4

T i n I V


17/18

CHEMISTRY NAME-O

N A M E O

FREE

CHEMIC LS

Use the following names to fill in your NAME-O Card:

Copper (II) chloride Sodium chloride Carbon tetrachloride

Silver nitrate Potassium permanganate Carbon monoxideIron (III) phosphate Mercury (II) chromate Diphosphorous pentaoxide

Lead (II) iodide Magnesium chloride Sulfur hexafluoride

Iron (II) oxide Calcium hydroxide Dinitrogen trioxideSodium silicate Iron (III) sulfide Tetraphosphorous decaoxide

Ammonium hydroxide Zinc acetate Tricarbon hexahydride

Manganese (II) phosphite Calcium carbonate Sulfur trioxideAluminum oxalate Lead (IV) hydrogen sulfate Oxygen dichloridePotassium chlorate Cobalt (III) nitride Carbon dioxide

Magnesium bromide Tin (II) nitrate Iodine monochloride

Copper (I) dichromate Sodium perchlorate Carbon disulfideManganese (III) hydrogen phosphate Aluminum oxide Nitrogen tribromide

Tin (IV) cyanide Lead (II) sulfate Sulfur triiodide

Cobalt (II) selenide Ammonium phosphate Selenium dichloride


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SeCl2 CuCl2 Mn3(PO3)2

SI3 NaCl Al2(C2O4)3 NBr 3 AgNO3 Pb(HSO4)4

CS2 FePO4 KClO3ICl KMnO4 CoN3 CO2 HgCrO4 MgBr 2

OCl2 PbI2 Sn(NO3)2

SO3 MgCl2 NaClO4C3H6 Ca(OH)2 Cu2Cr 2O4P4O10 FeO Mn2(HPO4)3 N2O3 Na2SiO3 Al2O3

SF6 Fe2S3 Sn(CN)4 P2O5 NH4OH PbSO4

CO ZnC2H3O2 (NH4)3PO4

CCl4 CaCO3 CoSe

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