C Chemical Nomenclature right · Objectives Students will: Learn to apply the rules of chemical...

Chemical Nomenclature

Chemical Nomenclature Naming and Writing Chemical Formulas

About this Lesson This activity is a guided lecture to teach students the rules for naming and writing various types of chemical formulas. This lesson is more in depth than many high school texts including the introduction of organic nomenclature early on in the course. This lesson is included in the LTF Chemistry Module 4. Objectives Students will:

Learn to apply the rules of chemical nomenclature.

Practice naming and writing formulas.

Level Chemistry

Common Core State Standards for Science Content LTF Science lessons will be aligned with the next generation of multi-state science standards that are currently in development. These standards are said to be developed around the anchor document, A Framework for K–12 Science Education, which was produced by the National Research Council. Where applicable, the LTF Science lessons are also aligned to the Common Core Standards for Mathematical Content as well as the Common Core Literacy Standards for Science and Technical Subjects.

Code Standard Level of Thinking

Depth of Knowledge

(LITERACY) RST.9-10.3

Follow precisely a multistep procedure when carrying out experiments, taking measurements, or performing technical tasks, attending to special cases or exceptions defined in the text.

Apply II


Translate quantitative or technical information expressed in words in a text into visual form (e.g., a table or chart) and translate information expressed visually or mathematically (e.g., in an equation) into words.

Apply II


Assess the extent to which the reasoning and evidence in a text support the author’s claim or a recommendation for solving a scientific or technical problem.

Apply II

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Connections to AP* AP Chemistry:

Chemical nomenclature is fundamental to the AP Chemistry, AP Biology and AP Environmental Science courses

*Advanced Placement and AP are registered trademarks of the College Entrance Examination Board. The College Board was not involved in the production of this product.

Materials and resources

Each lab group will need the following: bag, zipper-lock, quart copy of student formula manipulatives scissors

Assessments The following types of formative assessments are embedded in this lesson:

Assessment of prior knowledge. Guided practice through the lesson.

The following additional assessments are located on the LTF website: Chemistry Assessment: Nomenclature 2006 Chemistry Posttest, Free Response Question 1 and 2 AP Style Free Response

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Teaching suggestions This activity is designed to enhance a student’s ability to write and name chemical formulas. The students must be assigned the list of polyatomic ions for memorization. Ideally this memorization is done as a summer assignment or at least a few weeks before this activity. Quiz students over the list of ions each class period to encourage their participation. Once they have mastered the memory work, continue quizzing them weekly to ensure retention.

The students will create a set of manipulatives using the templates provided in the student section of this activity. These manipulatives will help students determine correct chemical formulas. It is recommended that you enlarge the template on a copy machine and make a demonstration set of the manipulatives for use on the chalk or white board in your classroom. If possible, make your set of manipulatives out of colored card stock and laminate them for durability. If the chalkboard or white board surface is magnetic, a small piece of adhesive magnetic strip may be added to the back of the manipulatives. Magnetic strip is readily available in hobby stores and is relatively inexpensive. If the board surface is not magnetic, masking tape may be used but must be replaced regularly.

This activity instructs the students to carefully cut out the pieces of Template 1 and arrange them by similar valence or oxidation state. They are to then trace over the element’s symbol and oxidation state with colored markers using the chart given. You may want to use colored card stock for your enlarged set of demonstration manipulatives. Alternatively, you may use the colored markers in the same way that the students do. Template 2 is used during the organic section and does not need to be colored.

Give each student a copy of the activity. The background information is essential to their success.

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RTeacher Overview – Chemical Nomenclature

Answer Key

Conclusion Questions

Table 8. Naming Acids

Acid Formula Acid Name

HCl hydrochloric acid

HClO hypochlorous acid

HClO2

chlorous acid

HClO3

chloric acid

HClO4

perchloric acid (or “hyperchloric” acid)

HNO3

nitric acid

HBr hydrobromic acid

H3PO

4phosphoric acid

H3PO

3phosphorous acid

HCN hydrocyanic acid

HC2H

3O

2acetic acid

H2CO

3carbonic acid

HI hydroiodic acid

HF hydrofl uoric acid

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Answer Key (continued)

Tab

le 9

. Nam

ing

Hyd

roca

rbon

Com

pou

nds

CnH

2n+1

OH

(–a

nol)

CH

3OH

met

hano

l

C2H

5OH

etha

nol

C3H

7OH

prop

anol

C4H

9OH

buta

nol

C5H

11O

Hpe

ntan

ol

C6H

13O

Hhe

xano

l

C7H

15O

Hhe

ptan

ol

C8H

17O

Hoc

tano

l

C9H

19O

Hno

nano

l

C10

H21

OH

deca

nol

CnH

2n−

2 (–y

ne)

cann

ot f

orm

C2H

2

ethy

ne

C3H

4

prop

yne

C4H

6

buty

ne

C5H

8

pent

yne

C6H

10

hexy

ne

C7H

12

hept

yne

C8H

14

octy

ne

C9H

16

nony

ne

C10

H18

decy

ne

CnH

2n (

–ene

)

C2H

4

ethe

ne

C3H

6

prop

ene

C4H

8

bute

ne

C5H

10

pent

ene

C6H

12

hexe

ne

C7H

14

hept

ene

C8H

16

octe

ne

C9H

28

none

ne

C10

H20

dece

ne

CnH

2n+

2 (–a

ne)

CH

4

met

hane

C2H

6

etha

ne

C3H

8

prop

ane

C4H

10

buta

ne

C5H

12

pent

ane

C6H

14

hexa

ne

C7H

16

hept

ane

C8H

18

octa

ne

C9H

20

nona

ne

C10

H22

deca

ne

Prefi x

or

Stem

met

h–

eth–

prop

–

but–

pent

–

hex–

hept

–

oct–

non–

dec–

Nu

mbe

r of

C

arbo

n A

tom

s (n

)

1 2 3 4 5 6 7 8 9 10

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Tab

le 1

0. N

amin

g B

inar

y Io

nic

Com

pou

nds

Mn

2+

Mn 3N

2

man

gane

se(I

I)

nitr

ide

MnO

man

gane

se(I

I)

oxid

e

MnB

r 2

man

gane

se(I

I)

brom

ide

MnS

man

gane

se(I

I)

sulfi

de

MnS

O4

man

gane

se(I

I)

sulf

ate

Mn(

ClO

2)2

man

gane

se(I

I)

chlo

rite

Mn 3(

PO3)

2

man

gane

se(I

I)

phos

phite

Al3+

AlN

alum

inum

ni

trid

e

Al 2O

3

alum

inum

ox

ide

AlB

r 3

alum

inum

br

omid

e

Al 2S

3

alum

inum

su

lfi de

Al 2(

SO4)

3

alum

inum

su

lfat

e

Al(C

lO2)

3

alum

inum

ch

lori

te

AlP

O3

alum

inum

ph

osph

ite

NH

4+

(NH

4)3N

amm

oniu

m

nitr

ide

(NH

4)2O

amm

oniu

m

oxid

e

NH

4Br

amm

oniu

mbr

omid

e

(NH

4)2S

amm

oniu

m

sulfi

de

(NH

4)2S

O4

amm

oniu

m

sulf

ate

NH

4ClO

2

amm

oniu

m

chlo

rite

(NH

4)3P

O3

amm

oniu

m

phos

phite

Ba2+

Ba 3N

2

bari

um n

itri

de

BaO

bari

um o

xide

BaB

r 2

bari

um

brom

ide

BaS

bari

um s

ulfi d

e

BaS

O4

bari

um s

ulfa

te

Ba(

ClO

2)2

bari

um c

hlor

ite

Ba 3(

PO3)

2

bari

um

phos

phite

Cu+

Cu 3N

copp

er(I

) ni

trid

e

Cu 2O

copp

er(I

) ox

ide

CuB

rco

pper

(I)

brom

ide

Cu 2S

copp

er(I

) su

lfi de

Cu 2S

O4

copp

er(I

) su

lfat

e

CuC

lO2

copp

er(I

) ch

lori

te

Cu 3P

O3

copp

er(I

) ph

osph

ite

Pb2+

Pb3N

2

lead

(II)

nit

ride

PbO

lead

(II)

oxi

de

PbB

r 2

lead

(II)

br

omid

e

PbS

lead

(II)

sulfi d

e

PbSO

4

lead

(II)

sul

fate

Pb(C

lO2)

2

lead

(II)

chl

orite

Pb3(

PO3)

2

lead

(II)

ph

osph

ite

Ag+

Ag 3N

silv

er n

itri

de

Ag 2O

silv

er o

xide

AgB

rsi

lver

bro

mid

e

Ag 2S

silv

er s

ulfi d

e

Ag 2S

O4

silv

er s

ulfa

te

AgC

lO2

silv

er c

hlor

ite

Ag(

PO3)

3

silv

er p

hosp

hite

N3−

O2−

Br− S2−

SO42−

ClO

2−

PO

33−

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Table 11. Naming Molecular Compounds

Formula Name

[Al(OH)4]− tetrahydroxoaluminate(III) ion

[Ag(NH3)

2]+ diamminesilver(I) ion

[Zn(OH)4]2− tetrahydroxozincate(II) ion

[Zn(NH3)

4]2+ tetramminezinc(II) ion

[Cu(NH3)

4]2+ tetramminecopper(II) ion

[FeSCN]2+ thiocyanatoiron(III) ion*

[FeSCN]Cl2

thiocyanoiron(III) chloride

[Cd(NH3)

4]2+ tetramminecadmium(II) ion

[Ag(CN)2]− dicyanoargentate(I) ion

Mg[Ag(CN)2]

2magnesium dicyanoargentate(I)

[Cu(Cl2Br

2I

2)]4− dibromodichlorodiiodocuprate(II) ion

[Co(NH3)

5Cl]Cl

2pentaamminechlorocobalt(III) chloride

K3[Fe(CN)

6] potassium hexacyanoferrate(III)

[Pt(NH3)

3Br]Cl triamminebromoplatinum(II) chloride

[Cu(Cl2Br

2INH

3)]4− amminedibromodichloroiodocuprate(I) ion

K3[CoF

6] potassium hexafl uorocobaltate(III)

[Co(NH3)

6]Cl

2hexaamminecobalt(II) chloride

[Fe(CN)6]4− hexacyanoferrate(II)

* In reality, it is the nitrogen that is the donor atom so you may see SCN− written as NSC−, which instead makes this formula [FeNSC]2+ and name isothiocyanatoiron(III) ion.



VOCABULARY Ion — an atom or group of atoms that has gained or lost electrons Monatomic ion — an atom that has gained or lost electrons and has a charge Polyatomic ion — a group of covalently bound atoms that has a charge Anion — a negatively charged ion Cation — a positively charged ion Charge — the positive or negative value assigned to an ion as a result of having lost or gained electrons Oxidation number — hypothetical charge a covalently bound atom would have IF its bonds were ionic Acid — a compound that donates a H+ ion during a reaction Ionic compound — a compound made of positively and negatively charged ions Molecular compound — a compound held together by shared pairs of electrons Hydrocarbon — a compound composed of carbon and hydrogen Alcohol — a hydrocarbon that has had one or more of its hydrogens replaced with –OH groups Complex ion — a metal ion that has been surrounded by ligands to form a large polyatomic ion Ligand — a neutral or charged molecule that covalently bonds to a metal ion to form a complex ion Coordination compound — a neutral ionic compound formed between a complex ion and another ion

INTRODUCTION Writing chemical formulas will open your eyes to the chemical world. Once you are able to write correct chemical formulas there are four naming systems you will need to master. The trick lies in recognizing which naming system to use! Use the following guidelines when making your decisions about how to name compounds. If the chemical formula for the compound starts with H, it is an acid. Use the Naming Acids

rules. If the chemical formula for the compound starts with C and contains quite a few H’s and

perhaps some O’s, it is organic. Use the Naming Organic Compounds rules. If the chemical formula for the compound starts with a metal it is most likely ionic. Use the

Naming Binary Ionic Compounds rules. If the chemical formula for the compound starts with a nonmetal other than H or C, use the

Naming Binary Molecular Compounds rules. It is essential that you memorize at least 9 common polyatomic ions. Polyatomic ions are groups of atoms that behave as a unit and possess an overall charge. If more than one copy of a polyatomic ion is needed to create a chemical formula, the ion must be enclosed in parentheses before adding the subscripts. You need to know their names, formulas and charges. If you learn the nine that follow, you can determine the formula and charges for many others from applying two simple patterns.



Name of Polyatomic Ion: Formula & Charge: Ammonium ion NH4

+

Acetate ion C2H3O2

− Cyanide ion CN−

Hydroxide ion OH− Nitrate ion NO3

− Chlorate ion ClO3

−

Sulfate ion SO4

2− Carbonate ion CO3

2−

Phosphate ion PO43−

Pattern 1: The -ates “ate” one more oxygen than the -ites however, their charge does not change as a result. For instance, if you know nitrate is NO3

−, then nitrite must be NO2−. If you know

phosphate is PO43−, then phosphite must be PO3

3−. You can also use the prefixes hypo- and per- with the chlorate series. Perchlorate, ClO4

−, was really “hyper and -ate yet another oxygen” when compared to chlorate, ClO3

−. Hypochlorite is a double whammy. It is -ite and therefore “ate” one less oxygen than chlorate and it is hypo- which means “below” so it “ate” even one less oxygen than plain chlorite so its formula must be ClO−. You can substitute the other halogens for chlorine and make similar sets of this series. Pattern 2: The -ates with charges less than negative one, meaning ions with charges of −2, −3, etc., can have an H added to them to form new polyatomic ions. For each H added the charge is increased by a +1. For instance, CO3

2− can have an H added and become HCO3−. HCO3

− is called either the bicarbonate ion or the hydrogen carbonate ion. Since phosphate is negative three, you can add one or two hydrogens to make new polyatomic ions, HPO4

2− and H2PO4−. The names are

hydrogen phosphate and dihydrogen phosphate, respectively. If you continue adding hydrogen ions until you reach neutral, you’ve made an acid! That means you need to see the Naming Acids rules.



Pattern 3: Use of the following periodic table will also come in handy. Notice the simple patterns for determining the most common oxidation states of the elements based on their family’s position on the periodic table. Notice the IA family is +1 while the IIA family is +2. Skip across to the IIIA family, and notice that aluminum is +3. Working backwards from the halogens, or VIIA family, they are most commonly −1 while the VIA family is −2 and the VA family is −3. The IV A family is “wishy-washy,” and can be several oxidation states, the most common being 4.

NAMING ACIDS How do I know it is an acid? The compound’s formula begins with a hydrogen, H, and water doesn’t count. Naming acids is extremely easy, if you know your polyatomic ions. There are three rules to follow: H + element: If the acid has only one element following the H, then use the prefix hydro-

followed by the element’s root name and an -ic ending. HCl is hydrochloric acid. H2S is hydrosulfuric acid. When you see an acid name beginning with “hydro”, think “Caution, element approaching!” (HCN is an exception since it is a polyatomic ion without oxygen, and it is named hydrocyanic acid.)

H + -ate polyatomic ion: If the acid has an “-ate” polyatomic ion after the H, then it makes an “-ic” acid. H2SO4 is sulfuric acid.

H + -ite polyatomic ion: If the acid has an “-ite” polyatomic ion after the H, then it makes an “-ous” acid. H2SO3 is sulfurous acid.

When writing formulas for acids you must have enough H+ added to the anion to make the compound neutral. Also note that -ate and -ite polyatomic ions contain oxygen so, their acids are often referred to as oxyacids.



NAMING ORGANIC COMPOUNDS How do I know it is organic? The chemical formula will start with a C followed by hydrogens and may even contain some oxygen. Most of the organic carbons you will encounter will be either hydrocarbons or alcohols. These are the simplest of all to name. Memorize the list of prefixes in Table B found in the conclusion questions. The prefixes correspond to the number of carbons present in the compound and will be the stem for each organic compound. Notice that the prefixes are standard geometric prefixes once you pass the first four carbons. This silly statement will help you remember the order of the first four prefixes: “Me Eat Peanut Butter.” This corresponds to meth-, eth-, prop-, and but- which correspond to 1, 2, 3, and 4 carbons, respectively. Now that we have a stem, we need an ending. There are three common hydrocarbon endings that you will need to know as well as the ending for alcohols. The ending changes depending on the structure of the molecule. -ane - alkane (all single bonds & saturated) CnH2n+2; The alkanes are referred to as saturated

hydrocarbons because they contain only single bonds and thus, the maximum number of hydrogen atoms.

-ene = alkene (contains one double bond & unsaturated) CnH2n; The alkenes are referred to as unsaturated hydrocarbons because a pair of hydrogens have been removed to create the double bond.

-yne ≡ alkyne (contains one triple bond & unsaturated) CnH2n−2; The alkynes are also referred to as unsaturated, because two pairs of hydrogens have been removed to create the triple bond. The term polyunsaturated means that the compound contains more than one double or triple bond.

-ol – alcohol (one H is replaced with a hydroxyl group, -OH group, to form an alcohol) CnH2n+1OH; Do not be fooled—this looks like a hydroxide ion, but is not! It does not make this hydrocarbon an alkaline or basic compound. Do not name these as a hydroxide! C2H6 is ethane while C2H5OH is ethanol.

NAMING BINARY IONIC COMPOUNDS How do I know it is ionic? The chemical formula will begin with a metal cation (+ ion) or the ammonium cation. The ending is often a polyatomic anion. If only two elements are present, they are usually from opposite sides of the periodic table, like KCl. If the metal can have more than one oxidation state, be prepared to use a Roman numeral indicating which oxidation state the metal is exhibiting. Group IA alkali metals, Group IIA alkaline earth metals, aluminum (Al), silver (Ag), cadmium (Cd) and zinc (Zn) are exceptions to the Roman numeral rule because their charges are constant. Group IA metals are always +1, Group IIA metals are always +2, Al is always +3, Ag is always +1, and Cd and Zn are always +2 in chemical compounds. In order to name these compounds, first name the ions.



Naming positive ions: Metals commonly form cations. Monatomic positive ions in Group A are named by simply writing the name of the metal from

which it is derived. Al3+ is the aluminum ion. Metals often form more than one type of positive ion so Roman numerals (in parentheses)

follow the ion’s name. Cu2+ is the copper(II) ion. Remember the exceptions — IA, IIA, Al, Ag, Cd, Zn.

NH4+ is the ammonium ion. It is the only positive polyatomic ion that you will encounter.

Naming negative ions: Nonmetals commonly form anions (− ions). Most of the polyatomic ions are also negatively-charged. Monatomic negative ions are named by adding the suffix -ide to the stem of the nonmetal’s

name. Group VIIA, the Halogens are called the halides. Cl− is the chloride ion. Polyatomic anions are given the names of the polyatomic ion. You must memorize these as

instructed. NO2− is the nitrite ion.

Naming the Compound: The + ion (cation) name is given first followed by the name of the negative ion (anion). Remember, to include the Roman numeral that indicates a metal’s charge for the many metals that have more than one oxidation state. No prefixes are used in naming ionic compounds.

NAMING BINARY MOLECULAR COMPOUNDS How will I know it is a molecular compound? The chemical formula will contain a combination of nonmetals, both lying near each other on the periodic table. No polyatomic ions will be present. Use the following set of prefixes when naming molecular compounds.

Subscript Prefix 1 Mono-

[usually used only on the second element; such as carbon monoxide or nitrogen monoxide]

2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

Naming the Compound: The name of the element with the positive oxidation state is given first, followed by the name of the element with the negative oxidation state. Use prefixes to indicate the number of atoms of each element. Don’t forget the -ide ending. If the second element’s name begins with a vowel, then the “a” at the end of the prefix is usually dropped. N2O5 is dinitrogen pentoxide not dinitrogen pentaoxide. PCl5 is phosphorous pentachloride not phosphorous pentchloride.



FORMULA WRITING Naming is the trickiest part! Once you have been given the name, the formula writing is easy as long as you have memorized the formulas and charges of the polyatomic ions. The prefixes of a molecular compound make it really easy to write the formula since the prefix tells you how many atoms are present for each element. Roman numerals are your friend; they tell you the charge of the metal ions that can have more than one oxidation state and thus form positive ions with different charges. Remember that Group IA, Group IIA, Al, Ag, Cd, & Zn are usually not written with a Roman numeral; you must know their charges. The most important thing to remember is that, the sum of the charges must add up to zero in order to form a neutral compound. The crisscross method is very useful—the charge on one ion becomes the subscript on the other. If you use this method, you must always check to see that the subscripts are in their lowest whole number ratio! Here are some examples: potassium oxide K1+ O2− K1 O2 K2O

iron(III) chlorate Fe3+ ClO31− Fe3 ClO3

1 Fe(ClO3)3

tin(IV) sulfite Sn4+ SO3

2− Sn4 SO32 Sn2(SO3)4 Sn(SO3)2

zinc acetate Zn2+ C2H3O2

1− Zn 2 C2H3O21 Zn(C2H3O2)2

COORDINATION CHEMISTRY NOMENCLATURE These are actually quite fun! The rules are simple and you will really feel like you are speaking chemistry. Square brackets are used to enclose a complex ion or neutral coordination species. A complex ion is composed of a single central atom or ion with other atoms or molecules attached. The atoms or molecules attached are known as ligands. The number of ligands attached is called the coordination number of the complex ion. The naming of complex cations and complex anions is similar, except that anions are always made to end in -ate. Coordination compounds, like other ionic compounds, are named with the cation preceding the anion regardless of which (if either) one of them is a complex ion.

The rules for naming complex ions or compounds are as follows: As with any ionic compound, the cation is named before the anion. In naming a complex ion, the ligands are named before the central metal ion. In naming ligands, an “-o” is added to the root name of any anion. For example, the halides as

ligands are called fluoro, chloro, bromo, and iodo; hydroxide is hydroxo; cyanide is cyano; nitrite is nitrito, etc. If the ligands are neutral, omit the “-o” ending. Neutral ligands take the name they normally use as neutral molecules. There are four exceptions which must be memorized: H2O as a ligand is known as aqua, NH3 is named ammine [note the “mm” in the spelling so it is not confused with the functional group –NH2, an amine group], CO is named carbonyl, and NO is nitrosyl.

The number of each kind of ligand is specified by the usual Greek prefix: mono-, di-, tri-, tetra-, penta-, and hexa-.

The oxidation number of the central metal atom is designated by a Roman numeral in parentheses.



When more than one type of ligand is present, they are named in alphabetical order with no regard for the Greek (numerical) prefix.

If the complex has a negative charge, the suffix -ate is added to the name of the metal. When a Latin symbol is used for the element, the element takes the Latin name in complex anions but not in complex cations. For example, [Cu(NH3)4]

2+ is called the tetraamminecopper(II) ion but [Cu(CN)6]

4− is called the hexacyanocuprate(II) ion. Likewise [Al(NH3)6]3+ is called

the hexaamminealuminum(III) ion but [Al(OH)4]− is called the tetrahydroxoaluminate(III) ion.

Common Neutral Ligands

Formula Name H2O aqua NH3 ammine CO carbonyl NO nitrosyl

Common Anion Ligands Formula Name

F− fluoro Cl− chloro Br− bromo I− iodo

OH− hydroxo CN− cyano

SCN− thiocyano S2O3

2− thiosulfato C2O4

2− oxalato Latin Names Used for Some Metal Ions in Anionic Complex Ions

iron ferrate copper cuprate

lead plumbate silver argentate gold aurate tin stannate



PURPOSE To master the skill of writing and naming chemical formulas.

MATERIALS

Each lab group will need the following: bag, zipper-lock, quart copy of student formula manipulatives scissors

PROCEDURE

1. Carefully cut out the models on Template 1. Group them by similar charge or oxidation state.

2. Trace over the symbol and oxidation state of each element using colored markers and apply the color scheme below:

3. Notice how the models fit together. If an element has a +3 oxidation state, it requires three elements with a −1 oxidation state to create a complete compound and the subscripts would reflect a 1:3 ratio.

4. Review the rules for naming acids and complete Table A on your student answer page. Use the models you created from Template 1 as needed. Supply either the acid’s name or its formula to complete Table A.

5. Review the rules for naming binary ionic and molecular compounds. Use the models you created from Template 1 as needed. Supply the compound’s formula and name to complete Table C. If the charge or oxidation state is missing from the table, it is because you should already know them or be able to determine them due to their position in the periodic table.

6. Carefully cut out the shapes on Template 2. Each carbon model has 4 inward notches. The model “bonds” found on Template 2 are for connecting the carbons. These shapes will be used to help you with organic compounds. There is no need to color them.

7. Review the rules for naming organic hydrocarbons and alcohols. Use your models from Template 2 as needed. Fill in the missing formulas and names for each compound in Table B.

Safety Alert Use care when handling scissors.

Color Oxidation StateBlue +1 Red −1

Yellow +2 Green −2 Purple +3 Pink −3




All You Really Need to Know About Chemical Names and Formulas SUMMARIZED In this flowchart, D and J in the general formula DxJy can represent atoms, monatomic ions, or polyatomic ions.

D = Group IA, IIA, _Al, Cd, Ag, or Zn?

D = Group IA, IIA, _ Al, Cd, Ag, or Zn?

DxJy

Yes

No

Compound is an acid;use the table below

Compound MUSTcontain a polyatomicicon its name ends in-ite or -ate

Name the ions; usea Roman numeral toindicate the chargeon the cation

Name the ions

Compound is binarymolecular; useprefixes in the name

Name the ions; usea Roman numeral toindicate the charge on the cation

Name the ions

Compound isbinary its name

ends in -ide

No

NoYes

No Yes

Yes

No

Yes

D = metal

More thanTWO elements?

D = H

NamingAcids

Anion ending Example Acid name Example

hydrosulfuric acid

sulfurousacid

sulfuric acid

(stem)-icacid

(stem)-ousacid

Hydro-(stem)-icacid

–ate

–ite

–ide

SO32-

sulfite

S2-

sulfide

SO42-

sulfate



CONCLUSION QUESTIONS

Table A

Acid Formula Acid Name

HCl

hypochlorous acid

chlorous acid

chloric acid

perchloric acid (“hyperchloric” acid)

HNO3

hydrobromic acid

H3PO4

H3PO3

hydrocyanic acid

HC2H3O2

carbonic acid

hydroiodic acid

HF



Table B

# of carbon atoms = n prefix or stem -ane

CnH2n+2

-ene

CnH2n

-yne

CnH2n−2

-anol

CnH2n+1OH

1 meth-

None here because you must have at least 2 carbons for multiple

bonding

CH3OH

methanol

2 eth-

3 prop- C3H6

propene

4 but-

5 pent- C5H12

pentane

6 hex-

7 hept- C7H15OH

heptanol

8 oct- C8H14

octyne

9 non-

10 dec-



Table C

Ag+ Pb2+ Cu+ Ba2+ NH4+ Al3+ Mn2+

N3−

O2−

Br−

S2−

SO42−

ClO2−

PO33−



Table D

Formula Name

tetrahydroxoaluminate(III) ion

[Ag(NH3)2]+

tetrahydroxozincate(II) ion

[Zn(NH3)4]2+

tetramminecopper(II) ion

[FeSCN]2+

[FeSCN]Cl2

tetramminecadmium(II) ion

[Ag(CN)2]−

Mg[Ag(CN)2]2

dibromodichlorodiiodocuprate(II) ion

[Co(NH3)5Cl]Cl2

potassium hexacyanoferrate(III)

triamminebromoplatinum(II) chloride

[Cu(Cl2Br2INH3)]4−

K3[CoF6]

[Co(NH3)6]Cl2

hexacyanoferrate(II)



Al3+

NH4+

Mn2+

H+

H+H+

H+

H+H+

Ag+Cl-

NO3-

Br-

Pb2+

Cu+

Ba2+

N3-

O2-

S2-

SO42-

H+

H+

H+

H+H+

Template 1



ClO-

C2H3O2-

PO33-

S2-

CO32-

ClO2-

ClO3-

ClO4-

F-

I-

CN-

PO43-



Template 2

CCC C

C

C

C

C

C

C

CC HHH

HH

HH

H

HHH

H

H

HH

HH

HH

H

HHH

H

OH

OH

OH

Use the models below as single, double and triple

bonds for connecting carbons.

Remember, DO NOT allow C to have more

than FOUR total bonds!


C Chemical Nomenclature right · Objectives Students will: Learn to apply the rules of chemical...

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