crhs academic chemistry unit 6 - nomenclature … 6... · unit 6 - nomenclature notes &...

Name ____________________ Period ____

CRHS Academic Chemistry

Unit 6 - Nomenclature

Notes & Practice Problems

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____ 6.1 _____ _____

____ 6.2 _____ _____

____ 6.3 _____ _____

____ 6.4 _____ _____

____ Warm Up _____

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of 24 Unit 6 Notes

WARM-UPS

#1 #6

#2 #7

#3 #8

#4 #9

#5 #10

Unit 6 Notes of 24

of 24 Unit 6 Notes

6.1 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - GROUP 1-3 METALS

1. Chemical nomenclature is a set of ____________________ used to generate systematic _______________

for chemical compounds.

2. Fill in the missing information in each of the cells of the table.

Element Group Number? Metal or

Nonmetal?

Group Name? Oxidation

Number?

Gain or Lose

Electrons?

How Many

Electrons Gained

or Lost?

Rb 1 Metal Alkali Metal +1 Lose 1

Al

O

I

Sr

Be

S

N

Br

F

Ne

Xe

Ra

P

Ar

Na

Ca

Ba

Unit 6 Notes of 24

Name the Ionic compound

1. SrCl2

2. MgI2

3. Li2O

4. CaBr2

5. MgS

6. Al2O3

7. BCl3

8. CaO

9. Al2S3

Fill in the table

Chemical Name Elements Charge of Ions Formula

Barium nitride Ba & N Ba+2 N–3 Ba3N2

Magnesium sulfide

Aluminum oxide

Sodium iodide

Lithium sulfide

Radium chloride

Calcium oxide

Potassium nitride

of 24 Unit 6 Notes

HW 6.2 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - POLYATOMIC IONS Indicate the type of compound then name the compound! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)

1. Na2SO4

2. Ca3(PO4)2

3. KMnO4

4. K2S

5. NaI

6. Rb2N3

7. K2CO3

8. Cs2SO4

9. Ba(NO3)2

10. LiC2H3O2

11. Ca3P2

12. Li2CrO4

13. KCN

Unit 6 Notes of 24

Indicate the type of compound then write the formula! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)

1. potassium permanganate

2. calcium hydroxide

3. sodium fluoride

4. sodium perchlorate

5. ammonium hydroxide

6. calcium carbonate

7. lithium nitride

8. calcium chlorate

9. barium sulfide

10. ammonium sulfate

11. sodium sulfite

12. ammonium chromate

13. potassium chromate

of 24 Unit 6 Notes

HW 6.3 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS – TRANSITION METALS Indicate the type of compound then name the compound! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)

1. NiF2

2. Cu2O

3. FeI2

4. CuBr2

5. FeSO4

6. SnS2

7. Na2S

8. CrSe

9. MgBr2

10. MnO

11. Mn2Se3

12. Na2SO3

13. AuI

14. PbO

15. KC2H3O2

16. CoCl3

Unit 6 Notes of 24

17. Fill in the table

Indicate the type of compound then write the formula! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)

18. copper (II) fluoride

19. sulfurous acid

20. dinitrogen pentoxide

21. barium chloride

22. hydronitric acid

23. lithium perchlorate

24. phosphorus trihydride

25. chromium (III) oxide

26. sodium peroxide

Compound Name Ions Formed Formula

iron (III) chloride Fe+3 & Cl–1 FeCl3

tin (IV) fluoride

chromium (III) oxide

manganese (II) sulfide

copper (II) nitride

lead (II) oxide

lead (IV) oxide

titanium (III) chloride

tin (II) sulfide

iron (III) selenide

of 24 Unit 6 Notes

HW 6.4 NAMING AND WRITING FORMULAS OF COVALENT COMPOUNDS Fill in the table of numerical prefixes

=1 =2 =3 =4 =5

=6 =7 =8 =9 =10

Name the following covalent compounds using the appropriate prefixes.

1. SO2

2. S3F7

3. N2O5

4. SiCl4

5. AsH3

6. H2O

7. SO3

Write the formula of the given covalent compound.

8. nitrogen triiodide

9. silicon tetrafluoride

10. arsenic pentafluoride

11. xenon hexafluoride

12. triiodine nonafluoride

13. sulfur trioxide

14. diiodine pentoxide

15. dinitrogen tetroxide

Unit 6 Notes of 24

Indicate the type of compound then write the name Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT) or Covalent (C)

1. Li2O

2. N2O5

3. HBr

4. Co2SO3

5. Ba(NO2)2

6. HClO4

7. H2C2O7

8. NiO2

Indicate the type of compound then write the formula Ionic (I) or Polyatomic Ion(P) or Ionic Transition Metal Polyatomic (IPT) or Covalent (C)

9. trinitrogen pentasulfide

10. hydrochloric acid

11. zirconium(III)bromide

12. strontium chromate

13. cesium nitride

14. chloric acid

15. nitrous acid

of 24 Unit 6 Notes

6.1 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - GROUP 1-3 METAL

CATIONS There are millions of known chemical substances. Without a universal, international system, naming them reliably would

be impossible. The system used in naming substances is called chemical nomenclature.

Chemical nomenclature is a set of rules used to generate systematic names for chemical compounds.

The governing body responsible for chemical nomenclature is the International Union of Pure and Applied Chemistry

(IUPAC). There are two major divisions to the IUPAC system:

1. Organic nomenclature – contain carbon, usually bonded with hydrogen, oxygen, nitrogen, and sulfur. Organic

chemistry and naming organic compounds is a topic for a college chemistry course.

2. Inorganic nomenclature – everything else is inorganic and is divided into three categories…

Covalent (a.k.a. molecular) compounds

Ionic compounds

Acids

This unit covers inorganic nomenclature for covalent compounds and ionic compounds. Nomenclature of acids

will be done in the acid and base unit.

Review Practice: Fill in the missing information

Group Number Group Name Oxidation Number Gain or Lose

Electrons

How Many Electrons

Gained or Lost?

Anion or Cation

1 Alkalai Metals +1 lose 1 Cation

2 Alkali Earth Metals +2 lose 2 Cation

13 ---- +3 lose 3 Cation

14 ---- +4,-4 Lose/Gain 4 -----

15 ---- -3 gain 3 Anion

16 ---- -2 gain 2 Anion

17 Halogens -1 gain 1 Anion

18 Noble Gases 0 Neither gain nor

lose electrons

0 -----

3-12 Transition Metals +1, +2, +3, +4 Gain 1, 2, 3, 4 Cation

Unit 6 Notes of 24

___Ionic_____________ compounds are made of a _____metal_______________ cation (+) and a

_______nonmetal____________ anion (–).

First element is from the __left____ of the zig-zag line (METAL)

Second element is from the RIGHT of the zig-zag line (NONMETAL).

The ___metal_______ is always written first.

The Ionic Naming Rules

1) Confirm the compound is ionic

2) The number of atoms _does_not__matter___ and there are __No___ PREFIXES.

3) Name the ___cation____________ (metal).

4) Name the ___anion____________ (nonmetal), using the root of the element and changing the ending to

___-ide____.

Examples:

NaBr sodium bromide

Practice:

K3N potassium nitride

Ca3P2 calcium phosphide

SrO strontium oxide

LiCl lithium chloride

STEPS to Writing Formulas

1. Identify the first term. This will be a __metal___ cation (+) and written exactly as it is on the periodic table.

2. The second term is a _____nonmetal_______ anion (–) and its ending has been changed to “___ide______”.

Determine the element name from the root of the word.

3. Write the cation and anion by finding their __charges_____.

4. Use the ___criss-cross_____ method.

of 24 Unit 6 Notes 5. __Reduce______ subscripts to lowest whole numbers.

Example:

Barium Iodide: Ba I → Ba+2 I–1 → Ba1I2 → BaI2

Practice

magnesium fluoride MgF2

aluminum iodide AlI3

calcium sulfide CaS

lithium oxide Li2O

beryllium phosphide Be3P2

francium sulfide Fr2S

Unit 6 Notes of 24

of 24 Unit 6 Notes

6.2 NAMING AND WRITING FORMULAS OF IONICS COMPOUNDS – POLYATOMIC IONS

Ionic compounds also form with groups of nonmetals acting as a cation or anion called Polyatomic Ions. (ex. NO3 –1,

nitrate)

Naming Rules for Ionic Compounds with Polyatomic Ions

1) __Never___ change the name of a polyatomic ion (PI)

2) This is ionic bonding, so NO PREFIXES.

3) If the PI comes _first_, name it, then name the anion by changing the ending to “ide”. (Ex. NH4Cl - ammonium

chloride)

4) If the PI comes ___last___, name the cation and then the PI. No changes necessary. (Ex. Na2SO4 – sodium

sulfate)

5) All but one PI are ANIONS (–). Ammonium, NH4+ is a cation.

Examples:

Mg(MnO4)2 magnesium permanganate

NH4Br ammonium bromide

Mixed Practice –indicate I (nonmetal anion) or IP (polyatomic ion). Name it.

1) NaNO3 IP sodium nitrate

2) BaCl2 I barium chloride

3) NH4ClO4 IP ammonium perchlorate

4) LiCl I lithium chloride

The most common PI’s list is found at the back of your packet. You will always be given this list, but you need to know how

to use it!

Unit 6 Notes of 24

Steps to Writing Formulas of Ionic Compounds with Polyatomic Ions

STEPS

1. Identify the cation (+), and the anion (–)

a. the cation, anion, or BOTH may be polyatomic ions.

2. Write the cation and anion by finding their ___charges_____

a. Place parentheses around the PI to remind you to ___NEVER CHANGE___________ a polyatomic ion!

3. Use the ____criss-cross_________ method.

4. ___Reduce______ subscripts to lowest whole numbers.

Examples:

Ammonium Bromide: NH4 Br → (NH4)+1 Br–1 → (NH4)1Br1 → NH4Br

Magnesium Nitrate: Mg NO3 → Mg+2 (NO3)–1 → Mg1(NO3)2 → Mg(NO3)2

Mixed Practice: Write I, IP(polyatomic). Write the formula.

sodium cyanide IP NaCN

radium fluoride I RaF2

barium oxide I BaO

aluminum nitrite IP AlNO2

calcium sulfite IP CaSO3

aluminum dichromate IP Al2(Cr2O7)3

ammonium silicate IP (NH4)2SiO3

of 24 Unit 6 Notes

6.3 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - TRANSITION METAL

CATIONS

Periodic table __transition_______________________ metals (and nearby poor metals) also form ionic compounds with

nonmetals and PI’s.

Transition metals are __metals_________, which means they can exhibit __>1_____ oxidation state, or charge:

ex. Fe+2, Fe+3.

They are named according to their cation charge using the __Stock___________ system.

The Stock System is a Roman numeral used to indicate the charge of a multivalent ion.

Roman Numerals 1 through 6

1 = I 2=II 3=III 4=IV 5=V 6=VI

Naming Rules for Ionic Compounds with Transition Metals

1) From the chemical formula, find the charge of the _anion____.

2) _Multiply________ the anion charge by its subscript to calculate the overall negative charge of the compound.

3) The cation(s) __equals_____ this charge to make the compound’s net charge equal zero (neutral).

4) Divide the overall positive charge by the subscript on the cation to find the charge on each metal cation.

5) Write the Roman numeral of the numerical charge in parentheses _after____________ the transition metal name.

6) Normal __ionic___ naming rules apply.

7) Example Fe2O3

Fe2O3 Fe2O3

Fe2O3

Iron (III) Oxide Examples:

CuO copper(II)oxide

FeS iron(II)sulfide

TiCl4 titanium (IV) Chloride

Ni(OH)3 nickel (III) hydroxide

+6 by 2 (atoms of Fe) = each Fe has a +3 charge, so…

–2

–6

–2

–6 +6

The 3 oxygens have a total –6 charge

–2 +3

+6 –6

Unit 6 Notes of 24

Mixed Practice – indicate I, or IP, or IT (transition metal) or IPT (polyatomic & transition metal). Name it.

1) VCl3 IT vanadium (III) choride

2) BaSO3 IP barium sulfite

3) FeBr2 IT iron (II) bromide

4) CuSO4 IPT copper (II) sulfate

5) NaI I sodium iodide

Steps to Writing Formulas for Ionic Compounds with Transition metals

1) Identify the transition metal and the anion.

2) Form the cation and anion by finding their _charge_______

a. cation charge is the ____Roman Numeral________________________

__________________________________________

3) Use the ___criss-cross_________________________ method to form the compound.

___Reduce__________________ subscripts to lowest whole numbers

Example:

Manganese(IV) oxide: Mn O → Mn+4 O–2 → Mn2O4 → MnO2

Mixed Practice: indicate I, or IP, or IT (transition metal) or IPT (polyatomic & transition metal). Write the formula.

tin (IV) iodide IT SnI4

mercury (II) sulfide IT HgS

lithium chloride I LiCl

iron (III) oxide IT Fe2O3

manganese (II) chloride IT MnCl2

chromium (VI) phosphate IPT Cr3(PO4)4

copper (III) permanganate IPT Cu(KMnO4)3

of 24 Unit 6 Notes Extra Mixed Practice: indicate I, or IP, or IT (transition metal) or IPT (polyatomic & transition metal). Write the formula.

barium fluoride I BaF

aluminum phosphate IP Al2(PO4)3

sodium acetate IP NaOC2H3O2

lead (II) oxide IT PbO

sodium hydroxide IP NaOH

calcium bromide I Ca(OH)2

potassium dichromate IP K2Cr2O7

manganese (III) oxide IT Mn2O3

sodium nitride I Na3N

tin (II) oxide IT SnO

Unit 6 Notes of 24

6.4 NAMING AND WRITING FORMULAS OF COVALENT COMPOUND

Binary ___covalent_________ compounds are made of TWO___nonmetals_______(Ex. P2O5) bound together. Nonmetals

are ___right____ of the zig-zag line (except _hydrogen___).

Covalent Compound Naming Rules

1) Confirm the compound is __covalent________.

2) Check the number of atoms of each element by the ___subscript___. If there is no subscript, there is one atom.

Ex. P2O5 – __2__ phosphorus, _5___oxygen

3) Name the _first_____ element using the prefix (page bottom) with the element name. (Ex. P2O5 –

diphosphorus…)

NEVER use “_mono___” on the first element.

4) Name the ___second________ element. Choose the prefix, write the root of the element, and change the

ending to “___ide_________”. (Ex. P2O5 – diphosphorus pentoxide…)

Practice:

1) SF6 sulfur hexaflouride

2) CS carbon monosulfide

3) S3N2 trisulfur dinitride

STEPS for Writing Formulas for Covalent Compounds

STEPS

1. Check the elements in the compound. Confirm they are both ____nonmetals___________________________.

2. Use the ______prefixes________________________ to determine how many _______________ of each

element are in the compound.

3. Use _____subscripts_____________________ to indicate how many atoms of each element are in the formula

4. Example: carbon dioxide has __1__ carbon(s) and __2_ oxygen(s) = C1O2 = CO2 (1 subscripts are understood)

Mono = 1 Di = 2 Tri = 3 Tetra = 4 Penta = 5

Hexa = 6 Hepta = 7 Octa = 8 Nona = 9 Deca = 10

of 24 Unit 6 Notes 5. Example: nitrogen trifluoride NF3

Practice:

1) selenium tetrafluoride SeF4

2) octaphosphorus pentabromide P8Br5

3) heptanitrogen hexachloride N7Cl6

Mixed Practice

Formula Name Type of Compound

P2O5 diphosphorus pentaoxide C

KClO2 potassium chlorite IP

CrCl2 chromium (II) chloride IT

Ba(OH)2 barium hydroxide IP

(NH4)2Se ammonium selenide IP

CCl4 carbon tetrachloride C

PbI2 lead (II) iodide IT

CaSO3 Calcium sulfite IP

CaSO4 calcium sulfate IP

Ra3(PO4)2 radium phosphate IP

Na3N sodium nitride I

Li2O lithium oxide I

(NH4)2S ammonium sulfide IP

Fe2O3 iron (III) oxide IT

Mg3P2 magnesium phosphide I

KCl potassium chloride I

BaSO4 barium sulfate IP

PI5 phosphorous pentiodide C

SO2 sulfur dioxide C

NO nitrogen monoxide C

Unit 6 Notes of 24

Prefixes for Covalent Compounds

Mono = 1 Di = 2 Tri = 3 Tetra = 4 Penta = 5

Hexa = 6 Hepta = 7 Octa = 8 Nona = 9 Deca = 10

Common Polyatomic Ions List

Name Ion Name Ion

acetate C2H3O2– or CH3COO– hypochlorite ClO–

ammonium NH4+ nitrate NO3

–

carbonate CO32– nitrite NO2

–

chlorate ClO3– perchlorate ClO4

–

chlorite ClO2– permanganate MnO4

–

chromate CrO42– phosphate PO4

3–

cyanide CN– phosphite PO33–

dichromate Cr2O72– silicate SiO3

2–

hydrogen carbonate HCO3– sulfate SO4

2–

hydroxide OH– sulfite SO32–

Roman Numerals for Transition Metals 1-6

1 = I 2 = II 3 = III 4 = IV 5 = V 6 = VI

20 Common Polyatomic Ions

of 24 Unit 6 Notes

crhs academic chemistry unit 6 - nomenclature … 6... · unit 6 - nomenclature notes &...

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