Chemistry HP Unit 4 Chemical Nomenclature and Chemical ...4... · Acids are compounds which most often begin with _____, such as H 2 SO4 (sulfuric acid) and HCl (hydrochloric acid),

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Chemistry HP Unit 4 – Chemical Nomenclature and Chemical Reactions

Learning Targets (Your exam at the end of Unit 4 will assess the following:)

4. Nomenclature and Chemical Reactions

4-1. Name and write formulas for ionic compounds including compounds with multivalent ions (using roman numerals) and

those with polyatomic ions.

4-2. Name and write formulas for covalent compounds (using prefixes).

4-3. Name and write formulas for acids.

4-4. Given any compound, classify as ionic, acid, or covalent and determine the appropriate name.

4-5. Identify diatomic elements and give each with the correct name and formula.

4-6. Identify the reactants and products in a chemical equation.

4-7. State the Law of Conservation of Mass.

4-8. Balance chemical equations beginning with either chemical names or formulas.

4-9. Classify reactions as synthesis, decomposition, single replacement, double replacement, neutralization, or combustion.

4-10. Predict the products of a reaction given the formulas or names of reactants.

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4-1. Name and write formulas for ionic compounds including compounds with multivalent ions (using roman numerals) and those

with polyatomic ions.

Naming Compounds

Ionic compounds, covalent compounds and acids all have different naming conventions, so, in order to name chemical compounds,

you first need to determine whether your compound is ionic, covalent or an acid.

Ionic compounds are compounds consisting of __________________ __________________, a __________________ cation and a

__________________ anion, or a __________________ cation or anion.

Covalent compounds are compounds consisting of __________________ __________________.

Acids are compounds which most often begin with __________________, such as H2SO4 (sulfuric acid) and HCl (hydrochloric acid),

though not all compounds which begin with hydrogen are acids.

Naming Ionic Compounds

Ionic compounds are compounds consisting of either a __________________ and a __________________, or a polyatomic ion and

another ion. We will consider three different cases.

Case 1: Single valent metals and nonmetals.

Single valent metals are metals that only form __________________ type of cation. All alkali metals and alkaline earth metals are

single valent. All alkali metals form __________________ ions and all alkaline earth metals form __________________ ions.

__________________ and __________________ __________________usually form multiple types of ions, so we refer to them as

__________________. Though, some transition metals are also single valent and you need to memorize them:

__________________, __________________and __________________.

To name an ionic compound made of a single valent metal and a nonmetal, name the _________________ first, followed by the

_________________, changing the ending of the anion to _________________.

For example:

NaCl is called _________________ _________________

CaBr2 is called _________________ _________________

Al2O3 is called _________________ _________________

Notice that you DO _________________ indicate _________________ _________________of each ion you have. CaBr2 is NOT

called calcium dibromide, just calcium bromide.

Let’s practice.

Name the following ionic compounds:

AgBr ________________________________

CdO ________________________________

Na2S ________________________________

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Case 2: Multi-valent metals and nonmetals.

All transition and inner transition metals are _________________, meaning they form _________________ _________________

_________________cation, with the exception of _________________, _________________ and _________________. Further,

there are 4 representative metals that have multi-valences. These are: Sn2+/Sn4+, Pb2+/Pb4+, Sb3+/Sb5+, Po2+/Po4+.

Since these metals form different cations, you MUST include the _________________ of the cation in the compound’s

_________________. You do so by writing the charge of the cation as a _________________ _________________in

_________________ following its name.

For example:

NiS is called _________________ _________________

CuCl is called _________________ _________________

CuCl2 is called _________________ _________________

But, how do you know its charge?

You know its charge because all ionic compounds are _________________ and you know the charge of the anion.

For example:

In NiS, you may not know what nickel’s charge is, but you know that sulfur forms the sulfide ion, _________________-. Since the

total charge of the compound must equal _________________, nickel must have the charge _________________, Ni2+.

In CuCl, you know that chlorine forms the chloride ion, _________________. Since the total charge of the compound must equal

_________________, copper must have the charge _________________, Cu+.

In CuCl2, since chlorine forms the chloride ion, Cl-, and this compound contains 2 chloride ions, totaling a _________________

charge, copper must have the charge _________________, Cu2+.

Let’s practice.

Name the following ionic compounds:

CrCl3 ________________________________

Pb3N2 ________________________________

SnO2 ________________________________

Case 3: Ionic compounds containing Polyatomic Ions.

A polyatomic ion is a group of _____________ ___________ ___________ ___________– ___________-- acting together as

___________ ___________ ___________. Polyatomic cations form ionic compounds when combined with non-metallic anions, and

polyatomic anions form ionic compounds with metallic cations.

When naming an ionic compound containing a polyatomic ion, the name of the polyatomic ion remains _________________.

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CaCO3 consists of the Ca2+ cation and the carbonate CO32- polyatomic anion. Its name is _________________ _________________.

Notice that we do _________________ add the “-ide” ending to the polyatomic ion.

NaNO3 consists of the Na+ cation and the nitrate NO3- polyatomic anion. Its name is _________________ _________________.

NH4Cl consist of the ammonium polyatomic cation and the chloride anion. Its name is _________________ _________________.

Notice that ammonium chloride ends with “-ide,” because the chloride part of the name is from Cl, NOT from a polyatomic ion.

Name the following ionic compounds (Use your list of polyatomic ions to help):

Zn(NO3)2 ________________________________

KIO3- ________________________________

V2(HPO3)3 ________________________________

Writing Formulas from Names

When writing the formulas of ionic compounds given their names, you MUST ensure that the resulting compound is

_________________.

For example:

Example 1. Determine the chemical formula of sodium bromide.

We know from the Periodic Table that sodium forms the ion _________________ and bromide forms the ion

_________________. We determine the neutral chemical formula of sodium bromide using the “criss-cross” method.

Example 2. Determine the chemical formula of sodium oxide.

Example 2. Determine the chemical formula of calcium phosphate.

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WS #1 (Learning Target 4.1: Name and write formulas for ionic compounds including compounds with multivalent ions (using

roman numerals) and those with polyatomic ions.)

I. Name the compound.

(1) ZnI2 _________________________________ (11) Sc2O3 _______________________________

(2) MgBr2 _______________________________ (12) Fr2O _______________________________

(3) Na3N ________________________________ (13) BaF2 _______________________________

(4) BaO _________________________________ (14) SrS ________________________________

(5) CaS _________________________________ (15) Al2S3 _______________________________

(6) RbF _________________________________ (16) LaCl3 _______________________________

(7) Li3P _________________________________ (17) TaBr5 _______________________________

(8) Cs2S ________________________________ (18) Ga2O3 ______________________________

(9) KCl _________________________________ (19) KBr ________________________________

(10) ZrBr4 _______________________________ (20) Ag2S _______________________________

II. Write the formula for each compound.

(1) lithium bromide________________________ (11) cadmium oxide ______________________

(2) barium iodide _________________________ (12) zirconium sulfide ___________________

(3) scandium chloride _____________________ (13) tungsten iodide ______________________

(4) potassium oxide _______________________ (14) strontium sulfide ___________________

(5) silver oxide __________________________ (15) hafnium phosphide ___________________

(6) magnesium fluoride ____________________ (16) zinc nitride _________________________

(7) francium bromide ______________________ (17) calcium sulfide _____________________

(8) calcium phosphide _____________________ (18) sodium phosphide ____________________

(9) beryllium oxide _______________________ (19) cesium nitride _______________________

(10) sodium sulfide ______________________ (20) thorium oxide _______________________

Answers:

I. II. (1) zinc iodide (11) scandium oxide (1) LiBr (11) CdO (2) magnesium bromide (12) francium oxide (2) BaI2 (12) ZrS2 (3) sodium nitride (13) barium fluoride (3) ScCl3 (13) WI6 (4) barium oxide (14) strontium sulfide (4) K2O (14) SrS (5) calcium sulfide (15) aluminum sulfide (5) Ag2O (15) Hf3P4 (6) rubidium fluoride (16) lanthanum chloride (6) MgF2 (16) Zn3N2 (7) lithium phosphide (17) tantalum bromide (7) FrBr (17) CaS (8) cesium sulfide (18) gallium oxide (8) Ca3P2 (18) Na3P (9) potassium chloride (19) potassium bromide (9) BeO (19) Cs3N (10) zirconium bromide (20) silver sulfide (10) Na2S (20) ThO2

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WS #1 (p. 2) (Learning Target 4.1: Name and write formulas for ionic compounds including compounds with multivalent ions

(using roman numerals) and those with polyatomic ions.)

Multi-Valent Metal Ionic Compounds


(1) PbI2 ________________________________ (11) SnS ________________________________

(2) CoCl3 _______________________________ (12) NiBr2 ______________________________

(3) Cr2O3 _______________________________ (13) FeCl3 ______________________________

(4) CuS ________________________________ (14) CrO _______________________________

(5) PbO2 _______________________________ (15) UCl6 _______________________________

(6) TiP _________________________________ (16) PtO ________________________________

(7) FeBr2 _______________________________ (17) PbS2 _______________________________

(8) Ni2O3 _______________________________ (18) MoBr3 ______________________________

(9) MnO2 _______________________________ (19) SnI4 ________________________________

(10) VI2 ________________________________ (20) MnF2 _______________________________

II. Write the formula for each compound. (1) lead (II) bromide _____________________ (11) vanadium (III) phosphide ______________

(2) copper (II) oxide _____________________ (12) titanium (IV) iodide __________________

(3) plutonium (V) chloride ________________ (13) mercury (II) oxide ____________________

(4) manganese (IV) sulfide _______________ (14) palladium (IV) fluoride ________________

(5) chromium (III) nitride _________________ (15) chromium (II) bromide ________________

(6) lead (II) sulfide _____________________ (16) cerium (III) nitride ____________________

(7) gold (I) oxide ________________________ (17) manganese (II) sulfide ________________

(8) tin (IV) oxide ________________________ (18) gold (III) iodide ______________________

(9) nickel (III) chloride ___________________ (19) niobium (V) oxide ____________________

(10) iron (III) oxide ______________________ (20) nickel (II) fluoride ____________________

Answers: Multivalent Ionic Compounds

I. II. (1) lead (II) iodide (11) tin (II) sulfide (1) PbBr2 (11) VP (2) cobalt (III) chloride (12) nickel (II) bromide (2) CuO (12) TiI4 (3) chromium (III) oxide (13) iron (III) chloride (3) PuCl5 (13) HgO (4) copper (II) sulfide (14) chromium (II) oxide (4) MnS2 (14) PdF4 (5) lead (IV) oxide (15) uranium (VI) chloride (5) CrN (15) CrBr2 (6) titanium (III) phosphide (16) platinum (II) oxide (6) PbS (16) CeN (7) iron (II) bromide (17) lead (IV) sulfide (7) Au2O (17) MnS (8) nickel (III) oxide (18) molybdenum (III) bromide (8) SnO2 (18) AuI3 (9) manganese (IV) oxide (19) tin (IV) iodide (9) NiCl3 (19) Nb2O5 (10) vanadium (II) iodide (20) manganese (II) fluoride (10) Fe2O3 (20) NiF2

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Polyatomic Compounds


(1) NaNO3 ______________________________ (11) CuS2O3 _____________________________

(2) Mg(OH)2 ____________________________ (12) Ni(IO3)3 ____________________________

(3) CaCO3 ______________________________ (13) ScPO3 ______________________________

(4) KMnO4 _____________________________ (14) HgClO2 _____________________________

(5) Sr(NO2)2 ____________________________ (15) Ag2C2O4 ____________________________

(6) NH4Cl ______________________________ (16) BaHPO4 _____________________________

(7) LiClO3 ______________________________ (17) Cr(C2H3O2)3 _________________________

(8) KCN ________________________________ (18) (NH4)2SO4 ___________________________

(9) Ba3(PO4)2 ____________________________ (19) Fe(OCN)3 ___________________________

(10) SrCO2 ______________________________ (20) V(HSO3)2 ___________________________


(1) barium sulfate ________________________ (11) vanadium (III) iodate __________________

(2) ammonium sulfide ____________________ (12) iron (III) hydrogen carbonate ____________

(3) potassium hydroxide ____________________ (13) tin (IV) nitrite ________________________

(4) lithium carbonate ______________________ (14) rubidium hypochlorite _________________

(5) zirconium iodite _______________________ (15) manganese (II) bromate ________________

(6) sodium hydrogen sulfite ________________ (16) titanium (III) nitrate ___________________

(7) nickel (II) oxalate ______________________ (17) cobalt (II) phosphate ___________________

(8) chromium (II) acetate ___________________ (18) strontium borate ______________________

(9) cesium dihydrogen phosphate ____________ (19) mercury (II) carbonite __________________

(10) scandium borate ______________________ (20) beryllium cyanide _____________________

Answers: Polyatomic Compounds

I. II. (1) sodium nitrate (11) copper (II) thiosulfate (1) BaSO4 (11) V(IO3)3 (2) magnesium hydroxide (12) nickel (III) iodate (2) (NH4)2S (12) Fe(HCO3)3 (3) calcium carbonate (13) scandium phosphite (3) KOH (13) Sn(NO2)4 (4) potassium permanganate (14) mercury (I) chlorite (4) Li2CO3 (14) RbClO (5) strontium nitrite (15) silver oxalate (5) Zr(IO2)4 (15) Mn(BrO3)2 (6) ammonium chloride (16) barium hydrogen phosphate (6) NaHSO3 (16) Ti(NO3)3 (7) lithium chlorate (17) chromium (III) acetate (7) NiC2O4 (17) Co3(PO4)2 (8) potassium cyanide (18) ammonium sulfate (8) Cr(C2H3O2)2 (18) Sr3(BO3)2 (9) barium phosphate (19) iron (III) cyanate (9) CsH2PO4 (19) HgCO2 (10) strontium carbonite (20) vanadium (II) hydrogen sulfite (10) ScBO3 (20) Be(CN)2

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Review: Ionic Compounds


(1) MgCl2 _______________________________ (11) Cr(IO3)2 _____________________________

(2) AlF3 ________________________________ (12) V(C2H3O2)2 __________________________

(3) CrBr3 _______________________________ (13) SnS ________________________________

(4) Ca(NO2)2 ____________________________ (14) ZnCO3 ______________________________

(5) NaOH _______________________________ (15) MoCl3 ______________________________

(6) ZnCrO4 ______________________________ (16) HgF ________________________________

(7) CuBr ________________________________ (17) U(BrO)4 ____________________________

(8) Li3PO3 ______________________________ (18) ScBO3 ______________________________

(9) Zr(NO3)4 _____________________________ (19) Cs2O _______________________________

(10) Fe2O3 _______________________________ (20) Ti3(PO4)4 ____________________________


(1) aluminum sulfide ____________________ (11) nickel (III) arsenate ___________________

(2) barium fluoride _______________________ (12) gold (I) bromide _____________________

(3) scandium nitride ______________________ (13) ammonium hydroxide _________________

(4) sodium bromite _______________________ (14) copper (II) carbonate __________________

(5) manganese (II) iodide __________________ (15) calcium oxalate ______________________

(6) lithium phosphide _____________________ (16) gallium sulfate ______________________

(7) strontium sulfite _____________________ (17) yttrium bromide ______________________

(8) beryllium nitrate ______________________ (18) platinum (II) perchlorate ________________

(9) rubidium hydrogen phosphate ____________ (19) cesium cyanide _______________________

(10) lead (IV) iodate ______________________ (20) osmium (IV) oxide ___________________

Answers: Review Ionic Compounds

I. II. (1) magnesium chloride (11) chromium (II) iodate (1) Al2S3 (11) NiAsO4 (2) aluminum fluoride (12) vanadium (II) acetate (2) BaF2 (12) AuBr (3) chromium (III) bromide (13) tin (II) sulfide (3) ScN (13) NH4OH (4) calcium nitrite (14) zinc carbonate (4) NaBrO2 (14) CuCO3 (5) sodium hydroxide (15) molybdenum (III) chloride (5) MnI2 (15) CaC2O4 (6) zinc chromate (16) mercury (I) fluoride (6) Li3P (16) Ga2(SO4)3 (7) copper (I) bromide (17) uranium (IV) hypobromite (7) SrSO3 (17) YBr3 (8) lithium phosphite (18) scandium borate (8) Be(NO3)2 (18) Pt(ClO4)2 (9) zirconium nitrate (19) cesium oxide (9) Rb2HPO4 (19) CsCN (10) iron (III) oxide (20) titanium (IV) phosphate (10) Pb(IO3)4 (20) OsO2

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4-2. Name and write formulas for covalent compounds (using prefixes).

Covalent compounds, also known as molecular compounds, are different from ionic compounds in two significant respects. First of all, covalent compounds are between _________________ _________________. Secondly, whereas ionic compounds consist of bonds between ions, covalent compounds contain bonds between _________________ _________________. Since covalent compounds do NOT contain ions, we cannot use their charges to determine their chemical formulas. Rather, we must convey that information in the way we name them. To indicate the number of each atom included in a covalent compound, we use the following prefixes:

Number of atoms Prefix

1 Mono-

2 Di-

3 Tri-

4 Tetra-

5 Penta-

6 Hexa-

7 Hepta-

8 Octa-

9 Nona-

10 Deca-

11 Undeca-

12 Dodeca-

To Name a Molecular Compound:

1. Name the first element and use a prefix if there is more than one atom (if there is only one atom of the first element

(NOT use the prefix “mono”).

2. Do not change the ending of the first element.

3. Name the second element and use a prefix to indicate the number of atoms (if there is only one atom of the second

element, the prefix "mono" must be used).

4. Change the ending to “ide”.

Examples:

Formula Name

NF3

N2O4

PH3

H2O

Sulfur hexafluoride

Cl2O7

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4-3. Name and write formulas for acids.

4-4. Given any compound, classify as ionic, acid, or covalent and determine the appropriate name.

Acids are compounds which give off a _________________ ion (_________________) when dissolved in water

(Arrhenius definition).

Acid = H+ + anion

The name of the acid will be determined by the anion.

Anion Ending Acid Name

“-ide” hydro-________-ic acid

“-ate” ________-ic acid

“-ite” ________-ous acid

Name the following acids:

Acid Anion Name

HClO4

HIO3

HI

H2SO4

H3PO3

Determine the formulas of the following acids:

Acid Anion Name

Hydrofluoric acid

Nitric acid

Bromous acid

Acetic acid

Periodic acid

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WS #2 (Learning Targets 4.2 and 4.3)

Acids

I. Name the acid.

(1) HCl _________________________________ (6) HC2H3O2 _____________________________

(2) HNO3 _______________________________ (7) HClO3 _______________________________

(3) H3PO3 _______________________________ (8) H2CO3 _______________________________

(4) HCN ________________________________ (9) H3AsO4 ______________________________

(5) H2SO3 _______________________________ (10) HIO2 _______________________________

II. Write the formula for each acid.

(1) hydrofluoric acid _______________________ (6) hydroiodic acid ________________________

(2) phosphoric acid ________________________ (7) bromic acid ___________________________

(3) nitrous acid ___________________________ (8) chlorous acid __________________________

(4) sulfuric acid _________________________ (9) periodic acid __________________________

(5) oxalic acid ____________________________ (10) carbonous acid _______________________

Covalent Compounds


(1) N2O3 _______________________________ (8) PI3 _________________________________

(2) P2O4 _______________________________ (9) F2O2 ________________________________

(3) SO3 ________________________________ (10) CO2 ________________________________

(4) IF5 _________________________________ (11) SF6 ________________________________

(5) SiCl4 _______________________________ (12) O2 _________________________________

(6) Cl2 _________________________________ (13) PF5 ________________________________

(7) PCl3 ________________________________ (14) CO ________________________________


(1) nitrogen trioxide _______________________ (8) oxygen difluoride ______________________

(2) carbon tetrabromide ____________________ (9) nitrogen trichloride _____________________

(3) sulfur monoxide ______________________ (10) fluorine _____________________________

(4) carbon disulfide ______________________ (11) phosphorus triiodide ___________________

(5) nitrogen ______________________________ (12) sulfur dioxide _______________________

(6) silicon dioxide _________________________ (13) diphosphorus pentoxide_________________

(7) sulfur hexabromide ___________________ (14) silicon tetraiodide _____________________

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WS #2 (p. 2) (Learning Targets 4.2 and 4.3)

Review: Covalent Compounds and Acids


(1) HI __________________________________ (7) NI3 _________________________________

(2) H2 __________________________________ (8) CF4 _________________________________

(3) PBr5 _________________________________ (9) HClO _______________________________

(4) HIO3 ________________________________ (10) N2H4 _______________________________

(5) CS2 _________________________________ (11) HOCN _____________________________

(6) P2S3 _________________________________ (12) H2C2O4 _____________________________


(1) perchloric acid ________________________ (7) tetraphosphorus decoxide _______________

(2) silicon tetrabromide ____________________ (8) carbon tetrachloride ___________________

(3) tetraphosphorus octasulfide _____________ (9) hydrosulfuric acid ___________________

(4) boron triiodide ________________________ (10) dinitrogen tetrasulfide _______________

(5) phosphorus pentafluoride ________________ (11) sulfur hexaiodide ___________________

(6) arsenous acid __________________________ (12) boric acid ___________________________

Answers: Acids

I. II. (1) hydrochloric acid (6) acetic acid (1) HF (6) HI (2) nitric acid (7) chloric acid (2) H3PO4 (7) HBrO3 (3) phosphorous acid (8) carbonic acid (3) HNO2 (8) HClO2 (4) hydrocyanic acid (9) arsenic acid (4) H2SO4 (9) HIO4 (5) sulfurous acid (10) iodous acid (5) H2C2O4 (10) H2CO2

Answers: Covalent Compounds

I. II. (1) dinitrogen trioxide (8) phosphorous triiodide (1) NO3 (8) OF2 (2) diphosphorus tetroxide (9) difluorine dioxide (2) CBr4 (9) NCl3 (3) sulfur trioxide (10) carbon dioxide (3) SO (10) F2 (4) iodine pentafluoride (11) sulfur hexafluoride (4) CS2 (11) PI3 (5) silicon tetrachloride (12) oxygen (5) N2 (12) SO2 (6) chlorine (13) phosphorus pentafluoride (6) SiO2 (13) P2O5 (7) phosphorus trichloride (14) carbon monoxide (7) SBr6 (14) SiI4

Review: Covalent Compounds and Acids

I. II. (1) hydroiodic acid (7) nitrogen triiodide (1) HClO4 (7) P4O10 (2) hydrogen (8) carbon tetrafluoride (2) SiBr4 (8) CCl4 (3) phosphorus pentabromide (9) hypochlorous acid (3) P4S8 (9) H2S (4) iodic acid (10) dinitrogen tetrahydride (4) BI3 (10) N2S4 (5) carbon disulfide (11) cyanic acid (5) PF5 (11) SI6 (6) diphosphorus trisulfide (12) oxalic acid (6) H3AsO3 (12) H3BO3

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Chemical reactions observe the ____________ _______ _________________ _______ _________________,which states

that the total amount of mass is the _________________ _________________ and _________________ a chemical

change.

A chemical reaction ___________________ the atoms, but does not create new atoms or destroy old atoms.

What a balanced chemical reaction tells us: C3H8 (g) + 5O2 (g) 4H2O (l) + 3CO2 (g)

Example 1. Balance this reaction.

H2 (g) + O2 (g) H2O (g)

Example 2. Balance this reaction.

CH4(g) + O2 (g) CO2 (g) + H2O(g)

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Balancing Word Equations

Requires knowledge of nomenclature AND the BrINClHOF’s.

BrINClHOF are all the naturally existing diatomic elements. Diatomic means ___________ ________________.

Example 3. Balance the following word equation.

Barium sulfide + water barium oxide + hydrogen sulfide


Example 4. Balance the following word equation.

Calcium carbonate + hydrochloric acid calcium chloride + hydrogen carbonate

The Algebraic Method of Balancing Chemical Reactions

Example 3. Balance this reaction. C4H10 + O2 → CO2 + H2O

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WS #3 (Learning Target 4-8: Balance chemical equations beginning with either chemical names or formulas.)

Balance the following equations.

1) ____ Na3PO4 + KOH NaOH + ____ K3PO4

2) ____ MgF2 + ____ Li2CO3 ____ MgCO3 + LiF

3) ____ P4 + O2 P2O3

4) RbNO3 + ____ BeF2 ____ Be(NO3)2 + RbF

5) AgNO3 + ____ Cu ____ Cu(NO3)2 + Ag

6) ____ CF4 + Br2 ____ CBr4 + F2

7) HCN + ____ CuSO4 ____ H2SO4 + ____ Cu(CN)2

8) ____ GaF3 + Cs CsF + ____ Ga

9) ____ C6H14 + ____O2 ____ CO2 + ____H2O

10) ____ N2 + H2 NH3

Balance the following word equations. ((Remember the following are diatomic: Br2, I2, N2, Cl2, H2, O2, F2)

11) sodium hydroxide + phosphoric acid sodium phosphate + water

12) antimony + chlorine antimony trichloride

13) sodium chlorate sodium chloride + oxygen

14) sodium carbonate + water sodium oxide + carbonic acid

15) silver + sulfur silver sulfide

16) potassium + water potassium hydroxide + hydrogen

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17) barium chloride + magnesium sulfate barium sulfate + magnesium chloride

18) sodium bromide + chlorine sodium chloride + bromine

19) ammonium carbonate ammonia (NH3) + carbonic acid

20) calcium carbonate + hydrochloric acid calcium chloride + carbonic acid

Answers.

1) ____ Na3PO4 + 3 KOH 3 NaOH + ____ K3PO4 11. 3NaOH + H3PO4 Na3PO4 + 3H2O

2) ____ MgF2 + ____ Li2CO3 ____ MgCO3 + 2 LiF 12. 2Sb + 3Cl2 2SbCl3 3) ____ P4 + 3 O2 2 P2O3 13. 2NaClO3 2NaCl + 3O2 4) 2RbNO3 + ____ BeF2 ____ Be(NO3)2 + 2 RbF 14. Na2CO3 + H2O Na2O + H2CO3 5) 2 AgNO3 + ____ Cu ____ Cu(NO3)2 + 2 Ag 15. 2Ag + S Ag2S 6) ____ CF4 + 2 Br2 ____ CBr4 + 2 F2 16. 2K + 2H2O 2KOH + H2 7) 2 HCN + ____ CuSO4 ____ H2SO4 + ____ Cu(CN)2 17. BaCl2 + MgSO4 BaSO4 + MgCl2 8) ____ GaF3 + 3 Cs 3CsF + ____ Ga 18. 2NaBr + Cl2 2NaCl + Br2 9) 2 C6H14 + 19 O2 12 CO2 + 14H2O 19. (NH4)2CO3 2NH3 + H2CO3 10) ____ N2 + 3H2 2 NH3 20. CaCO3 + 2HCl CaCl2 + H2CO3

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4-9. Classify reactions as synthesis, decomposition, single replacement, double replacement, neutralization, or

combustion.

Types of Chemical Reactions CLOZE

Synthesis Two elements or ________________ __________________ into ___________________ new

compound. If both reactants are compounds, usually one of the reactants is

___________________.

Example:

Decomposition __________________ reactant breaks down into its components.

Example:

Single Replacement __________________ element replaces another in a __________________.

Example:

Double Replacement

The cations and anions in two compounds __________________ __________________ with

each other.

Example:

Neutralization A special type of double replacement reaction between an _acid (begins with H+) and a base

(contains OH- polyatomic ion). The H+ of the acid combines with the OH- of the base, producing

a salt and water.

Example: HCl + NaOH HOH + NaCl

Combustion One of the reactants is O2. The other reactant is usually a hydrocarbon (compound made of

hydrogen and carbon). The products of the combustion of a hydrocarbon are CO2 and H2O.

Example:

Sample Problems:

The reaction 2Fe + 3Cl2 2FeCl3 is an example of which type of reaction?

The reaction Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) is an example of which type of reaction?

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WS #4 (Learning Target 4-9: Classify reactions as synthesis, decomposition, single replacement, double replacement,

neutralization, or combustion.)

Directions: Balance the following reactions and identify them as synthesis, decomposition, single replacement or double

replacement.

1. Mg + I2 MgI2

2. CuCl2 + H2S CuS + HCl

3. Sodium hydroxide + perchloric acid sodium perchlorate + water

4. Zinc carbonate zinc oxide + carbon dioxide

5. HCl + Zn ZnCl2 + H2

6. Na + MgCl2 NaCl + Mg

7. Calcium chloride + potassium carbonate calcium carbonate + potassium chloride

8. potassium + chlorine potassium chloride

9. BaCl2 + K3PO4 Ba3(PO4)2 + KCl

10. H2SO4 + KOH H2O + K2SO4

11. Al2(CO3)3 Al2O3 + CO2

12. Al + O2 Al2O3

13. Lead (II) nitrate + potassium hydroxide lead (II) hydroxide + potassium nitrate

14. H2SO4 + BaCl2 BaSO4 + HCl

15. Calcium + silver chloride calcium chloride + silver

16. H3PO4 + FeBr3 FePO4 + HBr

17. Li + N2 Li3N

18. HCl + Mg(OH)2 MgCl2 + H2O

19. Magnesium hydroxide magnesium oxide + water

20. Iron (III) hydroxide iron (III) oxide + water

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Answers.

1. Synthesis: Mg + I2 MgI2

2. Double displacement: CuCl2 + H2S CuS + 2HCl

3. Double displacement: NaOH + HClO4 NaClO4 + H2O

4. Decomposition: ZnCO3 ZnO + CO2

5. Single replacement: 2HCl + Zn ZnCl2 + H2

6. Single replacement 2Na + MgCl2 2NaCl + Mg

7. Double replacement CaCl2 + K2CO3 CaCO3 + 2KCl

8. Synthesis 2K + Cl2 2KCl

9. Double replacement 3BaCl2 + 2K3PO4 Ba3(PO4)2 + 6KCl

10. Double replacement H2SO4 + 2KOH 2H2O + K2SO4

11. Decomposition Al2(CO3)3 Al2O3 + 3CO2

12. Synthesis 4Al + 3O2 2Al2O3

13. Double replacement Pb(NO3)2 + 2KOH Pb(OH)2 + 2KNO3

14. Double replacement H2SO4 + BaCl2 BaSO4 + 2HCl

15. Single replacement Ca + 2AgCl CaCl2 + 2Ag

16. Double replacement H3PO4 + FeBr3 FePO4 + 3HBr

17. Synthesis 6Li + N2 2Li3N

18. Double replacement 2HCl + Mg(OH)2 MgCl2 + 2H2O

19. Decomposition Mg(OH)2 + heat MgO + H2O

20. Decomposition 2Fe(OH)3 + heat Fe2O3 + 3H2O

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4-10. Predict the products of a reaction given the formulas or names of reactants.

Reactants Type of Reaction Products Example

One compound Decomposition Two compounds Al2O3

Two elements Synthesis H2 + Cl2

One element and one ionic compound

Single Replacement New ionic compound + one element F2 + KCl

Two ionic compounds Double Replacement Switch Partners Pb(NO3)2 + K2S

Acid and Base Neutralization Switch Partners (salt and water) HCl + Ca(OH)2

Oxygen and hydrocarbon Combustion CO2 + H2O CH4 + O2

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WS #5 (Learning Target 4-10: Predict the products of a reaction given the formulas or names of reactants.)

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Documents

Chemistry HP Unit 4 Chemical Nomenclature and Chemical ...4... · Acids are compounds which most often begin with _____, such as H 2 SO4 (sulfuric acid) and HCl (hydrochloric acid),