Chemistry Honors Chapter 7 Section 1: Nomenclature Naming Compounds

Cations

(+) "element name" ion.

Anions

(-) Change last syllable on element name to -ide then ion.

Mono

1

Deca

10

# mol. Cu=10 g.*1 mol. Cu/63.55 g. Cu=0.157 mol. Cu # mol. O=2.52 g. O*1 mol. O/16 g. O=0.1575 mol. O Cu(0.157/0.157)O(0.1575/0.157) CuO

10.00 grams of copper is heated strongly in air. The sample gains 2.52 grams of oxygen. Calculate the empirical formula of the resulting product. Show your work!

Di

2

Tri

3

Tetra

4

Penta

5

Hexa

6

Hepta

7

Octa

8

Nona

9

# mol. Ca=2.004 g. Ca*1 mol. Ca/40.08 g. Ca=0.05 mol. Ca # mol. N=0.467 g. N*1 mol. N/14.01 g. N=0.033 mol. N Cu(0.05/0.033)N(0.033/0.033) 2(Cu1.5N) Cu3N2

A 2.004 g. sample of Cu is heated in steam of pure N gas. It gains 0.4670 g. of nitrogen. Calculate the empirical formula.

# mol. C=54.5 g. C*1 mol. C/12.01 g. C= 4.538 mol. C/2.27=2 # mol. H=13.6 g. H*1 mol. H/1.01 g. H=13.465 mol. H/2.27=6 # mol. N=31.8 g. N*1 mol. N/14.01 g. N=2.27 mol. N/2.27=1 C2H6N->2(40.08)+5(1.01)+14.01 80.16+5.05+14.01 100.23 g/mol. 88/100.23=0.88 0.88(C2H6N) C2H5N

A compound has a % composition of 54.5% carbon, 13.6% H, and 31.8% nitrogen. Its mm was found to be 88.0 g/mol. Calculate the empirical and molecular formulas.

# mol. Na=21.6 g. Na*1 mol. Na/22.99 g. Na=0.9395 mol. Na # mol. Cl=33.31 g. Cl*1 mol. Cl/35.45 g. Cl=0.9396 mol. Cl # mol. O=45.09 g. O*1 mol. O/16 g. O=2.8181 mol. O Na(0.9395/0.9395)Cl(0.9396/0.9395)O(2.8181/0.9395) NaClO3

A compound has a composition of 21.60% sodium, 33.31% chlorine, and 45.09% oxygen. Calculate the empirical formula.

HgCl->200.59+35.45=236.04 g/mol. 472.2/236.04=2 2(HgCl)=Hg2Cl2

A compound has an empirical formula of HgCl. Its molecular mass was found to be 472.2 g/mol. What is the molecular formula of the compound? Show your work!

0.4(100) 0.067(100) 0.533(100) 40 g. C 6.7 g. H 53.3 g. O # mol. C=40 g. C*1 mol. C/12.01 g. C=3.33 mol. C # mol. H=6.7 g. H/1 mol. H/1.01 g. H=6.63 mol. H # mol. O=53.3 g. O*1 mol. O/16 g. O=3.33125 mol. O C3.33/3.33H6.63/3.33O3.33125/3.33 CH2O

A compound is determined to be 40% C, 6.7% H, and 53.3% O. Find the emp. formula. Show your work!

0.158(100) 0.842(100) 15.8 g. C 84.2 g. S # mol. C=15.8 g. C*1 mol. C/12.01 g. C=1.32 mol. C # mol. S=84.2 g. S*1 mol. S/32.07 g. S=2.63 mol. S C(1.32/1.32)S(2.63/1.32) CS2; Carbon Disulfide

A compound is determined to have 15.8% Carbon and 84.2% Sulfur. Find the empirical formula and name it.

Tertiary Ionic Compounds

A compound that contains 3 or more different elements.

# mol. C=75.95 g. C*1 mol. C/12.01 g. C= 6.324 mol. C # mol. N=17.72 g. N*1 mol. N/14.01 g. N=1.265 mol. N # mol. H=6.33 g. H*1 mol. H/1.01 g. H=6.267 mol. H C(6.324/1.265)N(1.265/1.265)H(6.267/1.265) C5NH5 5(12.01)+14.01+5(1.01) 60.05+14.01+5.05 79.11 g/mol. (240/79.11)=3 3(C5NH5) C15N3H15

A yellow dye is found to be 75.95% C, 17.72% N, and 6.33% H. Its molar mass is 240 g/mol. What is the molecular formula? Show your work!

CH3COOH

Acetic Acid

Molecular Compound

Also known as covalent compounds, typically consists 2 nonmetals.

Salt

Any compound composed of a cation and an anion from an acid. NaCl contains the chloride anion from hydrochloric acid.

2(22.99)+32.07+4(16) 45.98+32.07+64 142.05 g/mol. 100(45.98/142.05)=32.37% Na 100(32.07/142.05)=22.58% S 100(64/142.05)=45.05% O

Calculate the percent composition of Na2SO4.

H2CO3

Carbonic Acid

HClO3

Chloric Acid

HClO2

Chlorous Acid

Ionic Compound

Compound formed between a cation and anion. Typically consists of one metal and one nonmetal.

Binary Molecular Compounds

Compounds containing two nonmetals. Charges are ignored.

Binary Ionic Compounds (Type I)

Compounds of 2 elements. 1 metal and 1 nonmetal. Metal has a charge (typically positive). Metal will receive elemental name. Nonmetals (typically negative) receive elemental name ending in -ide. Sum of charges must be 0.

NH3 14.01+3(1.01) 14.01+3.03 17.04 g/mol. NH3 # g. NH3=6.82*10^26 molecules NH3*1 mol. NH3/6.022*10^23 molecules NH3*17.04 g. NH3/1 mol. NH3=19,298.04 NH3

Determine the mass of 6.82*10^26 molecules of ammonia? Show your work!

# mol. Mg=28.03 g. Mg*1 mol. Mg/24.31 g. Mg=1.153 mol. Mg # mol. 21.6 g. Si*1 mol. Si/28.09 g. Si=0.769 mol. Si # mol. H=1.16 g. H*1 mol. H/1.01 g. H=1.149 mol. H # mol. O=49.21 g. O*1 mol. O/16 g. O=3.076 mol. O Mg(1.153/0.769) Si(0.769/0.769) H(1.149/0.769) O(3.076/0.769) 2(Mg1.5SiH1.5O4) Mg3Si2H3O8 EFM=3(24.31)+2(28.03)+3(1.01)+4(16) EFM=72.93+56.18+3.03+64 EFM=260.14 g/mol. MM/EFM=(520.8/260.14)=2 2(Mg3Si2H3O8) Mg6Si4H6O16

Determine the molecular formula of a compound that is 28.03% Mg, 21.6% Si, 1.16% H, 49.21% O. The molecular mass is 520.8 g/mol. Show your work!

Na2C2O4 2(22.99)+2(12.01)+4(16) 45.98+24.02+64 134 g/mol. Na2C2O4 45.98/134=34.31% Na 24.02/134=17.93% C 64/134=47.76% O

Find the % comp. of Sodium Oxalate. Show your work!

2(26.98)+3(32.07) 53.96+96.21 150.17 g/mol.

Find the molar mass for this compound: Al2S3. Show your work!

137.33+2(16)+2(1.01) 137.33+32+2.02 171.35 g/mol.

Find the molar mass for this compound: Ba(OH)2. Show your work!

22.99+14.01+3(16) 37+48 85 g/mol.

Find the molar mass for this compound: NaNO3. Show your work!

3(207.2)+2(30.97)+8(16) 621.6+61.94+128 811.54 g/mol.

Find the molar mass for this compound: Pb3(PO4)2. Show your work!

Percent Composition

Gives the percent by mass of each element contained in a compound.

Polyatomic Ions

Group of atoms that function as a unit and carries a charge. It will bond with a positive cation.

1

How any many atoms are assumed to be when there is no subscript next to an atom?

Add the mass of each atom present.

How do we calculate a formula mass?

H2SO3 # H atoms=10.2 mol. H2SO3*6.022*10^23 molecules H2SO3/1 mol. H2SO3*2 H atoms/1 molecule H2SO3=1.23*10^25 molecules H2SO3

How many Hydrogen atoms are in a 10.2 mol. sample of sulfurous acid? Show your work?

N=3, H=12, P=1, and O=4.

How many atoms in each element are in (NH4)3PO4?

# H atoms=20.1 g. H2O*1 mol. H2O/18.02 g. H2O*6.022*10^23 molecules H2O/1 mol. H2O*2 H atoms/1 molecule H2O=1.34*10^24 H atoms

How many atoms of hydrogen are found in 20.1 grams of H2O? Show your work!

#g.K2CO3=0.345 mol. K2CO3*138.21 g. K2CO3/1 mol. K2CO3=47.68245 g.K2CO3

How many grams are in 0.345 mol. K2CO3? Show your work!

#g. CoCl2=2.1 mol. CoCl2*129.83 g. CoCl2/1 mol. CoCl2=272.643 g. CoCl2

How many grams are in 2.1 moles of cobalt (II) chloride? Show your work!

#g.=2.4 mol. O*16 g./1 mol. O=38.4 g. O

How many grams are in 2.4 moles of Oxygen? Show your work!

NH4NO3 2(14.01)+4(1.01)+3(16) 28.02+4.04+48 80.06 g/mol. N2H4O3 #g. N2H4O3=3.2 mol. N2H4O3*80.06 g. N2H4O3/1 mol. N2H4O3= 256.192 g. N2H4O3

How many grams of Ammonium Nitrate are in 3.2 moles? Show your work!

#g. NF2=3.4 mol. NF2*52.01 NF2/1 mol. NF2=176.834 g. NF2

How many grams of nitrogen difluoride are in 3.4 moles?

# molecules H2SO4=25 g. H2SO4*1 mol. H2SO4/98.09 g. H2SO4*6.022*10^23 molecules/1 mol. H2SO4=1.53*10^23 molecules H2SO4

How many molecules are there in 25.0 g. H2SO4? Show your work!

Cu2SO4 2(63.55)+32.07)+4(16) 127.1+32.07+64 223.17 g/mol. Cu2SO4 # molecules Cu2SO4=100 g. Cu2SO4*1 mol. Cu2SO4/223.17 g. Cu2SO4*6.022*10^23 molecules Cu2SO4/1 mol. Cu2SO4=2.7*10^23 molecules Cu2SO4

How many molecules of Copper (I) Sulfate are in 100 g.?

#mol.=21.7 g. C*1 mol. C/12.01 g. C=1.81 mol. C

How many moles are in 21.7 grams of Carbon?

# mol. Ca(NO3)2=50.29 g. Ca(NO3)2*1 mol. Ca(NO3)2/164.1 g. Ca(NO3)2=0.31 mol. Ca(NO3)2

How many moles are in 50.29 g. of Ca(NO3)2? Show your work!

# mol. Ca(NO3)2=81.2 g. Ca(NO3)2*1 mol. Ca(NO3)2/164.1 g. Ca(NO3)2=0.49 mol. Ca(NO3)2

How many moles are in 81.2 g. of calcium nitrate? Show your work!

# mol. K2CO3=56.2 g. K2CO3*1 mol. K2CO3/138.21 g. K2CO3=0.41 mol. K2CO3

How many moles of potassium carbonate are in 56.2 grams? Show your work!

# O atoms=3.2 mol. CO2*6.022*10^23 molecules CO2/1 mol. CO2*2 atoms O/1 molecule CO2=3.85*10^24 O atoms

How many oxygen atoms are in 3.2 moles of carbon dioxide? Show your work!

1. Convert grams to moles (if given percents, assume 100 g, then your percent becomes grams). 2. Make mole values into subscripts. 3. Divide all subscripts by the smallest subscript. 1. If resulting subscripts aren't whole numbers, multiply by appropriate number so that they all become whole numbers (1/2 multiply by 2, 1/3 multiply by 3).

How to find an empirical formula?

1. Calculate the empirical formula of the compound. 2. Determine the empirical formula mass. 1. HO->17 g/mol. 2. CH2O->30 g/mol. 3. Divide the given molecular mass (mm) by the empirical formula mass (EFM). 4. Multiply all subscripts in empirical formula by rule obtained in step 3.

How to find molecular formulas?

HBr

Hydrobromic Acid

HCl

Hydrochloric Acid

HF

Hydrofluoric Acid

HI

Hydroiodic Acid

HClO

Hypochlorous Acid

-ic

If the ending of an ion is -ate, then what does it become for the acid?

Hydro-root-ic

If the ending of an ion is -ide, then what does it become for the acid?

-ous

If the ending of an ion is -ite, then what does it become for the acid?

There are 8 carbon atoms in this compound. There are 18 hydrogen atoms in this compound.

In a chemical formula what does the following chemical compound, C8H18 read?

Monotomic Ions

Ions formed from single atoms. Periodic trend for ion charges on the perioidic table.

Aluminum Phosphide

Name this compound: AlP.

Barium Oxide

Name this compound: BaO.

Barium Selenide

Name this compound: BaSe.

Beryllium Chloride

Name this compound: BeCl2.

Carbon Tetrachloride

Name this compound: CCl4.

Carbon Dioxide

Name this compound: CO2.

Calcium Bromide

Name this compound: CaBr2.

Calcium Carbonate

Name this compound: CaCO3.

Chromium (III) Oxide

Name this compound: Cr2O3.

Calcium Phosphate

Name this compound: Cu2(PO4)2.

Copper (II) Sulfate

Name this compound: CuSO4.

Iron (II) Hydroxide

Name this compound: Fe(OH)2.

Iron (III) Chromate

Name this compound: Fe2(CrO4)3.

Iron (II) Iodide

Name this compound: FeI2.

Sulfuric Acid

Name this compound: H2SO4.

Hydrocyanic Acid

Name this compound: HCN.

Perchloric Acid

Name this compound: HClO4.

Iodine Trichlorine

Name this compound: ICl3.

Potassium Nitride

Name this compound: K3N.

Potassium Hypochlorite

Name this compound: KCIO.

Potassium Chloride

Name this compound: KCl.

Magnesium Bromide

Name this compound: MgBr2.

Magnesium Sulfide

Name this compound: MgS.

Manganese (V) Sulfide

Name this compound: Mn2S5.

Dinitrogen Tetraiodide

Name this compound: N2I4.

Ammonium Hydroxide

Name this compound: NH4OH.

Sodium Phosphide

Name this compound: Na3P.

Sodium Chlorite

Name this compound: NaClO2.

Sodium Nitrate

Name this compound: NaNO3.

Nickel (I) Permanganate

Name this compound: NiMnO4.

Nickel (III) Nitride

Name this compound: NiN.

Diphosphorus Pentoxide

Name this compound: P2O.

Triphosphorous Heptoxide

Name this compound: P3O7.

Tetraphosphorus Decoxide

Name this compound: P4O10.

Phosphorus Pentabromine

Name this compound: PBr5.

Lead (II) Sulfide

Name this compound: PbS.

Rubidium Hydroxide

Name this compound: RbOH4.

Tin (IV) Iodide

Name this compound: SnI4.

Tin (IV) Oxide

Name this compound: SnO2.

Titanium (IV) Oxide

Name this compound: TiO2.

Aluminium Ion

Name this ion: Al+3.

Phosphide Ion

Name this ion: P-3.

Rubidium Ion

Name this ion: Rb+.

Selenide Ion

Name this ion: Se-2.

HNO3

Nitric Acid

HNO2

Nitrous Acid

HClO4

Perchloric Acid

H3PO4

Phosphoric Acid

Molecular Formulas

Represents the actual whole number ratio of atoms in a compound. Will either the same as the empirical formula or a whole number multiple of it.

Empirical Formula

Simplest formula for a compound. Gives the lowest whole number ratio of subscripts.

Binary (Type II)

Some metals can have multiple charges. Nonmetal gets elemental name ending in -ide. Metal gets elemental name followed by roman numerals designating the charge. The charge depends on what anion it is bonded to. Mostly occurs with transition metals. Lead and Tin also require roman numerals. Sum of charges=0. Some transition metals only have one charge and will not require roman numerals.

H2SO4

Sulfuric Acid

H2SO3

Sulfurous Acid

Subscripts

The number that indicates the number of atoms in the molecule.

Formula Mass

The sum of average atomic masses of all atoms represented in a formula.

Hydrocarbons

These compounds contain only hydrogen and carbon. The key focus of organic chemistry.

F-->Fluoride Ion and O^2->Oxide Ion

What are examples of anions?

Cul=Copper (I) Iodide and Cul2=Copper (II) Iodide

What are examples of binary (Type II) compounds?

Na+Cl-->NaCl->Sodium Chloride and K+Sl2-->K2S->Potassium Sulfide

What are examples of binary ionic compounds (type I)?

CO (Carbon Monoxide) and P4O10 (Tetraphosphorus Decoxide)

What are examples of binary molecular compounds?

HO is the empirical formula for H2O2. CH2O is the empirical formula for C6H12O6.

What are examples of empirical formulas?

NaCl->NaCl and HO*2->H2O2

What are examples of molecular formulas?

Na^+, Ca^2+, Cl^-, and N^3-

What are examples of monotomic ions?

Copper (I) Chloride (Cuprous Chloride), Copper (II) Chloride (Cupric Chloride), Iron (II) Oxide (Ferrous Oxide), and Iron (III) Oxide (Ferric Oxide)

What are examples of other naming methods?

NaNO3 (Sodium Nitrate) and CaCO3 (Calcium Carbonate)

What are examples of tertiary ionic compounds?

SF6 (Sulfur Hexafluoride) and N2O3 Dinitrogen Trioxide

What are examples of the second rule?

Dihydrogen Monoxide (H2O)=Water and Nitrogen Trihydride (NH3)=Ammonia.

What are examples of the third rule in terms of common names?

Mono-oxide->Monoxide and Penta-oxide->Pentoxide

What are examples of the third rule?

Some textbooks use a form of the Latin or Greek name to distinguish between charges. Lower charge has -ous ending. Higher charge has -ic ending.

What are other naming methods?

Metal gets elemental name. Polyatomic ion gets its name. Sum of charges must equal zero.

What are the rules for naming?

1. Make subscripts into mole values. 2. Convert moles into grams. 3. Divide the grams of each element by the total weight of the compound, then multiply by 100. Mass of element in compound*100 Mass of Total Compound Always check your work. The sum of your percentages should equal 100%.

What are the rules of percent composition?

+2

What charge does cadmium (cd) always have?

+1

What charge does group 1 have?

-3

What charge does group 15 have?

-2

What charge does group 16 have?

-1

What charge does group 17 have?

+2

What charge does group 2 have?

+3

What charge does group 3 have?

+1

What charge does silver (ag) always have?

+2

What charge does zinc (zn) always have?

An extra step after using Avogadro's number.

What does converting to atoms require?

Al2 refers to 2 atoms of Al. SO4 refers to 4 oxygen atoms in a sulfate ion. 3 refers to everything in parenthesis, giving a total of 3 sulfur atoms and 12 O. Al=2, S=3, and O=12.

What does the following compound read: Al2(SO4)3? How many atoms are there in each element?

Na^+->Sodium Ion

What is an example of a cation?

CH4

What is an example of a hydrocarbon?

CO

What is an example of a molecular compound?

Ca2+NO3-->Ca(NO3)2

What is an example of a polyatomic ion bonded with a positive cation?

No3-

What is an example of a polyatomic ion?

NaCl

What is an example of an ionic compound?

H2O Mass of Hydrogen: 2 moles H*1.007 g/mol.=2.014 g/mol. Mass of Oxygen: 1 mole O*16.00 g/mol.=+16.00 g/mol. 18.014 g/mol.

What is an example of formula mass?

SO2 (Sulfur Dioxide)

What is an example of the first rule?

#g. CO=2.5 mol. CO*28 g. CO/1 mol. CO=70 g. CO

What is an example of the molar mass conversion factor?

The element with the smallest group number is usually given first. If both are in the same group, the element with the greatest period number is listed first. If the first element only has one atom, prefix is not used.

What is the first rule for naming?

g/mm->mol. g<-mm*mol. mm=molar mass

What is the formula for the conversion of mass to moles?

The molar mass of a compound can be used to find convert between moles, grams, atoms, and molecules. Remember, atoms and molecules can be found by Avogado's number.

What is the molar mass conversion factor?

2(39.10)+51.99+4(16) 78.2+51.99+64 194.19 g/mol. 100(78.2/194.19)=40.27% K 100(51.99/194.19)=26.77% Cr 100(64/194.19)=32.96% O

What is the percent composition of Potassium Chromate? (K2CrO4)

The second atom will have a prefix representing the number of atoms.

What is the second rule for naming?

The o or a at the end of a prefix is usually dropped when the following word begins with another vowel. Some compounds go by "common names."

What is the third rule for naming?

6.022*10^23 molecules/mol. instead of atoms/mol.

When converting to molecules for compounds, what is Avogadro's number?

NH4Cl

Write the formula for ammonium chloride.

AsO2

Write the formula for arsenic dioxide.

CrPO4

Write the formula for chromium (III) phosphate.

CuBr2

Write the formula for copper (II) bromide.

CuO

Write the formula for copper (II) oxide.

IF5

Write the formula for iodine pentafluoride.

FeCl3

Write the formula for iron (III) chloride.

Pb(NO2)2

Write the formula for lead (II) nitrate.

Hg(C2H3O2)2

Write the formula for mercury (II) acetate.

HgO

Write the formula for mercury (II) oxide.

Ni3P2

Write the formula for nickel (II) phosphide.

PCl3

Write the formula for phosphorous trichloride.

K2SO3

Write the formula for potassium sulfite.

NaC2H3O2

Write the formula for sodium acetate.

Na2C2O4

Write the formula for sodium oxalate.

SF

Write the formula for sulfur monofluoride.

SF3

Write the formula for sulfur trifluoride.

C2H4O2

Write the formula for this compound: Acetic Acid.

(NH4)2SO3

Write the formula for this compound: Ammonium Sulfite.

Ca3N2

Write the formula for this compound: Calcium Nitride.

CaO

Write the formula for this compound: Calcium Oxide.

CsF

Write the formula for this compound: Cesium Fluoride.

GaN

Write the formula for this compound: Gallium Nitride.

FePO4

Write the formula for this compound: Iron (III) Phosphate.

MNI4

Write the formula for this compound: Manganese (IV) Iodide.

NBr2

Write the formula for this compound: Nitrogen Dibromide.

NF3

Write the formula for this compound: Nitrogen Trifluoride.

H3PO3

Write the formula for this compound: Phosphorous Acid.

K2C2O4

Write the formula for this compound: Potassium Oxalate.

AlCl3

Write the formula for this compound: aluminum chloride?

Al2S3

Write the formula for this compound: aluminum sulfide?

BaI2

Write the formula for this compound: barium iodide?

CaCl2

Write the formula for this compound: calcium chloride?

Li^+Br^-

Write the formula for this compound: lithium bromide.

Na3P

Write the formula for this compound: sodium phosphide?

V2O5

Write the formula for vanadium (V) oxide.