Chapter 5: Molecules and Compounds

SaltSodium – shiny, reactive, poisonousChlorine – pale yellow gas, reactive,

poisonousSodium chloride – table salt

SugarCarbon – pencil or diamondsHydrogen – flammable gas

Oxygen – a gas in airCombine to form white crystalline

sugar

5.2 Compounds Display Constant Composition

FIGURE 5.4 A mixture This balloon is filled with a mixture of hydrogen and oxygen gas. The relative amounts of hydrogen and oxygen

are variable.

FIGURE 5.5 A chemical compound This balloon is filled with water, composed of molecules that have a fixed ratio of hydrogen to oxygen. (Source: JoLynn E. Funk.)

Compounds Display Constant Composition

If we decompose water by electrolysis, we find 16.0 grams of oxygen to every 2.00 grams of hydrogen.

Water has a constant Mass Ratio of Oxygen to Hydrogen of 8.0.

0.8g 2.0g 0.16hydrogen of massoxygen of mass Ratio Mass

Why do Compounds ShowConstant Composition

the smallest piece of a compound is called a molecule

every molecule of a compound has the same number and type of atoms

since all the molecules of a compound are identical, every sample will have the

same ratio of the elementssince all molecules of a compound are

identical, every sample of the compound will have the same properties

Formulas Describe Compounds

H2OWater: 2 Hydrogen atoms and 1 Oxygen atom

C12H22O11

Sucrose (table sugar):12 atoms of Carbon, 22 atoms of Hydrogen and 11 atoms Oxygen

4 Mg(NO3) 2

A number in front of a molecule means that you have more than one molecule; it is often referred to as coefficient

A subscript number after an element means that you have more than 1 atom for that element

A subscript number after a parenthesis means that all the atoms in the parenthesis are present in that molecule multiple times.

If the molecule is an ion a superscript number represents the charge of the molecule

The specific order for listing nonmetal elements in a chemical formula is shown in Table 5.1.

There are a few historical exceptions in which the most metallic element is named first, such as the hydroxide

ion, which is written as OH−.

Classifying Materialsatomic elements = elements whose

particles are single atomsmolecular elements = elements whose

particles are multi-atom moleculesmolecular compounds = compounds

whose particles are molecules made of only nonmetals

ionic compounds = compounds whose particles are cations and anions

Molecular ElementsCertain elements occur as 2 atom molecules

Rule of 7’s there are 7 common diatomic elements

find the element with atomic number 7, Nmake a figure 7 by going over to Group 7A, then down

don’t forget to include H2

H2

Cl2

Br2

I2

7

VIIA

N2 O2 F2

Molecular Compounds

• two or more nonmetals

• smallest unit is a molecule

Ionic Compounds

• metals + nonmetals• no individual molecule

units, instead have a 3-dimensional array of cations and anions made of formula units

Molecular View of Elements and Compounds

Step1 - Common Names - Exceptions

• H2O = water, steam, ice

• NH3 = ammonia

• CH4 = methane• NaCl = table salt• C12H22O11 = table sugar

Step 2 - Classifying Compounds• Compounds containing a metal and a nonmetal =

binary ionic– Type I and II

• Compounds containing a polyatomic ion = ionic with polyatomic ion

• Compounds containing two nonmetals = binary molecular compounds

• Compounds containing H and a nonmetal = binary acids

• Compounds containing H and a polyatomic ion = oxyacids

Step 3 - Formula-to-NameRules for Ionic

• Made of cation and anion• Name by simply naming the ions

– If cation is:• Type I metal = metal name• Type II metal = metal name(charge)• Polyatomic ion = name of polyatomic ion

– If anion is:• Nonmetal = stem of nonmetal name + ide• Polyatomic ion = name of polyatomic ion

Monatomic Nonmetal Anion• determine the charge from position on the

Periodic Table• to name anion, change ending on the element

name to –ide4A = -4 5A = -3 6A = -2 7A = -1

C = carbide N = nitride O = oxide F = fluoride

Si = silicide P = phosphide S = sulfide Cl = chloride

Metal Cations• Type I

– metals whose ions can only have one possible charge

• IA, IIA, (Al, Ga, In)– determine charge by position on the

Periodic Table• IA = +1, IIA = +2, (Al, Ga, In = +3)

• Type II– metals whose ions can have more than

one possible charge– determine charge by charge on anion

How do you know a metal cation is Type II?

its not Type I !!!

Type I Binary Ionic Compounds• Contain Metal Cation + Nonmetal Anion• Metal listed first in formula & name

1. name metal cation first, name nonmetal anion second

2. cation name is the metal name3. nonmetal anion named by changing the ending

on the nonmetal name to -ide

Type II Binary Ionic Compounds• Contain Metal Cation + Nonmetal Anion• Metal listed first in formula & name

1. name metal cation first, name nonmetal anion second2. metal cation name is the metal name followed by a

Roman Numeral in parentheses to indicate its charge– determine charge from anion charge– Common Type II cations in Table 5.5

3. nonmetal anion named by changing the ending on the nonmetal name to -ide

Some Common Polyatomic IonsName Formulaacetate C2H3O2

–

carbonate CO32–

hydrogen carbonate(aka bicarbonate) HCO3

–

hydroxide OH–

nitrate NO3–

nitrite NO2–

chromate CrO42–

dichromate Cr2O72–

ammonium NH4+

Name Formulahypochlorite ClO–

chlorite ClO2–

chlorate ClO3–

perchlorate ClO4–

sulfate SO42–

sulfite SO32–

hydrogensulfate(aka bisulfate) HSO4

–

hydrogensulfite(aka bisulfite) HSO3

–

Step 3- Formula-to-NameRules for Molecular

• we will not learn the rules for molecular compounds with more than 2 elements

• for binary molecular:– name first nonmetal– then name second nonmetal with ide ending– then give each name a prefix to indicate its

subscript in the formula

Binary Molecular Compounds of 2 Nonmetals

1. Name first element in formula first – use the full name of the element

2. Name the second element in the formula with an -ide

– as if it were an anion, however, remember these compounds do not contain ions!

3. Use a prefix in front of each name to indicate the number of atoms

a) Never use the prefix mono- on the first element

Subscript - Prefixes• 1 = mono-;

– not used on first nonmetal• 2 = di-• 3 = tri-• 4 = tetra-• 5 = penta-• 6 = hexa-• 7 = hepta-• 8 = octa-• drop last “a” if name begins with vowel

Acids• Contain H+1 cation and anion

– in aqueous solution• Binary acids have H+1 cation

and nonmetal anion• Oxyacids have H+1 cation and

polyatomic anion

Formula-to-NameAcids

• acids are molecular compounds that often behave like they are made of ions

• All names have acid at end• Binary Acids = hydro prefix + stem of the name of the

nonmetal + ic suffix • Oxyacids

– if polyatomic ion ends in –ate = name of polyatomic ion with –ic suffix

– if polyatomic ion ends in –ite = name of polyatomic ion with –ous suffix

Formula-to-Name Flow Chart

Writing the Formulas from the Names

• For binary molecular compounds, use the prefixes to determine the subscripts

• For Type I, Type II, Ternary Compounds and Acids

1. Determine the ions present2. Determine the charges on the cation and

anion3. Balance the charges to get the subscripts

Compounds that Contain Ions• compounds of metals with nonmetals are made

of ions– metal atoms form cations, nonmetal atoms for

anions• compound must have no total charge, therefore

we must balance the numbers of cations and anions in a compound to get 0 charge

• if Na+ is combined with S2-, you will need 2 Na+ ions for every S2- ion to balance the charges, therefore the formula must be Na2S

Writing Formulas for Ionic Compounds

1. Write the symbol for the metal cation and its charge2. Write the symbol for the nonmetal anion and its charge3. Charge (without sign) becomes subscript for other ion4. Reduce subscripts to smallest whole number ratio5. Check that the sum of the charges of the cation cancels

the sum of the anions

Write the formula of a compound made from aluminum ions and oxide ions

1. Write the symbol for the metal cation and its charge

2. Write the symbol for the nonmetal anion and its charge

3. Charge (without sign) becomes subscript for other ion

4. Reduce subscripts to smallest whole number ratio

5. Check that the total charge of the cations cancels the total charge of the anions

Al+3 column IIIA

O2- column VIA

Al+3 O2-

Al2 O3

Al = (2)∙(+3) = +6O = (3)∙(-2) = -6

Formula Mass• the mass of an individual molecule or

formula unit• also known as molecular mass or molecular

weight• sum of the masses of the atoms in a single

molecule or formula unit– whole = sum of the parts!

mass of 1 molecule of H2O = 2(1.01 amu H) + 16.00 amu O = 18.02 amu