Lead II carbonateFormulas:

SnO2NAMING:

Period 8 Day 5

11-5

Naming:

Acids are named for their anions

Binary: hydro – anion base – ic ending – the word “acid”

Acid - Compound that yields H+ ions (always starts with an H) – molecular compounds that act like ionics

Naming:

Acids are named for their anions

Binary: hydro – anion base – ic ending – the word “acid”

Non-binary: ate ending becomes ic, ite ending becomes ous

Examples:HF HBr HNO3 HNO2

Naming:

Acids are named for their anions

Binary: hydro – anion base – ic ending – the word “acid”

Non-binary: ate ending becomes ic, ite ending becomes ous

Examples:Hydrochloric acid

Sulfurous acid

sulfuric acid

hydrofluoric acid

carbonic acid

Formulas:

HC2H3O2

HCl

H2SO3

NAMING:

# 2.57 (parts a-g) AND 2.58 (parts a-e) AND 2.59 (parts a-f)

BINDERS!!!

Lead II carbonate

Phosphoric acid

Formulas:

H2SO4

SnO2

NAMING:

Periods 1 + 3 Day 5 11-5

Phosphorous acid

nickel III oxide

Formulas:

Pb(CO3)2

HClO3

NAMING:

Periods 3 + 8 Day 6 11-6

Ionic Compounds & Polyatomic Ions

Oxyanions – polyatomic ions that contain oxygen

ate = ending for most common ion (ClO3- Chlorate)

ite = ending for one less oxygen (ClO2- Chlorite)

hypo = prefix for another less oxygen (ClO - Hypochlorite)

per = prefix for one more than most common (ClO4-

Perchlorate)

Molecule – group of atoms united by covalent bonds (molecules = molecular substance)

FORMULAS

Empirical - simplified ratio Molecular - How many atoms in a

single molecule (not always a simplified ratio, glucose = C6H12O6)

FORMULAS

Empirical - Simplified ratio Molecular - How many atoms in a

single molecule (not always a simplified ratio, glucose = C6H12O6)

Structural - Specifies which atoms are bonded to each other (organic chem)

Molecular Element – molecule of atoms of same element – NOT a compound - like O2, Cl2, O3

H BrONClIF = diatomic molecules - these elements naturally occur as diatomic molecules and not

singular atoms

Binary Molecular CompoundsBased on Prefixes

1. Less electronegative first – prefix only if more than one atom

2. Second element – prefix, root of name, ending ide (if only two elements)

3.o or a @ the end of prefix is dropped if name begins with a vowel (monooxide, monoxide)

PAGE 60

Mono 1

Di 2

Tri 3

Tetra 4

Penta 5

Hexa 6

Hepta 7

Octa 8

Nona 9

Deca 10

Binary Molecular

Compounds – prefix system

Write the Name:N2O5

SbF3

Dinitrogen pentoxide

Antimony trifluoride

Binary Molecular Compounds

Write the Formula:

Germanium tetraiodide

diphosphorous trioxide

GeI4

P2O3

Binary Molecular Compounds

Write the Name:As2O5

ICl3

diarsenic pentoxide

iodine trichloride

Write the Formula:

carbon tetraiodide

dinitrogen trioxide

CI4

N2O3

Phosphorous acid

nickel III oxide

Formulas:

Pb(CO3)2

HClO3

NAMING:

Period 1 Day 6

11-6

For each compound below, what type is it (covalent, acid, or ionic), and write the name.

NO2

HNO3

Co3(PO4)2

Day 1 11-9

Green = halogens

Black = carbons

White = hydrogens

Red = oxygen

Blue = nitrogen

Grey / purple = metal

Formulas Names

For each compound below, what type is it (covalent, acid, or ionic), and write the name.

HC2H3O2

Cu3PO3

SF6

Day 2 11-10

23

• Molecular compounds− Nonmetals or nonmetals + metalloids− Common names

− H2O, NH3, CH4

− Element furthest to the left in a period and closest to the bottom of a group on periodic table is placed first in formula

− If more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom

− Last element name ends in -ide

24

HI hydrogen iodide

NF3 nitrogen trifluoride

SO2 sulfur dioxide

N2Cl4 dinitrogen tetrachloride

NO2 nitrogen dioxide

N2O dinitrogen monoxide

Molecular Compounds

Example 2.7

Name the following molecular compounds:

(a)SiCl4

(b)P4O10

Example 2.7

Strategy

We refer to Table 2.4 for prefixes.

In (a) there is only one Si atom so we do not use the prefix “mono.”

Solution

(a)Because there are four chlorine atoms present, the compound is silicon tetrachloride.

(b)There are four phosphorus atoms and ten oxygen atoms present, so the compound is tetraphosphorus decoxide. Note that the “a” is omitted in “deca.”

Example 2.8

Write chemical formulas for the following molecular compounds:

(a)carbon disulfide

(b) disilicon hexabromide

Example 2.8

Strategy

Here we need to convert prefixes to numbers of atoms (see Table 2.4).

Because there is no prefix for carbon in (a), it means that there is only one carbon atom present.

Solution

(a)Because there are two sulfur atoms and one carbon atom present, the formula is CS2.

(b) There are two silicon atoms and six bromine atoms present, so the formula is Si2Br6.

29

30

An acid can be defined as a substance that yields hydrogen ions (H+) when dissolved in water.

For example: HCl gas and HCl in water

•Pure substance, hydrogen chloride

•Dissolved in water (H3O+ and Cl−), hydrochloric acid

31

32

An oxoacid is an acid that contains hydrogen, oxygen, and another element.

HNO3 nitric acid

H2CO3 carbonic acid

H3PO4 phosphoric acid

33

Naming Oxoacids and Oxoanions

34

The rules for naming oxoanions, anions of oxoacids, are as follows:1. When all the H ions are removed from the “-ic”

acid, the anion’s name ends with “-ate.” 2. When all the H ions are removed from the “-ou

s” acid, the anion’s name ends with “-ite.”3. The names of anions in which one or more but

not all the hydrogen ions have been removed must indicate the number of H ions present.

For example:– H2PO4

- dihydrogen phosphate– HPO4 2- hydrogen phosphate– PO4

3- phosphate

35

Example 2.9

Name the following oxoacid and oxoanion:

(a)H3PO3

Example 2.9

Strategy To name the acid in (a), we first identify the reference acid, whose name ends with “ic,” as shown in Figure 2.15.

Solution

(a)We start with our reference acid, phosphoric acid (H3PO4). Because H3PO3 has one fewer O atom, it is called phosphorous acid.

38

A base can be defined as a substance that yields hydroxide ions (OH-) when dissolved in water.

NaOH sodium hydroxide

KOH potassium hydroxide

Ba(OH)2 barium hydroxide

Hydrate – ionic substances that absorb water into their solid structures

Anhydrous substance – opposite of hydrates (water-free)

Namin

g1. Name ionic compound

2. use prefix to name hydrate

Name

CuSO4 • 5 H2O

MgSO4 • 7 H2O

Copper (II) sulfate pentahydrate

Magnesium sulfate heptahydrate

Formula

Calcium sulfate dihydrate CaSO4 • 2 H2O

41

Hydrates are compounds that have a specific number of water molecules attached to them.

BaCl2•2H2O

LiCl•H2O

MgSO4•7H2O

Sr(NO3)2 •4H2O

barium chloride dihydrate

lithium chloride monohydrate

magnesium sulfate heptahydrate

strontium nitrate tetrahydrate

CuSO4•5H2O CuSO4

42

43

Organic chemistry is the branch of chemistry that deals with carbon compounds.

C

H

H

H OH C

H

H

H NH2 C

H

H

H C OH

O

methanol methylamine acetic acid

Functional Groups:

44