NAME THAT COMPOUND

ACTIVITY

1

Minute to Name It!

A list of chemical formula and names

would be shown on the screen.

Each student would need to identify the

corresponding name (if a formula is given)

or formula (if a name is given).

2

Li2Se

AlCl3

Sr3P2

BaI2

Mg2N2

Ferric oxide

Ferrous oxide

Chromium(II) sulfide

Chromium(III) oxide

Lead(IV) oxide

CsCl

NaBr

BeCl2

Al2O3

BaS

Copper(II) telluride

Mercury(II) oxide

Stannic fluoride

Plumbous bromide

Copper(I) chloride

KF

CaC2

MgH2

BeCl2

Cd3P2

Cobalt(II) fluoride

Lead(IV) oxide

Nickel(II) phosphide

Lead(IV) sulfide

Nickel(II) iodide

Li2Se Lithium selenide

AlCl3 Aluminum chloride

Sr3P2 Strontium phosphide

BaI2 Barium iodide

Mg3N2 Magnesium nitride

KF Potassium fluoride

CaC2 Calcium carbide

MgH2 Magnesium hydride

BeCl2 Beryllium chloride

Cd3P2 Cadmium phosphide

CsCl Cesium chloride

NaBr Sodium bromide

BeCl2 Beryllium chloride

Al2O3 Aluminum oxide

BaS Barium sulfide

Fe2O3 Ferric oxide

FeO Ferrous oxide

CrS Chromium(II) sulfide

Cr2O3 Chromium(III) oxide

PbO2 Lead(IV) oxide

CuTe Copper(II) telluride

HgO Mercury(II) oxide

SnF4 Stannic fluoride

PbBr2 Plumbous bromide

CuCl Copper(I) chloride

CoF2 Cobalt(II) fluoride

PbO2 Lead(IV) oxide

Ni3P2 Nickel(II) phosphide

PbS2 Lead(IV) sulfide

NiI2 Nickel(II) iodide

Stoichiometry of Formulas and

Equations

CHAPTER 3

Burning Magnesium

7

Chemical reaction:

2 Mg(s) + O2(g) 2 MgO(s)

How do we look at this in terms of mass?

48 amu 32 amu 80 amu

? grams ? grams ? grams

Mole (abbreviated mol)

8

SI unit for amount of substance

Number of entities as there are atoms in exactly 12 g of 12C

Equal to 6.022 x 1023 entities

Called the Avogadro’s number

How big is Avogadro’s Number?

9

Spreading 1 mole of marbles over the entire surface of the earth

would produce a blanket of marbles almost 5 km high.

Avogadro’s Number: 602,200,000,000,000,000,000,000

College

tuition

World

population

Distance from

earth to sun (cm)

Age of the

earth (s)

Volume of world’s

oceans (L)

A mole of water

10

A mole of other substances

11

O2 (g)

32.00 g

H2O (l)

18.02 g

Cu (s)

63.55 g

CaCO3

100.09 g

1 mole of Fe vs 1 mole of S

12

The mole allows us to count out exactly the same number of things but use mass to do it!

1 mole Fe

6.022 x 1023 Fe atoms

55.85 g Fe

1 mole S

6.022 x 1023 S atoms

32.07 g S

Molecular Mass and Molar Mass

13

The molecular mass (or molecular weight) is the sum of the

atomic masses (in amu) in a single molecule.

The molar mass of a covalent compound is numerically equal

to the molecular mass, but in grams per mole.

Formula Mass and Molar Mass

14

The formula mass (or formula weight) is the sum of the

atomic masses (in amu) in a formula unit.

The molar mass of an ionic compound is numerically equal

to the formula mass, but in grams per mole.

Summary of Different Mass Terms

15

Term Definition Unit

Isotopic Mass Mass of an isotope of an

element

amu

Atomic Mass

(aka Atomic Weight)

Weighted average mass of an

element’s naturally occurring

isotopes

amu

Molecular or

Formula Mass

(aka Molecular or

Formula Weight)

Sum of the atomic masses of

the atoms (or ions) in a

molecule (or formula unit)

amu

Molar Mass Mass of 1 mole of a chemical

entity (e.g. atoms, ions,

molecules, or formula units)

grams per

mole (g/mol)

Practice Problem

16

What is the molecular mass of glucose (C6H12O6)?

Molecular Mass:

6 x 12.011 + 12 x 1.007 + 6 x 15.99 = 180.16 amu

Practice Problem

17

Complete the table below for glucose (C6H12O6,

MW = 180.16 g/mol)

Carbon Hydrogen Oxygen

Atoms in 1

glucose molecule

Mass C/H/O in 1

glucose molecule

Atoms per mole

of compound

Moles of atoms

in 1 mole cmpd

Mass per 1 mole

of compound

6 12 6

6 x 12.01 =

72.06 amu

12 x 1.008 =

12.10 amu

6 x 15.99 =

96.00 amu

6 (6.022x1023)

atoms 12 (6.022x1023)

atoms

6 (6.022x1023)

atoms

6 moles of

atoms

12 moles of

atoms

6 moles of

atoms

72.06 g 12.10 g 96.00 g

What’s in a Chemical Formula?

18

2 atoms of Al and 3 molecules of (SO4)2-

1 formula unit of Al2(SO4)3 = 342.17 amu

1 mole Al2(SO4)3 = 342.17 g Al2(SO4)3

1 mole Al2(SO4)3 = 6.022 x 1023 formula units Al2(SO4)3

1 mole Al2(SO4)3 = 2 moles Al3+ ions

1 mole Al2(SO4)3 = 3 moles (SO4)2- ions

1 mole Al2(SO4)3 = 12 moles O atoms = 12 x A.N. O atoms

1 mole Al2(SO4)3 = 3 moles S atoms = 3 x A.N. S atoms

1 mole Al2(SO4)3 = 2 moles Al atoms = 2 x A.N. Al atoms

Al2(SO4)3 (s)

Conversion Factors in a Molecular Formula

19

1 molecule of H2O = 2 H atoms and 1 O atom

Molecular mass = (2 x 1.008) + 15.99 = 18.00 amu

Molar mass = 18.00 g/mol H2O

1 mole of H2O = 6.022 x 1023 molecules of H2O

1 mole of H2O = 2 mol H atoms = 2 (6.022x1023) H atoms

1 mole of H2O = 1 mol O atoms = 1 (6.022x1023) O atoms

H2O (l)

Conversion Among Different Quantities

20

Practice Problem

21

1. Silver is often used in jewellery and tableware.

How many grams of Ag are in 0.0342 mol Ag?

2. Iron, the main component of steel, is the most

important metal in industrial society. How many

Fe atoms are in 95.8 g of Fe?

3. Urea, (NH2)2CO, is a nitrogen-containing

compound used as a fertilizer. How many

molecules of urea are in a 25.6 g sample?

4. How many hydrogen atoms are present in a

25.6 g sample of urea, (NH2)2CO?

Practice Problem

22

The plant photosynthetic pigment

chlorophyll contains 2.68% magnesium by

weight. How many atoms of Mg will there

be in 1.00 g of chlorophyll?