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Chapter 2 Chapter 2 Atoms, Molecules, Atoms, Molecules, and Ions and Ions

Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

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Page 1: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Chapter 2Chapter 2

Atoms, Molecules, and Atoms, Molecules, and IonsIons

Page 2: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Chapter #2 – Atoms, Molecules and Ions

2.1 The Early History of Chemistry2.2 Fundamental Chemical laws2.3 Dalton’s Atomic Theory2.4 Cannizzaro’s Interpretation2.5 Early experiments to Characterize the Atom2.6 The Modern View of Atomic Structure: An Introduction2.7 Molecules and Ions2.8 An Introduction to the Periodic Table2.9 Naming Simple Compounds

Page 3: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Computer simulation of the interior view of a twisted nanotube.

Page 4: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 5: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Priestley Medal

Source: Roald Hoffman, Cornell University

Page 6: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 7: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Laws of Mass Conservation & Definite Proportions (Composition)

Law of Mass Conservation:

The total mass of substances does not change

during a chemical reaction.

Law of Definite ( or constant ) Composition:

No matter what its source, a particular

chemical compound is composed of the same

elements in the same parts (fractions) by mass.

Page 8: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 9: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.2: John Dalton

Source: Manchester Literary & Philosophical Society

Page 10: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Mass of Oxygen that Combines with 1.00g of Carbon

Compound #1 1.33g

Compound #2 2.66g

Page 11: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 12: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Law of Multiple Proportions

If elements A and B react to form two compounds,the different masses of B that combine with a fixed mass of A can be expressed as a ratio of small wholenumbers:

Example: Nitrogen Oxides I & II

Nitrogen Oxide I : 46.68% Nitrogen and 53.32% OxygenNitrogen Oxide II : 30.45% Nitrogen and 69.55% Oxygen

in 100 g of each Cpd: g O = 53.32 g & 69.55 g g N = 46.68 g & 30.45 g

g O /g N = 1.142 & 2.2842.284 2

1.142 1=

Page 13: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Mass of Nitrogen that Combines with 1.00g of Oxygen

Compound #1 1.750 g

Compound #2 0.8750 g

Compound #3 0.4375 g

I 1.750 2 Cpd #1 N2O NO N4O2

II 0.8750 1 II 0.8750 2 Cpd #2 NO or NO2 or N2O2

III 0.4375 1 I 1.750 4 Cpd #3 NO2 NO4 N2O4

III 0.4375 1

=

=

=

=

=

=

Page 14: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Dalton’s Atomic Theory

Postulates:

1. Each element is made up of tiny particles called atoms.

2. The atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways.

3. Chemical compounds are formed when atoms combine with each other. A given compound always has the same relative numbers and types of atoms.

4. Chemical reactions involve reorganization of the atoms – changes in the way they are bound together. The atoms themselves are not changed in a chemical reaction.

Page 15: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 16: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.3 (P19): Combining gases on a Molecular Level

Page 17: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Avogadro’s Hypothesis

At the same temperature and Pressure, equal volumes of different gases contain the same number of particles (Molecules).

Page 18: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Stanislao Cannizzaro

Source: Corbis

Page 19: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Cannizzaro’s Relative Atomic(Molecular) Masses of Carbon and Hydrogen

Compound Relative Percent Carbon Relative mass of Molecular Mass by Mass Carbon Present

Methane 16 75 12Ethane 30 80 24Propane 44 82 36Butane 58 83 48Carbon Dioxide 44 27 12

Compound Relative Percent Hydrogen Relative mass of Molecular Mass by Mass Hydrogen Present

Methane 16 25 4Ethane 30 20 6Propane 44 18 8Butane 58 17 10

Page 20: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Comparison of Several of Berzelius’sAtomic Masses with Current Values

Element Atomic Mass Berzelius’s Value Current Value

Chlorine 35.41 35.45Copper 63.00 63.55Hydrogen 1.00 1.01Lead 207.12 207.2Nitrogen 14.05 14.01Oxygen 16.00 16.00Potassium 39.19 39.10Silver 108.12 107.87Sulfur 32.18 32.07

Page 21: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.4: An STM image of nickel atoms placed on a copper surface.

Source: IBM Research

Page 22: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.5: Image of a ring of cobalt atoms placed on a copper surface.

Source: IBM Research

Page 23: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.6: A cathode-ray tube. The fast-moving electrons

Page 24: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.7: Deflection of cathode rays by an applied electric field.

Page 25: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 26: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 27: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.8: (P24)Thomson’sPlum Pudding model

Page 28: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.9: Schematic representation of the apparatus Millikan

Page 29: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 30: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 31: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Marie Sklodowska Curie

Source: Corbis

Page 32: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Rutherford Experiment

• Alpha particles bombarding the atom.

• Rationale - to study the internal structure of the atom, and to know more about the mass distribution in the atom!

• Bombarded a thin Gold foil with Alpha particles from Radium.

Page 33: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.11 (P25): Rutherford’s experiment

Page 34: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.12: The expected results of the metal foil experiment

Page 35: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 36: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 37: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 38: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Ernest Rutherford (1871-1937)

• Won the Nobel Prize in Chemistry in 1908

• “It was quite the most incredible event..... It was almost as if a gunner were to fire a shell at a piece of tissue and the shell bounced right back!!!!! ”

Page 39: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.13 (P26): Nuclear atom cross section

Page 40: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Modern Reassessment of the Atomic Theory

1. All matter is composed of atoms. Although atoms are composed of smaller particles (electrons, protons, and neutrons), the atom is the smallest body that retains the unique identity of the element.

2. Atoms of one element cannot be converted into atoms of another element in a chemical reaction. Elements can only be converted into other elements in Nuclear reactions in which protons are changed.

3. All atoms of an element have the same number of protons and electrons, which determines the chemical behavior of the element. Isotopes of an element differ in the number of neutrons, and thus in mass number, but a sample of the element is treated as though its atoms have an average mass.

4. Compounds are formed by the chemical combination of two or more elements in specific ratios, as originally stated by Dalton.

Page 41: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Atomic Definitions I: Symbols, Isotopes,Numbers

XA

Z

X = Atomic symbol of the element, or element symbol

A = The Mass number; A = Z + N

Z = The Atomic Number, the Number of Protons in the Nucleus

N = The Number of Neutrons in the Nucleus

Isotopes = atoms of an element with the same number of protons, but different numbers of Neutrons in the Nucleus

The Nuclear Symbol of the Atom, or Isotope

Page 42: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.2 (P 27) The Masses and Charges of the Electron Proton and Neutron

Particle Mass Charge*

Electron 9.11 x 10 – 31 kg -1

Proton 1.67 x 10 – 27 kg +1

Neutron 1.67 x 10 – 27 kg none

•The magnitude of the charge on the electron and proton is 1.60 x 10-19 coulombs .

Page 43: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 44: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.14(P28) Isotopes of sodium

Page 45: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 46: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Neutral ATOMS• 51 Cr = P+ (24), e- (24), • N (27)

• 239 Pu = P+(94), e- (94), • N (145)

• 15 N = P+(7), e-(7), N(8)

• 56 Fe = P+(26), e-(26),• N (30)

• 235 U =P+(92), e-(92), • N (143)

Page 47: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Definitions for Components of Matter

Pure Substances - Their compositions are fixed! Elements and compounds are examples of Pure Substances.Element - Is the simplest type of substance with unique physical and chemical properties. An element consists of only one type of atom. It cannot be broken down into any simpler substances by physical or chemical means.Molecule - Is a structure that is consisting of two or more atoms that are chemically bound together and thus behaves as an independent unit.Compound - Is a substance composed of two or more elements that are chemically combined.Mixture - Is a group of two or more elements and/or compounds that are physically intermingled.

Page 48: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.15: Space-filling model of the methane molecule

Page 49: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.17 : Ball-and-stick model

Page 50: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Chemical Formulas

Empirical Formula - Shows the relative number of atoms of each element in the compound. It is the simplest formula, and is derived from masses of the elements.

Molecular Formula - Shows the actual number of atoms of each element in the molecule of the compound.

Structural Formula - Shows the actual number of atoms, and the bonds between them ; that is, the arrangement of atoms in the molecule.

Page 51: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Definitions

Chemical Bonds – The forces that hold atoms together in compounds

Covalent Bonds – The sharing of electrons in a chemical bond

Molecule – A group of atoms held together by covalent bonds

Chemical Formula – The symbols of for the elements are used to indicate the types of atoms present, and the subscripts are used to indicate the relative numbers of atoms presentStructural Formula – a Formula in which the bonds are shown along with the elemental symbols and order of atom arrangement

Page 52: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Chemical Compounds and Bonds

Chemical Bonds - The electrostatic forces that hold the atoms of elements together in the compound.

Ionic Compounds - Electrons are transferred from one atom to another to form Ionic Cpds.

Covalent Compounds - Electrons are shared between atoms of different elements to form Covalent Cpds.

“Cations” - Metal atoms lose electrons to form “ + ” ions.

“Anions” - Nonmetal atoms gain electrons to form “ - ” ions.

Mono-atomic ions form binary ionic compounds

Page 53: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 54: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Molecular model: Electron transferred from sodium to chlorine (neutral sodium to

neutral sodium ion)

Page 55: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Molecular model: Electron added to chlorine (neutral chlorine to chloride ion)

Page 56: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.18 : Sodium metal reacts with chlorine gas

Page 57: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.19 (P31) :Na/Cl arrangement

Page 58: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.16 : Space-filling models of various molecules.

Page 59: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.20: Ball-and-stick models of the ammonium ion and nitrate ion.

Page 60: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Definitions• ELEMENT - A substance that cannot be separated into

simpler substances by chemical means

• COMPOUND - A substance composed of atoms of two or more elements chemically united in fixed proportions

• PERIODIC TABLE - “MENDELEEV TABLE” - A tabular arrangement of the elements, vertical groups or families of elements based upon their chemical properties - actually combining ratios with oxygen

Page 61: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

TABELLE IIR

EIH

EN GRUPPE I GRUPPE II GRUPPE III GRUPPE IV GRUPPE V GRUPPE VI GRUPPE VII GRUPPE VIII

RH4 RH3 RH2 RH R2O RO R2O3 RO2 R2O3 RO3 R2O7 RO4

12

34

56

78910

1112

H=1 Li=7 Be=9,4 B=11 C=12 N=14 O=16 F=19

Na=23 Mg=24 Al=27,3 Si=28 P=31 S=32 Cl=35,5K=39 Cd=40 ---=44 Ti=48 V=51 Cr=52 Mn=55 Fe=56, Cu=59 Ni=59, Cu=53 (Cu=63) Zn=65 ---=68 ---=72 As=75 Se=78 Br=80Rb=85 Sr=87 ?Yt=88 Zr=90 Nb=94 Mo=96 ---=100 Ru=104, Rh=104, Pd=106, Ag=108 (Ag=108) Cd=112 In=113 Sn=118 Sb=122 Te=125 J=127Cs=183 Ba=137 ?Di=138 ?Ce=140 --- --- --- --- --- --- --- (---) --- --- --- --- --- --- --- --- ?Er=178 ?Lo=180 To=182 W=184 --- Os=195, Ir=197 Pt=198, Au=199 (Au=199) Hg=200 Tl=204 Pb=207 Bi=208 --- --- -- --- --- Th=231 --- U=240 --- --- --- --- ---

Page 62: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Metals

Non Metals

Semi - metals Metalloids

B

Si

Ge As

Sb Te

C N

P

O

S

Se

F

Cl

Br

I

At

He

Ne

Ar

Kr

Xe

RnPoBi

Al

Ga

Sn

Pb

In

Tl

Zn

Cd

Hg

Cu

Ag

Au

NiCoFeMn

Pd

Pt

Rh

Ir

Ru

Os

Tc

Re

Sg

W

Mo

CrV

Nb

Ta

Ti

Zr

Hf

Rf

Sc

Y

La

Ac

Be

Mg

Ca

Sr

Ba

Ra

H

Li

Na

K

Rb

Cs

Fr

Ce Pr

Th

Nd Pm SmEu Gd Tb Dy Ho Er

Pa U Np PuAmCm Bk Cf Es FmMd

TmYb Lu

No Lr

Db Bh Hs Mt Ds

Page 63: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

O

S

Se

Te

Po

N

P

As

Sb

Bi

C

Si

Ge

Sn

Pb

B

Al

Ga

In

Tl

ZnCu

Cd

Hg

Ag

Au

Ni

Pd

Pt

Co

Rh

Ir

Fe

Ru

Os

Mn

Tc

Re

Cr

Mo

W

V

Nb

Ta

Ti

Zr

Hf

Sc

Y

La

Ac

The Periodic Table of the Elements

The Alkali Metals

The Alkaline Earth Metals

Ce Pr Nd PmSmEu Gd Tb Dy Ho Er TmYb Lu

Th Pa Np PuAmCmBk Cf Es FmMd No LrU

H

Li

Na

K

Rb

Cs

Fr

Be

Mg

Ca

Sr

Ba

Ra Rf Sg

The Halogens

The Noble Gases

He

Ne

Ar

Kr

Xe

Rn

F

Cl

Br

I

At

Db Bh Hs Mt Ds

Page 64: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Samples of the alkai metals

Source: Tom Pantages

Page 65: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Three members of the halogen family

Source: Tom Pantages

Page 66: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the ElementsH

Li Be

NaMg

K Ca Sc

Rb

Cs

Fr

Sr

Ba

Ra

Ti V CrMn Fe

Y

La

Ac

Co Ni Cu Zn

Zr

Hf

Nb

Ta

Rf

Mo

W

Tc

Re

Ru

Os

Rh

Ir

Pd

Pt

Ag

Au

Cd

Hg

F

He

Ne

ArCl

Br Kr

Xe

Rn

I

At

Ce Pr Nd Pm

Th

SmEu Gd Tb Dy Ho Er Tm Yb Lu

Pa U Np PuAmCm Bk Cf Es FmMd No Lr

Boron family

B

Al

Ga

In

Tl

Carbon Family

C

Si

Ge

Sn

Pb

Nitrogen family

N

P

As

Sb

Bi

Oxygen Family

O

S

Se

Te

Po

Db Sg Bh Hs Mt Ds

Page 67: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

O

S

Se

Te

Po

N

P

As

Sb

Bi

C

Si

Ge

Sn

Pb

B

Al

Ga

In

Tl

The Periodic Table of the Elements

Lanthanides: The

Rare Earth ElementsThe Actinides

F

Cl

Br

I

At

H He

Ne

Ar

Kr

Xe

Rn

Li

Na

K

Rb

Cs

Fr

Be

Mg

Ca

Sr

Ba

Ra

Ce

The Transition Metals

Pr Nd PmSmEu Gd Tb DyHo Er TmYb Lu

Th Pa U Np PuAmCmBk Cf Es FmMd No Lr

Sc Ti V CrMn

Y

La

Fe Co Ni Cu Zn

Zr NbMo Tc Ru Rh PdAg Cd

Hf Ta W Re Os Ir Pt Au Hg

Ac Rf Sg HsDb Bh MtDs

Page 68: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Groups in the Periodic Table

Main Group Elements (Vertical Groups) Group IA - Alkali Metals Group IIA - Alkaline Earth Metals Group IIIA - Boron Family Group IVA - Carbon Family Group VA - Nitrogen Family Group VIA - Oxygen Family (Calcogens) Group VIIA - Halogens Group VIIIA - Noble GasesOther Groups ( Vertical and Horizontal Groups)Group IB - 8B - Transition MetalsPeriod 6 Group - Lanthanides (Rare Earth Elements)Period 7 Group - Actinides

Page 69: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.21: The periodic table continues to expand as new elements are synthesized

Page 70: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the ElementsH

Li Be

NaMg

K Ca Sc

Rb

Cs

Fr

Sr

Ba

Ra

Ti V CrMn

Y

La

Ac

Co Ni Zn

Zr

Hf

Nb

Ta

Rf Db Sg

Mo

W

Tc

Re

Ru

Os

Rh

Ir

Pd

Pt

Cd

B N O F

He

Ne

ArAl Si Cl

Ga Ge Se Br Kr

Xe

Rn

ITe

AtPo

In

Tl

Ce Pr Nd Pm

Th

SmEu Gd Tb Dy Ho Er Tm Yb Lu

Pa U Np PuAmCm Bk Cf Es FmMd No Lr

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

1600 - 1700

C

Bh Hs Mt Ds

P

Page 71: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Sc

Rb

Cs

Fr

Sr

Ba

Ra

Ti V CrMn

Y

La

Ac

Ni

Zr

Hf

Nb

Ta

Rf Db Sg

Mo

W

Tc

Re

Ru

Os

Rh

Ir

Pd Cd

B N O F

He

Ne

ArAl Si Cl

Ga Ge Se Br Kr

Xe

Rn

ITe

AtPo

In

Tl

Ce Pr Nd Pm

Th

SmEu Gd Tb Dy Ho Er Tm Yb Lu

Pa U Np PuAmCm Bk Cf Es FmMd No Lr

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

CLi

Na

CaK ZnCo

Pt

H

Be

Mg

1600 - 1700

P

Bh Hs Mt Ds

Page 72: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Sc

Rb

Cs

Fr

Ba

Ra

V

La

Ac

Hf

Nb

Ta

Rf Db Sg

Tc

Re

Ru

Os

Rh

Ir

Pd Cd

B F

He

Ne

ArAl Si

Ga Ge Se Br Kr

Xe

Rn

I

AtPo

In

Tl

Ce Pr Nd Pm

Th

SmEu Gd Tb Dy Ho Er Tm Yb Lu

Pa Np PuAmCm Bk Cf Es FmMd No Lr

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

CLi

Na

CaK ZnCo

Pt

H

Be

Mg

Sr Y

Ti

Zr

CrMn

Mo

W

Ni

N O

Cl

1600 - 1700

P

Te

U

Bh Hs Mt Ds

Page 73: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Sc

Rb

Cs

Fr Ra Ac

Hf

Rf Db Sg

Tc

Re

F

He

Ne

Ar

Ga Ge Kr

Xe

RnAtPo

In

Tl

Pr PmSmEu Gd Dy Ho Tm Yb Lu

Pa Np PuAmCm Bk Cf Es FmMd No Lr

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

C

ZnCo

Pt

H

Be

Mg

Sr Y

Ti

Zr

CrMn

Mo

W

Ni

N O

Cl

1600 - 1700

P

Te

Li

Na

K Ca

Ba La

V

Nb

Ta

Ce

Os

Rh

Ir

Pd Cd

B

Al Si

Se Br

I

Nd Tb Er

Ru

Th U

Bh Hs Mt Ds

Page 74: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Fr

Hf

Rf Sg

Tc

Re At

Pm Lu

Pa Np PuAmCm Bk Cf Es FmMd No Lr

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

C

ZnCo

Pt

H

Be

Mg

Sr Y

Ti

Zr

CrMn

Mo

W

Ni

N O

Cl

1600 - 1700

P

Te

Li

Na

K Ca

Ba La

V

Nb

Ta

Ce

Os

Rh

Ir

Pd Cd

B

Al Si

Se Br

I

Nd Tb Er

Ru

Th

Sc

Rb

Cs

Ra Ac

Ga Ge

In

Tl Po

F

He

Ne

Ar

Kr

Xe

Rn

Pr SmEu Gd Dy Ho Tm

U

Yb

BhDb Hs Mt Ds

Page 75: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Rf Db Sg

At

Es FmMd No Lr

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

C

ZnCo

Pt

H

Be

Mg

Sr Y

Ti

Zr

CrMn

Mo

W

Ni

N O

Cl

1600 - 1700

P

Te

Li

Na

K Ca

Ba La

V

Nb

Ta

Ce

Os

Rh

Ir

Pd Cd

B

Al Si

Se Br

I

Nd Tb Er

Ru

Th

Sc

Rb

Cs

Ra Ac

Ga Ge

In

Tl Po

F

He

Ne

Ar

Kr

Xe

Rn

Pr SmEu Gd Dy Ho Tm

U

Tc

ReHf

Fr

Pa

Pm Yb Lu

Np PuAmCm Bk Cf

Bh Hs Mt Ds

Page 76: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

1700 - 1750

1750 - 1800

1800 - 1850

1850 - 1900

1900 - 1950

1950 - 2000

Before 1600

Fe

S

As

Sb

BiPb

Sn

HgAu

Ag

Cu

Date of Discovery of the Elements

C

ZnCo

Pt

H

Be

Mg

Sr Y

Ti

Zr

CrMn

Mo

W

Ni

N O

Cl

1600 - 1700

P

Te

Li

Na

K Ca

Ba La

V

Nb

Ta

Ce

Os

Rh

Ir

Pd Cd

B

Al Si

Se Br

I

Nd Tb Er

Ru

Th

Sc

Rb

Cs

Ra Ac

Ga Ge

In

Tl Po

F

He

Ne

Ar

Kr

Xe

Rn

Pr SmEu Gd Dy Ho Tm

At

Tc

ReHf

Fr

Pm Yb Lu

Pa U Np PuAmCm Bk Cf

Rf Sg Ds 111

LrEs FmMd No

Db Bh HsMt

Page 77: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the Elements

Number of Stable IsotopesH2Li2

Be1

Na1

Mg3

K2

Ca6

Sc1

Rb2

Cs1

Fr0

Sr4

Ba7

Ra0

Ti5

V2

Cr4

Mn1

Y1La2

Ac0

Co1

Ni5

Zn4

Zr5

Hf6

Nb1

Ta2

Rf0

Db0

Sg0

Mo7

W5

Tc0

Re2

Ru7

Os7

Rh1

Ir2

Pd6

Pt6

Cd8

B2

N2

O3

F1

He2

Ne3

Ar3

Al1

Si3

P1

Cl2

Ga2

Ge5

Se6

Br2

Kr6

Xe9

Rn0

I1

Te8

At0

Po0

In2

Tl2

Ce4

Pr1

Nd7

Pm0

Th0

Sm7

Eu2

Gd7

Tb1

Dy7

Ho1

Er6

Tm1

Yb7

Lu2

Pa0

U0

Np0

Pu0

Am0

Cm0

Bk0

Es0

Fm0

Md0

No0

Lr0

Fe4

S4

As1Sb2

Bi1

Pb4

Sn10

Hg7

Au1

Ag2

Cu2

C2

Bh0

Hs0

Mt Ds0 0

Cf0

There are a Total of 282 Stable Isotopes. If we look at the even to odd Isotopes we have a very great disparity, for odd numbered Isotopes there are 61 stable Isotopes, or 1.45 per Z#, for even numbered Isotopes there are 224 stable Isotopes, or 5.46 per Z#!

Page 78: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Newly Discovered Elements

Atomic No.

1994

ACS Slate IUPAC Slate

RevisedIUPAC Slate

104 Rutherfordium Dubnium Rutherfordium

105 Hahnium Joliotium Dubnium

106 Seaborgium Rutherfordium Seaborgium

107 Neilsbohrium Bohrium Bohrium

108 Hassium Hahnium Hassium

109 Meitnerium Meitnerium Meitnerium

110 Darmstadium Darmstadium Darmstadium

111 ? ? GSI

112 ? ? GSIFinal Slate 9/12/04

Page 79: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

The Periodic Table of the ElementsH

Li Be

Na Mg

K Ca Sc

Rb

Cs

Fr

Sr

Ba

Ra

Ti V CrMn Fe

Y

La

Ac

Co Ni Cu Zn

Zr

Hf

Nb

Ta

Rf Db Sg

Mo

W

Tc

Re

Ru

Os

Rh

Ir

Pd

Pt

Ag

Au

Cd

Hg

B C N O F

He

Ne

ArAl Si P S Cl

Ga Ge As Se Br Kr

Xe

Rn

ITe

At

Sb

PoBi

SnIn

PbTl

Ce Pr Nd Pm

Th

SmEu Gd Tb Dy Ho Er Tm Yb Lu

Pa U Np PuAmCm Bk Cf Es FmMd No Lr

Bh Hs Mt

“1997- 2004”

Ds

Page 80: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

He

Ne

Ar

Kr

Xe

Rn

The Periodic Table of the Elements

CrMn Fe Co Ni

Mo

W

Tc

Re

Ru

Os

Rh

Ir

Pd

Pt

Most Probable Oxidation State

+1

+2

+3 +4

+3 +_4 - 3 - 2 - 1

0

H

Li

Na

K

Rb

Cs

Fr

Sc

Y

Be

Mg

Ca

Sr

Ba

Ra

La

Ac

B

Al

Ga

In

Tl

Ti

Rf

Hf

Zr

C

Si

Ge

Sn

Pb

F

Cl

Br

I

At

O

S

Se

Te

Po

N

P

As

Sb

Bi

Zn

CdHg

+ 2+1

Cu

Ag

Au

+5

V

Nb

Ta

CeTh

Pr Nd PmSmEu Gd Tb Dy Ho Er TmYb LuPa U Np Pu AmCmBk Cf Es FmMd No Lr

+3

+3

Db Sg Bh Hs Mt Ds

Page 81: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 82: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.3(P35) Common Monatomic Cations and Anions

Cation Name Anion Name

H+ hydrogen H- hydride Li+ lithium F- fluoride Na+ sodium Cl- chloride K+ potassium Br- bromide Cs+ cesium I- iodide Be2+ beryllium O2- oxide Mg2+ magnesium S2- sulfide Ca2+ calcium N3- nitride Ba2+ barium P3- phosphide Al3+ aluminum Ag+ silver Zn2+ zinc

Page 83: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.4(P36) Common Type II Cations

Ion Systematic Name Alternate Name

Fe3+ iron (III) ferric Fe2+ iron (II) ferrous Cu2+ copper (II) cupric Cu+ copper (I) cuprous Co3+ cobalt (III) cobaltic Co2+ cobalt (II) cobaltous Sn4+ tin (IV) stannic Sn2+ tin (II) stannous Pb4+ lead (IV) plumbic Pb2+ lead (II) plumbous Hg2+ mercury (II) mercuric Hg2

2+ * mercury (I) mercurous

*Note that mercury (I) ions always occur bound together to form Hg22+

Page 84: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

A dish of copper (II) sulfate.

Source: Tom Pantages

Page 85: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Crystals of copper (II) sulfate

Page 86: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Like Example 2.2 (P 37)Give the systematic name of each of the following compounds:

a) Fe Cl3 d) B2O3 g) Na2O

b) SrF2 e) SnBr4 h) CsBr

c) MgS f ) Ca3N2

Solution:

a) iron (III) chloride e) Tin (IV) bromide

b) Strontium fluoride f ) Calcium Nitride

c) Magnesium Sulfide g) Sodium Oxide

d) Boron Oxide h) Cesium bromide

Page 87: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Does the compound contain Type I or Type II cations

Page 88: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Various chromium compounds dissolved in water

CrCl2

K2Cr2O7

Cr(NO3)3CrCl3

K2CrO4

Page 89: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.5 (P 38) Common Polyatomic IonsIon Name Ion Name

NH4+ ammonium CO3

2- carbonateNO2

- nitrite HCO3- hydrogen carbonate

NO3- nitrate (bicarbonate is a

SO32- sulfite used common name)

SO42- sulfate ClO- hypochlorite

HSO4- hydrogen sulfate ClO2

- chlorite (bisulfate is a widely ClO3

- chlorate used common name) ClO4

- perchlorateOH- hydroxide C2H3O2

- acetateCN- cyanide MnO4

- permanganatePO4

3- phosphate Cr2O72- dichromate

HPO42- hydrogen phosphate CrO4

2- chromateH2PO4

- dihydrogen phosphate O22- peroxide

Page 90: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.6 (P 39) Prefixes Used to Indicate Number in Chemical Names

Prefix Number Indicated

mono- 1di- 2tri- 3tetra- 4penta- 5hexa- 6hepta- 7octa- 8nana- 9deca- 10

Page 91: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.22: Flowchart for naming binary compounds

Page 92: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.23: Flowchart for overall strategy

for naming chemical compounds

Page 93: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Microtaggants

Source: Microtrace, Minneapolis, MN 55449

Page 94: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Like Example 2.3 (P 40) Give the systematic name of each of the following compounds

Compounds

a. Na3PO4 d. KClO4 g. NaIO3 b. K2SO4 e. KHCO3 h. NaOH c. CuCO3 f. Cs2SO3 Names

a. Sodium Phosphate e. Potassium Hydrogen Carbonate

b. Potassium Sulfate f. Cesium Sulfite c. Copper (II) Carbonate g. Sodium Iodiate

d. Potassium Perchlorate h. Sodium Hydroxide

Page 95: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Like Example 2.4 (P 42) Give the chemical formula of each of the following compounds

Names

a. Sodium Peroxide e. Lithium Hydrogen Carbonate b. Chromium (VI) Oxide f. Calcium Carbonate c. Aluminum Oxide g. Copper (II) Chloride d. Ammonium Carbonate h. Magnesium Perchlorate Compounds

a. Na2O2 e. LiHCO3

b. CrO3 f. CaCO3

c. Al2O3 g. Cu(Cl)2

d. (NH4)2CO3 h. Mg(ClO4)2

Page 96: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Naming Acids

1) Binary acids solutions form when certain gaseous compounds dissolve in water. For example, when gaseous hydrogen chloride (HCl) dissolves in water, it forms a solution called hydrochloric acid. Prefix hydro- + anion nonmetal root + suffix -ic + the word acid hydrochloric acid

2) Oxoacid names are similar to those of the oxoanions, except for two suffix changes: Anion “-ate” suffix becomes an “-ic” suffix in the acid. Anion “-ite” suffix becomes an “-ous” suffix in the acid. The oxoanion prefixes “hypo-” and “per-” are retained. Thus, BrO4

-

is perbromate, and HBrO4 is perbromic acid; IO2- is iodite, and

HIO2 is iodous acid.

Page 97: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Figure 2.24(P44): Naming acids

Page 98: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.7 (P 44) Names of Acids that do not Contain Oxygen

Acid Name

HF hydrofluoric acid

HCl hydrochloric acid

HBr hydrobromic acid

HI hydroiodic acid

HCN hydrocyanic acid

H2S hydrosulfuric acid

Page 99: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Table 2.8 (P 44) Names of some Oxygen- Containing Acids

Acid Name

HNO3 nitric acid

HNO2 nitrous acid

H2SO4 sulfuric acid

H2SO3 sulfurous acid

H3PO4 phosphoric acid

HC2H3O2 acetic acid

Page 100: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Naming of the Oxoacids of Chlorine

Acid Anion Name

HClO4 perchlorate perchloric acid

HClO3 chlorate chloric acid

HClO2 chlorite chlorous acid

HClO hypochlorite hypochlorous acid

Page 101: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Rules for Families of OxoanionsFamilies with Two Oxoanions

The ion with more O atoms takes the nonmetal root and the suffix “-ate”.

The ion with fewer O atoms takes the nonmetal root and the suffix “-ite”.

Families with Four Oxoanions (usually a Halogen)The ion with most O atoms has the prefix “per-”, the nonmetal root and the suffix “-ate”.

The ion with one less O atom has just the suffix “-ate”.

The ion with two less O atoms has the just the suffix “-ite”.

The ion with three less O atoms has the prefix “hypo-” and thesuffix “-ite”.

Page 102: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

NAMING OXOANIONS - EXAMPLES

Prefixes Root Suffixes Chlorine Bromine Iodine

per “ ” ate perchlorate perbromate periodate [ ClO4

-] [ BrO4-] [ IO4

-] “ ” ate chlorate bromate iodate [ ClO3

-] [BrO3-] [ IO3

-]

“ ” ite chlorite bromite iodite [ ClO2

-] [ BrO2-] [ IO2

-]

hypo “ ” ite hypochlorite hypobromite hypoiodite [ ClO -] [ BrO -] [ IO -]

No.

of

O a

tom

s

Page 103: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Predicting the Ion an Element will form in Chemical Reactions

Problem: What monoatomic ions will each of the elements form?(a) Barium(z=56) (b) Sulfur(z=16) (c) Titanium(z =22) (d) Fluorine(z=9)Plan: We use the “z” value to find the element in the periodic table and which is the nearest noble gas. Elements that lie after a noble gas will lose electrons, and those before a noble gas will gain electrons.Solution: (a) Ba+2, Barium is an alkaline earth element, Group 2A, and is expected to lose two electrons to attain the same number of electrons as the noble gas Xenon! (b) S -2, Sulfur is in the Oxygen family, Group 6A, and is expected to gain two electrons to attain the same number of electrons as the noble gas Argon! (c) Ti+4, Titanium is in Group 4B, and is expected to loose 4 electrons to attain the same number of electrons as the noble gas Argon! (d) F -, Fluorine is in a halogen, Group 7A, and is expected to gain one electron, to attain the same number of electrons as the noble gas Neon!

Page 104: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Give the Name and Chemical Formulas of the Compounds formed from the following pairs of Elements

a) Sodium and Oxygen Na2O Sodium Oxide

b) Zinc and Chlorine ZnCl2 Zinc Chloride c) Calcium and Fluorine CaF2 Calcium Fluoride

d) Strontium and Nitrogen Sr3N2 Strontium Nitride

e) Hydrogen and Iodine HI Hydrogen Iodide

f) Scandium and Sulfur Sc2S3 Scandium Sulfide

Page 105: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Determining Names and Formulas of Ionic Compounds of Elements That Form More Than One Ion.

Give the systematic names for the formulas or the formulas for the names of the following compounds.

a) Iron III Sulfide - Fe is +3, and S is -2 therefore the compound is: Fe2S3

b) CoF2 - the anion is Fluoride (F -1) and there are two F -1, the cation is Cobalt and it must be Co+2 therefore the compound is: Cobalt (II) Fluoridec) Stannic Oxide - Stannic is the common name for Tin (IV), Sn+4, the Oxide ion is O-2, therefore the formula of the compound is: SnO2

d) NiCl3 - The anion is chloride (Cl-1), there are three anions, so the Nickel cation is Ni+3, therefore the name of the compound is: Nickel (III) Chloride

Page 106: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Hydrates Compounds containing Water molecules

MgSO4 7H2O Magnesium Sulfate heptahydrate

CaSO4 2H2O Calcium Sulfate dihydrate

Ba(OH)2 8H2O Barium Hydroxide octahydrate

CuSO4 5H2O Copper II Sulfate pentahydrate

Na2CO3 10H2O Sodium Carbonate decahydrate

Page 107: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Examples of Names and Formulas of Oxoanions and Their Compounds - I

• KNO2 Potassium Nitrite BaSO3 Barium Sulfite

• Mg(NO3)2 Magnesium Nitrate Na2SO4 Sodium Sulfate

• LiClO4 Lithium Perchlorate Ca(BrO)2 Calcium Hypobromite

• NaClO3 Sodium Chlorate Al(IO2)3 Aluminum Iodite

• RbClO2 Rubidium Chlorite KBrO3 Potassium Bromate

• CsClO Cesium Hypochlotite LiIO4 Lithium Periodate

Page 108: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Examples of Names and Formulas ofOxoanions and their Compounds - II

• Calcium Nitrate Ca(NO3)2 Ammonium Sulfite (NH4)2SO3

• Strontium Sulfate SrSO4 Lithium Nitrite LiNO2

• Potassium Hypochlorite KClO Lithium Perbromate LiBrO4

• Rubidium Chlorate RbClO3 Calcium Iodite Ca(IO2)2

• Ammonium Chlorite NH4ClO2 Boron Bromate B(BrO3)3

• Sodium Perchlorate NaClO4 Magnesium Hypoiodite Mg(IO)2

Page 109: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions

a) BaCl2 5 H2O Ba+2 is the cation Barium, Cl- is the Chloride anion. There are five water molecules thereforethe name is: Barium Chloride Pentahydrate

b) Magnesium Perchlorate Magnesium is the Mg+2 cation, and perchlorate is the ClO4

- anion, therefore we need two perchlorate anions for each Mg cation therefore the formula is: Mg( ClO4)2

c) (NH4)2SO3 NH4+ is the ammonium ion, and SO3

-2 is the sulfite anion, therefore the name is: Ammonium Sulfite

d) Calcium Nitrate Calcium is the Ca+2 cation, and nitrate is the NO3

- anion, therefore the formula is: Ca(NO3)2

Page 110: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Determining Names and Formulas ofAnions and Acids

Problem: Name the following anions and give the names and

formulas of the acid solutions derived from them:

a) I - b) BrO3- c) SO3

-2 d) NO3- e) CN -

Solution: a) The anion is Iodide; and the acid is Hydroiodic acid, HI

b) The anion is Bromate; and the acid is Bromic acid, HBrO3

c) The anion is Sulfite; and the acid is Sulfurous acid, H2SO3

d) The anion is Nitrate; and the acid is Nitric acid, HNO3

e) The anion is Cyanide; and the acid is Hydrocyanic acid, HCN

Page 111: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Determining Names and Formulas of Binary Covalent Compounds

Problem: What are the name or Chemical formulas of the followingChemical compounds:

a) Carbon dioxide b) PCl3 c) Give the name and chemical formula of the compound formed from two P atoms and five O atoms.

Solution:

a) The prefix “di-” means “two.” The formula is CO2

b) P is the symbol for phosphorous; there are three chlorine atoms which require the prefix “tri-.” The name of the compound is: phosphorous trichloride

c) P comes first in the name (lower group number). The compound is diphosphorous pentaoxide ( commonly called “phosphorous pentaoxide”)

Page 112: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Calculating the Molecular Mass of a Compound

Problem: Using the data in the periodic table, calculate the molecular mass of the following compounds: a) Tetraphosphorous decoxide b) Ammonium sulfatePlan: We first write the formula, then multiply the number of atoms (or ions) of each element by its atomic mass, and find the sum.Solution:

a) The formula is P4O10. Molecular mass = (4 x atomic mass of P ) +(10 x atomic mass of O ) = ( 4 x 30.97 amu) + ( 10 x 16.00 amu) = 283.88 = ___________amub) The formula is (NH4)2SO4

Molecular mass = ( 2 x atomic mass of N ) + ( 8 x atomic mass of H) + ( 1 x atomic mass of S ) + ( 4 x atomic mass of O) = ( 2 x 14.01 amu) + ( 8 x 1.008 amu) + ( 1 x 32.07 amu) + ( 4 x 16.00 amu) = 132.154 amu = ____________ amu

Page 113: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

Calculate the Molecular Mass of Glucose: C6H12O6

• Carbon 6 x 12.01 g/mol = 72.06 g

• Hydrogen 12 x 1.008 g/mol = 12.096 g

• Oxygen 6 x 16.00 g/mol = 96.00 g

g

Page 114: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s
Page 115: Chapter 2 Atoms, Molecules, and Ions. Chapter #2 – Atoms, Molecules and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical laws 2.3 Dalton’s

A space-filled model of C60 containing

a "caged" methanol molecule

Source: Photo Researchers


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