Atomic Theory and Structure

Unit 2

Atomic Theory Based on experimental data

Elements are made of only one kind of particle.

This basic particle is called an atom

Dalton’s Atomic Theory All matter is composed of very small particles called atoms.

Atoms of a given element are identical; atoms of different elements are different.

Atoms cannot be subdivided, created or destroyed. [LAW OF CONSERVATION OF MATTER]

Atoms of different elements combine in simple whole-number ratios (1:1, 1:2, 3:5, etc.) to form chemical compounds. [Law of Definite Proportions]

In chemical reactions, atoms are combined, separated, or rearranged.

Modern Atomic Theory Atoms of the same element may have

different masses (isotopes), but will always have the same atomic #.

Atoms are made of smaller particles.

Changing Models of the Atom

Dalton’s Model 1830

Major change: particle model

Physical model: solid spheres, billiard balls Could not be created,

divided into smaller particles, or destroyed

J.J. Thomson Model 1898

Major change: protons and electrons

Physical model: plum pudding Negatively charged

electrons were distributed throughout a uniform positive charge

Rutherford’s Model 1911

Major change: nucleus

Physical model: solar system model Electrons orbit around

the nucleus which contains proton and neutrons

Bohr’s Model 1931

Major change: energy levels

Physical model: energy level model Protons and neutrons

located within the nucleus but electrons are located on orbitals with different energy levels

Quantum, Wave mechanical,Schrodinger Late 1930’s

Major change: uncertainty principle

Physical model: cloud model Atom consist of cloud of

electrons around a very small nucleus of protons and neutrons

Evolution of the Atom

Properties of Particles That Make-Up the AtomParticle Mass Rel.

MassCharge Rel.

ChargeLocation

Electron 9.110 x 10-28 0 -1.602x10-19 -1 e-

cloud

Proton 1.673 x 10-24 1 +1.602x10-19 +1 Nucleus

Neutron 1.675 x 10-24 1 zero 0 Nucleus

STOP

Atomic Structure Continued…

Facts About The Atom All atoms are electrically neutral; therefore an

atom must have equal numbers of protons and electrons.

Any atom of a given element contains the same number of protons as any other atom of that element. (this also applies to electrons.)

For a given element, two different atoms of that element may contain differing numbers of neutrons. (definition of an isotope)

Characteristics of Atoms Atomic number- The number of protons in the nucleus of the atom. In a neutral atom,

this is also the number of electrons.

Mass number- The total number of particles in the nucleus of the atom. # protons + # neutrons

AZX

A: mass number & z: atomic number

Isotopes- Atoms with the same atomic numbers but different mass numbers. That is, with the same number of electrons and protons, but different numbers of neutrons.

Nucleus- Very small and very positive. Contains most of the mass of the atom. Made up of protons and neutrons.

Nuclear forces- Hold the protons and neutrons together in the nucleus.

Isotopes atoms of the same element with different numbers

of neutrons and therefore different atomic mass. Example: carbon-12 and carbon-14 Isotopes of Hydrogen

Protium Hydrogen-1 Protons___ Electrons___ Neutrons___

Deuterium Hydrogen-2 Protons___ Electrons___ Neutrons___

Tritium Hydrogen-3 Protons___ Electrons___ Neutrons___

Law of Multiple ProportionsA compound consists of molecules of integral

numbers of atoms. In a series in which one element forms more than one compound with a second element, the atoms must

combine in small integral numbers. Hence, the weights of the second element

combining with a fixed weight of the first element will be in the ratio of small integral

numbers.

Compound g of oxygen combining with 1g of nitrogen

Ratio of weights

Atomic grouping

Nitrous oxide

0.57 1 NO

Nitricoxide

1.14 2 NO2

Nitrogen trioxide

1.71 3 NO3

Nitrogen tetroxide

2.28 4 NO4

Nitrogen pentoxide

2.85 5 NO5