Chapter 3. Brief History of Electricity 1. Ancient Greeks discovered that if a piece of amber were...

Chapter 3

Brief History of Electricity1. Ancient Greeks discovered that if a piece of amber were rubbed with fur- pieces attracted each other. Later attributed to opposite charges (+ and -) – called static electricity

2. Benjamin Franklin – mid 1700’s – showed that lightning was a form of static electricity

Alessandro Volta – 1800 – First battery

G. Johnstone Stoney – 1874 – coined the word “electron” for the basic unit of electricity

By the end of the 19th Century scientists had discovered that the atom was not solid and indivisible as Dalton had proposed. Several important experiments led to these discoveries. Let’s look at 2 of them:

1. J.J. Thompson and the Crookes Tube Experiment

A) Led to discovery of electrons as basic unit of negative charge, found randomly inside atom.

B) Plum-Pudding Model of the atom

Cathode Rays are electrons

2. Ernest Rutherford and discovery of the nuclear atom

A) Natural radioactivity – 3 types – alpha particles (), beta particles () and gamma radiation ()

B) Gold foil Experiment

C) Nuclear Model of the atomElectrons m

ake up only about 1%

of the total mass o

f the atom

atom

Nucleus: positive charge very dense[very

small(less than 1% of the entire

space in the atom) but contains

almost all the mass of the atom]

C) Nuclear Model of the atom

First modelAfter discovery of neutrons

Summary of particles inside atom:

Particle Symbol Location Relative Charge Relative Mass

(Mass #)

Electron e- Outside nucleus - 1 0.005 ≈ 0

Proton p+ Inside nucleus + 1 1.000Neutron n0 Inside nucleus 0 1.000

Atomic Number (Z) – The number of protons in an atom.

Also the number of electrons in a neutral atom. Unique for

each element. Identifies the element.

•Mass Number – The number of protons + the number of neutrons in an atom. For example: An atom with 5 protons and 7 neutrons•Mass # = 5p+ + 7n0 = 12•This number is not unique for each element. All but one element have atoms with different numbers of neutrons and therefore different mass numbers. •For example, there are 3 different atoms of C found in Nature, all having 6 protons, but one having 6 neutrons, one 7 neutrons and one with 8 neutrons. What are their Mass Numbers? •These 3 atoms are called isotopes of C. Isotopes are atoms of the same element with different Mass Numbers.

Isotopic Symbols - C126

Mass #Atomic #

•Atomic Weight (AW) or better Atomic Mass – The relative

weight of an average atom of one element compared to that

of another atom chosen to be the standard.

•The modern standard is the C-12 isotope (arbitrarily

assigned a value of 12.0000 amu (atomic mass unit).

Actually the AW of an element is the average (taking into

account the relative amount of each) mass of all the naturally

found isotopes.

•This is the non-whole # found under each element in the

Periodic Table.

Bohr Model – Also called Solar System Model. Nucleus

with electrons revolving around in orbits of specific energies

(called Energy levels)

Niels Bohr – Danish - 1912

•Each successive orbit has a maximum # of electrons that

can exist (2, 8, 18, 32, 50 etc) We will only worry about the

first 20 elements. For these the maximum # of electrons is 2

for the first and 8 for the rest (actually 18 in the third, but the

last 10 are not important for us in this course).

•For every atom the electrons fill up the orbits in order

beginning with the lowest energy. The closer to the nucleus,

the lower the energy. In other words Li has an atomic # of 3,

therefore 3 electrons (2 in the first level and 1 in the next).

•See the following table. The electrons in the outermost energy

level are called Valence electrons and that level is called the

Valence Shell.

Dimitri Mendeleev and the Periodic Table

Modern Version

• Names of Families

• Metals, Non-metals and metalloidsand Noble Gases

• Representative elements and transition metals

Modern Periodic Table:

1. Metals – Left side - a) Properties – Shiny, malleable, ductile, conduct

electricity & heat

2. Non-Metals – Right Side b) Properties – Brittle as solids, non-conductors

3. Metalloids – In between c) Properties – Some of both metals & non-metals

4. Noble Gases – Far Right Column d) Properties – All are gases even at very low temperatures, non-conductors, very little tendency to chemically react

Representative Elements – Those in columns headed by an A (IA, IIA etc). We will spend most of our time dealing with these elements.

Transition Metals – Those in columns headed by a B.

Inner Transition Elements – Bottom 2 rows