Chapter 5 – Atomic Structure

Atoms Structure of An

Atom Distinguish Between

Atoms The Periodic Table

Ch 5.1 Atoms

Democritus of Abdera (Greece)

4th Century BC Coined the term

“atom” Could not prove

because no scientific research was being done

John Dalton (1766-1844)

Conducted research as to the ratios of elements in compounds

From the research he came up with Daltons Atomic Theory

Dalton’s Atomic Theory

1. All elements are composed of tiny indivisible particles called atoms.

Dalton’s Atomic Theory

2. Atoms of the same element are identical. The atoms of one element are different from those of any other element.

Dalton’s Atomic Theory

3. Atoms of different elements can physically mix together or can chemically combine with one another in simple whole number ratios to form compounds.

Dalton’s Atomic Theory

4. Chemical reactions occur when atoms are separated, joined or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction.

                                                           

Atom

The smallest particle of an element that retains the properties of that element.

Just How Small is an Atom

A pure copper coin about the size of a penny has 2.4 x 1022 atoms

2,400,000,000,000,000,000,000,000 atoms Earths population is only 6 x 109 people

Just How Small is an Atom

A 1cm long line of copper atoms has 100,000,000 atoms

Ch 5.2 Structure of the Nuclear Atom Particle Accelerators

are used to smash particles at speeds near the speed of light into each other in order to break them apart

A bubble chamber is used to track the paths of the broken particles

Cant ever see the actual particles

Electrons

Negatively charged subatomic particle

e-

Electrons

J.J. Thomson (1856-1940) discovered electrons in 1897

Invented cathode ray tubes (used in TVs)

Electrons

Robert Millikan (1868 – 1953)

Determined an accurate mass of an electron

Mass 1/1840 of a hydrogen atom

Protons

E. Goldstein (1886) discovered protons in a cathode ray tube

Protons are positively charged

Mass is 1840 times an electron

Neutrons

James Chadwick (1932) discovered neutrons

No Charge Mass the same as a

proton

Particle Symbol Charge Relative Mass

Actual Mass (g)

Electron e- 1- 1/1840 9.11x10-28

Proton p+ 1+ 1 1.67x10-24

Neutron n0 0 1 1.67x10-24

Atomic Nucleus

Rutherfords Gold Foil Experiment Shot rays of alpha particles at thin gold foil Most passed straight through Some bounced off at large angles Some bounced straight back Suggested that an atom is mostly empty

space with most of the mass and the positive charge in the center (nucleus)

Ch 5.3 Distinguish Between Atoms Atoms are made up

of Electrons Protons Neutrons

Nucleus contains protons and neutrons

Atomic Number

The number of protons in the nucleus of an element

Every element has a different atomic number

Atomic Number

The number of protons equals the number of electrons

Protons are positive, electrons are negative, therefore the total net charge of an atom is 0

Mass Number

The number of protons and neutrons.

Number of neutrons equals mass number minus atomic number

Mass Number

The number of protons does not always equal the number of neutrons

Oxygen Beryllium

Isotopes

There are different types of neon

What is different?

Isotopes

All of the neon's have the same number of protons and electrons, but different number of neutrons

Ne-20 has 10 Ne-21 has 11 Ne-22 has 12

Isotopes

Atoms that have the same number of protons and electrons but different numbers of NEUTRONS.

This also creates a different mass number for each.

Hydrogen

Atomic Mass

AMU (Atomic Mass Units) defined as 1/12 the mass of carbon-12 or 1 amu.

Atomic Mass

The weighted average mass of the atoms in a naturally occurring sample of the element.

Based on the percent of each isotope present on earth.

Atomic Mass

Chlorine 35 – 75.77% Chlorine 37 – 24.23 %

Average Mass based on Percents = 35.453