The Atom.

Slides:



Advertisements
Similar presentations
History of Atomic Theory
Advertisements

Atomic Theory.
Atomic Structure History of Atomic Theory. Democritus ( BC) Was the first person to come up with the idea of atom Believed that all matter was.
Atomic Structure.
Atomic Structure History and Theories. The Greeks 4 th century B.C. Democritus “Atomists” school of thought Matter is composed of tiny indivisible particles.
History and Structure of the Nuclear Atom
Atomic Structure.  Democritus (460 BC – 360 BC)  Ancient Greek philosopher ▪ No experiments performed!  Major Contribution: The Atom ▪ He proposed.
Class Notes: Atomic Models. Democritus= 400 B.C. – said the world was made of two things: empty space and tiny particles called “atoms” --said atoms were.
Atomic Theory. English scientist John Dalton, suggested that matter was made up of elements An Element is a pure substance Each element is composed of.
Atomic Structure Timeline
History of Atomic Theory
History of the Atom SWBAT #1: Describe the development of the model of the atom through history SWBAT #2: Identify the main components of the nuclear atom.
History of Atomic Theory
Atoms.
What is an atom? Try to come up with your own definition. Now turn to your partner and discuss.
Democritus/Leuccippos 400 BC
AIM: Models of the Atom DO NOW: Element Y has two isotopes: Y-27 and Y-29. Y-27 has an abundance of 43% and Y-29 has an abundance of 57%. What is the average.
History of Atomic Theory
Aim: Models of the Atom.
Atomic Theory “History of. . . ”.
Early Models of the Atom
Chemistry – Oct 30, 2017 P3 Challenge- Objective –
Unit 2 – Atomic Theory Chapter 4 & 11.2 Unit Test:
The evolution of the atom
Chemistry – Oct 26, 2017 P3 Challenge- Objective –
Atomic Structure.
Old Dead Guys.
Origin of the idea of atom…
Atomic Theory Nucleus 2s orbital p orbitals
Atomic Structure Timeline
Work in partners and grab a textbook or your phone and make a timeline of the main scientists who contributed to the atomic structure. Include Democritus,
Matter Unit Structure of an Atom.
SCH3U Unit 1: Matter, Chemical Trends and Chemical Bonding
1.3 History of the Atom Objectives 3:a,c,d; 5
Atom Model History - Democritus a fifth century B.C. Greek philosopher proposed that all matter was composed of indivisible particles called atoms (Greek.
Warm-Up Draw a picture of an atom. Be as specific as you can!
History of Atomic Theory
Models of the Atom   S Investigate the historical progression of the atomic model. Include: Dalton, Thompson, Rutherford, Bohr, quantum model.
Models of the Atom.
1.3 Atomic Theory.
Atomic Theory.
Origin of the idea of atom…
BELLWORK 9/11/17 What is the atom?
UNDERSTANDING THE PROPERTIES OF ELEMENTS
Atomic Theory A Brief History.
Atomic Structure Timeline
Atom Model History - Democritus a fifth century B.C. Greek philosopher proposed that all matter was composed of indivisible particles called atoms (Greek.
Unit 2: History of the Atom
Atomic Structure Timeline
2.1 History of the Atom Objectives S1 and S2
The Building Blocks of Matter
Chemistry – Nov 7, 2018 P3 Challenge- Objective –
Chemistry – Nov 1, 2018 P3 Challenge- Objective –
The History of Atomic Theory
Atomic Structure Timeline
Chapter 4 Atoms 1. Atomic Structure Timeline
Atomic Structure Timeline
Atoms & the Periodic Table
Historical Development of the Atomic Theory
Chapter 4 Atomic Structure and Theory
Atomic Structure An atom is the smallest particle of an element that retains its identity in a chemical reaction. Although early philosophers and scientists.
Chapter 4 Atoms.
Chapter 4: Atomic Structure
SCH3U Unit 1: Matter, Chemical Trends and Chemical Bonding
Atomic Structure Timeline
Chapter 4 Atoms.
Atomic Structure.
Atomic Structure Timeline
Presentation transcript:

The Atom

Greek Model One group of Greek philosophers who lived in the forth and fifth centuries B.C. believed that matter is composed of tiny indestructible particles which they called atoms. However, this theory was never verified by experiments and was discarded. More than 2000 years later, in 1804, John Dalton, an English school teacher, reintroduced the model or theory and developed it to such an extent that it was able to explain the laws of chemical change.

Dalton Model Dalton proposed that elements are composed of identical, indivisible atoms in his “billiard ball model” of the atom. He devised a system of atomic symbols. He correctly predicted the Law of Multiple Proportions (if the same elements combine to form different compounds, the ratio of the elements in the compounds are in simple multiples.

The discovery of subatomic particles showed that Dalton’s proposal that atoms were indivisible was wrong.

J.J. Thomson 1900 Thomson revised Dalton’s theory with his raisin bun or plum pudding model of the atom. Thomson proposed that an atom could be considered a sphere of positive electricity in which negative electrons are embedded like raisins in a bun. Most of the mass of the atom in this model is associated with the positive electricity.

Rutherford Model 1911-1912 In 1911, Rutherford’s gold foil experiment lead to another revision of the atomic model. Rutherford proposed that An atom has a nucleus in which its positive charge (protons) and mass are concentrated. The vast majority of the atom’s volume would be empty space occupied only by the moving negatively charged electrons.

Rutherford also postulated the existence of uncharged particles (neutrons)

Problems with Rutherford’s Model (1) If electrons are not moving, then the attraction of the negative electrons for the positive nucleus should collapse the atom. (2) If the electrons are moving (to counteract the pull of the nucleus), then the electrons should radiate energy and in time spiral down to the nucleus.

Bohr Model 1913 Bohr studied the atomic spectra of the elements and discovered the each spectrum showed a series of lines of definite energies. Bohr proposed that electrons of specific energy moved in circular orbits around the central atomic nucleus and that electrons could not exist between the orbits.

Bohr’s model worked well for hydrogen, but it did not work well for multi-electron atoms.

Quantum Mechanical Model 1920’s This is the most recent model of the atom. This model supports Bohr for the most part, but suggests that electrons do not exist in fixed orbits or a fixed definite path. Instead, they electrons exist anywhere within an electron cloud. Determining where an electron will be at any given moment is very difficult and can only be theorized using mathematical equations.

The Atom The model of the atom has evolved from Dalton’s “billiard ball” model to a highly complicated quantum mechanical model. It was first believe that an atom could not be broken down into smaller parts. We now know that it can, mostly by nuclear reactions. The three main sub-atomic particles are the proton, electron, and neutron.

Charge and Mass of Subatomic Particles Mass (kg) Mass (u) Proton (p) +1 1.672 x 10-27 1.00728 Neutron (n) 1.675 x 10-27 1.00783 Electron -1 9.110 x 10-31 0.000055

The proton and neutron are about equal in mass The proton and neutron are about equal in mass. These two types of particles are found together in the nucleus (center) of the atom. This explains Rutherford’s gold foil experiment. The electron is much smaller then the other two particles. It is found in orbits or shells surrounding the nucleus and does not contribute significantly to the mass of the atom.

Atomic Number Atomic number refers to the number of protons in the nucleus of the atom. It is represented by the symbol Z. Atomic number determines the identity of the element. Every atom of a given element has the same unique number of protons. In a neutral atom, atomic number is also equal to the number of electrons surrounding the nucleus.

Atomic Mass An atom’s mass is expressed in Atomic Mass Units (u or a.m.u.) It was impossible for scientists to determine the mass of individual atoms (they are too small) so they assigned relative atomic masses that agreed with the known composition of compounds.

Atomic Mass continued A new unit was developed to mass atoms. Carbon-12 (C-12) was chosen as the reference standard. An atom of C-12 was arbitrarily assigned a mass of 12 atomic mass units. The masses of all other atoms are compared with the mass of this type of carbon atom. According to this definition, an atomic mass unit is defined as 1/12 the mass of a carbon-12 atom.

Mass Number Mass number is the total number of protons and neutrons in an atom. The symbol for mass number is A. For now, we will round the atomic mass to the nearest whole number to get the mass number of an element.

Elements and the Periodic Table All elements can be represented as symbols that are organized in the periodic table. In addition to the symbols, the periodic table provides us with the atomic number and the mass number of an element.

Summary Atomic Number (Z) = # of protons Mass Number (A) = # of protons + # of neutrons Neutral Atom: # of protons = # of electrons