Bellwork08/20/2012 How long have people been interested in understanding matter and its structure? A.Thousands of years B.Hundreds of years C.A few years D.Never

History of Atomic Structure

Ancient Philosophy Who: Aristotle, Democritus When: More than 2000 years ago Where: Greece What: Aristotle believed in 4 elements: Earth, Air, Fire, and Water. Democritus believed that matter was made of small particles he named “atoms”. Why: Aristotle and Democritus used observation and inference to explain the existence of everything.

Democritus Matter is composed of empty space through which atoms move. Atoms are solid, homogeneous, indestructible, and indivisible. Different kinds of atoms have different sizes and shapes. The differing properties of matter are due to the size, shape, and movement of atoms. Apparent changes in matter result from changes in the groupings of atoms and not from changes in the atoms themselves.

Aristotle Democritus

Alchemists Who: European Scientists When: 800 – 900 years ago Where: Europe What: Their work developed into what is now modern chemistry. Why: Trying to change ordinary materials into gold.

Alchemic Symbols

Particle Theory Who: John Dalton When: 1808 Where: England What: Described atoms as tiny particles that could not be divided. Thought each element was made of its own kind of atom. Why: Building on the ideas of Democritus in ancient Greece.

Dalton Atoms of an element are not changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions. Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. BILLIARD BALL MODEL

John Dalton

Discovery of Electrons Who: J. J. Thompson When: 1897 Where: England What: Thompson discovered that electrons were smaller particles of an atom and were negatively charged. Why: Thompson knew atoms were neutrally charged, but couldn’t find the positive particle.

The Atom, circa 1900: PLUM PUDDING MODEL “Plum pudding” model, put forward by Thompson. Positive sphere of matter with negative electrons imbedded in it.

J. J. Thompson

Atomic Structure I Who: Ernest Rutherford When: 1911 Where: England What: Conducted an experiment to isolate the positive particles in an atom. Decided that the atoms were mostly empty space, but had a dense central core. Why: He knew that atoms had positive and negative particles, but could not decide how they were arranged.

Discovery of the Nucleus Ernest Rutherford shot  particles at a thin sheet of gold foil and observed the pattern of scatter of the particles.

The Nuclear Atom Since some particles were deflected at large angles, Thompson’s model could not be correct.

THE NUCLEAR MODEL According to Rutherford, most of the atom consists of electrons moving rapidly through empty space and a very dense, positively charged nucleus.

Ernest Rutherford

Other Subatomic Particles By 1920, Rutherford had refined his concept of the nucleus: He concluded that the very dense nucleus contained positively particles called protons. James Chadwick, a coworker, showed that the nucleus also contained a neutral particle in This was the neutron – a particle with nearly equal mass as a proton.

Atomic Structure II Who: Niels Bohr When: 1913 Where: England What: Proposed that electrons traveled in fixed paths around the nucleus. Scientists still use the Bohr model to show the number of electrons in each orbit around the nucleus. Why: Bohr was trying to show why the negative electrons were not sucked into the nucleus of the atom.

Niels Bohr

Electron Cloud Model Electrons travel around the nucleus in random orbits. Scientists cannot predict where they will be at any given moment. Electrons travel so fast, they appear to form a “cloud” around the nucleus.

Electron Cloud Model

Atomic Structure Timeline Requirements: Must include a title. Must include a spot for each of the 7 items. Must include at least the Who, When, and What. Must have a picture (color is preferred) for each item. Options: 1.Comic book format 2.Standard timeline

Properties of Subatomic Particles ParticleSymbolLocationCharge Relative mass Actual mass (g) Electrone-e- Around nucleus 1– × Protonp+Nucleus × Neutronn0n0 nucleus ×10 -24

Atomic Structure and the Periodic Table 14 Si Silicon Atomic number = # protons Symbol Name Atomic Mass: Round to a whole #: 28 = Relative mass of nucleus -14 = # protons 14 = # neutrons

Practice From the Periodic Table Complete the following chart: NameSymbol Relative mass # protons # neutrons # electrons Lithium Mg 26 16