The Atom Section 4.1-4.3 Notes.

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Presentation transcript:

The Atom Section 4.1-4.3 Notes

Some videos… http://www.youtube.com/watch?v=caYxrueCHiQ You might be giants - Elements

History of Atomic Models Democritus (~400BC) atomos = small, solid, indestructible particles of different shapes & sizes These were just ideas, not truly science… Dalton’s Atomic Theory Billiard Ball Model - small solid sphere Developed notion of conservation of mass and that atoms combine in specific ratios

History of Atomic Models J.J. Thomson Plum Pudding Model - positive and negative particles dispersed throughout the atom Used Cathode Ray tubes to discover the electron - first subatomic particle discovered! http://www.youtube.com/watch?v=XU8nMKkzbT8

Cathode Ray Tube A tube that contains a stream of electrons going from a negative disk (cathode) to a positive disk. Deflected stream showed that electrons are negative.

Rutherford Nuclear Model Discovered dense positively charged nucleus of the atom while working with alpha particles Gold Foil Experiment

History of Atomic Models Neils Bohr - Also Solar System Model Electrons travel in specific, circular orbits Schrodinger & Heisenburg - Quantum Mechanical Model Dense nucleus w/ protons & neutrons Electrons exist in ‘clouds’ called orbitals w/ specific energy levels Mathematical predictions for probability of finding electrons Electrons have particle and wave properties

What do you already know about atoms? Brainstorm about what you already know (or are pretty sure of…) about atoms. Write it down on your paper, then we’ll discuss.

How big is the nucleus?!? Go to atoms videoclip

Comparing subatomic particles…

sToP & tHinK If an atom has 2 protons and 2 neutrons, what is its atomic mass in atomic mass units (amu)? What is the charge on an atom that has 7 protons and 7 electrons?

Atomic Number # of protons # of electrons in a NEUTRAL atom Always a whole number

Mass Number # of protons + neutrons in atomic mass units (amu) Isotopes - atoms of the same element with different masses differ in number of neutrons Examples: Carbon-13 & Carbon-14, Boron-10 & Boron-11 Element-mass#

Calculating # of neutrons Subtract atomic # from mass # Example: Aluminum 13 protons 27-13 = 14 neutrons

sToP & tHinK What element has the atomic number 8? How many protons, neutrons, and electrons are in a neutral atom of Potassium (K)? How many protons, neutrons, and electrons are in a neutral atom of Boron-11?

Average Atomic Mass & Molar Mass Average mass of all the atoms of a sample for an element In amu’s for individual atom In grams for a mole of that element = molar mass

Relative Abundance The atomic mass on the PT is the average of the isotopes for that element. Example: Lithium has two isotopes, one has a mass of 6 amu & one has a mass of 7 amu. Lithium-7 occurs 92.5% of the time… Multiply the mass by the abundance Add the two together to get the atomic mass for the element What is Lithium’s average atomic mass?

sToP & tHinK The published average atomic mass of phosphorus is 30.97. If it has two isotopes, phosphorus-30 and phosphorus-31, which one is more abundant. Explain.

sToP & tHinK An element has two isotopes. One has a mass of 24 amu and represents 70% of the atoms of the element, the other has a mass of 25 amu and represents 30% of the atoms of the element. What is the average atomic mass?