Atomic Structure.

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Presentation transcript:

Atomic Structure

Atom Definition – smallest particle of an element that retains the chemical identity of that element Term proposed by Democritus in 450 BC Democritus proposed that all matter is composed of tiny, indivisible particles Rejected by Aristotle because Democritus could not explain how particles “stuck together”

Dalton’s Atomic Theory of Matter- 1803 Based on observations made by scientists during the 1700’s, John Dalton proposed a theory that could explain the properties of matter Four postulates: Each element is made of small particles called atoms All atoms of a given element are identical, but different from those of any other element Atoms are neither created nor destroyed in a chemical reaction A given compound always has the same relative numbers and kinds of atoms

Are the four postulates all true? What do we know about atoms that means we might need to re-state one of the postulates?

Postulate Number 2 – not all atoms of the same element are the same You can have different Isotopes of the same element Example: Iodine-125 and Iodine-127 are both iodine, but are different from each other. Iodine-125 is radioactive and Iodine-127 is not.

History of Discovering about Atomic Structure Dalton thought atoms were hard and round like tiny marbles Early 1800’s – Franklin- two kinds of electric charges (positive and negative)

Electrons were First Particles Found An English scientist discovered electrons and named them. An Amercian scientist found their mass. Mass of an electron to be 9.11 x 10-28 grams

Protons were next particles found Atoms are electrically neutral so the negative electrons must be balanced by an equal number of positive particles An English scientist found these particles and called them protons. He also discovered these positively charged particles were all concentrated in the center of the atom – called it the nucleus

Modern Atomic Theory Atoms are composed of protons, neutrons, and electrons At first, scientists visualized electrons orbiting the nucleus much like planets orbiting the sun

Last particle found was the neutron Neutrons have a mass approximately equal to that of a proton Neutrons have no charge Neutrons help “glue” the nucleus together

Fundamental Subatomic Particles Particle Location Charge Mass (amu) Proton Nucleus +1 1 Neutron Nucleus 0 1 Electron Outside -1 0 Nucleus

Moseley’s Discovery Found that atoms of each element contain a unique positive charge in their nucleus Conclusion: atom’s identity comes from the number of protons in the nucleus Called “Atomic Number” Neutral atoms – positive charges must equal negative charges Conclusion – for neutral atoms, no. of electrons equals no. of protons

Information in Periodic Table 7 Atomic Number (sometime not in center) N Chemical Symbol Nitrogen 14.0067 Atomic Mass

Mass Number Hydrogen -1 The 1 after the hydrogen is the mass number. Used to help keep track of what isotope you have. Definition Sum of the neutrons and protons Always a whole number Another way to represent Mass Number 1 2 3 H H H 1 1 1 Atomic Number

Mass of an Atom Atomic Mass Unit – approximately the weight of one neutron or proton Used because the weight in grams is very small 1 a.m.u. = 1.66 x 10-24 g.

Element’s atomic mass Weighted average of all of the isotopes of an element 7 N Nitrogen 14.0067 Atomic Mass Nitrogen contains mostly Nitrogen-14 with a small amount of Nitrogen-15

Practice Find sodium (Na) on the periodic table I gave you Find the atomic number. What does that number mean? Find the atomic mass. What does that number mean?

How many electrons does one sodium atom have? I have one atom of sodium represented by 46V 23 How many protons does it have? How many neutrons does it have?