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Name: ____________________________ Date: ______ Per: _______ Properties and Interactions of Matter Advances in Atomic Theory Democritus (400 B.C.) - was the first person to use the term “________” to describe the tiny units of matter that make up all things. ATOM Derived from the Greek word “________”meaning unable to ______ Smallest part of an element 1. Ancient Greek Model of the Atom Aristotle proposed the existence of the four elements: _______, ____, ______, _______. All matter was a __________________ of those elements. (Draw Ancient Greek model of the four elements) 2. Thompson’s Plum Pudding Model of the Atom John Dalton (1803) English chemist who developed the first ________________ of atoms based on laboratory experiments. J.J. Thompson (1897) English physicist who discovered a _________ charged subatomic particle. Thompson named this particle the ___________. (Draw Plum Pudding Model of the Atom) 3. Rutherford’s Positive Nucleus Model of the Atom Ernest Rutherford (1911) - Gold foil experiment showed that atoms have a ______ but _______ center called the _______________. The nucleus contains positively (+) charged __________ and neutrally charged ___________. (Draw Positive Nucleus Model of the Atom) 4. Bohr’s Electron Shell Model of the Atom Neils Bohr (1913) - Danish physicist who showed that electrons __________ the nucleus in welldefined orbits called ____________________. ( Draw Electron Shell Model of the Atom) Draw for Carbon 5. Electron Cloud Model of the Atom Electron Cloud Model (1926) - electrons move about around the nucleus in a region called an ________________. It describes the region where an electron is _________________ to be. (Draw Electron Cloud Model of the Atom) Unit Four Introduction: Properties and Interactions of Matter Parts of an Atom An atom consists of two parts: 1) _________ – positively (+) charged center that has __________ - (+) charge __________ - no charge (Mass of protons and neutrons is __________ ) 2) ________________ - surrounds nucleus ____________ – negative (-) charge Electron Cloud Model electrons _______ nucleus have ______ energy electrons __________ away have ___________ energy each region (energy level) can hold a _____________ number of electrons Energy Levels 1 (lowest energy) 2 3 4 Max # of Electrons In an atom, the number of protons (+) __________ the number of electrons (-). Therefore, the atom is electrically ______________. Atomic Number The number of __________ in the nucleus (In a _______ atom, this also equals the number of ___________ ) Masses of the Atoms Mass of proton or neutron is about ______________ the mass of an electron. Most of the mass of an atom is a result of the protons and neutrons. Mass Number The sum of the number of ___________ and the number of ______________ in the nucleus of an atom Ex. Sodium, Na 11 P 12 N Mass # Lead, Pb 82 P 125 N Mass # If Uranium has a mass # of 238 how many neutrons does it have? Mass # = # protons + # neutrons # neutrons = mass # - # protons # neutrons = _____ - ____ # neutrons = ______ Given the table below, fill in the missing information. ELEMENT AT. # # PROT. # NEUT. Boron Carbon Oxygen Sodium Copper Iron Sulfer 5 6 5 6 6 8 12 8 11 29 26 29 # ELEC. 6 16 11 29 MASS # 11 12 23 63 56 32 AT. MASS 10.81 12.01 16.00 22.99 63.55 55.85 32.07 Atoms of a particular element must always have the same number of ___________ but the number of _____________ may vary. Isotopes - Atoms of the ________ element that have different numbers of __________________. Isotopes can be written two ways: 1. The name of the element followed by the mass number. Ex. Carbon - 12 2. The chemical symbol with the mass number as a superscript Ex. 12C Given the isotopes listed below, enter the correct number of protons, neutrons, and electrons for each. Hydrogen - 1 or 1H #P = #N = #E = Hydrogen - 2 or #P= #N= #E= Hydrogen - 3 or #P = #N = #E = 2 H 3 H Average Atomic Mass The ______________________ of all the isotopes of an element. This value is the same as the atomic mass listed on the periodic table. Ex. CARBON ELEMENT MASS ABUNDANCE Carbon-12 12.000 98.89% Carbon-13 13.003 1.11% Average Atomic Mass Ex. OXYGEN ELEMENT MASS ABUNDANCE Oxygen- 16 15.995 99.76% Oxygen- 17 16.999 0.04% Oxygen- 18 17.999 0.20% Average Atomic Mass