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Atoms Family Story In the center of Matterville, there is a place called the Nucleus Arcade, where two members of the Atoms Family like to hang out. Name Picture Perky Patty Proton, like her sisters, is quite large with a huge smile and eyes that sparkle (+). Patty is always happy and has a very positive personality. Patty spends all her time in the arcade. Description Favorite Activity Name Picture Nerdy Nelda Neutron is large like Patty, but she has a boring, flat mouth and eyes with zero expression (o). Her family is very apathetic and neutral about everything. Like Patty, Nelda, and their sisters spend all their time in the arcade. Description Favorite Activity Around the Nucleus Arcade, you will find a series of roadways that are used by another member of the Atoms Family, Patty and Nelda’s VERY little brother, Enraged Elliott Electron. Name Description Favorite Activity Picture Elliott races madly around the Arcade on his bright red chrome-plated HarleyDavidson. He rides so fast that no one can be sure where he is at any time. Elliott is much smaller than Patty and Nelda and he is always angry because these bigger relatives will not let him in the Arcade. He has a frown on his face, eyes that are squinted with anger, and a very negative (-) attitude. MM/MG 09-10 The morale of Matterville is stable as long as each negative Electron brother is balanced out by one positive Proton sister. The number of residents in Matterville depends on the Proton and Neutron families. Morale of Matterville + = Morale Challenge: What would happen to the morale of Matterville if one Elliott Electron was kidnapped? + = - = Morale Challenge: What would happen to the morale of Matterville if one Elliott Electron moved to Matterville? + = - = The first energy street can only hold only two Electron brothers. The second energy street, called the Energy Freeway, can hold 8 brothers. The third energy street, called the Energy Superhighway, can hold 18 of the brothers. Matterville: MM/MG 09-10 Chapter 17 Atoms and the Periodic Table Objectives 17-1 Define and describe protons, neutrons and electrons. (Mass, location, charge) 17-2 Draw a Bohr model showing the correct number and placement of electrons. 17-3 Know where to find atomic number and average atomic mass for an element on a periodic table. 17-4 Calculate the number of protons, neutrons and electrons for an element. 17-5 Calculate the number of atoms of each element in a chemical compound. 17-6 Differentiate between atoms and isotopes. 17-7 Identify the subatomic particle that determines the identity of the element. Section 1 - Structure of the Atom Objectives Structure Particle Relative Mass Charge Location Proton Neutron Electron Models of Atom MM/MG 09-10 History of the Atomic Model • Democritus – 4th century BC philosopher thought atoms were whole • In 1808 John Dalton came up with a theory that was developed with a scientific basis. Dalton’s Theory • Matter was made up of atoms that could not be divided. • All atoms of a given element are exactly the same. • Atoms of given elements could join to form compounds. More Theories • • In 1877 JJ Thomson theorized on particles smaller than an atom. Electrons In 1911 Ernest Rutherford theorized a nucleus in an atom with a positive charge. History of the Atomic Model • In 1913 Niels Bohr proposed a model of the atom where electrons moved in definite orbits around the nucleus. Bohr’s Model MM/MG 09-10 Drawing an Atomic Model # of protons Equal to _______________________ # of neutrons Equal to atomic mass (rounded) atomic # # of electrons Equal to # of protons – 1st energy level holds _______ e– 2nd energy level holds ______ e– 3rd energy level holds _______ e– 4th energy level holds _______ e- MM/MG 09-10 Chapter 17 Section 2 - Masses of Atoms Objectives Atomic Mass Definition Atomic Number Sum of masses of the _____________________ and _____________________ The number of _____________________ Concentrated in the Identifies each ___________________. _____________________ in the nucleus. If you change the number of Extremely small protons, then you change the Atomic mass unit is smaller than _____________________ you have. a _________________. Other information AMU Masses of Proton = _____________ Neutron = ____________ Electron = ___________ Where to find it on the periodic table Examples Calcium – Ca – Zinc – Zn – Tungsten – W – Lithium – Li - MM/MG 09-10 Isotopes Mass Number Average atomic mass Sum of Weighted average of _____________________ _____________________ Atoms of the same element have different number of _____________________ but the same number of Definitions _____________________ and and _____________________ in the nucleus of an isotope. of all naturally occurring _____________________ _____________________ Have different Different __________________ __________________ for each isotope Due to different number of _____________. Other Can have different information ___________________ (variety) of an element. Depends on ______________ and _______________ of isotopes Based on the __________________ Round to a whole properties number Showing Isotopes Name + mass number Where to find it on the periodic table Hydrogen – Nitrogen – N – Beryllium – Be – Hydrogen – Neon – Ne– Iron – Fe - Examples MM/MG 09-10 What’s the difference between Average Atomic Mass and Mass Number? o Average Atomic Mass is based on ______________________ isotopes of the element. o Mass number is for just _____________________ isotope of the element. Counting Atoms During chemical reactions you need to know how many atoms are involved. Remember, more than one element bonded together is a compound. – H2O CO O2 = 2 Oxygen atoms bonded together. It’s now a molecule. The 2 is called a____________________________________. 7H2O The 7 is called a ____________________________________. This means there are 7 water molecules, each molecule having 2 Hydrogen and 1 Oxygen 2 How many Carbon atoms are present? ___________________ How many Oxygen atoms? ___________________ 3SO 4 How many Oxygen atoms? ___________________ How many Sulfur atoms? ___________________ Practice S(H20)2 o S = __ o H = __ o O = __ 12H2SO4 o S = __ o H = __ o O = __ 8Na2(OH4)6 o Na = __ o H = __ o O = __ 10C6H12O6(OH)12 o C = __ o H = __ o O = __ 3(Mg,Fe)7Si8 o Mg = __ o Fe = __ o Si = __ Periodic Acid – 12H5IO6 o I = __ o H = __ o O = __ MM/MG 09-10