Ch. 4 section 1 Notes 11-1-11 Item #53/56 honors.

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Ch. 4 section 1 Notes 11-1-11 Item #53/56 honors

Atoms Atom = is the smallest particle of an element Existence theorized and named by Democritus in 4th century B.C.! Atomic Theory grew as a series of models developed from experimental evidence, over time the theories and models were revised

Dalton’s Atomic Theory In 1808 Dalton developed the atomic theory: Atoms cannot be divided (now false) All atoms of one element are exactly alike (now false) Atoms cannot be changed into an atom of a different element. Atoms cannot be created nor destroyed, only rearranged. Atoms of different elements join in specific ratios to form compounds

The next 4 slides are for your information…you do not need to write down 

Thompson’s Model In 1897, Thompson discovered the electron, a negatively charged particle within an atom. Proposed model of atom with negative charges scattered throughout a ball of positive charge – like berries in a muffin.

Rutherford’s Model In 1911, Rutherford used his gold foil experiment to find the nucleus, a tiny region in the center which contained positively charged protons.

Bohr’s Model In 1913, Bohr showed the electrons moved in orbits like planets orbiting around the sun.

Cloud Model In the 1920’s scientists found electrons do NOT orbit around the nucleus like planets, instead they can be anywhere in a designated “cloud” region, called an energy level.

Modern Atomic Model In 1932, Chadwick discovered the neutron, a neutral particle within the nucleus. Modern model = at the center of the atom is a tiny nucleus containing protons and neutrons. Surrounding the nucleus is a cloudlike region of moving electrons.

Scientist/Model QUIZ Match the atomic structure/model with the scientist: Dalton, Rutherford, Thompson, Bohr, Chadwick, Democritus Orbiting planet model Gold foil experiment Nucleus Electron Proton Neutron Energy level “Atom”

Parts of the Atom Nucleus: atom’s central core, made up of protons and neutrons, is positive in charge Proton (p+): subatomic particle that has positive charge, has some mass Neutron (n): subatomic particle that has no charge or is neutral, same mass as proton Electron (e-): subatomic particle that has a negative charge, relatively no mass

Comparison Chart Atoms have no charge overall since protons balance out electrons. Particle Symbol Charge Mass Location Proton p+ +1 ~ 1amu Nucleus Neutron n Electron e- -1 ~ 0amu Outside nucleus

Atomic Structure Atomic Number: number of protons in the nucleus of an atom Atomic # = # of p+ Determines the identity of the element Periodic table is organized by atomic number Ex: What is the atomic number of… He ______ C ______ N ______ O ______

Summary: Create a BRACE MAP to illustrate the structure of the ATOM Use the following words: electrons atom electron cloud Neutrons nucleus protons

Organizing The Elements 11-2-12 Page # Meet the Elements Song Chapter 4 Section 2 Notes Organizing The Elements 11-2-12 Page #

I. Mendeleev’s Periodic Table By 1869, 63 elements had been discovered. Mendeleev found a way to organize them. He arranged them by atomic mass, the average mass of all the isotopes of an element. He noticed a pattern of properties in the table and was able to predict where future elements would occur!

II.Modern Periodic Table The modern periodic table is organized by the number of protons or atomic number. The properties of an element can be predicted from its location on the periodic table. According to periodic law, when elements are arranged this way, similarities in their properties will occur in a regular pattern.

III. Finding Your Way Around The Periodic Table: Classes of Elements: Elements are classified as metals, semimetals, or nonmetals. The zigzag line on the periodic table separates the metals from the nonmetals

III. Finding Your Way Around The Periodic Table: Periods: The horizontal rows. The properties of elements in a row follow a repeating pattern as you move across each period.

III. Finding Your Way Around The Periodic Table: Groups (Families): The vertical columns (top to bottom). Elements in the same group have similar characteristics.

III. Finding Your Way Around The Periodic Table: Reading the Data: Each square in the table gives: atomic number chemical symbol element name atomic mass Chemical Symbol = representation of an element usually consisting of 1 or 2 letters

Meet The Elements… Meet the Elements Song

State of Matter Periodic Table displays the state of matter element is in at room temperature Solids: Most common on table Liquids: Only 2-5 total on table Gases: in upper, right hand corner

Classification Metals: elements that are shiny, bendable, conduct heat and electricity well. Most common, take up left and middle of table Nonmetals: elements that conduct heat and electricity poorly. Located in upper, right corner of table Metalloids: located in between metals and nonmetals, on “staircase” Semiconductors: element that conducts fairly well

Chapter 4 section 3 Notes Metals November 6th Notebook page 81

Properties of Metals The Reactivity of metals tends to decrease as you move from left to right across the periodic table Physical Properties: Luster (shiny) Malleability = material can be hammered or rolled into sheets/shapes Ductility = material can be pulled out into wire Thermal conductivity = ability to transfer heat Electric conductivity = ability to transfer electric current

Properties of Metals Chemical Properties: Reactivity = ease and speed substance reacts with other substances Decreases as you move from left to right on table! Corrosion = gradual wearing away of a metal due to chemical reaction

Alkali Metals Group 1: Alkali Metals React w/ other elements by losing 1 electron Super reactive; always found in compounds, never alone in nature Soft, shiny Ex: sodium, lithium, potassium

Group 1: Alkali Metals Turn to page 76 in your notebook and label your periodic table.

Alkaline Earth Metals Group 2: Alkaline Earth Metals Hard, gray-white, good conductor of electricity, fairly reactive Form compounds found in limestone and in human body React by losing 2 electrons Ex: magnesium, calcium, barium

Group 2: Alkaline Earth Metals Turn to page 76 in your notebook and label your periodic table.

Transition Metals Groups 3-12, Group that contains the MOST elements Conduct heat and electricity Hard, shiny, colorful Ex: copper, iron, mercury, silver, gold, nickel

Metals in Mixed groups Groups 13-15, some are metals (Aluminum, Gallium, Indium, Thallium, tin, lead, bismuth) Never found uncombined in nature

Metals in Mixed Groups

Lanthanides Atomic numbers 57-71, rare earth metals, used to make alloys

Actinides Atomic numbers 89-103 radioactive, some are synthetic (man-made), unstable (Uranium)

Synthetic Elements Synthetic elements are made by scientists by forcing nuclear particles to crash into one another. The nuclei break apart quickly so this makes it difficult to determine properties of newly discovered elements Elements numbered 92 and greater Particle accelerator = moves atomic nuclei at high speeds causing them to crash into each other, sometimes combine into single nuclei

November 7, 2012 Notebook Page 83 Chapter 4 Section 4 Nonmetals, Inert Gases, and Semimetals November 7, 2012 Notebook Page 83

Nonmetals Physical Properties: Dull Brittle Poor conductor of heat and electricity Basically the OPPOSITE of metals! Chemical Properties: Gain or share electrons Metals and nonmetals often react together

Nonmetals Located on the right side of table Abundant on Earth Oxygen and Nitrogen make-up 99% of atmosphere Carbon is in more compounds than any other elements combined!

Group 17: Halogens Very reactive Dangerous to humans Ex: Fluorine, Chlorine, Bromine, Iodine, Astatine Group 18: Noble/Inert gases: Unreactive Do not usually form compounds Ex: Helium, Neon, Argon, Krypton…

Semimetals/Metalloids Contains only 8 elements, found along boundary between metals and nonmetals Have properties of both metals and nonmetals Ex: Boron, Silicon, Arsenic… Are semiconductors: conduct heat and electricity under certain conditions Silicon used in computer chips to speed up conduction

Radioactive Elements 4-5

Radioactivity Radioactive decay = atomic nuclei of unstable isotopes release fast-moving particles and energy. Radioactivity = element which spontaneously emits radiation First discovered by Becquerel in 1896 with uranium.

Types of Radioactive Decay Radioactive decay can produce 3 types of radiation: Alpha Decay: an alpha particle consists of 2 protons and 2 neutrons and is positively charged. Can be stopped by a thin layer Beta Decay: a neutron is converted into a beta particle, a fast-moving electron Can be stopped by thick material Gama Decay: high-energy waves Can only be stopped by thick concrete or lead

As uranium decays it becomes multiple elements releasing multiple types of radiation!

Uses of Radioactive Isotopes Radioactive isotopes can include the tracing steps of a chemical reactions, industrial processes, and diagnosing and treating disease.