CHEMISTRY. Objectives 1-9
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1 CHEMISTRY Objectives 1-9
2 Matter anything that has mass and takes up space (volume). It can be in the form of a solid, liquid or gas (States of Matter)
3 Determine Particle Arrangement of solids, liquids, and gases from the video. Bill Nye: Phases of Matter
4 Particle Arrangement Solid Liquid Gas
5 Matter is made of Atoms When all atoms that make up a substance are the same, then that substance is an element. Elements are made of only one kind of atom. Because of this, elements are called "pure" substances. An atom is the smallest piece of an element that still has the properties of that element.
6 Sodium Element Sodium Element All the atoms within this substance are sodium atoms
7 Matter is made up of Elements. Elements are substances that contain one type of matter and cannot be broken down or separated into simpler substances.
8 Example The element aluminum is a lightweight, shiny metal. If we took a piece of aluminum and cut it into small pieces, it would still be aluminum.
9
10 Activity Refer to the periodic table and locate the elements; Aluminum Tungsten Gold Titanium Americium Lead Record the elements symbol Record a fundamental use of each element (Text Pg 21)
11 Describing Matter
12 Describing Matter #1. Physical Properties (Text Page 18) Characteristics of matter that are often observed or measured. Can be either qualitative (observed) or quantitative (measured).
13 Physical Properties of Matter Qualitative State Color Malleability Ductility Texture Magnetism Quantitative Solubility Conductivity Viscosity Density Melting point Boiling point lustre
14 Physical Properties & Physical Change Characteristics that don t change the substance no new substance formed Ex: sugar dissolving in water
15
16 #2. Chemical Properties (Text Page19) Observed when substances react with each other. Determines a substances usefulness.
17 Chemical Properties of Matter Reactivity Combustibility Toxicity
18
19 Chemical Properties & Chemical Change Characteristics that change the substance A new substance is formed Ex: Burning paper
20 Atoms of different elements can combine to make new substances. If atoms combine that are of two or more different elements, we call that a compound.
21 Example Iron oxygen Iron oxide Rust
22 Assignment Properties of Matter (Physical or Chemical Property)
23 Physical & Chemical Property Computer Lab ual_labs/bl01/bl01.swf
24 Physical & Chemical Property Lab
25 Theory vs Law A theory is less well supported than a law. Most laws are supported by different and robust experimental evidence.
26 Science Laws Descriptions of events, patterns, or relationships that have been observed over and over again. Laws do not provide explanations, they simply state what happens
27 Science Theories Explanations of observations supported by evidence. Theories may change as new facts become available. Laws are constant.
28 Atomic Theory The descriptions of matter and how it behaves. Has undergone many modifications as new facts became available.
29 Early ideas years ago Empedocles: matter was composed of four elements ; earth, air, water, and fire.
30 Democritus eventually a substance will be cut into a piece that can no longer be cut. He called this piece atomos.
31 Development of Atomic Theory John Dalton ( ) He suggested that the particles that make up matter are like small, hard spheres that are different for different elements. He defined an atom as the smallest particle of an element.
32 Dalton s Model... Billiard Ball Model He believed atoms were small, hard spheres like a billiard ball! (draw the ball)
33 J.J. Thomson ( ) He suggested that all atoms must contain electrons(negative charge). His model pictured a positively charged ball with the negatively charged electrons embedded in it.
34 Thomson s Model... Raisin Bun Model
35 Ernest Rutherford ( ) He discovered that atoms have a nucleus. two kinds of particles in the nucleus; 1. protons (positive charge) 2. neutrons (neutral)
36 Rutherford s Model... Planetary Model
37 Niels Bohr ( ) He proposed that electrons surround the nucleus in specific energy levels or shells. Each electron has a particular amount of energy.
38 Bohr s Model... Orbital Model
39 Rutherford was able to develop Thomson s model due to the development of new technologies. (gold foil experiment) The development of cyclotrons and proton accelerators have further developed the model accepted today.
40 Billiard s Ball Plum Pudding Planetary Orbital
41 Inside the Atom
42
43 Board Work Atom Components (subatomic particles)
44 Atomic Number = the number of protons in the nucleus. It also represents the mass of the protons. (amu) It also equals The number of electrons surrounding the nucleus. All atoms are neutral in charge, so the # of positive charges (protons) = the # of negative charges (electrons) Atomic Mass The average mass of the atoms of an element. Mass is the number of protons and neutrons in an atom. # of neutrons = Mass number atomic # Example: 7 3 = 4 neutrons.
45 Worksheet Requires booklet and textbook page 50. Review subatomic particles on the periodic table Worksheet - Interpreting Atomic Theorists Models
46 Project Introduction Due at the end of Chemistry unit (booklet 3) Start researching ideas to complete a home experiment. (Video Project) MythBusters: S13E05 - Do Try This At Home (FULL EPISODE) - YouTube SciGuys: Elephant toothpaste: Rock Candy Burning steel wool Ms. Dawe will go into more detail with you!
Chemistry. Objectives 1-9
Chemistry Objectives 1-9 Matter anything that has mass and takes up space (volume). It can be in the form of a solid, liquid or gas (States of Matter) Determine Particle Arrangement of solids, liquids,
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