Chapter 14: Inside the Atom Pages 404 - 423. First Thoughts of the Atom “Cannot be divided” Keep dividing matter until only one particle remains Chemistry.

Slides:

Advertisements

Similar presentations

Chapter 11 Radioactive Elements.

Advertisements

Ch. 3.2 Atomic Structure On your bell work sheet, answer the following. When are zeros significant? When do you use the fewest number of Significant Figures?

Chapter 4 Atomic Structure

4-1: Introduction to Atoms

ATOM Chapter 14. I CAN IDENTIFY THE PROPERTIES OF THE THREE SUBATOMIC PARTICLES OF ATOMS. I CAN USE A MODEL TO REPRESENT THE STRUCTURE OF AN ATOM AND.

THE ROAD TO THE ATOM.

Atomic Theory “History of. . . ”.

UNIT FOUR: Matter and its Changes  Chapter 12 Atoms and the Periodic Table  Chapter 13 Compounds  Chapter 14 Changes in Matter  Chapter 15 Chemical.

Model of the Atom.

Radioactive Decay.

History of Atomic Theory

Introduction to Atoms.

Chapter 9 pages And Chapter 18 pages

Atomic Structure History of Atomic Theory. Democritus ( BC) Was the first person to come up with the idea of atom Believed that all matter was.

Models of the Atom The Nucleus. Early Beliefs 2500 ya, early Greek philosophers believed that if you continued to divide matter eventually you would have.

Monday August 20 Describe subatomic particles. Models of the Atom John Dalton—pictured the atom as a hard sphere that was the same throughout.

The Atom Chapter 11 Notes and Review By: Mr. Steffen.

Atomic Structure Chapter 4

Chapter 9: Radioactivity and Nuclear Reactions The last chapter we will study!

Atomic Structure and The Periodic Table of Elements

Flashbacks 1. A place where an earthquake originates is called the __________. A Epicenter B Starting point C Quake zone D Shaking place 2. When only a.

Introduction to Atoms Chapter 4.

Chapter 16: The Properties of Atoms and the Periodic Table

Using the Periodic Table

A History of Atomic Theory & Basic Atomic Structure Chapter 3: The Atom Big Idea: Physical, chemical and nuclear changes are explained using the location.

Section 1- Discovering the parts of the atom

Mullis1 Democritus ( B.C.) Democritus was one of a few Greek philosophers who believed that all matter in the world was made of of indivisible parts.

The Structure of the Atom Chemistry 1. 2 Learning Objectives for this Chapter: 1.Describe changes in the atomic model over time and why those changes.

Nuclear Reactions.

For each scientist you need to know  Approximate date of discovery  Discovery  Experiment/Theory  Atomic Structure from their perspective FOCUS.

HISTORY OF THE ATOM. Aristotle 400 BC 400 BC - Claimed that there was no smallest part of matter - Claimed that there was no smallest part of matter -

Scientists in the late 1800s determined that there were different types of radiation in addition to visible light. Some types of radiation have mass, some.

Radioactive Decay. What do you know about Radioactivity? 1.All atoms are made up of __________. 2.What are some radioactive isotopes? 3.Why do some isotopes/atoms.

Radioactivity SPS3. Students will distinguish the characteristics and components of radioactivity. Differentiate among alpha and beta particles and gamma.

Chapter 3 Atoms: The Building Blocks of Matter. Objectives: Students should be able to: Summarize the essential points of Dalton’s atomic theory. Describe.

Chapter 4 Atomic Structure

INSIDE THE ATOM. Three Topics: Section 1 How scientists model the atom What are charged particles What were Rutherford’s experiments REVIEW VOCABULARY.

Unit 10: Atoms and Periodicity. An atom is the smallest particle in which matter can be divided and still be the same substance. The same type of atoms.

 Atoms are small hard particles made of a single material that can’t be divided.  Developed his ideas by thinking.

Structure of Atom Atom Smallest particle of an element Atomic Structure – arrangement of smaller particles within an atom.

How did the atomic theory develop and change into the modern model of the atom?

Jeopardy Scientist Model of Atoms NucleusIsotopes 2 Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Jeopardy.

Chapter TED:Radioactivity-Expect the Unexpected by Steve Weatherall hDvDlD3b85zmvERO_rSSUj3FVWScEA _X.

Radioactivity Nucleus – center of the atom containing protons and neutrons –How are the protons and neutrons held together? Strong Force - an attractive.

The Atomic Theory Democritus Dalton 440 B.C. – Thought matter was made of tiny particles – Believed these particles could not be cut into anything smaller.

Atomic Models: Developing the Structure of the Atom.

Chapter 5 Atoms: Building Blocks of Matter. Evidence Direct evidence is when you do something to gather the evidence Examples are Doing an experiment.

Unit: Chemistry Lesson 1: Introduction to Atoms Essential Questions: 1.) How did atomic theory develop? 2.) What is the modern model of the atom?

Chapter 11 Introduction to Atoms. Section 1: Objectives  Describe some of the experiments that led to the current atomic theory.  Compare the different.

The Nucleus Chapter 14 Section 2.

Atomic Concepts How the building blocks of life work; and where they came from Brought to you by Erica Stevens.

Section 1: Introduction to Atoms

Radioactivity and Nuclear Decay Test on Friday March 1.

 What are the limitations of relative age dating?  What do you think Absolute age dating is?

Historical Development of an Atom. Democritus B.C Democritus was a Greek philosopher ( B.C.) who is the father of modern atomic thought.

Chapter 10 Nuclear Decay. Objectives 〉 What happens when an element undergoes radioactive decay? 〉 How does radiation affect the nucleus of an unstable.

(8th) Chapter 4-1 Cornell Notes “Introduction to Atoms”

DEVELOPMENT OF THE ATOMIC THEORY Atom- smallest particle into which an element can be divided and still be the same substance Called the building blocks.

The Atomic Theory – p Democritus  Democritus, 440 B.C.  Thought matter was made of tiny particles  Believed these particles could not be cut.

Unit E Chapter 1 “Atoms, Elements and Compounds” Lesson 1.

{ Models of the Atom Ms. Fauss 8 th Grade.  Some of the early philosophers thought that matter was composed of tiny particles.  They reasoned that you.

Atomic Theory and Atomic Structure

Chapter 2 Section 1: Models of the Atom Section 2: The Nucleus

Chapter 2 Section 1 8th Grade.

Chapter 10- Introduction to Atom

Presentation transcript:

Chapter 14: Inside the Atom Pages

First Thoughts of the Atom “Cannot be divided” Keep dividing matter until only one particle remains Chemistry – study of matter

A Model of the Atom Element – matter made of atoms of only one kind Dalton’s Concept – –Matter is made up of atoms –Atoms cannot be divided into smaller pieces –All atoms of an element are exactly alike –Different elements are made of different kinds of atoms *Thought was like tiny marble

William Crookes Experiment –Showed particles were traveling in a straight line from the negative electrode to the positive –CRT – once used in TV’s and computer monitors

Discovering Charged Particles J.J. Thomsom – used magnet on CRT and beam was bent towards it Proved that this was not light, but made of charged particles of matter Electrons – negatively charged particles Particles smaller than atoms do exist

Atomic Model: –Sphere of positive charge –Negatively charged electrons spread evenly throughout positive charge –Positive=Negative –Atom is neutral –Later discovered not all atoms are neutral –More positive electrons = + atom –More negative electrons = - atom

Questions 1.What does the word atom mean? 2.What 4 concepts did Dalton propose about atoms? 3.What did William Crookes experiment show? 4.How did Thomson prove particles were in the CRT and not light? 5.What type of particle did Thomson discover? 6.Describe what an atom looks like. 7.How do we know if an atom is neutral or has a positive or negative charge?

Rutherford’s Experiments Tested Thomson’s model to see if correct Alpha particles bombarded gold foil Most passed through or veered slightly, but some bounced right back!

A Model with a Nucleus Hypothesized that almost all mass of an atom and all positive charge is crammed into one small space in the center called the nucleus Proton – positively charged particle in the nucleus of an atom The rest of the atom is empty space occupied by almost massless electrons

Neutron: –Same mass as a proton –Neutral charge –Located in nucleus –Neutral atom has equal number of protons and electrons

Further Developments Electrons – in constant, unpredictable motion, impossible to know precise location of an electron Electrons act as waves Electron Cloud – region surrounding nucleus where electrons travel Electron energy levels – Niels Bohr

Questions 1.What did Rutherford discover about the atom from his experiment? 2.What is a proton? 3.What is a neutron? 4.How does an atom get a neutral charge? 5.Describe the behavior of an electron in an atom. 6.Where are electrons located in an atom?

Chapter 14 Section 2: The Nucleus Pages

Identifying Numbers Atoms of different elements contain different #s of protons Atomic number is the number of protons in the nucleus of an atom of that element. Smallest: Hydrogen has 1 proton, atomic # is 1 Heaviest: Uranium has 92 protons, atomic # is 92 Elements are identified by their atomic # (doesn’t change for an element)

Number of Neutrons Atoms can have a varying # of neutrons in the nucleus. Isotopes are atoms of the same element that have different #s of neutrons. Mass #: the # of neutrons + protons. Strong nuclear force holds protons together that are tightly packed in the nucleus.

Radioactive Decay unstable nuclei have too many or too few neutrons. Radioactive decay: nucleus releases particles to become stable If protons are released the element is changed Transmutation is the changing of an element due to radioactive decay.

Alpha particle = 2 protons and 2 neutrons. Beta particle = high energy electron that comes from the nucleus, not from the electron cloud. Neutron becomes unstable and splits into a proton (+) and an electron (-) Electron (-) is given off Nucleus now has 1 more proton (+), and is a new element.

Questions 1.Define atomic number. 2.What are the smallest and heaviest elements? 3.Define Isotope. 4.What is mass number? 5.What is radioactive decay? 6.How could an element be changed during radioactive decay? 7.What is an alpha particle? 8.How does a beta particle being released affect an element?

Rate of Decay Half-life of a radioactive isotope is the amount of time it takes for half of a sample of the element to decay. Not affected by weather, pressure, magnetic/electric fields, or chemical reactions.

Carbon Dating Carbon 14 is used to find the age of once living things (fossils, dead animals, plants and humans.) Half-life of Carbon14 is 5,730 years Compare amounts of Carbon14 in old items with the amount of Carbon14 new items to determine age. Uraium 238 is used to date non living things (rocks)

Making Synthetic Elements Scientists create new elements by smashing atomic particles into a target element. Isotope iodine131 used to diagnose thyroid problems. Radioisotopes can help discover how pesticides move throughout an ecosystem

Questions 1.Define half-life. 2.What is Carbon14 used to date? 3.What is the half-life of Carbon14? 4.What is Uranium238 used to date? 5.How do scientists create new elements? 6.How are synthetic elements useful?