The Nucleus Topic 16.1.

Slides:

Advertisements

Similar presentations

Atomic Mass & Number Isotopes The Periodic Table.

Advertisements

Atomic Structure.  Describe the experiments of Thomson and Rutherford explain how they contributed to our present understanding of atomic structure.

Rutherford Experiment & Isotopes Mr. Rana 9/21/12.

The Structure of an Atom Chapter 4.2. Warm-up: KWL Chart - ATOMS What I Know About Atoms What I Would Like to Learn About Atoms What I Have Learned About.

The Atom. Dalton’s Atomic Theory 1.Elements are made of tiny particles called atoms. 2.All atoms of a given element are identical. 3.The atoms of a given.

Chapter 3 review With chalkboards. What is this called? z X A.

Atom – basic unit of matter 3 subatomic particles: protons, electrons, neutrons Atom is mostly empty space Atoms have small dense positive core (nucleus)

Journal #20 1. Who discovered the electron? 2. What did Rutherford discover?

Unit 3: The Atom. Atoms All matter is made of very tiny particles All matter is made of very tiny particles These particles have the same properties as.

Notes on Isotopes Remember Protons are (+) and Electrons are (-). Neutrons were the last subatomic particles to be discovered because they have no electrical.

{ Atom and Isotope Review Physical Science. An atom has 6 protons, 8 neutrons, and 6 electrons. What is the atomic mass?

Introduction to Atomic Particles. How will I know if I am successful? – I can name and describe three types of atomic particles Charge Location Mass –

Atomic Structure. Sub-Atomic Particles Nucleus – a dense, positively charged region at the center of the atom Proton p +  Positively charged particle.

Atomic Structure- Ch 4. Daltons Atomic Theory 1. All elements are composed of tiny indivisible particles called atoms. 2. Atoms of the same element are.

Radioactivity and the nucleus

Chapter 4 Atomic Structure 4.1 Defining the Atom

Atom-Building blocks of matter What are the main

Atomic Structure Notes

Atoms: The Building Blocks of Matter

All Need to Know About Atoms

Atomic Structure.

The structure of the atom.

Atomic Structure Concepts.

Parts of the Atom PSSA: A/S8.C.1.1.

Atomic Structure Subatomic Particles C. Johannesson.

4.2 -Atomic Structure Theory

Atomic Structure Notes

ELEMENTS, IONS AND ISOTOPES

STRUCTURE OF THE ATOM.

Introduction to Atomic Particles

SECTION III: A WORLD OF PARTICLES

Learning objective 2: I can understand the patterns found in the number of protons, neutrons, and electrons in an atom.

Bellwork or Teacher’s Pet – Atoms: Write 3 facts for the video.

Chapter 3 Atomic Theory.

Atomic Structure Chemistry, Unit 1.

Chapter 4 Atomic Structure.

The Chemistry of Life The Nature of Matter.

Chapter 3 Structure of the Atom

Atomic Particles Particle Charge Mass # Location Electron -1

Specific Charge of a Particle

Atomic Number Atomic Mass

Modern View of atom.

Atomic Structure Most of the mass of an atom is concentrated in an extremely small, dense, and positively charges core called the nucleus The nucleus contains.

Atomic Structure Chemistry.

Section 1 Structure of the atom and cells on the periodic table

Chapter 4 Atomic Structure 4.1 Defining the Atom

Warm Up #2 Label the following as a physical or a chemical change:

The Structure of an Atom

Intro to Atomic Structure

Chapter 4 Atomic Structure 4.1 Defining the Atom

Ch. 3 - Atomic Structure II. Masses of Atoms (p.75-80) Mass Number

Chapter 4 Atomic Structure 4.1 Defining the Atom

The Structure of an Atom

Topic: Structure of an Atom

Jeopardy Parts of the Atom How Many Atomic Models Q $100 Q $100 Q $100

Chapter 6-2 part 1 The Atom.

The Atom Unit 2 Topic 1.

Atomic Structure.

Ch. 4 - Atomic Structure II. Masses of Atoms Mass Number Isotopes

The Structure of an Atom

Chapter 6-2 part 1 The Atom.

Atomic Structure Atom = the smallest particle of an element that retains the properties of that element.

Topic: Structure of an Atom

The Atom Ch 3.1.

neutral equal electrons Atomic Number = Protons Element Symbol

Presentation transcript:

The Nucleus Topic 16.1

Outcomes There are no outcomes that correspond with this lesson…just some periodic table review.

Rutherford Rutherford’s gold foil experiment demonstrated that atoms contained a densely packed, positive charged core He called the tightly packed, positive particles protons

Discovering the Neutron Protons could not account for all the mass contained within the nucleus, in fact, the charge-to-mass ratio of a proton was twice that of a helium nuclei Rutherford suggested that the nucleus may also contain neutrons, neutral particles with about the same mass as a proton

Nuclear Definitions Proton- Positively charged particle in the nucleus (p+) Atomic number- Number of protons in the nucleus (equal to the number of electrons surrounding the nucleus in a neutral atom) Neutrons- Particle with no charge in the nucleus (n0) Nucleons- Number of protons and neutrons collectively Mass number- Sum of the number of protons and neutrons in a nucleus Electron- Particle with a negative charge surrounding the nucleus (e-)

Nuclear Terms and Notations Atomic Mass (A): number of nucleons (protons & neutrons) Atomic Number (Z): number of protons Element Symbol (X) Neutron Number (N): number of neutrons (A – Z)

Sample Problem How many protons and neutrons does a carbon atom have?

Isotopes Many elements have two or more isotopes Isotopes: same number of protons, but differing number of neutrons Their chemical properties are almost identical, however, their physical properties can differ dramatically. Some isotopes are very stable, while others are highly radioactive

Atomic Mass Units Atoms and nuclei, are incredibly small and therefore using kilograms is illogical For calculations involving subatomic particles the atomic mass unit (u) is used – which is 1/12 the mass of a carbon12 isotope 1 atomic mass unit () = 1.6605x10-27kg

(DON’T THINK OF ‘C’ AS A UNIT – WE MUST APPLY c2) Converting Mass The data sheet lists masses in units of MeV/c2. How do we convert this to kilograms? Example: An electron is listed as 0.511 MeV/c2 (DON’T THINK OF ‘C’ AS A UNIT – WE MUST APPLY c2)

Homework p. 167 #1-3