Figure: 21-T01.

Slides:



Advertisements
Similar presentations
Properties of nucleus 26.2 Binding energy and mass defect. UNIT 26 : NUCLEUS is defined as the central core of an atom that is positively charged.
Advertisements

Aim: How are protons held together within the nucleus? Essential Questions : Why do certain elements undergo radioactive decay and others don’t? How do.
Nuclear Physics Selected Topics  Properties of Nuclei.
Nuclear Science What is in a nucleus? Why do nuclei decay? Where does radiation come from?
Atomic Mass & Number Isotopes The Periodic Table.
 Protons, neutrons, electrons too  Make up the atoms all around you!
Atomic Structure and the Periodic Table
1. Nucleons. Protons and neutrons 2. Nuclide
Subatomic particles Electron Proton Neutron NameSymbolCharge Relative mass Actual mass (g) e-e- p+p+ n0n / x x
Nuclear Stability Notes
Known nuclides PROPERTIES OF FUNDAMENTAL PARTICLES Particle Symbol Charge Mass (x Coulombs) (x kg) Proton P Neutron N.
What is the smallest unit of matter? An atom What is an atom made of? Subatomic particles protons (p + ) – positive charge neutrons (n) – no charge.
– a unit of matter; the smallest unit of a chemical element.
PROTON Proton: the positively charged particle found in the nucleus of an atom.
Physics 12 Mr. Jean May 20th, 2014 The plan: Video clip of the day Question #1 –Visiting the Relatives Binding energy Energy Deflection Mass and energy.
Inorganic Chemistry May 12, Describe how the strong force attracts nucleons Relate binding energy and mass defect Predict the stability of a nucleus.
Types of Radioactive Decay Kinetics of Decay Nuclear Transmutations
Atomic Mass. Each element found on the periodic table of elements is given an atomic mass The atomic mass tells you the average mass of the atoms of an.
Nuclear Reactions Nuclear Reactions.
LAB #1 Radioactivity RADIOACTIVITY: is spontaneous transition of an atomic nucleus from a higher energy to a lower energy state. This transition is accompanied.
2. What are isotopes? Use two particles from the table above to illustrate your answer. (3 marks) 17 O & 18 O (1) Same Atomic mass / number of protons.
© OCR The periodic table is an essential tool for all chemists. It is full of useful information. RELATIVE ATOMIC MASS ATOMIC NUMBER SYMBOL helium.
 Atoms  Elements are made of particles called atoms  Atoms are the smallest pieces of matter that contain all the properties of a specific element.
Atom and Periodic Table Review. What is the atom’s atomic number?
Chapter 21 Nuclear Chemistry
Parts of the Atom.
The Periodic Table.
Mass of constituent parts of the nucleus:
Mass to Energy Energy to Mass
All Need to Know About Atoms
Aim # 25: What is Radioactivity?
Atomic Structure and Isotopes
ELEMENTS, IONS AND ISOTOPES
Aim: What is an atom? DRAW IMAGES DO NOW: Identify X, Y, and Z as
Nuclear Chemistry I The Nucleus II III IV C. Johannesson.
Ch. 21 Nuclear Chemistry.
Basic Atomic Structure
Nuclear Intro.
Visual Vocabulary Chemistry.
Nuclear Stability Nuclear Changes
Atomic Particles Particle Charge Mass # Location Electron -1
Specific Charge of a Particle
Structure and Properties of the Nucleus
Ch – 3-2 NUCLEAR PROPERTIES
Unit 3: Part 2 of the Atom Nuclear Chemistry
Nuclear Stability.
The Nucleus Objectives:
Name That Atom! Use your knowledge of atoms to find the name of each of the following atoms. Use a Periodic Table!
CHAPTER 22 Nuclear Chemistry
I. The Nucleus What is “nuclear” energy? Where does it come from?
Nuclear Chemistry.
Atomic Structure.
Standard Grade Chemistry Topic 3
e- p+ n0 0 amu 1 amu 1 amu Electron proton Neutron
Name:__________ Date:_________
Nuclear Chemistry Chapter 21.
22.1 The Nucleus Essential Questions:
P2 Radiation from Rocks Revision pt1 Mock 2015
THE NUCLEUS: A CHEMIST’S VIEW
Unit 4 Nuclear Chemistry.
Nuclear Chemistry Radioactive Decay.
How small is an atom? Parts of the Atom What do the numbers mean?
The Nucleus Objectives:
Physics 4 – Mar 8, 2019 Agenda: P3 Challenge – None. Re: Short class
Atomic Structure Final Examination Review
Unit 4 – Nuclear Reactions
Nuclear Chemistry Essential Question: What are the different types of radioactive decay? How does each type change the nucleus?
Nuclear Chemistry Essential Question: How do we determine stability of a nucleus to compare different atoms?
Atomic Particles Particle Charge Mass (kg) Location Electron -1
Counting Subatomic Particles
Presentation transcript:

Figure: 21-T01

Figure: 21-T02

Fundamental Atomic Particles Symbol Charge (10–19 C) Mass (10–27 kg) Molar Mass (g/mol) Proton p +1.60218 1.672622 1.007276 Neutron n 1.674927 1.008665 Electron e –1.60218 0.000911 5.486 × 10–4 Table 22-1. Properties of Fundamental Particles

Figure: 21-02

Figure: 21-03

Modes of Nuclear Decay for Nuclides on Either Side of the Belt of Stability Figure 22-5. A detailed view of one portion of the N vs. Z plot of nuclides, illustrating the modes of nuclear decay for nuclides on either side of the belt of stability.

Figure: 21-04

Figure: 21-T04

Figure: 21-10

Binding Energy Per Nucleon vs. A The most stable nuclides lie in the region around A = 60. Figure 22-3. Plot of the binding energy per nucleon vs. mass number A. The most stable nuclides lie in the region around A = 60.

Figure: 21-16

Figure: 21-19

Figure: 21-20C