Atomic theory Odds and ends. AMU 1.6 x 10 -27 Kg Mass of 1/12 of carbon – 12 isotope.

Slides:

Advertisements

Similar presentations

Topic A: Atoms and the Elements

Advertisements

Atomic Theory History of Atom Early Greeks believed that matter consisted of tiny particles – they called the “atoms”

» What is the name of this device? » Which scientist used this device?

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Stoichiometry Stoichiometry - The study of quantities of materials consumed.

Chapter 5: Atomic Theory: The Nuclear Model of the Atom

Atomic Structure Nucleus – contains protons and neutrons

Atoms: The building blocks of Matter

Basic Atomic Structure Democritus Dalton Subatomic Particles Symbol Notation Isotopes Average Atomic Mass.

Atomic Mass and the Mole. Relative Atomic Mass Units of grams are TOO LARGE for atoms! Relative atomic mass – compare to small particles – amu – “atomic.

Chapter 4.2 – The Structure of Atoms - protons have a positive charge -neutrons have no charge -protons and neutrons have almost the same size and mass.

C H E M I S T R Y Chapter 2 Atoms, Molecules, and Ions.

Classification of Matter. Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in the early 19th century,

THE BUILDING BLOCKS OF MATTER

Unit 3 Language of Chemistry Part 1 Zumdahl: Chapter 4 Holt: Chapter 3.

Stoichiometry Quantitative nature of chemical formulas and chemical reactions Chapter 3 (Sections )

Mass Number Atomic Number equals the # of... NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE ATOM.

Atomic Theory History of Atom Early Greeks believed that matter consisted of tiny particles – they called the “atoms”

Monday, Oct. 21 st : “A” Day Tuesday, Oct. 22 nd : “B” Day Agenda  Begin Chapter 3: “Atoms and Moles” Sec. 3.1: “Substances are Made of Atoms”  In-Class:

Midterm Review Chapter 3 Pg Atomic Theory pg  Atomic Theory – the idea that atoms are the building blocks of all matter  Everything is.

SURVEY OF CHEMISTRY I CHEM 1151 CHAPTER 2 DR. AUGUSTINE OFORI AGYEMAN Assistant professor of chemistry Department of natural sciences Clayton state university.

Weighing and Counting Atoms

Definite Proportions, Multiple Proportions and Atomic Theory

Atoms and Moles.  All matter is made of atoms  Law of definite proportions  Water is 88.8 % oxygen and 11.2 % hydrogen  Law of conservation of mass.

By: Andres Sanchez. Law Of Definite Proportions  Law of definite proportions states that two samples of a give compound are made of the same elements.

Unit 5: The Mole.

Quantitative Chemistry Chapter 3. Objectives Learning objective 1.2 The student is able to select and apply mathematical routines to mass data to identify.

C H E M I S T R Y Chapter 2 Atoms, Molecules, and Ions.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 3 Atoms: The Building Blocks of Matter.

Atoms and Compounds ICS III Week 4. How to read the Periodic Table.

Chapter 3 Atoms: The Building Blocks of Matter. The Atomic Theory  Law of conservation of mass  Mass is neither destroyed nor created  Law of definite.

CH. 3 - ATOMIC STRUCTURE The Atom: From Philosophical Idea to Scientific Theory OBJECTIVES EXPLAIN THE LAW OF CONSERVATION OF MASS, THE LAW OF DEFINITE.

Law of Conservation of Mass Law of Definite Proportions.

Determining the NUMBER of Protons Electrons and Neutrons in Atoms, Ions, and Isotopes.

Chapter 3 pages Modern Chemistry Chapter 3 Atoms: the building block of matter.

Atoms and Moles – Chapter 3 Substances are made of atoms 3.1.

The Atom Chapter 3. From Idea to Theory Democritus, Greek philosopher, 400 B.C., introduced the concept of an atom, an ‘indivisible’ particle. Democritus,

How is the mole concept related to chemical formulas?

Atoms Isotopes Average Atomic Mass Development of Atom

Chemical Foundations: Elements, Atoms, and Ions Atoms & Compounds.

Atoms and Molecules By Doba Jackson, Ph.D.. Outline of Concepts in this chapter Law of Constant Composition (sec. 2-4) –Mass Percentages Dalton’s Atomic.

Average Atomic Mass. Relative Atomic Masses  Masses of atoms (in grams) are very small, so for convenience we use relative masses.  Carbon-12 is our.

ATOMS: The Building Blocks of Matter Objectives 1.Law of conservation of mass 2.Law of definite proportions 3.Law of multiple proportions 4.Dalton’s Atomic.

MODERN CHEMISTRY CH 3 Atoms: The Building Blocks of Matter.

Chapter 3 Atoms: The Building Blocks of Matter. Sect. 3-1: The Atom: From Philosophical Idea to Scientific Theory  Democritus vs. Aristotle  Atom vs.

Chemistry – King William High School.  Foundations…  Law of conservation of mass – mass is neither created nor destroyed  Law of definite proportions.

1 Modern Chemistry Chapter 3 Atoms: The Building Block of Matter.

Atomic Structure. I. Atoms The atom is the basic unit of matter.

Chapter 3 Atoms and matter. laws The transformation of a substance or substances into one or more new substances is known as a chemical reaction. Law.

Law of conservation of mass states that mass can neither be created nor destroyed in a chemical reaction.

Dalton’s Atomic Theory. Law of Conservation of Mass The total mass of materials after a chemical reaction is the same as the total mass before the reaction.

Isotopes & Ions 4.7; Subatomic Particles Remember Dalton?  Remember Dalton’s atomic theory?  “All atoms of a given element are identical”. 

Atomic Structure. Subatomic Particles In the nucleus: Protons Mass  1 amu Charge = +1 Neutrons Mass  1 amu Charge = 0 In the electron cloud: Electrons.

The Atom CHAPTER 3.1 MS. COX’S CHEMISTRY CLASS. Lesson Objectives Explain the law of conservation of mass, the law of multiple proportions and the law.

Chapter Three ATOMIC THEORY NOTES. Important Concepts in a Nutshell First person to theorize that matter was made up of tiny particles was a Greek philosopher.

Chemistry Chapter Three – Atoms: The Building Blocks of Matter South Lake High School Science Department Ms. Sanders.

Atomic Theory & Periodic Table Unit 3 Part 1 (Ch. 4 & 5) Atomic Theory Introduction, Isotopes.

Chapter 3 The Atom. ____________ (450 B.C.) proposed that all matter is made up of tiny, indivisible particles. (atomos) 3-2.

C H E M I S T R Y Chapter 2 Atoms, Molecules, and Ions.

Atomic Unit Calculations. Calculating Atomic Mass Units (amu) Definition: A unit of mass used to express atomic and molecular weights.

Atomic Theory In 1808, the English Chemist John Dalton proposed the first theory of the nature of matter in stating that all matter was composed of atoms.

ATOMIC THEORY Honors Chemistry Topics of Discussion Summarize the Development of Atomic Theory Examine Atomic Structure.

Ch. 9 – Moles Law of definite proportions – for a pure substance, each element is always present in the same proportion by mass. Also, for a pure substance,

Atoms – The Building Blocks of EVERYTHING

Chapter 3 Atomic Theory.

Biology- The study of life and living things.

Atomic Structure.

Law of definite and multiple proportions

Q2 Name 3 subatomic particles. What particle has no charge?

The Atom Ch 3.1.

Presentation transcript:

Atomic theory Odds and ends

AMU 1.6 x Kg Mass of 1/12 of carbon – 12 isotope

Masses of particles Proton plus charge 1.6 x Kg = 1 amu Neutron no charge 1.6 x Kg = 1 amu Electron negative charge 9.11 x Kg = 0 amu

Atomic masses Average mass of various isotopes Found by multiplying isotope mass by its percentage in nature, then adding them all up.

examples Oxygen-16 x % = Oxygen-17 x 0.038% = Oxygen – 18 x 0.200% = Then add them up__________

example Copper 63 x 69.17% = Copper 65 x 30.83% = Then add _________________

example Argon % Argon % Argon % then add _________

FINAL EXAMPLE Naturally occuring Boron is 80.20% boron-11 and and % of some other isotope. The average mass is What is the mass of the other isotope?

MORE ATOM STUFF NOW THAT WE KNOW AN AMU IS 1.6 X Kg WHAT CAN WE DO WITH THAT INFO? IF WE KNOW THE AVERAGE AMU FOR AN ATOM, WE CAN TRANSLATE THAT INTO A QUANTITY WE CAN WORK WITH IN THE LAB!

THE MOLE The amount of a substance that contain as many particles as there are atoms in exactly 12g of carbon By experiment that amount is 6.02 x particles

calculation Average Amu of carbon = amu x 1.661x Kg x 1000 g = x Amu Kg x g x x particles = g mole mole

RESULT WE CAN NOW HANDLE ATOMS IN THE LABORATORY AND KNOW HOW MANY WE HAVE! IF I HAVE GRAMS OF CARBON, I HAVE 1 MOLE OF CARBON, I HAVE X ATOMS SAME WITH ANY OTHER MASS ON THE PERIODIC TABLE!!!!!

3 MAJOR LAWS OF CHEM CONSERVATION OF MATTER IN ANY ORDINARY CHEMICAL REACTION, MATT IS NOT CREATED OR DESTROYED DEFINITE PROPORTIONS IN A GIVEN COMPOUND, THERE ARE ALWAYS THE SAME ELEMNTS IN EXACTLY THE SAME MASS RATIO

MULTIPLE PROPORTIONS WHEN DIFFERENT COMPOUNDS ARE FORMED FROM THE SME TWO ELEMENTS, THE RATIOS ARE ALWAYS SMALL WHOLE NUMBERS. WATER H 2 0 vs peroxide H CARBON DIOXIDE CO 2 vs CARBON MONOXIDE CO