Ch. 3 – Atoms: The Building Blocks of Matter

Slides:

Advertisements

Similar presentations

Ch. 3 – Atoms: The Building Blocks of Matter An atom is the smallest matter that can’t be divided into smaller matter. What is an atom made up of? –Nucleus.

Advertisements

Chapter 3 Atoms: The Building Blocks of Matter. I. The Atom *Matter: anything that has mass and volume *Indirect Evidence: evidence you get without actually.

Development of the Atomic Theory

Basic concepts for general chemistry Lec.2. Important definitions Element  Any substance that contains only one kind of an atom.  Each element is represented.

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

CHAPTER 3 Atoms: The Building Blocks of Matter CHEMISTRY.

Mullis1 Atomic Model Review ( Match Theory to Scientist) 1. Atoms are solid spheres. 2. Electrons move around the nucleus in specific levels. 3. Protons.

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.

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

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.

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.

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

3.3: Counting Atoms How do I count and calculate the mass of atoms?

Chapter 4 – Atomic Structure. Greek Atomic Theory (400 BC) “There is no smallest among the small and no largest among the large, but always something.

A TOMS Chapter 16 and 17 Physical Science Honors.

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

CHAPTER 3 Atoms& Atomic Theory Brief History of Atomic Theory Particle Theory (400 BC) –A Greek philosopher named Democritus proposed that matter was.

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,

Ch. 3: Atoms 3.1 Foundations.

? ? What do atoms look like? ? ?.

Chapter 3 Atoms and Elements

Chapter 3 Atoms: The Building Blocks of Matter

Chapter 3 The Atom.

Unit 3 Atomic Structure.

The Building Blocks of Matter

Atoms: The Building Blocks of Matter

Atomic Structure.

4.2 -Atomic Structure Theory

Atoms: The Building Blocks of Matter

Atoms: The building blocks of matter

Physical Science Chapter 4 – Section 2

Chapter 3 – Atoms: The Building Blocks of Matter

SECTION III: A WORLD OF PARTICLES

Chapter 3-1: The Atom Summarize the five essential points of Dalton’s atomic theory Explain the relationship between Dalton’s Atomic Theory and the laws.

Subatomic Particles Subatomic particles - 3 important to chemistry

Atoms – The Building Blocks of EVERYTHING

Counting Atoms Section 3.3.

Chapter 3 Atomic Theory.

Atomic Structure Nat

Matter Unit Structure of an Atom.

Atoms: The Building Blocks of Matter

ATOMS Standard C-2 Students will demonstrate an understanding of atomic structure and nuclear processes.

Atoms & Molecules.

Presentation Properties of Atoms

Goal – 3 Atoms Students will be able to identify parts of the atom and how the parts of the atom play a role in the periodic table.

Foldables: Atoms Terms.

Atomic Structure Ch. 3.

Evolution of Atomic Theory & Counting Atoms

Bellwork Pick the handouts off the front table

ELEMENTS & ATOMS.

Mrs. Butsch 8th Grade Science

Warm Up 1.What did Rutherford’s scattering experiment show? Need to list 2 important findings. 2. What did Thomson discover? Describe the atomic model.

Atoms: The Building Blocks of Matter

Counting Atoms CHAPTER 3.3.

The Structure of an Atom

Atoms: The Building Blocks of Matter

Ch. 3 Atoms 3.3 Counting Atoms.

Atoms: The Building Blocks of Matter

Atomic Number, Mass Number, Atomic Mass and Isotopes

Here’s What Matters Matter Anything that takes up space

Atomic Structure Nucleus Protons Neutrons Electrons.

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

Structure of an Atom What is an ATOM??? Pg

Has mass and takes up space

Atomic Particles Particle Charge Mass (kg) Location Electron -1

Atoms: The Building Blocks of Matter

The Atom Ch 3.1.

Presentation transcript:

Ch. 3 – Atoms: The Building Blocks of Matter An atom is the smallest matter that can’t be divided into smaller matter. What is an atom made up of? Nucleus Proton – positive charge Neutron – neutral charge Electron clouds (energy levels) Electrons – negative charge Atom is Greek for indivisible

Bohr’s Model Dalton’s Theory Explains the make up of an atom. Nucleus  Protons & Neutrons Electron Clouds  Electrons Bohr’s Model Show’s the make up of an atom.

MASS # - ATOMIC # = NEUTRONS Atoms of different elements may combine to form chemical compounds. In chemical reactions atoms are either combined, separated, or rearranged Atoms cannot be created nor destroyed. Each element can have more than 1 atom. Ex. Cl2 MASS # - ATOMIC # = NEUTRONS

Atoms of the same element may have different masses Atoms of the same element may have different masses. These are called isotopes. Ex. Hydrogen has 3 isotopes  Protium, deuterium, tritium. What does the atomic number tell you? Number of protons in each atom of an element. What does the mass number tell you? Total number of protons and neutrons in the nucleus of an atom. If an element has isotopes for that element they are called nuclides.

An atomic mass unit is a standard unit used for comparison. Carbon has exactly 12 atomic mass units (U) and is used as a standard for comparison. Each element on the periodic table has an average atomic mass. Why do you suppose it is an average? Average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element. Ex. Cu  69.17% is Cu – 63; 30.83% is Cu – 65.

Mole, Molar Mass, and Avogadro’s number all help describe an element. CD ROM Mole – Roughly the mass of a substance that is has 6.02 x 1023 particles (atoms or molecules). All of the average atomic masses on the periodic table is equal to 1 mole (mol.). Ex. B 10.81g = 1 mol. Ex. Zn 65.39g = 1 mol.

Avogadro’s number is 6.02 X 1023 particles. The number of particles (atoms or molecules) in exactly one mole is always 6.02 X 1023. Ex. B 10.81g = 6.02 X 1023. Ex. Zn 65.39g = 6.02 X 1023. Molar mass – the mass in grams of one mol. Of a pure substance. Basically the average atomic mass in grams. Ex. B 10.81g = 1 mol. = 6.02 X 1023. Ex. Zn 65.39g = 1 mol. = 6.02 X 1023.

The molar mass of all elements will always contain the same number of atoms, which is 6.02 X 1023. Which atoms are heavier? Do the heavier atoms have more atoms in one mole? Pg. 90 Sample Problems from pg. 82-85.