The law of conservation of mass states that:. The law of conservation of mass states that: matter cannot be created or destroyed. Only changed in form.

Slides:

Advertisements

Similar presentations

Advertisements

ATOMIC STRUCTURE. Objectives: SWBAT Identify three subatomic particles and compare their properties. Distinguish the atomic number of an element from.

Introduction to the Atom and Atomic Models

Chapter 4 Atomic Structure

Part II Discovers the Electron Experimented with cathode rays Took a glass tube and pumped most of the air out of it. Applied a high voltage that.

ATOMIC STRUCTURE AND HISTORY

Atomic Theory “History of. . . ”.

Democritus: The Atom (around 400 BCE)

ATOMIC STRUCTURE. Atomic Structure All matter is composed of atoms. Understanding the structure of atoms is critical to understanding the properties of.

Dual Nature of Light. Light Quanta. Photoelectric Effect.

How Big is an Atom? Imagine that you could increase the size of an atom to make it as big as an orange. 

History of Atomic Theory

Learning Standards Atomic Structure Broad Concept: Atomic models are used to explain atoms and help us understand the interaction of elements and compounds.

Atomic Structure and The Periodic Table

Introduction to the Atom and Atomic Models

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.

Chemistry Atomic structure Chapter 4, and Chapter 5, p

Chemistry Sheds Light on Our Lives Unit 4 Atoms and Light

Chemistry: Matter and Chemical Bonding Early Atomic Theories.

Atomic Theory Chapter 3 Sections 1 &2 9/18/14.

The Physical Setting Chemistry.

1 The Physical Setting Chemistry Jerry Deutsch 2 New York State Education Department Core Curriculum

FAMOUS SCIENTISTS ATOMIC MASS ATOMIC NUMBER ATOMIC.

Chapter 4 Atomic Structure.

Atomic Theory Timeline

The History of the Atom…. went against, Aristotle, who believed that matter was composed of four qualities: earth, fire, air and water all matter is composed.

Atomic Theory “History of... ”. The Ancient Greeks Democritus and other Ancient Greeks were the first to describe the atom around 400 B.C. The atom was.

WHAT’S A THEORY?. Atomic Theory The Ancient Greeks Democritus and other Ancient Greeks were the first to describe the atom around 400 B.C. The atom was.

The History of the Atom. Atomic Theory Because we can not see atoms, we use models to teach and learn about atoms. The atomic theory has changed over.

History of the Atom Democritus Democritus: It was 400 BC when he came up with the idea that matter could not be divided indefinitely. This lead to the.

Chapter 4 Atomic Structure

Unit 2 - Lecture 1: Structure of the Atom

Quantum Physics Dalton’s Atomic Theory Dalton’s indivisible atom has not been disregarded—it has been modified to explain new observations. Two important.

Development of Atomic Theory Ancient Times | Dalton's Postulates | Thomson's Discovery of Electron Properties | Rutherford's Nuclear Atom | Bohr's Nuclear.

Development of the Atom A brief review of the history…

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.

History of the Atomic Model

Atomic Structure Subatomic Particles An atom is the smallest unit of an element. It consists of three major particles: Note:

Review Class #1.  Greeks ◦ Matter is made up of tiny, discrete particles  Fire, Earth, Wind, Water  Boyle ◦ Found gold and silver as being elemental.

What do I need to know for the test?. 460 BC-created the 1 st Atomic Theory of Matter (not modern atomic theory however) HIS THEORY Matter is composed.

Atomic Structure Models. Dalton’s Atomic Model Solid sphere Evidence: Conservation of matter Law of definite composition Law of multiple proportions.

MODELS OF THE ATOM A HISTORICAL PERSPECTIVE  Anything that has mass and takes up space  If you did not know this definition, how would you describe.

1 The Physical Setting Chemistry Jerry Deutsch 2 New York State Education Department Core Curriculum

CP Chemistry Chapter 8 Atomic Theory Subatomic Particles Protons Protons Neutrons Neutrons Electrons Electrons.

Chapter 4 “Atomic Structure”. Introduction to the Atom and Atomic Models.

Models of the Atom. Ancient Greece 300 BC in Greece School of thought that matter is made up of tiny indivisible, invisible, indestructible, fundamental.

The Atom - Scientists. Philosophers Democritus – believed matter was not infinitely divisible THERE WERE NO EXPERIMENTS TO TEST HIS IDEAS Matter is composed.

History of Atomic Theory Figuring Out Atoms. Dalton’s Atomic Theory 1.Matter is composed of extremely small particles called atoms. 2.Atoms are indivisible.

A good theory/model should :  Explain observed (empirical) evidence  Provide a reasonable, logical, theoretical explanation  Predict the results of.

THE STRUCTURE OF THE ATOM.  All atoms consist of 2 regions:  1) Nucleus: very small region located near the center of the atom  Proton: positively.

Greeks Before 400 BC Observers (not scientists) did not use scientific experiments Matter could be endlessly divided Matter is made of fire, water, air,

Essential Question: What type of model did Thompson, Rutherford, and Bohr propose about the atom. ATOMIC STRUCTURE Atom- smallest particle of an element.

Atoms CHAPTER 4 1. Let’s Review! o Matter is… o Anything that has mass and takes up space o All matter is made of elements – substances that cannot be.

POD Who were the major scientists involved in discovering the model of the atom?

Goal 5.01 Atomic Theory. Basic Laws of Chemistry Law of conservation of massLaw of conservation of mass: mass is neither created or destroyed during chemical.

ATOM Early Thoughts Greeks matter is made up of particles--4 elements 4 elements --air--fire--water- -- earth Aristotle-- Continuous theory Democritus.

UNIT 2 Atoms, Molecules, and Ions. 1. Each element is composed of extremely small particles called atoms. 2. All atoms of a given element are identical.

The law of conservation of mass states that:

Atomic Theory “History of. . . ”.

Unit 8: Introduction to Chemistry

The law of conservation of mass states that:

Atomic Theory Models and Particles.

Atomic Structure/ Periodic Table

ATOMIC STRUCTURE.

The law of conservation of mass states that:

Atomic Theory The idea that matter is made up of atoms, the smallest pieces of matter.

Presentation transcript:

The law of conservation of mass states that:

The law of conservation of mass states that: matter cannot be created or destroyed. Only changed in form.

Who was responsible for the Gold Foil Experiment? What where the results of the experiment? What did he conclude based on his results?

Ernest Rutherford.

The results were: most of the radiation passed through with little deflection a small portion was deflected at wide angles, including back at the source of the radiation.

He concluded that the atom contain a small positive center called the nucleus, which accounted for most of the mass of the atom (because of _________.) He also determined that most of the volume of an atom was empty space. (because of _______________.)

How many protons does the following atom have?

31 Protons Because………..

The atomic number, which is the number of protons, is 31 Atomic Number Mass Number

Which model of the atom did John Dalton create?

John Dalton was responsible for the “marble” model of the atom. A solid, neutral, indivisible sphere.

What are the main flaws with Dalton’s model of the atom?

1. A) He thought atoms were indivisible, proven later to be divisible (into____.) B) Also, thought the atom was solid. Later proven that the volume is mostly empty space.(by……) C) Thought atoms were neutral, actually “net neutral” which means…..

A) He thought atoms were indivisible, proven later to be divisible (into____.) a positive nucleus (which contain proton/neutrons) and electrons B) Also, thought the atom was solid. Later proven that the volume is mostly empty space.(by……Rutherford’s gold foil experiment. Found that most of the radiation passed straight through as though it had nothing to interact with. C) Thought atoms were neutral, actually “net neutral” which means…..the positive protons are balanced out by the negative electrons.

2. Thought all atoms of an element were identical to each other. There are ______ of all elements.

ISOTOPES: Dalton’s model believed that all atoms of a given element were identical to each other. He did not account for isotopes of the elements.

What distinguishes isotopes of an element from one another?

The number of neutrons (which helps determine the _____________) distinguishes one isotope from another. Mass number

Write the complete nuclear symbol for potassium ion with a +1 charge.

How many neutrons and electrons in this potassium ion?

20 neutrons 18 electrons

Calculate the average atomic mass of an element with the following isotopes: Element – 127 (67.02%) Element – 128 (25.67%) Element – 129 (7.31%)

amu 127 x.6702 = x.2567 = x.0731 = = amu

Who was responsible for the plum pudding model? What experiment did he use to arrive at this model?

JJ Thomson completed the cathode ray tube experiment.

What experimental results led Thomson to believe that Dalton’s model was incorrect?

He found that he could predictably alter the course of the cathode ray using magnetic and electric fields. The ray acted as a stream of negatively charged particles that were present in all substances and smaller than atoms.

Describe the Plum Pudding Model.

The plum Pudding model has negative electrons scattered evenly throughout a positive mass.

What was Max Planck’s view on energy? How was this different from the previous view? Who help prove Planck’s idea? How?

Suggested that energy could only be absorbed or emitted in pieces of certain size. (A quantum amount) Energy was thought to be continuous. Einstein used his idea to explain the Photoelectric effect. Bohr used his idea to explain emission spectra.

Explain the photoelectric effect.

In the photoelectric effect, electrons are ejected from a metal surface when light with a certain minimum energy (or frequency) strikes the surface of the metal. If the light did not have the correct energy (frequency) no effect was noticed.

What was Bohr’s model? How was it different from Rutherford’s model? How was it similar to Rutherford’s model?

Differences: Bohr solar system model suggested that the electrons were quantized, and therefore where only allowed certain orbits corresponding to certain energies around the nucleus of the atom. Rutherford’s model just had one general orbit for the electrons around the nucleus.

Similarities: Both believed that the atom contained a nucleus that accounted for most of the atom’s mass and all the positive stuff. Both believed that the electrons were around the nucleus, in orbit. Both believed that most of the volume was empty space, as supported by gold foil experiment

Based on the Bohr model of the atom, explain what happens to produced the yellow flame when sodium chloride is put into the Bunsen burner flame.

When the electron absorbs a quantum amount of energy, it “jumps” to a higher less stable energy level (excited state). If a lower level is open, the electron will release a photon of light with a quantum amount of energy, and fall back to a lower, more stable energy state (ground state). These released photon are the source of the color produced in the flame.

Write the : orbital diagram for beryllium electron configuration for iron noble gas notation for platinum

Be=1s __ 2s __ Fe=1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Pt= [Xe] 6s 2 4f 14 5d 8

What are the quantum numbers that describe the last electron in the following and identify the element (by name if possible) it describes: 4f 8 2p 3 1s 1 5d 8

n= l= m= m s = -1/2 +1/2 +1/2 -1/2 Tbnitrogen hydrogenplatinum

If the first QN=3, what are the possible values of the 2 nd QN? How many orbitals exist on the 3 rd energy level? How many electrons? If l=3: what type of orbital? What are the possible values of the 3 rd QN?

2 nd QN (l)= 2 or 1 or 0(n-1) to 0 3 rd energy level has 9 orbitals (#orbitals =n 2 ) has 18 electrons (#e - = 2n 2 ) In a f-orbital, and the 3 rd QN may be -3, -2, -1, 0, +1, +2, or +3. (- l to + l )