Unit 3. The Atom & Modern Atomic Theory
|
|
|
- Kelly Page
- 6 years ago
- Views:
Transcription
1 Unit 3 The Atom & Modern Atomic Theory
2 Theories of the Atom Early Models & Thoughts: Democritus Matter is made up of tiny particles called atoms. Smallest unit that retains the identity of the element
3 Theories of the Atom John Dalton: Hard Sphere model The main points of Dalton's atomic theory were: Elements are made of extremely small particles called atoms. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties. Atoms cannot be subdivided, created, or destroyed. Atoms of different elements combine in simple wholenumber ratios to form chemical compounds. In chemical reactions, atoms are combined, separated, or rearranged.
4
5 Theories of the Atom J.J. Thomson: Cathode Ray Tube experiment. Found the atom to be a positively charged sphere, negatively charge electrons embedded within the sphere. Discovered the electron Plum pudding model of the atom.
6 Cathode Ray Tube Experiment k
7
8 Gold Foil Experiment bc &feature=related
9 Theories of the Atom Ernest Rutherford Gold Foil experiment : Shot alpha particles at gold foil. Some went straight through others bounced back & deflected at odd angles. His 3 conclusions: 1. Atoms are mostly empty space, 2. Dense positive center. 3. Most of the mass of the atom is in the center (nucleus) Model of the atom has a nucleus with orbiting electrons.
10 Theories of the Atom Bohr Model: Planetary Model of the atom The atom contained a nucleus w/ protons and Neutrons Each electron in an atom is allowed to be in certain orbits that correspond to different amounts of energy. Electrons can jump orbits (energy levels)
11 Theories of the Atom Electron Cloud/ Wave Mechanical Model: Current model Protons & neutrons in the nucleus Electrons are in areas called orbitals and the model is based on the probability of finding an electron. Greater cloud density = increased probability of finding an electron. There is a greater chance of finding an electron in certain orbitals.
12 Theories of the Atom The modern model of the atom is based on the work of many scientists over a long period of time.
13 Venus Explains the Atom CM
14 Atomic Structure
15
16 Atomic Structure Moseley: Devised the concept of atomic number Said atomic number of an atom is equal to the number of protons in the atom's nucleus.
17 The Periodic Table can tell you about an atom. Atomic Mass = #Protons + #Neutrons # Protons
18 Atomic Structure 3 Important Ideas: 1 2 The atomic number is the ID of the element unique to each element). 3
19 Atomic Structure 3 Important Ideas: 1 2 The atomic number is the ID of the element unique to each element). In a neutral atom: # of Protons = # of electrons 3
20 Atomic Structure 3 Important Ideas: 1 2 The atomic number is the ID of the element unique to each element). In a neutral atom: # of Protons = # of electrons 3 When an atom gains or loses an electron, it is now an ion
21 Atomic Structure Charge = # of protons # of electrons
22 Atomic Structure Example 1. What is the name of the element whose atoms have 11 protons? Example 2: How many protons and electrons in an oxygen atom? Example 3: How many electrons and protons in Na +?
23 Atomic Structure Example 4: Write the symbol for the ion with 9 protons and 10 electrons. Example 5: Write the symbol for the ion with 13 protons and 10 electrons. Example 6: How many protons & electrons in S -2 ion?
24 Atomic Structure, Part II Reflect: Why use the a.m.u. scale to measure the mass of an atom?
25 Atomic Structure, Part II a.m.u. : Atomic Mass Unit To determine the number of neutrons: # of neutrons = mass number atomic number
26 Atomic Structure, Part II Example 1: How many neutrons, protons, and electrons are in an ion? Example 2: Determine the number of protons, electrons, and neutrons this ion:
27 Atomic Structure, Part II Example 3: Write the complete chemical symbol of an element with 21 protons, 24 neutrons, and 18 electrons. Example 4: Write the complete chemical symbol of an element with 53 protons, 74 neutrons, and 54 electrons.
28 Ar Element Symbol Mass Number # of Protons # of Neutrons # of Electrons Ion Charge Boron 5 0 Na Al Oxygen O -2 Calcium Sulfur 32 0
29 Element Symbol Mass Number # of Protons # of Neutrons # of Electrons Ion Charge Boron B Na Al Oxygen O -2 Calcium Sulfur 32 0 Ar 18 18
30 Element Symbol Mass Number # of Protons # of Neutrons # of Electrons Ion Charge Boron B Sodium Na Al Oxygen O -2 Calcium Sulfur 32 0 Ar 18 18
31 Element Symbol Mass Number # of Protons # of Neutrons # of Electrons Ion Charge Boron B Sodium Na Hydrogen H Al Oxygen O -2 Calcium Sulfur 32 0 Ar 18 18
32 Element Symbol Mass Number # of Protons # of Neutrons # of Electrons Ion Charge Boron B Sodium Na Hydrogen H Chlorine Cl Al Oxygen O -2 Calcium Sulfur 32 0 Ar 18 18
33 Element Symbol Mass Number # of Protons # of Neutrons # of Electrons Ion Charge Boron B Sodium Na Hydrogen H Chlorine Cl Aluminum Al Fluorine F Oxygen O Calcium Ca Sulfur S Argon Ar
34 Atomic Structure, Part II Isotope: Same element (same # of protons), but different number of neutrons. (So the mass of each isotope is different). Remember: atomic mass is the weighted average of masses of these isotopes.
35 Atomic Structure, Part II (isotope mass)(% abundance) + (isotope #2 mass)(% abundance) Example 1: Chlorine has two isotopes, chlorine 35 and chlorine 37. Approximately 75% is Cl-35 and 25% is Cl-37. Which isotope should the weighted average be closer to?
36 Atomic Structure & Isotopes (isotope mass)(% abundance) + (isotope #2 mass)(% abundance) Example 2: Boron-10 has a relative abundance of 19.78%. Boron-11 has a relative abundance of 80.22%. Calculate the average atomic mass.
37 Atomic Structure & Isotopes (isotope mass)(% abundance) + (isotope #2 mass)(% abundance) Example 3: The relative masses and abundances of Iodine are given below. Calculate the average atomic mass. Isotope % Abundance I % I % I %
38 Reviewing the Atom The Wave-Mechanical Model of the Atom
39 Reviewing the Atom Protons Neutrons Electrons Charge Mass Where found If you change the number of these particles, you get How to figure out how many an atom has
40 Bohr Model & Electron States
41 Bohr Model & Electron States Electron Configurations: Ordered sequence showing how many electrons are in each Principle Energy Level for a particular atom. Given in your reference table, starting from energy level 1 Note the * for elements 72 and up
42 Ex: or 2-4 or 2-7 Bohr Model & Electron States Valence Electrons: Outer most electrons found in the last Principle Energy Level that are used for bonding. Hint: Look at your periodic table. In each box is the Bohr e- configuration. The last number are the valence electrons.
43 Bohr Model & Electron States
44 Bohr Model & Electron States Practice: Write the electron configurations of the following atom and then state how many principle energy levels each element has. Element Electron Configuration # of Principle Energy Levels Neon Strontium Bromine Magnesium Copper
45 Bohr Model & Electron States Directions: Draw a Bohr model of the following neutral atoms using the electron configuration on the Periodic Table. Include the number of protons and neutrons in the nucleus and write the electron configurations in the box below.
46 Bohr Model & Electron States Directions: Draw a Bohr model of the following neutral atoms using the electron configuration on the Periodic Table. Include the number of protons and neutrons in the nucleus and write the electron configurations in the box below.
47 Bohr Model & Excited States
48 Ground State: Bohr Model & Electron States All electrons are in their lowest possible state. Ex: Magnesium Excited State: An electron has jumped to a higher principle energy level. Ex: Magnesium
49 Bohr Model & Electron States
50 Electromagnetic Spectrum
51 In different scenarios, light behaves as a continuous wave AND as individual particles.
52 Light & Quantum Theory Much of the understanding of how electrons behave in atoms comes from studies of how light interacts with matter.
53 One photon interacts with 1 atom of matter at a time.
54 Depending on what orbital the electrons jumped to and fell from, there will be photons of different energy emitted. We can see the color of those photons.
55 Electron Transitions Key Idea #1 Longer wavelengths (red end of spectrum) have less energy. Shorter wavelengths (violet end of spectrum) have more energy
56 Electron Transitions Key Idea #2 When electrons move up energy levels, this requires energy (remember protons and electrons attract!). (Ground Excited) When electrons move down energy levels (Excited Ground), they emit energy as light waves Different transitions result in different energy emissions (i.e. different colors)
57 Electron Transitions Key Idea #3 Each atom emits a specific number and pattern of bands based on its electron configuration when you pass its light through a prisim.
58
59 Bohr Model & Electron States Ground State: When electrons are at their lowest possible energy state. Example electron configuration: Excited State: When an electron gains energy (heat or electricity) and jumps to a higher PEL. Example electron configuration: 2 7 3
60 Bohr Model & Electron States How Light is Produced: 1. Electron(s) absorb energy in the form of heat or electricity 2. Electron(s) then jump up to a higher PEL & are in the excited state. 3. The electron(s) then fall back down to the ground state. 4. When the electron(s) falls back to the ground state it emits a photon of light (energy absorbed = energy emitted).
61 Bohr Model & Electron States Flame Test: Metallic salts are put in a flame A specific color of light is given off
62 Bohr Model & Electron States Bright Line Spectrum: Electricity is run through a gas tube A specific color of light is given off Light is passed through a prism A unique patter of colored lines are produced Ca be used to ID an element!
63 Red light has the least energy. Violet light has the greatest energy.
64 Review of Light & Quantum Theory Much of the understanding of how electrons behave in atoms comes from studies of how light interacts with matter.
65 In different scenarios, light behaves as a continuous wave AND as individual particles.
66 One photon interacts with 1 atom of matter at a time. Energy, wavelength, frequency are associated with each photon.
67 Bohr took his model of the atom and stated that electrons can absorb certain amounts of energy and then release that energy in the form of a photon.
68 Review of Light & Quantum Theory When all electrons are at their lowest possible energy, it is called the Ground State. When the electron absorbs a specific amount of energy, it moves to a higher orbital and is in the excited state.
69 Depending on what orbital the electrons jumped to and fell from, there will be photons of different energy emitted. We can see the color of those photons.
70 Every atom has a range of colors emitted when their electrons get excited and fall back down. Sodium: Orange Copper: Green Strontium: Drk. Orange Mercury: Blue
71 The colorful lights of fireworks are emitted by "excited" atoms; that is, by atoms that have absorbed extra energy. Different compounds within the fireworks give them their signature colors.
72 Light can be further analyzed by passing it through a prism. White light when passed through a prism breaks up into all the colors of the rainbow (ROYGBIV)
73 When the color of light emitted by an atom is passed through a prism, only certain colors are observed. These specific colors are called a Bright Line Spectrum. Each line spectra is different for every element and can serve to identify a particular element. Hydrogen:
74 Electron Configurations Reflect: Think of electrons, all negatively charged, in a cloud around the nucleus. How can they be organized to minimize repulsion?
75 Electron Configuration3 Wave Mechanical Model: Electrons are organized in orbitals, or areas of probable electron location
76 Electron Configurations Heisenberg Uncertainty Principle: We cannot know both the direction and location of electrons measuring one changes the other
77 Organized by: which is like Principle Energy levels (7 total, numbered 1, 2, etc) Floors in an apartment Sublevels (Named s, p, d, f) The actual apartment Orbitals (Can hold only 2 electrons) Rooms in the apartment
78 S 1 Orbital Holds 2 e- P 3 Orbitals Holds 6 e- d 5 Orbitals Holds 10 e-
79 Each sublevel holds a different number of orbitals: s = 1 orbital = 2 electrons p = 3 orbitals = 6 electrons d = 5 orbitals = 10 electrons f = 7 orbitals = 14 electrons
80 Electron Configurations Principal Energy Level Type of Sublevel (shape of orbitals) Number of Orbitals in Sublevel Electron Capacity of Sublevel
81 Electron Configurations
82
83 Electron Configurations Sublevel: Sublevels are contained within a PEL. There are 4 shapes /types that are labeled with letters (s, p,d, f). *sublevels are regions of space where the electrons w/ specific energies live. s sublevel
84 Electron Configurations p sublevel
85 Electron Configurations d sublevel
86 Electron Configurations f sublevel
87 Electron Configurations Orbital: Orbitals make up the sublevels. Each orbital can hold only 2 electrons max. The p sublevel contains 3 orbitals. Each holds 2 electrons for a total of 6 electrons in the p sublevel s sublevel has 1 orbital. 2 e- max d sublevel has 5 orbitals. 10 e- max f sublevel has 7 orbital2. 14 e- max
88 Electron Configurations When writing an electron configuration, the general format is to list the information in the following order: PEL then sublevel then # of Electrons 1,2,3 s,p,d,f write as an exponent You start with the innermost electrons and continue describing the location of all electrons as you move away from the nucleus. General Trend: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2
89 Analogy Electron Apartment Complex: Each floor represents a PEL. On the first floor (n =1)there is only 1 apartment. Apartment s. It is the cheapest apartment (lowest in energy). It is a studio (one room) and can only hold 2 occupants (electrons). s n = 1
90 Analogy Electron Apartment Complex: On the second floor (n = 2)there are 2 apartments. One studio apartment (s) that can hold 2 people (which costs more since it is on the 2 nd floor) and a p apartment that has 3 bedrooms (2 people to a room) for a total of 6 occupants, which costs more than the studio because it is bigger. (*cost = energy) s p p p n = 2 s
91 Analogy Electron Apartment Complex: On the 3 rd floor (n = 3)there are 3 apartments. One studio apartment (s) that can hold 2 people (which costs more since it is on the 3 nd floor) and a p apartment that has 3 bedrooms (2 people to a room) for a total of 6 occupants, which costs more than the studio because it is bigger. Then there is the d apartment that has 5 bedrooms, 2 people to a room for a total of 10 occupants. s p p p d d d d d n = 3 s p p p s
92 Analogy Electron Apartment Complex: On the 4 th floor (n = 4) there are a total of 4 apartments. 1 studio, 1 three bedroom, a 5 bedroom and lastly the Penthouse with a total of 7 bedrooms (2 occupants to a room) that can house up to 14 people. This apartment costs the most to occupy. (The s, p and d apartments are also more expensive than the ones on lower floors). n = 4 s p p p d d d d d f f f f f f f s p p p d d d d d s p p p s
93 Analogy
94 Be: Practice C: F: Ne+: * Exponents should add up to the total # of electrons in the atom!
95 Agenda Warm up Complete the top Reviewing the Atom In your work packet you got last week Notes on Orbital notation Practice notation H.W. 3.7
96 Orbital shapes
97 Using the Periodic Table to Write Sublevel Electron Configurations
98 Using the Periodic Table to Write Sublevel Electron Configurations
99 Practice Examples H: He: Li: Be: B: C: N:
100 Orbital Notation Electron Configurations: 1s 2 Orbital Diagrams:
101 Orbital Notation Orbital Diagram: A pictorial representation (using arrows to represent electrons) of sublevel electron configurations. Examples of Orbital Diagrams: Orbital diagram for Oxygen
102 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Aufbau: Electrons are added 1 at a time to the lowest energy orbitals available until all the electrons are used.
103 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Pauli Exclusion Principle: An orbital can only hold a maximum of two electrons.
104 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Hund s Rule: Electrons of the same energy spread out before pairing up.
105 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
106 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
107 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
108 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
109 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
110 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
111 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
112 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
113 Orbital Notation Rules for Electron Configurations & Orbital Diagrams: Example: Orbital Diagram for Fluorine 9 electrons 1s 2 2s 2 2p 5
114 Sodium: Practice
115 Sodium +1 ion: Practice
116 Chlorine: Practice
117 Atomic Structure Protons Neutrons Electrons Found in the nucleus (+) charge Mass of 1 amu # of protons = Atomic # # of protons = # of electrons in a NEUTRAL atom # of protons = the nuclear charge.
118 Atomic Structure Protons Neutrons Electrons Found in the nucleus (+) charge Mass of 1 amu # of protons = Atomic # # of protons = # of electrons in a NEUTRAL atom # of protons = the nuclear charge. Found in the nucleus (0) charge neutral mass of 1 amu
119 Atomic Structure Protons Neutrons Electrons Found in the nucleus (+) charge Mass of 1 amu # of protons = Atomic # # of protons = # of electrons in a NEUTRAL atom # of protons = the nuclear charge. Found in the nucleus (0) charge neutral mass of 1 amu Found in orbitals ( e- clouds) surrounding nucleus ( - ) charge Mass 1/1836th of a proton # of e- = # of protons in a NEUTRAL atom
What is a theory? An organized system of accepted knowledge that applies in a variety of circumstances to explain a specific set of phenomena
Atomic Structure What is a theory? An organized system of accepted knowledge that applies in a variety of circumstances to explain a specific set of phenomena Early Theories Democritus: 4 B.C.: atom He
Regents Chemistry Unit 1 Atomic Concepts. Textbook Chapters 3 & 4
Regents Chemistry Unit 1 Atomic Concepts Textbook Chapters 3 & 4 Atomic Theory- Atoms are the building blocks of matter Atomic Models Democritus ~440 BC a Greek Philosopher suggested that matter is made
Democritus s ideas don t explain chemical behavior & lacked experimental support.
A1: Atomic Structure Worksheet Key (Goals 1 3, Chapter 4) 1. Democritus, who lived in Greece during the 4 th century B.C., suggested that matter is made up of tiny particles that cannot be divided. He
a. According to Dalton, what is inside the atom? Nothing, the atom it the smallest
Unit 3: Review SCIENTIFIC THEORIES Dalton theorized that atoms were the smallest particle and could not be divided. Atoms can bond with one another in whole number ratios to form compounds but cannot be
The History of the Atom. How did we learn about the atom?
The History of the Atom How did we learn about the atom? The Atomic Theory of Matter All matter is made up of fundamental particles. What does fundamental mean? The Greek Philosophers, 400 B.C. Democritus
Atomic Structure Early Theories Democritus: 4 B.C.: atom Dalton: atoms cannot Thomson: Cathode Ray Tubes Rutherford:
Atomic Structure n a well-substantiated explanation of some aspect of the natural world; n an organized system of accepted knowledge that applies in a variety of circumstances to explain a specific set
Notes:&&Unit&4:&Atomics& & & & & & & & & & & & & & & & &
Name: RegentsChemistry:Mr.Palermo Notes:Unit4:Atomics! www.mrpalermo.com Name: $ Key$Ideas$ Themodernmodeloftheatomhasevolvedoveralongperiodoftimethroughtheworkofmany scientists.(3.1a) Eachatomhasanucleus,withanoverallpositivecharge,surroundedbyoneormorenegatively
UNIT 2 - ATOMIC THEORY
*KEY* *KEY* UNIT 2 - ATOMIC THEORY *KEY* *KEY* VOCABULARY: Allotrope Anion Atom Atomic Mass Atomic Mass unit (a.m.u.) Atomic number Bohr model Cation Compound Electron Electron Configuration Element Excited
Honors Ch3 and Ch4. Atomic History and the Atom
Honors Ch3 and Ch4 Atomic History and the Atom Ch. 3.1 The Atom is Defined 400 B.C. the Greek philosopher Democritus said that the world was made of two things: Empty space and tiny particles called atoms
UNIT 2 - ATOMIC THEORY
UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Electron Configuration Nuclear Charge Anion Element Nucleons Atom Excited state Nucleus Atomic Mass Ground state Orbital Atomic Mass unit (a.m.u.) Ion Proton
UNIT 2 - ATOMIC THEORY
UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Anion Atom Atomic Mass Atomic Mass unit (a.m.u.) Atomic number Bohr model Cation Compound Electron Electron Configuration Element Excited state Ground state
UNIT 2 - ATOMIC THEORY
UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Electron Configuration Nuclear Charge Anion Element Nucleons Atom Excited state Nucleus Atomic Mass Ground state Orbital Atomic Mass unit (a.m.u.) Ion Proton
Atomic Structure. How do you discover and study something you can t see?
Atomic Structure How do you discover and study something you can t see? WHAT IS A THEORY? A hypothesis is a proposed explanation made as a starting point for further investigation (It s bright outside
Teacher: Mr. gerraputa. Name: Base your answer to the question on the information below. Given the electron dot diagram:
Teacher: Mr. gerraputa Print Close Name: 1. Given the electron dot diagram: The valence electrons represented by the electron dot diagram could be those of atoms in Group 1. 13 3. 3 2. 15 4. 16 2. Which
Observation information obtained through the senses; observation in science often involves measurement
Review Sheet Unit 1: The Atom Chemistry the study of the composition of matter and the changes matter undergoes Scientific Method Scientific method a logical, systematic approach to the solution of a scientific
I. History and Development of the Atom
Unit 3: The Atom I. History and Development of the Atom A. Democritus (around 400 B.C.) Based on his observations of the natural world around him, Democritus was the first to suggest that all matter was
TEST REVIEW GCAA Chemistry Atoms. A. Excited B. Energy C. Orbital D. Plum Pudding Model
TEST REVIEW GCAA Chemistry Atoms From the Hangman Game-----Match the answers correctly! A. Excited B. Energy C. Orbital D. Plum Pudding Model E. Bohr F. Electron G. Frequency H. Neutron I. Thomson J. alpha
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS Atoms Atoms have protons and neutrons located in the nucleus of the atom. Electrons orbit around the nucleus in well-defined paths. Protons have
Atomic Class Packet Unit 3
The modern model of the atom has evolved over a long period of time through the work of many scientists.(3.1a) Each atom has a nucleus, with an overall positive charge, surrounded by one or more negatively
Atomic Structure. Chemistry Mr. McKenzie
Atomic Structure Chemistry Mr. McKenzie How was the understanding of the atom developed? John Dalton (1766-1844) - developed a model to explain observations made at the time 1. Elements are made of tiny
Atomic Structure. Defining the Atom. Defining the Atom. Sizing up the Atom. Structure of the Atom 9/18/2012
Atomic Structure Defining the Atom Atom smallest particle of an that retains the chemical of that element 1 2 Defining the Atom The Greek philosopher Democritus (460 B.C. 370 B.C.) was among the to suggest
Chapter 4 The Structure of the Atom
Chapter 4 The Structure of the Atom Read pg. 86-97 4.1 Early Theories of Matter The Philosophers Democritus Artistotle - Artistotle s influence so great and the science so primitive (lacking!) his denial
To remain valid, models and theories must:
Note Taking Guide: Episode 301 Model: A idea used to explain facts in. Theory: An of facts and. To remain valid, models and theories must: all known enable to make correct Democritus: proposed the of an
Collegiate Institute for Math and Science Day 57: December 9, 2016 Room 427
Unit 2: Atomic Concepts Outline Name: Period: Date: 1. The modern model of the atom has evolved over a long period of time through the work of many scientists. Dalton s Model: Elements are made of atoms
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS Atoms Atoms have protons and neutrons located in the nucleus of the atom. Electrons orbit around the nucleus in well-defined paths. Protons have
Section 3.1 Substances Are Made of Atoms
Section 3.1 Substances Are Made of Atoms Objectives: 1. State the three laws that support the existence of atoms. 2. List the five principles of John Dalton s atomic theory. Vocabulary: law of definite
Unit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct.
Unit Two Test Review Click to get a new slide. Choose your answer, then click to see if you were correct. According to the law of definite proportions, any two samples of water, H2O, A. will be made up
Elements, atoms, & the. discovery of atomic structure
Elements, atoms, & the discovery of atomic structure Chapter 4 EARLY MODELS OF THE ATOM One What is an atom? The smallest particle of an element that can keep the same properties of the element. Democritus
Practice Packet Level 3: Atomics
Name: Regents Chemistry: Mr. Palermo Practice Packet Level 3: Atomics Name: Unit Vocabulary: For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions.
4. The mass of a proton is approximately equal to the mass of A an alpha particle C a positron. B a beta particle D a neutron
1. Which particles have approximately the same mass? A an electron and an alpha particle B an electron and a proton C a neutron and an alpha particle D a neutron and a proton 2. Which phrase describes
Atomic Theory. Developing the Nuclear Model of the Atom. Saturday, January 20, 18
Atomic Theory Developing the Nuclear Model of the Atom Democritus Theory: Atom, the indivisible particle c. 300 BC Democritus Problem: No scientific evidence c. 300 BC Dalton Theory: The solid sphere model
Atomic Structure Chapter 4
Atomic Structure Chapter 4 Outline A History of the Atomic Model Electron Structure of the Atom Useful Element Notations Early Thoughts on the Structure of Matter Before the invention of high powered microscopes,
ATOM. Rich -Paradis. Early Thoughts Aristotle-- Continuous theory. Matter can be divided indefinitely. Greeks
ATOM Early Thoughts Aristotle-- Continuous theory Greeks Matter can be divided indefinitely matter is made up of particles--4 elements 4 elements --air--fire--water- -- earth Democritus --Discontinuous
A1: Atomic Structure Worksheet (Goals 1 3, Chapter 4)
Unit 3 Assignment Packet Name: Period: A1: Atomic Structure Worksheet (Goals 1 3, Chapter 4) 1. Democritus, who lived in Greece during the 4 th century B.C., suggested that is made up of tiny particles
Atomic Theory. H. Cannon, C. Clapper and T. Guillot Klein High School
Atomic Theory Unit 3 Development of the Atomic Theory 1. Where is the mass of the atom concentrated? 2. What is located in the nucleus? 3. What is the negative particle that orbits the nucleus? 4. What
Practice Packet Unit 4: Atomic Structure
Name: Regents Chemistry Practice Packet Unit 4: Atomic Structure Assess Yourself: Vocab: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Lesson 5: Lesson 6: Lesson 7: 1 Vocabulary: Check your understanding. Describe
EM SPECTRUM, WAVELENGTH, FREQUENCY, AND ENERGY WORKSHEET
EM SPECTRUM, WAVELENGTH, FREQUENCY, AND ENERGY WORKSHEET 1.) Look at the EM spectrum below to answer this question. As you move across the visible light spectrum from red to violet (A) Does the wavelength
Chemistry: Hood River Valley High School Unit 3 Note Packet and Goals. Description A1. Marble Lab. Nailon Isotope Lab A2.
Chemistry: Hood River Valley High School Unit 3 Note Packet and Goals Name: Period: Unit 3 Atomic Structure and Periodic Table Unit Goals- As you work through this unit, you should be able to: 1. describe
What is the current atomic model?
4.1 Atoms Basic Units of Matter What is the current atomic model? Matter is anything that has mass and takes up space, such as gases, solids, and liquids. Matter is not sound, heat, or light these are
Atomic Theory. Early models
Atomic Theory Early models Ancient Greece Late 18 th century 4 elements Earth, Water, Wind, Fire: Matter is made up in different combinations of these 4 elements. First atom proposed by Democritus (Greek)
: the smallest particle that has the properties of an element. In, this Greek philosopher suggested that the universe was made of.
Notes: ATOMS AND THE PERIODIC TABLE Atomic Structure: : the smallest particle that has the properties of an element. From the early concept of the atom to the modern atomic theory, scientists have built
The modern model of the atom has evolved over a long period of time through the work of many scientists.(3.1a) Each atom has a nucleus, with an
REGENTS CHEMISTRY 1 The modern model of the atom has evolved over a long period of time through the work of many scientists.(3.1a) Each atom has a nucleus, with an overall positive charge, surrounded by
Chapter #1 - Atomic Structure
Chapter #1 - Atomic Structure Atomic Theories Democritus (460-340 BC) Democritus believed that all matter consisted of extremely small particles that could not be divided. He called them atoms from the
Democritus & Leucippus (~400 BC) Greek philosophers: first to propose that matter is made up of particles called atomos, the Greek word for atoms
Chemistry Ms. Ye Name Date Block The Evolution of the Atomic Model Since atoms are too small to see even with a very powerful microscope, scientists rely upon indirect evidence and models to help them
Unit 1, Lesson 01: Summary of Atomic Structure so far
Unit 1, Lesson 01: Summary of Atomic Structure so far Atoms are made of sub-atomic particles: Protons: found in the nucleus, charge of 1+, mass of 1 amu (u) Neutrons: found in nucleus, no charge, mass
Chapter 2 Atoms and Elements. 2.4 The Atom
Chapter 2 Atoms and Elements 2.4 The Atom Atoms Dalton s Atomic Theory Are tiny particles of matter. Of an element are similar and different from other elements. Of two or more different elements combine
1. Based on Dalton s evidence, circle the drawing that demonstrates Dalton s model.
Various models of the ATOM Dalton Model John Dalton developed the first atomic model in 1808. Before him people, mostly philosophers, had speculated about the smallest unit of matter and two theories prevailed.
Dalton Thompson Rutherford Bohr Modern Model ("Wave. Models of the Atom
Dalton Thompson Rutherford Bohr Modern Model ("Wave Models of the Atom Mechanical" Model) Aim: To discuss the scientists and their contributions to the current atomic model. Focus: Rutherford's Gold Foil
Nuclear Chemistry. Atomic Structure Notes Start on Slide 20 from the second class lecture
Nuclear Chemistry Atomic Structure Notes Start on Slide 20 from the second class lecture The Birth of an Idea Democritus, 400 B.C. coined the term atom If you divide matter into smaller and smaller pieces,
Unit 2: Atomic Structure Practice Packet
Unit 2: Atomic Structure Practice Packet Dalton s Model: hard sphere model 1. I can describe John Dalton s contribution to our Thomson s Experiment: cathode ray experiment 2. I can describe JJ Thomson
CHAPTER 4: Matter is Made up of Atoms
CHAPTER 4: Matter is Made up of Atoms ATOMS & THEIR STRUCTURE Aristotle thought matter was made of air, earth, fire and water. Democritus (250 B.C.)- Said the world is made of empty space & tiny particles
protons electrons neutrons nucleus Center of the atom; contains protons and neutrons. The Atom Molecules are made up of two or more atoms.
_ Period: The Atom Ch. 18:1 Everything is made of atoms. Atoms are the smallest part of matter. Atoms are made up of 3 subatomic particles (particles smaller than the atom): electrons, protons, and neutrons.
Atom Practice Test (#1) 1) What is the total number of valence electrons in an atom with the electron configuration 2-8-5? a) 2 b) 5 c) 8 d) 15
Atom Practice Test (#1) Name Multiple Choice 1 pt. each 1) What is the total number of valence electrons in an atom with the electron configuration 2-8-5? a) 2 b) 5 c) 8 d) 15 2) A Ca 2+ ion differs from
Ch4 and Ch5. Atomic History and the Atom
Ch4 and Ch5 Atomic History and the Atom Ch4.2 What are atoms? Atoms are the smallest part of an element that still has the element s properties. Ch. 4.3 The Atom is Defined 400 B.C. the Greek philosopher
8.5 Atomic Structure
Views of the Atom Democritus (Greek philosopher from 460 BC to 370 BC) Believed that atoms were indivisible and indestructible. His approach was simply philosophy and was not based upon the scientific
5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.
1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added
Atomic Structure. For thousands of years, people had many ideas about matter Ancient Greeks believed that everything was made up of the four elements
An atom is the smallest particle of an element that retains its identity in a chemical reaction. Although early philosophers and scientists could not observe individual atoms, they were still able to propose
Chapter 4 Lesson 2 Notes
Chapter 4 Lesson 2 Notes How were electrons discovered? Scientists have put together a detailed model of atoms and their parts. Here is the journey of atom parts. How were electrons discovered? (cont.)
Development of Atomic Theory Elements of chemistry- Atoms, the building blocks of matter Video
Development of Atomic Theory Elements of chemistry- Atoms, the building blocks of matter Video 2 CH 4- Atoms 1 Discovering the Atom In this lesson we will take a look at the scientists who explored the
Duncan. Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1. Figure 2. Figure 3
Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1 Figure 2 Figure 3 Light Calculation Notes Here s how the type/form of EM radiation can be determined The amount
Light Study of light by Newton helped lead to the quantum mechanical model. INTRO AND BACKGROUND: Atomic Structure. Electromagne?
INTRO AND BACKGROUND: Atomic Structure Light Study of light by Newton helped lead to the quantum mechanical model All light exhibits WAVE properties -AMPLITUDE: height of a wave -WAVELENGTH: distance between
Unit 1 Part 1 Atomic Structure and The Periodic Table Introduction to Atomic Structure UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE
UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE PART 1 INTRODUCTION TO ATOMIC STRUCTURE Contents 1. Protons, Neutrons and Electrons 2. Early Models of the Atom 3. Isotopes and Atomic Mass 4. Atoms and Ions
CHAPTER 5 Electrons in Atoms
CHAPTER 5 Electrons in Atoms 5.1 Light & Quantized Energy Was the Nuclear Atomic model incomplete? To most scientists, the answer was yes. The arrangement of electrons was not determined > Remember...the
Notes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass
Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following
Early Models of the Atom
Early Models of the Atom An atom is the smallest particle of an element that retains its identity in a chemical reaction. Although early philosophers and scientists could not observe individual atoms,
Chapter 9: Electrons and the Periodic Table
C h e m i s t r y 1 2 C h 9 : E l e c t r o n s a n d P e r i o d i c T a b l e P a g e 1 Chapter 9: Electrons and the Periodic Table Work on MasteringChemistry assignments What we have learned: Dalton
Atomic Structure. Part 3: Wave-Mechanical Model of the Atom. Key Question: How does the wave mechanical model explain the location of electrons?
Name Chemistry Atomic Structure Essential Question: How was the structure of the atom determined? Vocabulary: bright-line spectrum electron configuration excited state ground state orbital wave-mechanical
Alchemy Unit Investigation III. Lesson 7: Life on the Edge
Alchemy Unit Investigation III Lesson 7: Life on the Edge The Big Question How does the atomic structure of atoms account for the trends in periodicity of the elements? You will be able to: Explain how
Chapter 2: The Structure of the Atom and the Periodic Table
Chapter 2: The Structure of the Atom and the Periodic Table 1. What are the three primary particles found in an atom? A) neutron, positron, and electron B) electron, neutron, and proton C) electron, proton,
Chap 4 Bell -Ringers
Chap 4 Bell -Ringers The Structure of the Atom The Atom has a Structure What we ve seen so far Chapter 1 The Science of Chemistry - Chemistry is about discovering and understanding natural laws using the
Quantum Theory and Electron Configurations
Chapter 5 Chapter 5 Quantum Theory and Electron Configurations It s all about color In terms of atomic models, so far: Dalton (1803) = Tiny, solid particle Thomson (1897) = Plum Pudding model Electrons
2015 Name: Test 1 Atomic Structure
2015 Name: Test 1 Atomic Structure 1. During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms A) return to lower energy
Atomic Structure Practice Questions
Atomic Structure Practice Questions 1. Experiments performed to reveal the structure of atoms led scientists to conclude that an atom s (1) positive charge is evenly distributed throughout its volume (2)
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals
Atoms, Electrons and Light MS. MOORE CHEMISTRY
Atoms, Electrons and Light MS. MOORE CHEMISTRY Atoms Remember Rutherford??? What did he discover with his gold foil experiment. A: Atoms contain a dense nucleus where the protons and neutrons reside. ATOMS
2. The mass of an electron is NOT REALLY ZERO, but it s so small, about 1/1750 of a proton or neutron, that we
Atomic Theory Notes OB: Students will examine basic structure of the atom, learn what the numbers on the Periodic table mean, and look at electron orbitals. All atoms are made up of three sub-atomic (smaller
E J The electron s energy difference between the second and third levels is J. = J
The wavelength of light emitted is 654 nm. = c f c 3.00 10 8 m/s f c 3.00 108 m 1s 6.54 10 7 m f 4.59 4.59 10 14 z 1 s 10 14 The frequency of the light emitted is 4.59 10 14 z. E hf h 6.63 10 34 J/z E
CHAPTER 5. Electrons in Atoms. Rutherford Model. Bohr Model. Plum Pudding Model. 5.1 Atomic Models
CHAPTER 5 Electrons in Atoms 5.1 Atomic Models The Chemical properties of atoms, ions, and molecules are related to the arrangement of the electrons within them. The first model of the atom was Dalton
4/14/2013 ATOMIC STRUCTURE THE ATOMIC MODEL
ATOMIC STRUCTURE R E G E N T S C H E M I S T R Y M R S. T I L A R O HISTORY OF THE ATOM O L D A N D M O D E R N A T O M THE ATOMIC MODEL Model of the atom is based on indirect experimental data. Model
Professor K. Atomic structure
Professor K Atomic structure Review Reaction- the formation and breaking of chemical bonds Bond- a transfer or sharing of electrons Electrons Abbreviated e - What are they? How were they discovered? Early
Name Chemistry-PAP Period. Notes: Electrons. Light travels through space as a wave. Waves have three primary characteristics:
Name Chemistry-PAP Period The Wave Nature of Light Notes: Electrons Light travels through space as a wave. Waves have three primary characteristics: Wavelength (λ): the distance between 2 consecutive crests
Accelerated Chemistry Study Guide Atomic Structure, Chapter 3
Accelerated Chemistry Study Guide Atomic Structure, Chapter 3 Terms and definitions atom ion law of constant composition isotope atomic theory of matter mass number cathode ray tube atomic mass electron
Focus Learning Targets Atomic Structure and Quantum Chemistry 1. Give the one main contribution to the development of the atomic model from each of
Atomic Structure Homework Packet Honors Chemistry Focus Learning Targets Atomic Structure and Quantum Chemistry 1. Give the one main contribution to the development of the atomic model from each of the
Chemistry 11 Early models of the atom 1. Structure of the Atom
Chemistry 11 Early models of the atom 1 Structure of the Atom Democritus Developed the idea of atom Thought things were made of atoms that have different Shapes Aristotle Matter is made of different amounts
UNDERLYING STRUCTURE OF MATTER
1 UNDERLYING STRUCTURE OF MATTER Chapter 4 Atomic Structure DEFINING THE ATOM Earlier theories of matter: A. Even though his hypothesis lacked evidence at the time, the Greek philosopher Democritus (460
1 Development of the Atomic Theory
CHAPTER 4 1 Development of the Atomic Theory SECTION Introduction to Atoms BEFORE YOU READ After you read this section, you should be able to answer these questions: What is the atomic theory? How has
Name Date Due Test Day! Unit 1: Atomic Theory. Pretest Practice K +
! 2017-2018 Name Date Due Test Day! Unit 1: Atomic Theory Pretest Practice 1.) Complete the following table: Work space (if needed)! 2.) What do the superscripts and subscript represent in the symbol below?
Unit 3: The Atom Part 1. DUE: Friday October 13, 2017
Unit 3: The Atom Part 1 The following pages are practice questions for this unit, and will be submitted for homework! You must complete: What is in an atom? ALL QUESTIONS Calculating the Number of Protons,
Name Period Date Engage-Atoms 1. What does Bill cut in half?
Name Period Date Engage-Atoms https://www.youtube.com/watch?v=fmuskig2exi 1. What does Bill cut in half? 2. By cutting this item in half he tries to prove that there are pieces that are uncut- table called
PROGRESSION OF THE ATOMIC MODEL
PROGRESSION OF THE ATOMIC MODEL By 1808, it was widely accepted that matter was made up of ELEMENTS, which consisted of tiny PARTICLES called ATOMS. After 2000 years - DEMOCRITUS was right all along John
Unit 2 Atomic Theory and Periodicity Review
Unit 2 Atomic Theory and Periodicity Review Section I: History In each box, write the name of the scientist(s) associated with the statement. Choose from among the following: Democritus Thomson Bohr Schroedinger
Unit 3: Atomic Structure. Particle Charge Location in the Atom Mass
Unit 3: Atomic Structure Name: Basics of the Atom Particle Charge Location in the Atom Mass a.m.u.: unit used to measure mass of atoms atomic number: mass number: To find net charge on an atom, consider
Where it came from and what we know now
Where it came from and what we know now History of the Atom The first mention of the atom came from Democritus in ancient Greece He suggested that the universe was made up of small, indivisible units called
Chapter 3 https://youtu.be/thndxfdkzzs?list=pl8dpuualjx tphzzyuwy6fyeax9mqq8ogr
Chapter 3 https://youtu.be/thndxfdkzzs?list=pl8dpuualjx tphzzyuwy6fyeax9mqq8ogr The smallest particle of an element that retains the chemical properties of that element. Regions: Nucleus: very small region
Chapter 5: Electrons in Atoms
Chapter 5: Electrons in Atoms Models of the Atom Rutherford used existing ideas about the atom and proposed an atomic model in which the electrons move around the nucleus, like the planets move around
UNIT TWO TEST HISTORY OF ATOM, STRUCTURE OF ATOM, ATOMIC MASS CARBON-12
KEY Review Sheet: UNIT TWO TEST HISTORY OF ATOM, STRUCTURE OF ATOM, ATOMIC MASS 1. Know which isotope is the standard for the atomic mass unit. CARBON-12 2. Know what the difference in masses of isotopes
DO NOT, under any circumstances, throw this away! This packet MUST be saved for the final exam.
Name: Period: Unit 10 Packet Atomic History/Structure and Quantum Mechanics Packet Contents Sheet with Objectives (This Page) Worksheet 1: Thermal energy, radiation, and color Early Discoveries About the
Name: Date: Blk: Dalton Thomson Rutherford Bohr THOMSON
Name: Date: Blk: NOTES: ATOMIC STRUCTURE I. History of the Atom Dalton Thomson Rutherford Bohr 1803 1897 1909 1913 1. DALTON - everything is made of atoms - different elements combine to form compounds
Units 1, 2 study guide- atomic structure
Name: Units 1, 2 study guide- atomic structure 1) Complete the required information for each subatomic particle (T1.3) symbol name charge location Mass (AMU) p + e - n 0 2) Define the following terms: