PowerPoints II-9 to III-16. De La Salle High School Mr. Puccetti
|
|
|
- Kerry Little
- 6 years ago
- Views:
Transcription
1 PowerPoints II-9 to III-16 De La Salle High School Mr. Puccetti
2 II-9 ChemCatalyst Create a Table Properties of the Elements HW#1 (42): 1-3 Lab Report due Friday 1. What patterns do you see in how the elements are organized? 2. What do the numbers represent?
3 Create a Table Properties of the Elements How did Mendeleyev organize the elements into the periodic table?
4 Create a Table Properties of the Elements II-9 Notes Periodic Table of the elements: An organization of the elements in rows ( ) and columns ( )
5 Create a Table Properties of the Elements II-9 Notes Atomic mass: A measure of the relative mass of an element Atomic mass units: The units used for atomic mass (amu).
6 Create a Table Properties of the Elements II-9 Notes Properties: The properties of elements include color, hardness, and reactivity. Iodine I 2 Sodium Na Sulfur S
7 Create a Table Properties of the Elements II-9 Notes Reactivity: The reactivity of an element is related to whether or not it will combine with other substances as well as the speed with which the products form. Iodine I 2 Sodium Na Sulfur S
8
9 Which of the following elements belong in a group? II-9 Check- In Cadmium Cd Moderately soft, silvery solid, metal React very slowly with water Found in CdCl 2 (s) Zinc Zn Moderately hard, silvery solid, metal Reacts very slowly with water Found in ZnCl 2 (s) Iodine I Purple solid, nonmetal Reacts slowly with metals Found in ICl (s) Mercury Hg Silvery liquid, metal Does not react with water Found in HgCl 2 (s)
10 II-10 ChemCatalyst Breaking the Code The Periodic Table Look at the periodic table poster. Where would you put copper on the periodic table? Explain your reasoning. Copper shiny, reddish metal HW#2 (50): 1, 2, 4-7 & Color Code your Periodic Table (instructions on webpage) Cu 63.5 Reacts slowly with oxygen Found in CuCl
11 HW#2 (50): 1, 2, 4-7 & Color Code your Periodic Table (instructions on webpage) Breaking the Code The Periodic Table Copper Cu 63.5 shiny, reddish metal Found in CuCl
12 Breaking the Code The Periodic Table Where did Mendeleyev put copper (Cu) in his periodic table?
13 Mendeleyev s table has ten elements like copper, with atomic masses between 40.1 and 69.7 Breaking the Code The Periodic Table
14 Breaking the Code The Periodic Table The periodic table opens up to make room for more elements
15 Breaking the Code The Periodic Table Then add Mendeleyev s remaining elements -- keeping them in their columns
16 Breaking the Code The Periodic Table The Modern Periodic Table
17 Breaking the Code The Periodic Table What information does the periodic table reveal about the elements?
18 Breaking the Code The Periodic Table What information does the periodic table reveal about the elements?
19 Key: Groups ( ) Periods ( ) Breaking the Code The Periodic Table
20 Breaking the Code The Periodic Table Groups ( ): Elements in a group have similar properties. They are arranged in vertical columns on the periodic table Key: Groups ( ) Periods ( ) I II III IV V VI VII VIII
21 Breaking the Code The Periodic Table Periods: The horizontal rows on the table. The patterns repeat over and over again at the start of each new row. Key: Groups ( ) Periods ( )
22 Breaking the Code The Periodic Table II-10 Check-in List 5 things to describe the element silver (Ag). Copper shiny, reddish metal Gold shiny, yellow metal Cu Au Reacts slowly with oxygen Found in CuCl not very reactive Found in AuCl
23 Breaking the Code The Periodic Table Use pens and/or colored pencils to label the following on your periodic table (make a key): groups (columns), periods (rows), metals, non-metals, gases, halogens, alkali metals, alkaline metals, noble gases, transition elements, metalloids Mark the 2 most reactive elements on your periodic table with a. Hint: One element is a metal and the other is a non-metal. HW#2 (50): 1, 2, 4-7 & Color Code your Periodic Table (instructions on webpage)
24 09/7/09: Atomic Pudding Models of the Atom HW#3 (57): 1-4 III-11 ChemCatalyst meters The drawing is a model of a very tiny cube of gold. 1. What does the model tell you about the element gold? What do the spheres represent? What are atoms? 2. How would you draw copper to show that it is different from gold? Explain your reasoning.
25 Atomic Pudding Models of the Atom Atoms: Extremely small particles, which cannot be seen. All matter is made up of atoms. III- 11 Note s Models: A simplified representation of something more complex, that facilitates understanding certain aspects of a real object or process.
26 Atomic Pudding Models of the Atom How are the smallest bits of matter described? III- 11 Note s In 1803, John Dalton proposed that atoms were simply solid spheres. In the decades that followed chemists collected a lot of evidence suggesting that there was more to the atom.
27 Atomic Pudding Models of the Atom How are the smallest bits of matter described? This lesson will introduce you to various models for the atom that have appeared over the past two hundred years. The descriptions of five models of the atom are on a separate handout.
28 The Progression of Models Solid Sphere Model Plum Pudding Model Nuclear Model Dalton, 1803 Thomson, 1897 Rutherford 1911 Solar System Model Bohr, 1913 Proton Model Rutherford, 1918
29 Atomic Pudding Models of the Atom III- 11 Note s Models S tructures Solid Sphere Model (Dalton, 1803) None a solid sphere Plum Pudding Model (Thomson, 1897) Electrons nega tive charge Fluid positive charge
30 Atomic Pudding Models of the Atom III-11 Notes Models S tructures Nuclear Model (Rutherford, 1911) Electrons nega tive charge Nucleus positive charge Electrons circle around the nucleus Solar System Mo del (Bohr, 1913) Electrons nega tive charge Nucleus positive charge Electron orbits at different distances from the nucleus Proton Model (Rutherford, 1918) Electrons nega tive charge Protons positive charge Nucleus of protons. Electrons circle around the nucleus
31 Atomic Pudding Models of the Atom III-11 Notes Model of the Atom electrons protons and neutrons in the nucleus Atoms: Extremely small particles, which cannot be seen. All matter is made up of atoms.
32 09/10/09 III-12 : Atoms By Numbers Atomic Number & Atomic Mass (1) III-11 ChemCatalyst HW#4 see board 1. Label the following diagram 2. What are the charges associated with each of these particles? (2) and (3) are in the nucleus Helium, He 3. List 3 similarities and 3 differences between the atomic models of He and Be. 4. Why do you think helium is #2 (the second element), and beryllium is #4 on the periodic table? Beryllium, Be
33 Atomic Pudding Models of the Atom III-11 Notes Model of the Atom Electrons (-) Protons (+) and neutrons (ø) in the nucleus The atom is composed of even smaller pieces called protons, neutrons, and electrons.
34 Atomic Pudding Models of the Atom III-11 Notes Model of the Atom electrons protons and neutrons in the nucleus The protons and neutrons are located in the dense nucleus of the atom. The electrons surround the nucleus.
35 Atomic Pudding Models of the Atom III-11 Notes Model of the Atom Electrons (-) Protons are positive (+). Neutrons are neutral (Ø). Electrons are negative (-). Atoms are neutral (Ø). The nucleus or an atom is positive (+). Protons (+) and neutrons (ø) in the nucleus
36 09/10/09 III-12 : Atoms By Numbers Atomic Number & Atomic Mass (1) 1. Label the following diagram 2. What are the charges associated with each of these particles? III-11 ChemCatalyst HW#4 see board (2) and (3) are in the nucleus Helium, He 3. List 3 similarities and 3 differences between the atomic models of He and Be. 4. Why do you think helium is #2 (the second element), and beryllium is #4 on the periodic table? Beryllium, Be
37 Atoms By Numbers Atomic Number and Atomic Mass III-12 Notes How are the atoms of one element different than the atoms of another element? Helium, He Berylium, Be
38 Atoms By Numbers Atomic Number and Atomic Mass III-12 Notes Atomic number is the number of protons in the nucleus of an atom. Atomic number = # protons Henry Mosely If you change the proton number, you change the element.
39 Atoms By Numbers Atomic Number and Atomic Mass III-12 Notes The atom is neutral so # protons (+) = # of electrons (-) electrons protons and neutrons in the nucleus Atomic number = # protons = # of electrons
40 Atoms By Numbers Atomic Number and Atomic Mass III-12 Notes The proton and neutron account for most of the mass in an atom.
41 Atoms By Numbers Atomic Number and Atomic Mass Atomic mass of an atom: The mass of an atom in amu s is approximately equal to the number of protons + the number of neutrons. protons and neutrons in the nucleus The mass of an atom is measured in amu (atomic mass units) Mass of one proton = 1 amu. Mass of one neutron = 1 amu. Mass of one electron = ~ amu (very tiny)
42 Atoms By Numbers Atomic Number and Atomic Mass The proton and neutron account for most of the mass in an atom. Atomic mass = protons + neutrons electrons protons and neutrons in the nucleus
43 Atoms By Numbers Atomic Number and Atomic Mass Atomic mass of an atom: The mass of an atom in amu is approximately equal to the number of protons added to the number of neutrons. Atomic mass = protons + neutrons electrons protons and neutrons in the nucleus To find neutrons: neutrons = Atomic mass (rounded to the nearest whole #) atomic number (protons)
44 Atoms By Numbers Atomic Number and Atomic Mass Symbols associated with elements Atomic number Atomic mass C B 10.8 Element Symbol C B
45 Atoms By Numbers Atomic Number and Atomic Mass Symbols associated with elements III- 12 Note s Atomic number Atomic mass C B 10.8 Atomic number = # protons = # of electrons Atomic mass = # protons + # neutrons # of neutrons?
46 Atoms By Numbers Atomic Number and Atomic Mass Each successive element in the periodic table has one more proton than the element preceding it. The atomic number of an atom is equal to the number of protons in its nucleus. The number of electrons in an atom is equal to the number of protons because an atom is neutral. The mass of a proton is 1 atomic mass unit or 1 amu. The mass of a neutron is also 1 amu. The atomic mass of an atom in amu is just the sum of the number of protons and neutrons. How are the atoms of one element different than the atoms of another element? The mass of the atom is found in the nucleus.
47 Atoms By Numbers Atomic Number and Atomic Mass III- 12 Note s Use your periodic table to identify the following elements: a) Atomic number 18 b) Has three electrons c) Atomic mass of 16.0
48 Subatomic Heavyweights Isotopes III- 13 Note s 1. What is different about the two atoms? 2. What is the atomic mass/atomic number of each atom? 3. Do you think they are both Lithium atoms? Why or why not?
49 N P Subatomic Heavyweights Isotopes How can atoms of the same atom differ? III- 13 Note s Protons = Neutrons = Electrons = Protons = Neutrons = Electrons =
50 Subatomic Heavyweights Isotopes How can atoms of the same atom differ? III- 13 Note s Protons = (6) same Neutrons = (6) Different Electrons = (6) same? Protons = (6) same Neutrons = (7) Different Electrons = 6 same?
51 Subatomic Heavyweights Isotopes III- 13 Note s Isotope: Atoms of the same element that have different numbers of neutrons. Protons = same Neutrons = Different Electrons = same Protons = same Neutrons = Different Electrons = same
52 Subatomic Heavyweights Isotopes III-13 Notes Isotopes: Atoms of the same element that have different numbers of neutrons Isotopes have the same number of protons and electrons but different numbers of neutrons. 3 Protons 3 Neutrons 3 Electrons 3 Protons 4 Neutrons 3 Electrons
53 Subatomic Heavyweights Isotopes III- 13 Note s The atomic mass of the element is the average of the masses of the atoms in the sample. Compared to the definition of the atomic mass of an atom Atomic mass of an atom: The mass of an atom in amu is approximately equal to the number of protons added to the number of neutrons. Atomic mass = protons + neutrons
54 Subatomic Heavyweights Isotopes III-13 Notes Atomic mass of an atom of Ne = 20, 21, or 22 Atomic mass of Ne = amu
55 Subatomic Heavyweights Isotopes III-13 Notes What is the average atomic mass of Ne? 90% of atoms weigh 20 amu 1% of Ne atoms weigh 21 amu 9% of atoms weigh 22 amu
56 Subatomic Heavyweights Isotopes III-13 Notes What is the average atomic mass of Ne? 90% of atoms weigh 20 amu 1% of Ne atoms weigh 21 amu 9% of atoms weigh 22 amu
57 Subatomic Heavyweights Isotopes III-13 Wrap Up Notes The atomic weight of an element listed on the periodic table is the average mass of the naturally occurring isotopes of that element.
58 Isotopia Stable and Radioactive Isotopes III-14 ChemCatalyst Predict the isotopes of carbon, C. Which isotope is more abundant? How do you know? C
59 Subatomic Heavyweights Isotopes 5 B 10.8 P N
60 Subatomic Heavyweights Isotopes III-13 Notes Isotope Symbols Atomic Number Atomic Mass 5 B B Boron B Boron-11
61 Subatomic Heavyweights Isotopes III-13 Notes Atomic Mass Atomic Number Chemical Name- Atomic Mass Isotope Symbols 10 5 B Boron-10 5 B 10.8
62 Subatomic Heavyweights Isotopes III-13 Notes Isotope Symbols Atomic Mass AM = p + n Atomic Number AN = # p Chemical Name- Atomic Mass AM AN Sy Symbol-AM
63 Subatomic Heavyweights Isotopes III-13 Wrap Up- Notes Isotopes are referred to by their mass numbers (not the neutron #). Example: boron-10 and boron B 11 B 5 5 Boron-10 Boron-11
64 Subatomic Heavyweights Isotopes III-13 Notes What types of isotopes do various elements have? 6 Li Li 3 3 Lithium-6 Lithium-7 7
65 Subatomic Heavyweights Isotopes III-13 Notes Isotopes have the same number of protons and electrons but different numbers of neutrons. The atomic weight of an element listed on the periodic table is the average mass of the naturally occurring isotopes of that element. Isotopes are referred to by their mass numbers. (example: boron-10 and boron-11)
66 Isotopia Stable and Radioactive Isotopes III-14 ChemCatalyst Predict the isotopes of carbon, C. Which isotope is more abundant? How do you know? C
67 Isotopia Stable and Radioactive Isotopes
68 Chart of Naturally Occurring Isotopes In Textbook
69
70 Isotopia Stable and Radioactive Isotopes Atoms must have at least one neutron for every proton in the nucleus (with the exception of hydrogen).
71 Isotopia Stable and Radioactive Isotopes Many isotopes have more neutrons than protons. The larger an atom is the more neutrons it needs in the nucleus to be stable.
72 Isotopia Stable and Radioactive Isotopes Radioactivity Radioactive isotope: Any isotope that has an unstable nucleus and breaks apart or decays over time. Compared to... Stable isotope: An isotope that does not break apart into smaller atoms.
73 Isotopia Stable and Radioactive Isotopes III-14 Wrap-up What types of isotopes do various elements have? There are somewhere between 1 and 10 isotopes of each element found in nature. The neutron to proton ratio is an important factor in determining the stability of a nucleus. Some elements have isotopes that are radioactive. The nuclei of radioactive isotopes are unstable and they break apart over time producing atoms with smaller masses.
74 III-15: Nuclear Quest Nuclear Reactions
75 Chem Catalyst Stable and Radioactive Isotopes Which of the following are isotopes of copper? Explain your reasoning. 63 Cu 197 Au 63 Cu 87 Cu 34 Cu 65 Cu
76 Alpha Decay III-15 Notes Alpha decay: A nuclear reaction in which an atom emits an alpha particle. Its atomic number decreases by 2, and its mass number decreases by 4.
77 Beta Decay III-15 Notes Beta decay: A nuclear reaction in which a neutron changes into a proton, and the atom emits a beta particle. The atom s atomic number increases by 1.
78 III-15: Nuclear Quest Nuclear Reactions III-15 Notes Nuclear chemistry is the study of changes to the nucleus. Nuclear reaction: A process that involves changes to the nucleus of an atom. Radioactive decay: A spontaneous process by which an atom emits radiation or a particle from its nucleus to become more stable. Fusion: The joining of two nuclei to form a larger nucleus accompanied by a release of energy. Fission: The splitting apart of an atomic nucleus into two smaller nuclei accompanied by a release of energy.
79 ChemCatalyst 09/15/09 1. What patterns do you notice in the fusion reactions? 2. Do you think gold can be created on Earth by a fusion reaction? Explain your thinking.
80 III-15: Nuclear Quest Nuclear Reactions III-15 Wrap- Up Changes in the nucleus of an atom can change the identity of an element. Alpha particle: A particle composed of two protons and two neutrons, equivalent to the nucleus of a helium atom. Beta particle: An electron emitted from the nucleus of an atom during beta decay. Gamma ray: A form of high-energy electromagnetic radiation emitted during nuclear reactions.
81 III-15: Nuclear Quest Nuclear Reactions III-15 Wrap- Up What are nuclear reactions? Alpha decay results in a in the atomic number by. results in an increase in the atomic number by. Gamma radiation usually accompanies alpha and beta decay and also fission. Gamma radiation can be quite harmful to humans.
82 III-15: Nuclear Quest Nuclear Reactions III-15 Wrap- Up Nuclear fission involves a single nucleus breaking apart into two smaller nuclei. Nuclear fusion involves two nuclei combining to form a nucleus with a larger atomic number. Nuclear fusion takes place in extremely hot environments, such as the cores of stars.
83 III-16: Old Gold Formation of Elements How are new elements formed? Radioactive decay, nuclear fusion, and nuclear fission are all nuclear processes that result in the creation of new elements. The mass of a nucleus changes when neutrons or protons are added or lost. The identity of an element changes when its nucleus gains or loses protons.
84 Check-In Write the nuclear equation showing technetium-100 undergoing alpha decay. Write the nuclear equation showing barium undergoing beta decay.
85 III-16: Old Gold Formation of Elements Radioactive decay happens in the natural world around us. Fission can be spontaneous for unstable nuclei, or it can be provoked using nuclear bombardment and other methods. Fusion of nuclei to form different isotopes happens in the stars.
All are made of atoms. The, your and even are made of atoms. Atoms are. One atom is only one of a meter wide!
Name: Atoms & The Periodic Table WHAT IS AN ATOM? What is an atom? All are made of atoms. The, your and even are made of atoms. Atoms are. One atom is only one of a meter wide! DEMOCRITIS The idea of an
Unit 2 Atomic Structure and Nuclear Chemistry
Chemistry 1 West Linn High School Unit 2 Packet and Goals Name: Period: Unit 2 Atomic Structure and Nuclear Chemistry Unit Goals: As you work through this unit, you should be able to: 1. describe Dalton
The Periodic Table. LESSON 10 Breaking the Code. Think About It. Exploring the Topic. The Modern Periodic Table
Printed Page 43 [Notes/Highlighting] LESSON 10 Breaking the Code Think About It The elements copper, Cu, and gold, Au, share many similarities. Both are relatively unreactive elements. They are soft so
1 amu 1 amu 0 amu. Chapter 2 part 1.notebook September 16, Modern Atomic Theory
Chapter 2 The Atom Elements are the basic substances that make up all matter. An atom is the smallest particle of an element. Average atoms are 10 10 m in diameter. If you could put 6.02 x 10 23 p + and
A. Element 1. The number of protons and neutrons of an atom.
Unit 03: Test Review Atoms and Elements Key Term Definition A. Element 1. The number of protons and neutrons of an atom. B. Atom 2. The smallest particle of an element. C. Atomic Number 3. A primary substance
Chapter 2. Atoms, Ions, and the Periodic Table. Chapter 2 Topics. 2.1 Dalton s s Atomic Theory. Evidence for Atoms. Evidence for Atoms
Chapter 2 Atoms, Ions, and the Periodic Table Chapter 2 Topics 1. Dalton s s Atomic Theory 2. Structure of the Atom 3. Ions 4. Atomic Mass 5. The Periodic Table Copyright The McGraw-Hill Companies, Inc.
Isotopes and Radioactive Decay
NAME PERIOD DATE CHAPTER 4 NOTES: ISOTOPES Isotopes and Radioactive Decay ISOTOPES: Atoms that contain the same number of protons but a different number of neutrons. Isotopes containing more neutrons have
Atomic Structure & Nuclear Chemistry Unit 3 Notes
Atomic Structure & Nuclear Chemistry Unit 3 Notes Academic Chemistry Name 52 24 Cr Mass Number Symbol Atomic Number Unit #3 Test Date You can never learn less, you can only learn more. R. Buckminster Fuller
Chapter 1: Atomic Structure and the Periodic Table 1.1 Atoms are the smallest form of elements.
Chapter 1: Atomic Structure and the Periodic Table 1.1 Atoms are the smallest form of elements. All matter is made of atoms. About 100 different atoms, or elements, make up everything on Earth. Hydrogen
Understanding the Atom
Name Date Period 3.1 Discovering Parts of an Atom Directions: On the line before each statement, write correct if the statement is correct or not correct if the statement is not correct. If the statement
UNIT 2: Matter and its changes. Mrs. Turner
UNIT 2: Matter and its changes Mrs. Turner Preassessment Take out a sheet of paper and number it from 1-25. Write down your answers to plug them into your clickers. Don t worry about not knowing an answer
Chemistry Review Unit 1 Study Guide
1. Draw and label a Bohr model of a C 14 atom. 2. Describe the following about a proton a. mass: the mass of a proton is 1 atomic mass unit (AMU) b. charge: protons have a positive charge c. location:
Properties of Atoms and The Periodic Table. Ch 16, pg
Properties of Atoms and The Periodic Table Ch 16, pg. 488-506 Today s Learning Objectives Describe the 5 models of the atom. Be able to arrange the 5 models of the atom in order. Explain why the models
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
The Structure of the Atom
The Structure of the Atom Section 4.1 Early Theories of Matter In your textbook, read about the philosophers, John Dalton, and defining the atom. For each statement below, write true or false. 1. Ancient
8. atomic mass: the mass of the element and represents the. 9. Atomic number: on top of the atomic symbol; represents the.
Intro To Chemistry Study online at quizlet.com/_2xw51k 1....:... 2. alkali metals: 8. atomic mass: the mass of the element and represents the number of protons plus the number of neutrons. 9. Atomic number:
Mass number i. Example U (uranium 235) and U (uranium 238) atomic number e. Average atomic mass weighted of the isotopes of that element i.
CP NT Ch. 4&25 I. Atomic Theory and Structure of the Atom a. Democritus all matter consists of very small, indivisible particles, which he named i. Atom smallest particle of an element that retains all
Unit Two: Atomic Structure
Unit Two: Atomic Structure TEKS 5: The student understands the historical development of the Periodic Table and can apply its predictive power. (b) use the Periodic Table to identify and explain the properties
Chapter 4 Atoms and Elements
Atoms and Elements Experiencing Atoms Atoms are incredibly small, yet they compose everything. Atoms are the pieces of elements. Properties of the atoms determine the properties of the elements. 2 The
UNIT 4 NOTES: ATOMIC THEORY & STRUCTURE
S T U D E N T N O T E S P r e - A P C h e m i s t r y U N I T 4 Page 1 NAME PERIOD UNIT 4 NOTES: ATOMIC THEORY & STRUCTURE STUDENT OBJECTIVES: Your fascinating teachers would like you amazing learners
Chapter 2 Atoms and Elements
Chapter 2 Atoms and Elements Law of Conservation of Mass in a chemical reaction, matter is neither created nor destroyed total mass of the materials you have before the reaction must equal the total mass
Notes:&&Unit&4:&Atomics& & & & & & & & & & & & & & & & &
Name: RegentsChemistry:Mr.Palermo Notes:Unit4:Atomics! www.mrpalermo.com Name: $ Key$Ideas$ Themodernmodeloftheatomhasevolvedoveralongperiodoftimethroughtheworkofmany scientists.(3.1a) Eachatomhasanucleus,withanoverallpositivecharge,surroundedbyoneormorenegatively
Modern Atomic Theory
Modern Atomic Theory Review of the Discovery of the Atom 1803 John Dalton discovered that elements are made of atoms. He thought that atoms were solid, like a marble. 1875 Crooks discovered the electron.
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
Exploring Atoms. Introduction
Exploring Atoms Introduction Atoms All physical entities are made of matter. Matter is anything which has mass and takes up space. There are three common states of matter--solid, liquid, and gas--on earth.
Atoms and Nuclear Chemistry. Atoms Isotopes Calculating Average Atomic Mass Radioactivity
Atoms and Nuclear Chemistry Atoms Isotopes Calculating Average Atomic Mass Radioactivity Atoms An atom is the smallest particle of an element that has all of the properties of that element. Composition
4.1 Structure of the Atom
4.1 Structure of the Atom How do atoms differ from each other? What are atoms composed of? What are the subatomic particles? 2-1 Structure of the Atom Atoms actually are divisible. They are composed of
Periodic Table Workbook
Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order
Textbook: Section B, Chapter 1
Atoms and the Periodic Table Review Sheet Textbook: Section B, Chapter 1 1. What is the Atomic number of nitrogen? 2. How many protons does nitrogen have? 3. How many electrons does nitrogen have? 4. How
ATOMIC STRUCTURE. Atoms are really small. Gold and Palladium Atoms
ATOMIC STRUCTURE Atoms are really small. Gold and Palladium Atoms Theory vs Model Models are diagrams or apparatuses used to simplify the description of a complicated idea John Dalton English scientist
Atomic Structure and The Periodic Table. Unit 3
Atomic Structure and The Periodic Table Unit 3 Lesson 1: Atoms Unit 5: Atomic Structure & The Periodic Table Atoms How small can things get? If you break a stone wall into smaller and smaller pieces, you
Chapter 4 Atoms Practice Problems
Chapter 4 Atoms Practice Problems 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Which of the following is a
2. Electrons: e - charge = negative -1 mass ~ 0
Notes Ch. and 5: Atomic Structure and Nuclear Chemistry History and Structure the Nuclear Atom The Atom smallest particle an element that retains all properties the element I. Early Models the Atom A.
Chapter 2 Atoms, Ions, and the Periodic Table. Law of Conservation of Mass. Law of Conservation of Mass
Chapter 2 Atoms, Ions, and the Periodic Table Dalton s Atomic Theory Structure of the Atom Ions Atomic Mass The Periodic Table Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction
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 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
Matter and Energy. Chapter 3
Matter and Energy Chapter 3 Matter Anything that has mass and takes up space Two categories Pure substances Mixtures Pure Substances Matter with a fixed composition Either an element or compound Element
5.1 Atoms are the smallest form of elements
5.1 Atoms are the smallest form of elements 1 All matter is made of atoms Same type of atoms = element There are approximately 100 elements known today 2 Each element has its own symbol & properties Hydrogen
Vocabulary QUIZ: 1. The total number of particles in the nucleus 2. 1 / 12
Sep 29 11:29 AM Vocabulary QUIZ: 1. The total number of particles in the nucleus 2. 1 / 12 th of the mass of a carbon atom 3. The weighted average mass of all the isotopes of a particular element 4. A
Chapter 5 Atomic Structure and the Periodic Table
Chemistry/ PEP Name: Date: Chapter 5 Atomic Structure and the Periodic Table Chapter 5: 1 16, 20, 21, 23, 24, 27-32, 35, 42, 44, 49, 50, 55 (32 total) Section Review 5.1 1. In your own words, state the
Test 3: Lab Safety, Measurements, Matter and Periodic Table
Name: Grade/Group: Subject: Chemistry-7 Teacher: Mrs. Raj Date: Test 3: Lab Safety, Measurements, Matter and Periodic Table Directions: Determine the best answer for each question. Circle your answer on
Nuclear Physics Questions. 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of?
Nuclear Physics Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?
Organizing the Periodic Table
Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements
UNIT (2) ATOMS AND ELEMENTS
UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called
Honors Chemistry Unit 2: The Atom & Its Nucleus
Honors Chemistry Unit 2: The Atom & Its Nucleus (2017-2018) Bunsen, I must tell you how excellent your study of chemical spectroscopy is, as is your pioneer work in photochemistry but what really impresses
Structure of the Nuclear Atom
Structure of the Nuclear Atom I. The II. A. The is the smallest particle of an element that retains its of the element. History of the Atom A. Democritus 1. Democritus (460 B.C. 370 B.C) was the first
Friday, 05/06/16 6) HW QUIZ MONDAY Learning Target (NEW)
Friday, 05/06/16 1) Warm-up: If you start with 100g of a radioactive substance, how much will be left after 3 half-lives? 2) Review HW & Nuclear Notes 3) Complete Modeling Energy Investigation 4) Complete:
Atoms and Elements Review
Atoms and Elements Review YOU ARE EXPECTED TO KNOW THE MEANING OF ALL THE FOLLOWING TERMS: ALCHEMY ELEMENT ATOM SUBATOMIC DEMOCRITUS DALTON THOMSON RUTHERFORD BOHR ELECTRON NEUTRAL PROTON NEUTRON ORBIT
Atomic Structure & the Periodic Table
Atomic Structure & the Periodic Table Basic Definitions smallest unit of an element that retains the properties of that element Atoms are made up of several subatomic particles called,, and Protons, Neutrons,
Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table
Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table Name /87 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statements by changing
CHEMISTRY. Matter and Change. Table Of Contents. Section 4.1 Early Ideas About Matter. Unstable Nuclei and Radioactive Decay
CHEMISTRY 4 Table Of Contents Matter and Change Section 4.1 Early Ideas About Matter Chapter 4: The Structure of the Atom Section 4.2 Section 4.3 Section 4.4 Defining the Atom How Atoms Differ Unstable
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
Chem 1A Chapter 5 and 21 Practice Test Grosser ( )
Class: Date: Chem A Chapter 5 and 2 Practice Test Grosser (203-204) Multiple Choice Identify the choice that best completes the statement or answers the question.. The periodic law states that the properties
Regents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
Note that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom?
Atomic Structure and the Periodic Table Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample
DATE: NAME: CLASS: BLM 1-9 ASSESSMENT. 2. A material safety data sheet must show the date on which it was prepared.
Chapter 1 Test Goal Demonstrate your understanding of the information presented in Chapter 1. What to Do Carefully read the instructions before answering each set of questions. True/False On the line provided,
What particles form the nucleus of an atom? CHEMISTRY OLYMPICS 2nd 6 weeks
CHEMISTRY OLYMPICS 2nd 6 weeks Class Battle Between: Bauer, Cannon, Hermsdorf, Lawton, and Muller What particles form the nucleus of an atom? A) protons and neutrons B) electrons only C) neutrons and electrons
Unit 4: Atomic Structure and the Periodic Table
1 Unit 4: Atomic Structure and the Periodic Table Vocabulary: Atom Proton Neutron Electron Nucleus Term Definition Sub-atomic particle with positive (+) charge; located in nucleus of atom; determines identity
2. Which is NOT considered matter? (A) air (B) lead (C) sugar (D) sunlight. 4. Which of the following is a metalloid? (A) Se (B) Sr (C) Si (D) Sn
Midterm Review Packet ANSWER KEY 01/26/2014 Multiple Choice Question 1. Which part of an atom is positively charged? (A) proton (B) neutron (C) electron (D) shells 2. Which is NOT considered matter? (A)
Name Date Class ATOMIC STRUCTURE
4 ATOMIC STRUCTURE SECTION 4.1 DEFINING THE ATOM (pages 101 103) This section describes early atomic theories of matter and provides ways to understand the tiny size of individual atoms. Early Models of
Chemistry Released Questions
Name: Date: 1. What was Niels Bohr s prediction about the location of the electrons in an atom? 3. An atom with which atomic diagram has chemical properties most similar to calcium? A. Electrons pair with
CHAPTER 3. Chemical Foundations
CHAPTER 3 Chemical Foundations 3.1 THE ELEMENTS 118 elements in 92 occur naturally, the rest are synthesized All matter in the universe can be chemically broken down into elements Compounds are made by
Honors Chemistry: Chapter 4- Problem Set (with some 6)
Honors Chemistry: Chapter 4- Problem Set (with some 6) All answers and work on a separate sheet of paper! Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Atoms of
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law
Unit 02 Review: Atomic Theory and Periodic Table Review
Practice Multiple Choice Questions Unit 02 Review: Atomic Theory and Periodic Table Review 1. The number of neutrons in an atom of radioactive C 14 is: a) 6 c) 8 b) 12 d) 14 2. When a radioactive nucleus
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
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
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
Scientist wanted to understand how the atom looked. It was known that matter was neutral. It was known that matter had mass
Atom Models Scientist wanted to understand how the atom looked It was known that matter was neutral It was known that matter had mass They used these ideas to come up with their models, however science
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
Chapter 3-1. proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small
Chapter 3-1 Sub-atomic Charge Location Mass Particle proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small The most mass of the atom
Atomic Theory & the Atom
Section III Atomic Theory & the Atom it s elemental Our view of the atom has changed over time the ATOM the smallest particle of an element that still retains the chemical properties of that element Here
UNIT 4 NOTES: ATOMIC THEORY & STRUCTURE
S T U D E N T N O T E S P r e - A P C h e m i s t r y U N I T 4 Page 1 UNIT 4 NOTES: ATOMIC THEORY & STRUCTURE STUDENT OBJECTIVES: Your fascinating teachers would like you amazing learners to be able to
ATOMS AND ELEMENTS. Evolution of Atomic Theory
ATOMS AND ELEMENTS Chapter Four Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on the smallest
Chemistry Notes: The Periodic Table
Warm-Up 1. What is the periodic table? 2. Who invented it? 3. How does the periodic table organize the elements? 4. Why did Mendeleev leave empty spaces when he constructed his periodic table? Chemistry
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate
Periodic Table of Elements
Periodic Table of Elements The Atomic Nucleus The nucleus is a small, dense region at the center of the atom. It consists of positive protons and neutral neutrons, so it has an overall positive charge.
AnswerIT! Atoms and isotopes. Structure of an atom Mass number, atomic number and isotopes Development of the model of the atom.
AnswerIT! Atoms and isotopes Structure of an atom Mass number, atomic number and isotopes Development of the model of the atom. Atoms and isotopes - AnswerIT 1. The diameter of an atom is about 0.000 000
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
NJCTL.org 2015 AP Physics 2 Nuclear Physics
AP Physics 2 Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?
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,
Atoms, Elements, and the Periodic Table Unit Assessment (2016) Page 1 of 13
TEST NAME:Atoms, Elements, and the Periodic Table Unit Assessment (2016) TEST ID:36063 GRADE:06-08 SUBJECT:Life and Physical Sciences TEST CATEGORY: Common Assessment Atoms, Elements, and the Periodic
Unit 7: The Periodic Table
Unit 7: The Periodic Table Name Class Website: http://pilarz.weebly.com PS:7 TLW categorize elements of the periodic table according to common properties and explain how elements differ in structural parts
Radioactive Decay What is Radioactivity? http://explorecuriocity.org/explore/articleid/3033 http://explorecuriocity.org/explore/articleid/3035 http://explorecuriocity.org/explore/articleid/2160 Quick Review
Atoms, Ions, and the Periodic Table
Atoms, Ions, and the Periodic Table 2-1 2.1 Dalton s Atomic Theory 2-2 1 2.1 Dalton s Atomic Theory The scanning tunneling microscope, STM, invented in 1981, allows us to create images of matter at the
Chapter 4 The Atom. Philosophers and scientists have proposed many ideas on the structure of atoms.
Chapter4 TheAtom 4.1 Early Models of the Atom An atom is the smallest particle of an element that retains its identity in a chemical reaction. Philosophers and scientists have proposed many ideas on the
ATOMIC STRUCTURE. Name: Period: Date: 1) = a generalization of scientific observations that what happens (does explain)
ATOMIC STRUCTURE Name: Period: Date: I. LAW vs. THEORY: 1) = a generalization of scientific observations that what happens (does explain) 2) (model) = a set of assumptions used to explain observations
Unit 2 Exam - Atomic Structure and Nuclear
1. The atomic number of an atom is always equal to the total number of. neutrons in the nucleus. protons in the nucleus 5. The mass number of an atom is equal to the number of. neutrons, only. protons,
Chemistry Unit 2 Quiz KEY
Form A (Master Copy) Chemistry Unit 2 Quiz KEY Standards: SC 1 a, 3 a, c, d DO NOT WRITE ON THIS TEST USE A SCRATCH SHEET OF PAPER! SAVE TREES, INCREASE SUTAINABILITY!! Directions: Please choose the best
Atoms and Elements Review KEY
Atoms and Elements Review KEY YOU ARE EXPECTED TO KNOW THE MEANING OF ALL THE FOLLOWING TERMS: ELEMENT ATOM WHMIS HHPS SDS PURE MIXTURE COMPOUND MOLECULE DIATOMIC HETEROGENEOUS HOMOGENEOUS METALS NON-METALS
CP/Honors Chemistry Unit 3: Atomic Theory Sections 4.1, 4.2, 4.3
CP/Honors Chemistry Unit 3: Atomic Theory Sections 4.1, 4.2, 4.3 Subatomic Particles Warm-Up Quiz 1. What are the three subatomic particles? 2. Where are the particles located in the atom? 3. What are
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
Elements and the Periodic Table
Chapter 7 Elements and the Periodic Table What are metals like? Think of things that are made with metals like aluminum, copper, iron, and gold. What do they have in common? They are usually shiny, and
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
new experimental data, and can be modified
Mass in grams 10 20 30 40 50 Name: Date: Period: CP Chemistry Semester 1 Final Test Review CHAPTERS 1 & 2: Scientific Method, Density, Metric Conversions, Accuracy/Precision, Significant Figures 1. Know
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
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
8th GRADE PHYSICAL SCIENCE: 2nd SEMESTER EXAM OUTLINE
1) Light is an wave. Electromagnetic LIGHT 2) Draw, label, and give an example of each section of the electromagnetic spectrum. Radio - Radios Micro The appliance in your house Infra- Thermal Visible What
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,