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ChemI Block-1st: 3.4.15 Infinite Campus: • Matter and Energy Exam-32 pts. • Mapping Atomic Structure Lab-10pts. Objectives: • I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab) • I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.) • I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.) Atomic Ranking Task Worksheet 1. What question(s) were you able to answer correctly using your background knowledge? 2. What question(s) did you have trouble with using your background knowledge? What did you learn from your research last night? Include the sources you used. Atomic Ranking Task Worksheet Answer qts. using: 1. Background Knowledge 2. Resources(textbook)-marker Atomic Structure: Ranking Task Atomic Number Mass Number Isotopes Atomic Mass ChemI Block-1st: 3.9.15 Due: Define the following vocabulary words: atomic number, mass number, and isotopes. Objectives: • I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab) • I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.) • I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.) Atomic Structure: Bell Ringer 1. What is the atomic number for an atom? 2. Rank the following atoms from smallest to largest based on atomic number? a. N b. H c. F d. O 3 . What is an atom’s mass number? Atomic Number • The number of protons within an atom’s nucleus. • Its an atom’s I.D. • Atoms of the same element always have the same number of protons. • Do you notice any patterns with atomic numbers on the periodic table? Subatomic Particles in an Atom Subatomic symbol charge Particle location Mass (g) mass # (amu) proton 1.674 x 10 -24 1 electron 9.11 x 10-28 0 neutron 1.675 x 10 -24 1 What is the mass number for an atom? Subatomic symbol charge location Particle Mass (g) mass # (amu) proton p+ +1 nucleus 1.674 x 10 -24 1 electron e- -1 electron cloud 9.11 x 10-28 0 neutron n0 0 nucleus 1.675 x 10 -24 1 Atomic Structure Lab education.jlab.org Mass Number? Mass Number Mass number : • The mass of a single atom. • Sum of the p+ and n0 within an atom. • Common unit: atomic mass unit (amu) *The mass number is NOT the same as atomic mass located on your periodic table. What is the mass number for an atom? Subatomic symbol charge location Particle Mass (g) mass # (amu) proton p+ +1 nucleus 1.674 x 10 -24 1 electron e- -1 electron cloud 9.11 x 10-28 0 neutron n0 0 nucleus 1.675 x 10 -24 1 Element’s Atomic Numbers ChemI Block-1st: 3.10.15 Due: • Elements Subatomic Differences Worksheet Objectives: • I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab) • I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.) • I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.) Elements: Subatomic Differences Bell Ringer: Atom’s Subatomic Particles 1. : A cesium (Cs) atom has a mass of 133 amu and an atomic number of 55. a. How many p+, e-, and n0 are there? b. Illustrate where the subatomic particles are located within the cesium atom. 2.: An iron(Fe) atom has an atomic number of 26 and consists of 30 neutrons. a. How many p+ and e- are there? b.What is iron’s mass number (amu)? Isotope Worksheet Homework: • Annotate the passage on isotopes. • Complete the worksheet (front and back) ChemI Block-1st: 3.11.15 Due: • Isotope Worksheet Objectives: • I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab) • I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.) • I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.) • I can calculate atomic mass for an element. Elements :Isotopes Isotopes • What is an isotope? ChemI Block : 2.25.15 Due: • Mapping Atomic Structure Lab-Post Lab Qts. Objectives: • I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab) • I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.) • I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.) • I can distinguish between mass number and atomic mass. Isotopic Symbols Isotope Applications 1. Calculate the number of protons, neutrons, and electrons in each neutral isotope below. Na-18 and Na-23 ChemI Block-1st: 3.12.15 Due: • Kandium Lab Objectives: • I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab) • I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.) • I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.) • I can calculate atomic mass for an element. • I can investigate the evolution of the atom. Chem I: Homework 1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles. a. Li-6 and Li-7 b. H-1 and H-2 c. O-16 and O-17 d. B-10 and B-11 Chem I: Homework 1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles. a. O-16 and O-17 b. B-10 and B-11 Chem I: Homework 1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles. a. Li-6 and Li-7 b. H-1 and H-2 c. O-16 and O-17 d. B-10 and B-11 2. Research and state the difference between the following atomic terms: mass number and atomic mass. *Record answers on separate sheet. Kandium Lab Purpose: To investigate an new element’s isotopes and to calculate its atomic mass Mass Number vs. Atomic Mass • Mass Number: • Atomic Mass: An Atom’s Mass Mass number : • The mass of a single atom. • Sum of the p+ and n0 within an atom. • Common unit: atomic mass unit (amu) *The mass number is NOT the same as atomic mass located on your periodic table. Calculating Atomic Mass of an Element Atomic mass: • It is an average mass calculated from all the isotopes of a particular element. • The average mass is weighted because there is NOT an equal amount of each isotope in a sample. • How do you calculate a weighted average mass? 1. For each isotope, multiply its mass (mass #) by its natural abundance (decimal form) to get the weighted mass for each isotope. 2. Add up the isotopes weighted masses to get the atomic mass (average mass) for the element. Calculating Atomic Mass Isotope Natural Abundance (%) Atomic Structure Review: Bell Ringer Rubidium’s Isotopes Natural Abundance (%) Rb-86 72.2 Rb-87 27.8 1. Identify the number of protons, neutrons, and electrons for each isotope of Rb. 2. Does Rb-86 and Rb-87 isotopes have similar chemical properties? Explain how you know this. 3. a.Calculate the atomic mass of Rubidium. b. What is the difference between mass number and atomic mass? 4. a. Distinguish between the two types of forces within an atom. b. Which force is stronger? Explain how you know this. ChemI Block : 3.13.15 Due: • Kandium Lab • Isotopes and Atomic Mass Worksheet Objectives: • Atomic Structure Quiz • I can identify forces within an atom. • I can investigate the evolution of the atom. Homework: Atomic Structure Study Guide-Test Tuesday Element’s Isotopes and Atomic Mass • Questions? Atomic Structure Quiz • Quiz includes the ranking task worksheet. ChemI Block : 3.16.15 Due: • Ranking Task Worksheet • Atomic Structure Study Guide-reviewed Objectives: • I can identify forces within an atom. • I can investigate the evolution of the atom. • Atomic Structure Test-Wednesday! Bell Ringer: Atomic Structure 1. If most of the atom is empty space, why is it matter (made of atoms) does not pass through one another? 2. What keeps the protons from leaving the nucleus and hooking up with the electrons? Atomic Properties • If most of the atom is empty space, why doesn’t matter pass through one another? • “The Space Between Atoms” video clip. spiff.rit.edu Atomic Forces • Electrostatic Forces : - Forces between charged particles. Types of electrostatic forces: a. Attractive: (p+ and e-) b. Repulsion: (p+ and p+ e- and e-) • Nuclear Forces: Forces that holds p+ and n0 together in nucleus. Evolution of the Atom • Rank the models of the atom from earliest to most recent. (only use your background; context clues). Evolution of the Atom • Rank the models of the atom from earliest to most recent. (only use your background; context clues). Democritus(400b.c.) Greek Philosopher 1) Observed matter to be made up of atoms. 2) Atoms are the smallest form of matter. 3. Atoms cannot be broken down. 4) The types of atoms in matter determine its properties. Aristotle: Greek Philosopher (300b.c.) • Aristotle observed matter to be made from four things: earth, water, air, and fire John Dalton’s Atomic Model Dalton’s Atomic Theory 1. Atoms are the building blocks of all matter. 2. Atoms cannot be subdivided. 3. Each element has the same kind of atoms. 4. A compound is composed of two or more atoms chemically combined in a fixed amount. Ex. NaCl 5. Atoms cannot be created or destroyed just rearranged during chemical reactions. Thomson’s Plum Pudding Model Thomson’s Cathode Tube Experiment l-esperimento-piu-bello-della-fisica.bo.imm.c... Subatomic Particle: Electron J.J. Thomson (pg. 105) • 1897 discovered electrons in gas atoms using a cathode ray tube. • Determined electrons have a negative charge. • Electrons have the same charge in all atoms. Robert Millikan: Determined the mass of the electron to be very tiny. J. J Thomson’s Plum Pudding Model • If atoms are made of electrons how come most matter does not shock us? • Atoms must have positive particles, too. • He proposed the Plum Pudding Atomic Model • An atom is equally made up of positive and negative particles. Goldstein’s Cathode Tube Experiment chemed.chem.purdue.edu reich-chemistry.wikispaces.com He discovered protons using a cathode ray tube. Observe particles moving in the opposite direction. Subatomic Particles: Protons • 1886 Eugen Goldstein observed particles traveling in the opposite direction of the cathode rays(electrons). • He knew these particles must be (+) charged. They were called protons. • Protons charge is the same for all atoms • Protons have a significant mass compared to the electron. Rutherford’s Model of the Atom green-planet-solar-energy.com Rutherford’s Gold Foil Experiment If positively charged light particles traveled through a sample of matter composed of atoms with protons and electrons evenly distributed throughout the atom, what would happen to the trajectory (path) of the + charged light particles as it passes through these atoms? Rutherford’s Gold Foil Experiment Rutherford’s Conclusion •Most of the atom is empty space. •Small dense region composed of (+) charged particles. (Nucleus) Rutherford’s Nuclear Atomic Model Subatomic Particle: Neutron •What keeps the protons within the nucleus ? (Like particles repel each other) •1932 - James Chadwick discovers that the nucleus also has neutral particles present. He called them neutrons. Chadwick’s Experiments: Neutron nobelprize.org Bohr’s Model of the Atom http://micro.magnet.fsu.edu Bohr’s Model of the Atom http://micro.magnet.fsu.edu/ Bohr’s Model of the Atom •Electrons travel in fixed, circular paths around the nucleus. •Each path has a specific energy requirement. •These circular paths are called energy levels. •Limited number of electrons on each energy level. (2n2 Rule) http://micro.magnet.fsu.edu/ Current Atomic Model Erwin Schrodinger Current Atomic Model Erwin Schrodinger blogs.stsci.edu science.howstuffworks.com Current Atomic Model Electrons do not travel in fixed paths around the nucleus Electrons constantly move to different energy levels in the electron cloud. Direction of movement is dependent upon how much energy an electron has. Observed several different paths electrons can take around the nucleus. Types of electron paths around nucleus Atomic Models Atomic Model Dalton’s Model Thomson’s Model Rutherford’s Model Bohr’s Model Schrodinger’s Model Illustration Description Atomic Models Dalton’s Atomic Model Bohr’s Planetary Model Thomson’s Plum Pudding Model Rutherford’s Nuclear Model Schrodinger’s Atomic Model (current model)