Atom review
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The document discusses the key components of atoms including the structure of an atom, atomic nucleus, atomic number, atomic mass, ions, isotopes, and how to calculate protons, electrons, and neutrons from the periodic table. It explains that atoms are made up of protons, neutrons, and electrons, the nucleus is heavy and small at the center of the much larger electron cloud, and the atomic number represents the number of protons and electrons in a neutral atom which determines its position on the periodic table.
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Atomic models are useful because they allow us to picture what is inside of an atom, something we will never be able to actually see. We're going to talk about two models, the Bohr model and the Quantum model. While we know that the Quantum model is the correct way to represent atoms, the Bohr model is still useful for a very basic understanding. Think of it as a stick figure sketch of an atom. The parts are all there, its just not quite filled in all of the way.
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Steps for Drawing a Bohr Model:
1. Count the number of protons, electrons, and neutrons for that atom.
2. Draw the nucleus. Indicate the correct number of protons and neutrons in the nucleus.
3. Draw energy levels around the nucleus, starting with the energy level closest to the nucleus. Fill up each energy level before moving on to the next.
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For example, here is a Bohr model for the average oxygen atom:
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Atomic models are useful because they allow us to picture what is inside of an atom, something we will never be able to actually see. We're going to talk about two models, the Bohr model and the Quantum model. While we know that the Quantum model is the correct way to represent atoms, the Bohr model is still useful for a very basic understanding. Think of it as a stick figure sketch of an atom. The parts are all there, its just not quite filled in all of the way.
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1. Count the number of protons, electrons, and neutrons for that atom.
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ATOMIC AND MOLECULAR STRUCTURE
This document provides a 3-paragraph summary of the contents of an inorganic pharmaceutical chemistry course titled "Atomic and Molecular Structure/Complexation". The course will cover 9 topics including atomic and molecular structure, electrolytes, essential and trace ions, non-essential ions, gastrointestinal agents, antacids, protective adsorbents, radiopharmaceutical preparations, and radio opaque and contrast media. It will examine the fundamental atomic structure including protons, neutrons, electrons, isotopes and quantum mechanics. The course will also cover electronic configurations, orbitals, quantum numbers, ionization, periodic trends, and transition metal ions. The instructor is Hayder R. Fadhil and the course is listed as the 1st semester, 3
Atomic structure
1. Atoms consist of protons and neutrons in the nucleus surrounded by electrons that reside in orbitals classified by quantum numbers.
2. Electrons fill orbitals systematically according to rules like the Aufbau principle. The configuration of electrons plays a vital role in chemistry as chemical interactions occur between valence electrons.
3. Atoms with similar electron configurations display similar chemical properties, explaining periodic trends in the periodic table. Properties like atomic size, ionization energy, and electronegativity follow periodic trends related to electron configuration.
D4_D5_Periodicity_Chemistry_8_pgs.docx
1. The document is a periodicity chemistry worksheet containing questions about periodic trends, atomic structure, ionization energy, electronegativity, and other periodic properties.
2. Key periodic trends addressed include ionization energy increasing across a period and decreasing down a group, atomic radius decreasing across a period and increasing down a group, and electronegativity generally increasing moving up and to the right on the periodic table.
3. Factors that influence periodic trends are discussed, such as the shielding effect increasing with greater nuclear charge, which causes atomic radius to decrease and ionization energy to increase moving across a period.
Unit 2 Physical Science
This document provides information about atomic structure and the periodic table. It defines key terms like isotope, nuclear reaction, atomic number, and explains that the number of protons determines an element's identity while the total number of protons and neutrons determines its mass. The document also discusses the periodic table, noting that periods indicate the number of occupied electron energy levels while groups indicate how many valence electrons an element has. It explains trends in the periodic table like atomic mass generally increasing as you read across or down.
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Atom review
- 1. List of topics to know: structure of an atom ( what is looks like and what the subatomic particles are) atom’s nucleus, size and relative mass Atomic number Atomic Mass Atoms, Ions, Isotopes Know how to calculate, p,e, and n, from periodic table
- 2. Structure of an atom Draw and label
- 3. atom’s nucleus, size and relative mass NUCLEUS : heavy, small, compact ELECTRON CLOUD: light, wide area
- 4. Atomic particles The 3 particles of the atom are: a.______________________ b.______________________ c.______________________ Their respective charges are: a.______________________ b.______________________ c.______________________
- 6. NUMBER OF PROTONS=NUMBER OF ELECTRONS
- 7. Atomic number The atomic number tells you the number of ______________________in one atom of an element. It also tells you the number of _____________________in a neutral atom of that element. The atomic number gives the “identity “ of an element as well as its location on the Periodic Table. No two different elements will have the _____________ atomic number.
- 8. Atomic Mass/Mass number The atomic weight is basically a measurement of the total number of particles in an atom's nucleus. Mass number= round off atomic weight
- 9. Number of neutrons Mass Number = (Number of Protons) + (Number of Neutrons)
- 10. IONS POSITIVE ( CATION) NEGATIVE (ANION)
- 11. ISOTOPE Same element , different neutrons
- 12. Number of Protons = Atomic Number Number of Electrons = Number of Protons = Atomic Number Number of Neutrons = Mass Number - Atomic Number