10/15 Review: Atomic Structure
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This document provides an overview of an upcoming chemistry class covering atomic structure. The weekly schedule outlines topics to be covered each day, including atomic radius, electronegativity, atomic structure, and a midterm exam on Friday. Students are instructed to sketch the periodic table and label families for homework. The document then reviews atomic structure, including the dense nucleus at the center containing protons and neutrons, and less dense electron shells. Examples are given to calculate protons, neutrons, and electrons in different atoms. Homework assigned is to make a study notecard and complete a review worksheet in preparation for the midterm.
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1) Atoms are the smallest particle into which an element can be divided and still retain its properties. Atoms are made up of even smaller particles called subatomic particles - protons, neutrons, and electrons.
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11. (Draws a picture of a nitrogen nucleus with 7 protons)
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This document summarizes the history and development of the atomic theory and periodic table. It discusses early Greek philosophers' ideas about atoms, John Dalton's atomic theory in the early 1800s, J.J. Thomson's discovery of electrons in the late 1800s, Ernest Rutherford's discovery of the nucleus in 1909, and the discovery of neutrons in 1930 which completed the modern atomic model. It also explains how atoms are composed of protons, neutrons and electrons, how atomic and mass numbers are used to identify elements and isotopes, and how average atomic masses are calculated based on the relative abundances of isotopes in nature.
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The document discusses the basic building blocks of matter at the atomic level. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and found in the atom's nucleus along with neutrons, which have no charge. Electrons are negatively charged and orbit the nucleus. It provides examples of hydrogen, oxygen, and sodium atoms, showing their proton, neutron, and electron composition. The atomic number is the number of protons, while the mass number includes protons and neutrons. Atoms can gain or lose electrons to become ions that are electrically charged.
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3) Atoms can have different numbers of neutrons forming isotopes of the same element.
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Atomic structure.ppt ishan
The document summarizes atomic structure. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and have a mass of about 1 atomic mass unit. Neutrons are neutral and also have a mass of about 1 atomic mass unit. Electrons are negatively charged and have a negligible mass. The nucleus of an atom contains protons and neutrons, and electrons orbit the nucleus in shells. For example, hydrogen has 1 proton, 1 electron, and no neutrons, while helium has 2 protons, 2 neutrons, and 2 electrons. The mass number of an atom is the total number of protons and neutrons, and the proton number indicates how many protons an atom contains. Electron shells
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Here are the answers:
1. Aluminum
2. Helium
3. Palladium
4. Gold
5. Oxygen
6. Calcium has 20 protons
7. Silver has 47 protons
8. Neon has 10 protons
9. Potassium has 19 protons
10. Iron has 26 protons
11. (Draws a picture of a nitrogen nucleus with 7 protons)
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This document provides a review of key concepts in atomic structure:
1) Protons have a positive charge and determine the atomic number, neutrons have no charge and determine isotope variations, electrons have a negative charge and determine ion charge state.
2) Atomic mass is the total number of protons and neutrons, while the atomic number indicates just the number of protons. Neutrons can be calculated by subtracting the atomic number from atomic mass.
3) Elements are arranged on the periodic table by atomic number, which identifies each unique atom, while isotopes of an element can vary in neutron number.
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The periodic table can be used to determine the structure of an atom. The atomic number indicates the number of protons in the nucleus, while the atomic mass provides the total number of protons and neutrons. By subtracting the atomic number from the atomic mass, we can calculate the number of neutrons. The periodic table also shows the arrangement of elements by increasing atomic number and energy levels which indicate where electrons are located around the nucleus.
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The charge of the ion is indicated
by the superscript number after the element
symbol. A positive number means the atom
lost electrons and is positively charged. A
negative number means the atom gained
electrons and is negatively charged.
Model: Na+ Ion
Sodium ion (Na) that lost 1 electron
Charge: +1
Protons: 11
Electrons: 10
Neutrons: 12
Mass: 22.9898
Model this ion in your notebook!
Model: Cl- Ion
Chlorine ion (Cl) that gained 1 electron
Charge: -1
Protons: 17
Electrons: 18
Neutrons: 18
Atomic chemistry
This document provides an overview of atomic chemistry, including:
1) Atomic structures such as shells, orbitals, suborbitals and electrons that make up the structure of an atom.
2) Concepts like the periodic table, atomic radius, ionization energy and electronegativity that describe atomic properties.
3) Bonding concepts including molecular forces, melting/boiling points and solubility that describe how atoms interact.
4) Radioactivity and the three types of radioactive particles: alpha, beta and gamma rays.
Atomic chemistry
This document provides an overview of atomic chemistry, including:
1) Atomic structures such as shells, orbitals, suborbitals and electrons that make up the structure of an atom.
2) Concepts like the periodic table, atomic radius, ionization energy and electronegativity that describe atomic properties.
3) Bonding concepts including molecular forces, melting/boiling points and solubility that describe how atoms interact.
4) Radioactivity and the three types of radioactive particles: alpha, beta and gamma rays.
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The document provides instructions on how to determine the number of protons, neutrons, and electrons in an atom using the atomic number and atomic mass from the periodic table. It gives examples of determining the particles in boron and chlorine atoms. Students are then asked exit slip questions to test their understanding of finding particles and identifying elements based on particle numbers.
12 14 Balancing Review1
The document contains information from a chemistry class, including:
- A practice exam average of 87% was achieved, with questions 5, 6, 7, 9, and 14 dropped.
- An upcoming unit exam on Thursday will cover balancing equations, the mole concept, and conversions between grams, moles, atoms, and grams.
- A snowman challenge activity had students work in groups to balance sample chemical equations.
- An exit slip posed sample questions testing the concepts of identifying reactants, calculating atoms in a formula, balancing equations, and determining missing coefficients.
2 4 What Is Pressure
The document instructs students to get their binders and take a seat. It reports that 96% of students answered yesterday's practice questions correctly. The objectives for the lesson are to describe how temperature relates to molecular motion and to convert between the Kelvin and Celsius temperature scales.
Lesson: Tuesday 9/1
Two quantities that define matter are volume and mass. Volume can be measured using units like liters, cubic centimeters. Mass is measured using standard units like grams.
The document discusses the history of atomic theory. Ancient Greek philosophers proposed the idea of atoms as the smallest indivisible units of matter. In the 1800s, John Dalton further developed atomic theory, proposing that atoms are the building blocks of all matter and composed of even smaller subatomic particles like protons, neutrons and electrons.
The size of an atom is incredibly small. For example, about 10 trillion atoms could fit in a single centimeter. Despite their small size, atoms are not truly indivisible as originally proposed, as they can be broken
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I apologize, upon reviewing the document again I do not see enough context to summarize it in 3 sentences or less. The document provides some details about an upcoming exam and homework assignments but does not have an overall topic or theme that can be succinctly summarized. Please provide more context if you would like me to attempt a summary.
12 15 Mole Review
Here are the steps to solve this problem:
1) Given: 12.04 X 1023 molecules of H2O
2) Conversion factors:
1 mol H2O / 6.02 X 1023 molecules H2O
18.02 g H2O / 1 mol H2O
3) Calculations:
12.04 X 1023 molecules H2O x (1 mol H2O / 6.02 X 1023 molecules H2O) x (18.02 g H2O / 1 mol H2O) = 36.04 g
The answer is d.
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10/15 Review: Atomic Structure
- 1. Launch Grab your binder and immediately take a seat Take out last night’s homework 1. From memory, sketch out the periodic table and label the 5 families. 2. What family do the following belong to? i. Sr ii. I iii. Fr iv. Xe
- 2. Weekly Schedule Monday: Atomic Radius Tuesday: Electronegativity & Ionization Energy Wednesday: Metals, nonmetals, special groups Thursday: Atomic structure & nuclear processes Friday: Mid-Term Exam Only excused absences, otherwise 0! No retakes! We don’t have much time! If you don’t understand something, ask!
- 3. Review Session Today During lunch After school (until 4:30pm)
- 4. How is the atom structured? Mr. Heffner 10/15/09
- 5. How is the atom structured? 0 Nucleus 0 Rings 0 • Protons (1 amu) • Electrons (0 amu) • Neutrons (1 amu) 0 valence = outermost
- 6. How is the atom structured? Density comparison: The nucleus Large mass Small volume Dense! The rings Small mass Large volume Not Dense!
- 7. How is the atom structured? 5 Atomic number Atomic B Boron Really important! mass 10.81
- 8. Example #1 How many protons, neutrons, and electrons does an atom of nitrogen have? Step 1: Find the # of protons Atomic number 7 Step 2: Find the # of neutrons Atomic mass – atomic number 14 - 7 = 7 Step 3: Find the # of electrons Same as # of protons 7 What about valence electrons?
- 9. Example #2 Isotope: different # of neutrons How many protons, neutrons, and electrons does an atom of nitrogen-15 have? # of protons Atomic number 7 # of neutrons Atomic mass – atomic number 15 - 7 = 8 # of electrons Same as # of protons 7
- 10. Nuclear Review Two forces in the nucleus: Strong force: holds the nucleus together “Bungees” Electrostatic repulsive force: tries to break it apart Protons fighting There are three types of radioactive decay: Alpha ( ) decay Beta ( ) decay Gamma ( ) decay
- 11. Practice Questions Review Worksheet #4
- 12. Notecard One notecard, front and back Things I would include: Definitions: isotope, atomic number, alpha particle, valence electron, density of nucleus… Pictures of the trends Families on the periodic table
- 13. Homework Make a notecard Finish Review Worksheet #4 Study hard! Review your notes Check out our exit slips online!