Mechel Golenberke: My First Website
Chapter 4 Atomic Structure
Check Out: http://www.nclark.net/Atom
4.1 Studying Atoms
4.1.1 Describe the ancient Greek models of matter
4.1.2 List the main points of Dalton’s atomic theory and describe his evidence for the existence of atoms
4.1.3 Explain how Thompson and Rutherford used data from experiments to produce their atomic models
nucleus – the dense, positively charged mass located in the center of an atom
- Dalton proposed the theory that all matter is made up of individual particles called atoms, which cannot be divided.
- Thompson’s experiments provided the first evidence that atoms are made of even smaller particles.
- According to Rutherford’s model, all of an atom’s positive charge is concentrated in its nucleus.
Day 1 & Day 2:
Chapter 4 Pre-Test (6 questions)
Chapter 4 Summary – Talking to the Text
4.1 Interest Grabber: Using Analogies (do on same page as pre-test)
BrainPOP: Atomic Model
See how the atomic model has developed over time in this BrainPOP animated movie.
4.1 PowerPoint (31 slides) & note guide
Check out this Website: Jefferson Lab
Jefferson Lab Question & Answers Atoms, Elements & Molecules
Day 3
Finish 4.1 Notes while I check homework
Go over 4.1 Homework
Go over PowerPoint: Atoms, Molecules, Elements & Compounds
Website: A Virtual Trip to the Center of the Atom
Virtual Physical Science: Lab 8 Thompson & Smaller Parts of Atoms
Lab 9 Rutherford & the Nucleus
4.2 The Structure of an Atom
4.2.1 Identify three subatomic particles and compare their properties
4.2.2 Distinguish the atomic number of an element from the mass number of an isotope, and use these numbers to describe the structure of atoms
- Protons, electrons, and neutrons are subatomic particles.
- Protons, electrons, and neutrons can be distinguished by mass, charge, and location in an atom.
- Atoms of different elements have different numbers of protons.
- Isotopes of an element have the same atomic number but different mass numbers because that have different numbers of neutrons.
proton – a positively charges subatomic particle that is found in the nucleus of an atom
electron – a negatively charged subatomic particle that is found in the space outside the nucleus of an atom
neutron – a neutral subatomic particle that is found in the nucleus of an atom
atomic number – a unique number for each element that equals the number of protons in an atom of that element
mass number – the sum of the number of protons and neutrons in the nucleus of an atom
isotopes – atoms of a given element that have different numbers of neutrons and different mass numbers
Day 4 & 5 – go over 4.2 SRW at end of Day 5
4.2 Interest Grabber: The “Rutherford” Atom
4.2 PowerPoint (21 slides)
BrainPOP: Isotopes
Tim and Moby explain how two atoms of the same element can have different numbers of neutrons in this animated BrainPOP movie about isotopes.
Brightstorm The Atom Atomic Structure (2:16)
The Bohr model is a simple model of atomic structure. It is now outdated, but is still useful at the basic level. An atom has a central core called its nucleus which contains its protons (positively charged particles) and neutrons (neutral particles). The Bohr model depicts electrons, tiny negatively charged particles, as orbiting the nucleus in concentric rings, representing energy levels. However, the electrons reside in atomic orbitals, which are more complicated.
Brightstorm The Atom Atomic Number - Isotopes (4:47)
Every element has a unique atomic number. The atomic number specifies how many protons an element has in its nucleus. In the periodic table of the elements, elements are arranged in order of ascending atomic number. Isotopes are atoms that have the same number of protons but different numbers of neutrons. Different isotopes have different nuclear stabilities.
Brightstorm The Atom Atomic Mass (4:19)
An element’s atomic mass is the mass of one atom of that element, measured in atomic mass units (amu). An element’s atomic mass in amu is equal to its molar mass in g/mol.
PhET: Build an Atom, Isotopes & Atomic Mass
4.3 Modern Atomic Theory
4.3.1 Describe Bohr’s model of the atom and the evidence for energy levels
4.3.2 Explain how the electron cloud model represents the behavior and locations of electrons in atoms
4.3.3 Distinguish the ground state from excited states of an atom based on electron configurations
- An electron in atom can move from one energy level to another when the atom gains or loses energy.
- Scientists use the electron cloud model to describe the possible locations of electrons around the nucleus.
- An electron cloud is a good approximation of how electrons behave in their orbitals.
- The most stable electron configuration is the one in which the electrons are in orbitals with the lowest possible energy.
energy levels – the possible energies that electrons in a atom can have
electron cloud – a visual model of the most likely locations for electrons in an atom
orbital – a region of space around the nucleus where an electron is likely to be found
electron configuration – the arrangement of electrons in the orbitals of an atom
ground state – a state in which all the electrons in a atom have the lowest possible energies
Day 6 & 7 – go over 4.3 homework @ end of day 7
4.3 PowerPoint (27 slides)
Investigation 4B Modeling the Location of an Electron in an Atom
**Vocabulary Quiz – only 12 words in chapter so do all together**
Brightstorm The Atom Atomic Orbitals (4:27)
Atomic orbitals are regions of space in which electrons can be found. Each orbital can fit two electrons and different orbitals have different shapes. The s sub-level has one spherically shaped orbital, while the p sub-level has three dumbbell shaped orbitals. The arrangement of electrons in orbitals can be depicted using either orbitals diagrams or electron configuration notation.
Brightstorm The Atom Orbital Diagrams (4:58)
Orbital diagrams are pictorial descriptions of the electrons in an atom. Three rules are useful in forming orbital diagrams. According to the Auf Bau Principle, each electron occupies the lowest energy orbital. The Pauli Exclusion Principle says that only two electrons can fit into an single orbital. Hund’s rule states that electrons go into different orbitals in the same sub-level before doubling up inside orbitals.
Brightstorm The Atom Electron Configuration (3:53)
Electron configuration is shorthand for the arrangement of electrons in atomic orbitals. It is written out, as opposed to orbital diagrams which are depicted pictorially. For elements with many electrons, noble gas configuration is a useful way to abbreviate the electron configuration.
Day 8
Forensic Lab: Using Flame Tests
Investigation 4A Constructing Models of Atoms
Day 9 – How to Build an Atom WebQuest
- Jefferson Lab: How Do I Build a Model of an Atom?
- McDougal Littell Interactive: Atomic Models, Build Atoms Yourself, Build More Atoms
- PhET Interactive Simulation: Build an Atom
(Teacher page with some easy instructions: http://fcweb.sd36.bc.ca/~hunter_s/Chemistry%2011)
Day 10
Supplement: What is Matter: Even smaller particles of matter (mesons, gluons, & quarks)
Review: Chapter 4 WordWise & Chapter 4 Crossword
Day 11 – Chapter 4 Test
Brightstorm The Atom Exceptions to Electron Configuration (2:58)
There are two main exceptions to electron configuration: chromium and copper. In these cases, a completely full or half full d sub-level is more stable than a partially filled d sub-level, so an electron from the 4s orbital is excited and rises to a 3d orbital.
Brightstorm The Atom Valence Electrons (2:19)
Valence electrons are the outer electrons that are involved in bonding. Only electrons in the s and p orbitals are valance electrons, so a given atom can have between 0 and 7 valance electrons. Atoms with 0 valence electrons are called noble gases and don’t like form bonds. An atom’s valence electrons can be depicted pictorially using Lewis Dot Diagrams.
more Brightstorm The Atom:
