(Long Form) Periodic Table and Writing Utensils and the Metallic Bonding Notes and Your ID
Please take out your folded (long form) Periodic table and writing utensils and the Metallic Bonding notes and your ID. Thank you.
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Metallic Bonding (8.4) ID || ||||| ||||| Per 3 Chemistry Class POWER Norms 1. Purpose Per 3 Chemistry Class POWER Norms 1. Purpose - to grow and develop: some Chemistry, some lab skills, communication skills (oral, written), collaboration skills (labs, discussions, study teams), think creatively, think critically, make connections (with each other, between all the skills) Whether it’s fun or easy or difficult or frustrating Per 3 Chemistry Class POWER Norms Evidence : 1. Purpose - to grow and Ready to start with develop: paper, pens etc. out on desk and bags
(with phones in them) away under the seat. • • • • • • Metallic Bonding All metals can conduct electricity
http://www.dur.ac.uk/p.m.johnson/electric_circuits/01_metallic_bonding.htm In a solid metal element the atoms are arranged in a regular repeating pattern (a lattice, or crystal lattice) and the outer energy levels of the metal atoms overlap.
This results in valence electrons that are free to move about through the lattice from one atom to another holding the lattice of atoms together. The freely moving electrons are often called “delocalized” electrons (because their position is not “localized” to one particular atom.)
This model of bonding in metals is called the “electron sea” model because the metal atoms are floating in a sea of delocalized (and moving) valence electrons. The physical properties of metals can be explained in terms of the “electron sea model.” Metals can conduct electricity (and heat) because the delocalized electrons can move to carry the electric current (or heat) quickly from one part of the metal to another. Metals are malleable (can be hammered into sheets) and ductile (can be drawn into wires) because the sea of electrons allows the metal atoms to slide over each other and the metal deforms rather than breaks Metals are shiny (have luster – when clean) the sea of delocalized electrons interacts with light, absorbing and then releasing photons (packets of light, quanta of light) which we see as the shine on the metal
mpts – moderately high metal atoms can move past each other without too much energy (heat) being needed the electron “sea” allows the atoms to move over each other and the solid to melt bpts – extremely high
metal atoms have to escape from each other to enter the gas phase, this takes a great deal of energy because all the attractions between the valence electrons and the atoms have to be overcome (Group 1A metals are softest – because they only have 1 valence electron per atom in the sea of delocalized electrons.) Transition metals Fold to hide the transition elements - Put a title on this format : Main Group Elements (Representative elements) Video: Periodic Table
Watch again as Prof. Radhakrishnan shows us valence shells for Alkali metals.
At 10:49 Main Group Elements: Valence Shell Electrons
Period 1
Period 2
Period 3
Period 4
Period 5
Period 6
Period 7 Main Group Electron dot diagrams Show only valence electrons - electrons available for bonding.
Notice all elements in a column (group) have same dot diagram. Video: Periodic Table
Make notes to answer the following questions while watching:
1. Which elements are named the alkali metals? What is the trend in reactivity for the alkali metals?
2. What two factors led to the development of the current periodic table?
3. How are new elements made and named? Patterns in the Periodic Table and Making Predictions Naming
Size
Mpts and Bpts
Density
(To finish at home for next time.)