Atoms and the Periodic Table
Day 1: Of what are atoms made?
DO NOW (10 min)
In classroom, complete the TIMELINE REFLECTION!
DISCOMFORT WHEN READING
The four chemically important types of atomic orbital correspond to values of l = 0, 1, 2, and 3. Orbitals with l = 0 are s orbitals and are spherically symmetrical, with the greatest probability of finding the electron occurring at the nucleus. All orbitals with values of n > 1 and l = 0 contain one or more nodes. Orbitals with l = 1 are p orbitals and contain a nodal plane that includes the nucleus, giving rise to a dumbbell shape. Orbitals with l = 2 are d orbitals and have more complex shapes with at least two nodal surfaces. Orbitals with l = 3 are f orbitals, which are still more complex. Because its average distance from the nucleus determines the energy of an electron, each atomic orbital with a given set of quantum numbers has a particular energy associated with it, the orbital energy. In atoms or ions with only a single electron, all orbitals with the same value of n have the same energy (they are degenerate), and the energies of the principal shells increase smoothly as n increases. An atom or ion with the electron(s) in the lowest-energy orbital(s) is said to be in its ground state, whereas an atom or ion in which one or more electrons occupy higher-energy orbitals is said to be in an excited state. The calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron shielding, in which intervening electrons act to reduce the positive nuclear charge experienced by an electron, allows the use of hydrogen-like orbitals and an effective nuclear charge (Zeff) to describe electron distributions in more complex atoms or ions. The degree to which orbitals with different values of l and the same value of n overlap or penetrate filled inner shells results in slightly different energies for different subshells in the same principal shell in most atoms.
Open 15-16 Reading… Discomfort...
Read the text, be ready to discuss.
EXPLAIN
Active Reading Strategy P-L-A-N
1) Predict
2) Locate
3) Add
4) Note
I will be modeling P-L-A-N using a reading on the Development of the Atomic Theory.
P = PREDICT - Before you read
Pre-read: predict the content and structure of the text using major headings and subheadings as well as bold-face terms
Create a “concept map” using headers and bold items to guide you
L = LOCATE - Before you read
Assess prior knowledge: locate known and unknown information to help decide how closely they need to read particular sections of text
Determine what you know and ( ) check it.
Put a ( ) question mark next to what you don’t know.
A = ADD - While you read
Use metacomprehension: briefly explain the new concepts or confirm and extend the known concepts
Add details to your map, explain new concepts, define terms
N = NOTE - After you read
Work with the information: they may reproduce the map from memory, reorganize the information, summarize the information in a paragraph,...
Summarize the information from the map in a paragraph or list!
EXPLORE (10 min)
Reading Selection Part 1:
Atoms and the Periodic Table
Day 2: How big is an atom?
What makes an atom?
ENGAGE
Take out your Graphic Organizer!
Turn to your neighbor and answer 2 of the following questions that were asked before you began reading…
Parts of the Atom:
Atomic Number - Number of protons in the nucleus of an atom.
Atomic Mass - Average number of protons and neutrons in the nucleus of an atom
NOTES
This is lithium.
Atomic Number = 3
Protons = 3
Neutrons = 4
Electrons = 3
Atomic Mass = 6.9
This Bohr model is a representation of the Lithium Atom however it is not factually correct. Why?
More Info
Why is hydrogen the only element that does not generally have neutrons?
In other words, why are neutrons important?
Notes LINK
Size of the Atom:
1 proton's mass = 1.7 x 10-24 g
This is so small that scientists made up a new unit called the AMU -- atomic mass unit and 1 proton's mass = 1 AMU
EXPLORE (cont...)
HW:
Reading Selection Part 2:
Atoms and the Periodic Table
Day 3: How are atoms of elements different? And what forces work inside the atom?
VOCABULARY
Electron Proton Neutron Nucleus | Isotope Atomic number Atomic mass Bohr model Ion | Valence electrons Periodic table Period Family Group Octet rule | Metal Metalloid Nonmetal Noble gas |
ENGAGE
Quick Check-In
Check Classroom
NOTES
Ion - charged atom made from losing or gaining electrons
NOTES
Isotopes - atoms with the same number of protons but a different number of neutrons
These are all hydrogens --- just different isotopes.
Isotopes share most of the same physical and chemical properties. For example, the most common isotope of Oxygen has 8 neutrons, but you can also have 9 or 10 neutrons. All are colorless, odorless, flammable gases and all can keep you alive.
However...
NOTES
When something
is written like this:
C-14, the “14” is
the MASS NUMBER
NOTES
HOWEVER WHAT???
There are some differences between isotopes.
Copper-63
Copper-65
(63 * 69%) + (65 * 31%) = 63.62 AMUs
NOTES
Four Basic Forces
More Practice...
CHECK-IN - (use your Periodic Table in your planner)
DECIDE with your table partner -
Quick Overview
How do I find…
HOMEWORK
Complete the Basic Atomic Structure Worksheet.
Atoms and the Periodic Table
Day 4: Putting it All Together
EXPLORE