Download Periodic Table Development

Unit 3: The Periodic Table
Lesson 1
Periodic Table Development
1.____________ ________________
1869 - Published a table of the elements organized by ___________ ________.
2. ____________ ________________
1913 – Reorganized the table of elements in order of _____________ _________
____________.
3.
________ ___ ________________
1944 - Co-discovered ____ elements and created the _____________ series.
Periodic Law:
Rows are called ________________________
Columns are called _____________________
Metals
Non – Metals
Semi-metals (Metalloids)
Ions by Group
To become stable, atoms ______________________ electrons to fill their outermost energy level
(valence shell) with 8 electrons (Octet rule).
Metals _______ electrons to achieve eight electrons in their valence shell.
Nonmetals ________ electrons to achieve eight electrons in their valence shell.
Examples
What is the electron configuration of Oxygen?
What is the electron configuration of Mg?
Alkali Metals (Group 1 or IA)
Hydrogen
Alkaline Earth Metals(Group 2 or IIA)
Boron Family (Group 13 or IIIA)
Carbon Family (Group 14 or IVA)
Nitrogen Family (Group 15 or VA)
Oxygen Family(Group 16 or VIA)
Halogens(Group 17 or VIIA)
Noble Gases(Group 18 or VIIIA)
Representative Elements
Lesson 2
Transition Metals (d subshells, Groups 3 – 12)
Inner Transition Metals (f subshells)
Post Transition Metals (P Block Metals)
Lesson 3
Periodic Table Trends
Atomic Radius
Distance from the center of the nucleus to __________________________________
Atoms get ___________ going down a group because each is ________________________ bigger
(“n” value increases)
Atoms get ____________going across a period because __________________________ the electrons
towards the nucleus
Z Efficiency: As you increase the number of ______________ in the nucleus of the atom, you increase
the _______________________________ of the atom (Zeff), and the nucleus pulls more strongly on the
entire electron cloud. This makes the atomic radius _________________ in size.
Ionic Radius
Size of _____________________
Atoms that _____________________, lose their whole outer shell, thus ________________________.
Atoms that _____________________ become bigger because the extra electrons ____________each
other and space out more.
Ionization Energy
Energy needed to _____________________________ (make an atom an ion) from a gaseous atom.
The __________________the ionization energy, the _________________ it is to remove an electron
Atoms with a _________________ atomic radius have a _____________________ ionization energy.
Why? –
Atoms with a __________________ electronegativity have a ______________ionization energy.
Why? –
Electronegativity
Ability to ________________________ electrons in a chemical bond
Electronegativity ___________________ from left to right across a period
Why? –
Electronegativity ____________________ as you go down a group
Why? –
Summary
Sample Problem
Boron, carbon, and aluminum occur near each other in the periodic table. Use the periodic table to
identify which of these elements is:
The largest atom
The atom with the highest ionization energy
Examples
Compare the following atoms: F, Br, At
Which has the largest:
Electronegativy?
Atomic Radius?
1st Ionization energy?
Examples
Compare the following atoms: K, Cu, Kr
Which has the largest:
Electronegativy?
Atomic Radius?
1st Ionization energy?
Metallic Character
Metals have a higher tendency to ___________ electrons order to achieve the ____________ of a
_________________________.
Valence electron _____________________________ = ______________ to lose electrons.
As electronegativity or ionization energy increases, metallic character ___________________.