Transcript Metals Non-metals Metalloids

Section 11.4
Electron Configuration and
Atomic Properties
PERIOD 6 Group #2
Background
- Electron; covers a broad area it also behaves like cloud in an
atom
• to understand how the principal energy levels fill with electrons in
atoms beyond hydrogen.
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to learn about valence electrons and core electrons.
to learn about the electron configurations of atoms with Z < 18.
to understand the general trend in properties in the periodic table.
Electron Configuration
• The electron arrangement in atoms from Z = 1 to Z = 18
can be described by placing electrons in principal
energy level
• Principal energy level – energy denoted by principal
quantum number n. ex. – n = 1 , n = 2, n = 3….
• The 1st element in the each period of the Periodic Table
represents a new principal energy level.
• Ex. – hydrogen has lone electron in 1s orbital / so
represents 1s^1 because it is in electron arrangement
• Electron arrangement – can be called electron
configuration in an atom
https://teach.lanecc.edu/gaudias/scheme.gif
http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/text_images/CH08/FG08_06.JPG
Question #1
• For the first 18 elements, what is the sublevel
order and the elements?
Answer #1
• 1s 2 s 2p 3s 3p
are the sublevels for the first 18 elements.
Orbital Diagram
• Also known as the box diagram
• Gives more detailed information
about electron configuration
• Arrows represent an electron
spinning in a particular direction.
• For each element’s orbital – takes
one electron before any orbital in
each sub level can receive another
electron.
• Pauli Exclusion Principle –
Question #2
• What is the electron configuration and orbital
diagram for silicon?
Example of Orbital Diagram
Answer #2
• Silicon –
1s^2 2s^2
2 ^6
3s^2
3p^2
Metal & Non-metal & Metalloids
Chart
All URL on “Reference” page
Metals
Non-metals
Gallium crystals
from left to right
He, Ne, Ar, Kr, Xe
Metalloids
Boron
Iron (Fe)
from left to right; F, Cl, Br, l
Copper(Cu)
Sulfur
Silicon
Germanium
Metals & Nonmetals & Metalloids
• Metals and nonmetals have relatively large ionization
energies.
• Metals gain electrons
• Lower left region of the periodic table have the lowest
ionization energies (are the most chemically active metals)
• Upper right region of the periodic table have the highest
ionization energies (are the most chemically active
nonmetals)
• Metalloids – found along the stair-steps line between the
metals and nonmetals.
• Metalloids have properties of both metals and nonmetals.
Question #3
• Name the physical properties of the metals.
Answer #3
• A lustrous appearance, the ability to change
shape without breaking, and excellent
conductivity of heat and electricity.
Atomic Size
•Increases down a group
•Decreases to the right of the period.
•The average distance of the electrons from the
nucleases increases.
•Atoms get bigger as electrons are added to larger
principal energy levels.
•The sizes of atoms vary
•The atoms in a particular period all have their
outermost electrons in a given principal level
http://www.avon-chemistry.com/p_table_atomic_rad.jpg
Question #4
• Which element has the smallest atomic size?
Answer #4
The element with the smallest atomic size is
helium.
Ionization Energy
http://nanotech.sc.mahidol.ac.th/genchem/bonding1/ie.jpg
Ionization Energy
• The energy required to remove an electron
from and individual atom in the gas phase.
• Increases up a group and to the right of a
period.
• Metals have relatively low ionization energies.
• Ionization energies tend to decrease in going
from the top to the bottom of a group.
Question #5
• What is the definition of ionization energy and
how does it related to the elements?
Answer #5
• It is the energy to remove an electron from an
individual atom in the gases phase of an
element and the energies tend to decrease
going down a group.
Quiz
1) What is the electron configuration for Cerium (Ce;
atomic #58)? Include a box diagram.
2) What is the Pauli Exclusion Principle and how does it
relate to the orbital diagram?
3) Out of the metals and non-metals, which has relatively
large ionization energy?
4) In which pattern so metals tend to lose electrons?
Explain.
5) Define atomic mass and atomic size.
Answer key
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5)
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2
4f^1
2 electrons in the same level cannot be in the same quantum state
so in the orbital diagram, the arrows cannot be in the same
direction, and each orbital can only hold up to 2 electrons.
Nonmetals
Metals tent to lose electrons going down a group because as we go
down a group, the electron being removed resides on average
farther and farther from the nucleus.
Atomic mass is the mass of an atom and atomic size is the size of
the atom.
Reference
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https://teach.lanecc.edu/gaudias/scheme.gif
http://www.avon-chemistry.com/p_table_atomic_rad.jpg
http://nanotech.sc.mahidol.ac.th/genchem/bonding1/ie.jpg
http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/text
_images/CH08/FG08_06.JPG
http://upload.wikimedia.org/wikipedia/commons/0/0c/Gallium1_640x480.jpg
http://upload.wikimedia.org/wikipedia/commons/0/03/Fe%2C26.jpg
http://upload.wikimedia.org/wikipedia/commons/a/a0/Burning-sulfur.png
http://upload.wikimedia.org/wikipedia/commons/d/d3/Edelgase_in_Entladungsroehre
n.jpg
http://upload.wikimedia.org/wikipedia/commons/f/f5/Halogene.jpg
http://upload.wikimedia.org/wikipedia/en/thumb/e/e9/SiliconCroda.jpg/800pxSiliconCroda.jpg
http://upload.wikimedia.org/wikipedia/commons/5/5e/Germanium.jpg
http://upload.wikimedia.org/wikipedia/commons/4/41/Schattenkreuzr%C3%B6hrein_use-lateral_view-standing_cross.jpg