IONIC BONDING

• Chemical Bond formed between 2 oppositely charged ions by the transfer of electrons.
• Involves a metal and a non metal element
• The farther two elements are across the periodic table; the more likely they are to form an ionic compound

Sodium  (on the left) loses its one valence electron to chlorine who has 7 valence electrons (on the right),

The Result is.. 

 A positively charged sodium ion (left) and a negatively charged chlorine ion (right).

NOTE: Chlorine became negatively charged because it gained an electron which has a negative charge. And Sodium became postively charged because it has more protons+ than electrons-

ILLUSTRATION

USING LEWIS ELECTRON DOT SYSTEM

Element Pair

             Lithium has 2 valence electrons .

Chlorine has 7 valence electrons 

 

Electron Transfer

Lewis Structure

The Ionic Compound

Covalent Bonding

• 
  
  Sharing of one or more pairs of electrons between atoms, in order to produce a mutual attraction
  
  
• 
  
        Covalent bonding occurs because the atoms in the compound have a similar tendency for electrons (generally to gain electrons).
  
  
• 
  
        This most commonly occurs when two nonmetals bond together. Because both of the nonmetals will want to gain electrons, the elements involved will share electrons in an effort to fill their valence shells
  
  
• 
  
  
  
        Neither atom completely loses or gains electrons as in ionic bonding

There are two types of covalent bonding:

1. Non-polar bonding

2. Polar bonding

Nonpolar Covalent Bonding

• 
  
  A nonpolar covalent bond is formed when an element has an equal attraction or affinity for electrons
• 
  
  It is also formed whenever two atoms of the same element bond together.
• 
  
  The H2 molecule is a good example of the first type of covalent bond, the non-polar bond. 

Polar Covalent Bonding

• 
  
  When electrons are unequally shared between two atoms, a polar covalent bond is formed
• 
  
  it also occurs when one atom has a stronger affinity for electrons than the other.
• • A good example of a polar covalent bond is the hydrogen-oxygen bond in the water molecule.

• 
  
  

  

  
  
  
  
  
  
  IMPORTANT TERMS!!
  
  
  
  
  
  

        - Single covalent bond

  It is the sharing of a single pair of electron between bonded atoms. 

  
  
  

  -          Double covalent bond

  Shares 2 electron pairs

  
  
  

  -          Triple covalent bond

  Shares 3 electron pairs

  
  

  
  

  -          Bonding electrons

  Electrons shared between the 2 atoms

  
  
  

  -          Lone Pairs

  Valence electron pairs that are not involved in bonding

  
  

GROUP 8
CHUA
CORNELIO
DUMPIT 
CATAPANG
CARBONEL

ATOMIC RADIUS AND METALLIC PROPERTIES

ATOMIC RADIUS

Atomic Radius is basically how wide an atom is, therefore it increases across the periodic table. The more electrons the bigger the radius. The atomic radius of a chemical element is the measure of the size of its atom usually the distance from the nucleus. The atomic Radius is also called the covalent radius. It is half the distance between the two like atoms that are covalently bonded.

EXCERCISES!

get a piece of paper and your periodic table

1. What can you observe (in the atomic radius) when you look at one period ?
2. How about the metallic properties?
3. Arrange the different sets of elements by its atomic radius (increasing)

-Br,Ar, Mo, Na
-Re,Ne,Li,N
-Po,Ag, Be, I
-He, Y ,S,O,
4.Arrange the different sets of elements by its metallic properties (increasing)
-Be,H, B,I
-H, O,Ni, Lu
-Ti, Fr, Si,C
-K,Kr,Ru,Au

METALLIC PROPERTIES AND ATOMIC RADIUS!

METALLIC PROPERTIES

ATOMIC RADIUS

REFERENCES ! 

http://www.chemicalelements.com/groups/nonmetals.html

http://www.sciencebyjones.com/periodic_table1.htm

http://www.tutorvista.com/content/science/science-ii/metals-non-metals/physical-properties-metals-non-metals.php

http://www.chem.lsu.edu/lucid/tutorials/Periodic_Table.html

https://chemistry.twu.edu/tutorial/PerTabSum.html

http://www.drsobhe.com/herostudents/metals_s_sc.html

http://www.saskschools.ca/curr_content/chem20/metals/chemprop.html

MADE BY:

Marquez

Lacanilao

Lagaya

Manacsa

Legazpi

Bonding and LEDS

L.E.D.S: Lewis Dot Structure


Facts:
a.k.a Lewis Dot Diagrams, Electron Dot Diagram and Electron Dot Structures
Shows the bonding between atoms and electrons
named after Gilbert Newton Lewis


How To Do It

• Determine the Valence Electrons

Something like this...

Red dots are the valence electrons.

• Electrons must be placed into the structure.

Something like this...

* Always follow the Octet Rule: atoms combined in such way the have 8 electrons giving them the same number of electrons as a noble gas.

• Bonding pair is shared between two atoms. Transferring of electrons.

Something like this...

Multiple Bondings

Facts:

used when in need of more electrons from one element

Just like this...

The electrons of Magnesium was transferred to th two chlorine's.

Results:

Lets try some exercises

Members:

Mendoza

Monsalud

Pacunayen

Pagkalinawan

Ponce

II-5

Group1: Modern Periodic Table

MODERN PERIODIC TABLE

     In 1869 Russian chemist Dimitri Mendeleev started the development of the periodic table, arranging chemical elements by atomic mass.

He predicted the discovery of other elements, and left spaces open in his periodic table for them.

        

     Dmitri Mendeleev, a Siberian-born Russian chemist, was the first scientist to make a periodic table much like the one we use today. Mendeleev arranged the elements in a table ordered by atomic weight, corresponding to relative molar mass as defined today.

·              Before 1800 (36 elements): discoveries during and before the 

          Enlightenment.

·              1800-1849 (+22 elements): impulse from scientific (empirical processes

          systematization and modern atomic theory) and industrial revolutions.

·              1850-1899 (+23 elements): the age of classifying elements received an 

           impulse from the spectrum analysis. Boisbaudran, Bunsen, Crookes, 

           Kirchhoff, and others "hunting emission line signatures".

·              1900-1949 (+13 elements): impulse from the old quantum theory, the

          consolidated periodic table, and quantum mechanics.

·              1950-1999 (+15 elements): "atomic bomb" and Particle physics issues, for 

          atomic numbers 97 and above.

 

PERIODS: 

     It tells about how many energy level an atom has.

Horizontal rows of the periodic table.

GROUPS/FAMILIES: Vertical columns of the periodic table.

Group- last electron configuration

Family- states the common properties

**the elements in any group of the periodic table have physical and chemical properties. **

Today's Periodic Table

     The most important difference between Mendeleev's table and today's table is the modern table is organized by increasing atomic number, not increasing atomic weight. Why was the table changed? In 1914, Henry Moseley learned you could experimentally determine the atomic numbers of elements. Before that, atomic numbers were just the order of elements based on increasing atomic weight. Once atomic numbers had significance, the periodic table was reorganized.

 Group1:

Dianne Ang

Androse Ansaldo

Micah Antonio

Oya Bautista

Angela Cansana

source:  http://chemistry.about.com/library/blperiodictable.htm

             http://www.aip.org/history/curie/periodic.htm