chemical bond science 9. discussion quarter 3

CHEMICAL BONDING

1. Formation of an Ionic Bond an Covalent Bond

2. Chemical bonding Is the process of linking or joining together of atoms to gain stability and to form a compound molecules Chemical bond Is a force of attraction that holds atoms together in compound or molecules

3. Types of Chemical Bonds Ionic Bonding - When atoms of one element give their electrons to atoms of another element so that both can have a full outer shell, this is called an ionic bond . Covalent Bonding - Electrons are always shared between two atoms in pairs. Neither atom loses or gains an electron during this type of bonding. Instead, they share their electrons so that their outer shells are full. 

4. Types of Chemical Bonds Ionic Bonding - When atoms of one element give their electrons to atoms of another element so that both can have a full outer shell, this is called an ionic bond . Covalent Bonding - Electrons are always shared between two atoms in pairs. Neither atom loses or gains an electron during this type of bonding. Instead, they share their electrons so that their outer shells are full. 

5. Forming an I onic Bond There is a total or net transfer of electron or electrons from a very reactive metal to a very reactive nonmetal.

6. Metals contain loosely held electrons that can be easily dislodges, which means these electron are easily removed from metals , like sodium atom. -electron Na Na Chlorine atom on the other hand is capable of accepting electrons and accommodate it on its shell. + electron CI CI

7. Properties and Characteristics of Ionic Bonds Involves the transfer of electrons from one atom to another Formed between a metal and nonmetal with sharp electronegativity difference so that the nonmetal can attract the electrons from the metal The attraction between the nuclei and electrons is electrostatic with charge separation. They are the most reactive of all the bonds in the appropriate medium. Strength is directly proportional to the quantity of the charges and inversely proportional to the distance between the charged ions. Ionic compounds have high melting and boiling points. The atoms are held together in a lattice structure, and much energy is needed to melt the compounds .

8. Examples of Ionic Bonds Sodium Chloride ( NaCl ) Sodium (Na) has a valency of one. It has only one electron in its outermost (valence) shell.  Chlorine  has seven electrons in its outermost shell and requires one electron to complete the shell. 2. Magnesium Oxide ( MgO ) Magnesium (Mg) has two electrons in its outermost shell, and oxygen (O) has six. Magnesium will donate the two electrons to achieve its nearest inert gas configuration, i.e., neon. As a result, magnesium will become a magnesium ion (Mg2+).  Oxygen  (O) is more electronegative than magnesium . It requires two electrons to complete its outermost shell and achieve its nearest inert gas configuration, neon.

9. Examples of Ionic Bonds 3. Calcium Chloride (CaCl 2 ) Calcium ( Ca ) has two valence electrons, and chlorine ( Cl ) has seven. The former will give off its two electrons to form a calcium ion ( Ca + ). Chlorine is more electronegative than calcium will attract those electrons . Hence, two chlorine atoms will combine with calcium 4. Potassium Oxide (K 2 O) Potassium (K) has one electron in its outermost shell. Oxygen (O) has six electrons in its outermost shell and requires two to complete the shell. It is more electronegative than potassium, and so it will attract two electrons from two potassium atoms forming an oxide ion (O – ). 

10. Examples of Ionic Bonds