Grade 10 - Chemistry - LO.5 - Types of bonds

 

We have in LO.5 Chemistry G10

First: the Concepts

Chemical bond.

Ionic and Covalent bond.

Electron dot diagram.

Nomenclature of alkanes (IUPAC common name).

Isomers of alkanes.

Cis and Trans.

Structure Isomers and Chains

Second: the References

Zumdahl: ch.8 sec.1,2,3,4,10,11

                   ch. 22 sec.1     

Third: the Videos links

Fourth: Skills

Correlate electron configuration with ionization energies and chemical properties 

Determine valence numbers from electron configuration 

Compare organization of the periodic table according to valence numbers with physical and chemical properties and predict formulas for binary compounds .

Contrast ionic bonding and covalent bonding .

Draw electron-dot diagrams for simple molecules with covalent bonding and ionic bonding . 

Student can compare between organic and inorganic substance.

Detect practically C and H in organic substance .

Distinguish between molecular, structural and empirical formula . 

Draw formulas for isomers of a compound. (structure chain, cis and trans). 

Name simple alkanes according to IUPAC nomenclature rules

Fifth: the materials as PPT., DOCX., and PDF

In the Drive from this link

Few Notes:

How to Draw a Lewis Structure

-Step 1:  Find the Total Number of Valence Electrons 

In this step, add up the total number of valence electrons from all the atoms in the molecule

-Step 2:  Find the Number of Electrons Needed to Make the Atoms "Happy“

An atom is considered "happy" when its outer electron shell is filled. Elements up to period four on the periodic table need eight electrons to fill their outer electron shell. This property is often known as the "octet rule".

-Step 3: Determine the Number of Bonds in the Molecule

Covalent bonds are formed when one electron from each atom forms an electron pair. Step 2 tells how many electrons are needed and Step 1 is how many electrons you have. Subtracting the number in Step 1 from the number in Step 2 gives you the number of electrons needed to complete the octets. Each bond formed requires two electrons, so the number of bonds is half the number of electrons needed or (Step 2 - Step 1)/2

-Step 4:  Choose a Central Atom

The central atom of a molecule is usually the least electronegative atom or the atom with the highest valence. To find electronegativity, either rely on periodic table trends or consult a table that lists electronegativity values. Electronegativity decreases moving down a group on the periodic table and increases moving from left to right across a period. Hydrogen and halogen atoms tend to appear on the outside of the molecule and are rarely the central atom

-Step 5: Draw a Skeletal Structure

Connect the atoms to the central atom with a straight line representing a bond between the two atoms. The central atom can have up to four other atoms connected to it.

-Step 6: Place Electrons Around Outside Atoms

Complete the octets around each of the outer atoms. If there are not enough electrons to complete the octets, the skeletal structure from Step 5 is incorrect. Try a different arrangement. Initially, this may require some trial and error. As you gain experience, it will become easier to predict skeletal structures.

-Step 7: Place Remaining Electrons Around the Central Atom

Complete the octet for the central atom with the remaining electrons. If there are any bonds left over from Step 3, create double bonds with lone pairs on outside atoms. A double bond is represented by two solid lines drawn between a pair of atoms. If there are more than eight electrons on the central atom and the atom is not one of the exceptions to the octet rule, the number of valence atoms in Step 1 may have been counted incorrectly. This will complete the Lewis dot structure for the molecule.

Chemical bond

TYPES OF CHEMICAL BONDING 

-Ionic Bonding - two atoms of opposite charge electrically attracted to one another

-Covalent Bonding - two atoms each sharing electrons within a molecular orbital 

-Metallic Bonding - positive metal ions held together in a lattice with a “sea of electrons”

 An actual chemical bond is a blend of all three types of bonding. Most often, one type is dominant over others. We will concentrate on ionic and covalent bonding. 

Ionic vs Covalent Bonding

IONIC

electron(s) leave one atom & gained by another atom to satisfy both atoms’ octets, this results in the formation of ions. The resulting opposite charges attracts each other.

COVALENT

Electrons are shared by two or more atoms to satisfy their octets.

LEWIS STRUCTURES 

Only valence electrons are important in bonding.

-Lewis dot structures show valence electrons surrounding atom. 

-We visualize the four valence orbitals of an atom as the sides of a box. Electrons are put into orbitals according to Hund’s rule

IONIC BONDING 

Oppositely charged ions attract each other.

Metal atoms lose e- and nonmetal atoms gain e- .

Ions attract each other to form ionic lattice. 

COVALENT BONDING 

-Atoms that are bonded “share” valence electrons. 

-Sharing is what creates covalent bond. 

-When atoms bond covalently, new entity termed molecule is formed. 

-Nuclei are bound together by their mutual attraction toward the shared electrons. 

-Bonding in Diatomic Molecules 

-Hydrogen 

Polar covalent

the electrons are shared, but one atom is pulling on the electrons a lot more. The electrons spend more time around that atom. 

Nonpolar covalent

the electrons are evenly shared between the two atoms.

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