Bonding Ionic Bonding & Metallic Bonding Keeping Track of Electrons l The electrons responsible for the chemical properties of atoms are those in the.

Bonding

Ionic Bonding

&

Metallic Bonding

Keeping Track of Electrons The electrons responsible for the

chemical properties of atoms are those in the outer energy level.

Valence electrons - The s and p electrons in the outer energy level.

Core (kernel)electrons -those in the energy levels below.

Keeping Track of Electrons Atoms in the same column Have the same outer electron

configuration. Have the same valence electrons. Easily found by looking up the group

number on the periodic table. Group 2A - Be, Mg, Ca, etc.- 2 valence electrons

Electron Dot diagrams A way of keeping track of

valence electrons. How to write them Write the symbol. Put one dot for each

valence electron Don’t pair up until they

have to

X

The Electron Dot diagram for Nitrogen

Nitrogen has 5 valence electrons.

First we write the symbol.

NThen add 1 electron at a time to each side.

Write the electron dot diagram for

Na Mg C O F Ne He

Electron Configurations for Cations

Metals lose electrons to attain noble gas configuration.

They make positive ions. (Cations) If we look at electron configuration it

makes sense. Na 1s22s22p63s1 - 1 valence electron Na+ 1s22s22p6 -noble gas configuration

Electron Dots For Cations Metals will have few valence electrons

Ca

Electron Dots For Cations Metals will have few valence electrons These will come off

Ca

Electron Dots For Cations Metals will have few valence electrons These will come off Forming positive ions

Ca+2

Electron Configurations for Anions

Nonmetals gain electrons to attain noble gas configuration.

They make negative ions. (Anions) If we look at electron configuration it

makes sense. S 1s22s22p63s23p4 - 6 valence electrons S-2 1s22s22p63s23p6 -noble gas

configuration.

Electron Dots For Anions Nonmetals will have many

valence .electrons. They will gain electrons to fill outer shell.

P P-3

Stable Electron Configurations All atoms react to achieve noble gas

configuration. Noble gases have 2 s and 6 p electrons. 8 valence electrons . Also called the octet rule.

Ar

Ionic Bonding Anions and cations are held together by

opposite charges. (metal and non-metal)

Ionic compounds are called salts. Simplest ratio is called the formula unit. The bond is formed through the transfer

of electrons. Electrons are transferred to achieve

noble gas configuration. Atoms are generally far apart on table EN difference of 1.7 or greater.

Ionic Bonding

Na Cl

Ionic Bonding

Na+ Cl-

Ionic Bonding All the electrons must be accounted for!

Ca P

Ionic Bonding

Ca P

Ionic Bonding

Ca+2 P

Ionic Bonding

Ca+2 P

Ca

Ionic Bonding

Ca+2 P-3

Ca

Ionic Bonding

Ca+2 P-3

Ca P

Ionic Bonding

Ca+2 P-3

Ca+2 P

Ionic Bonding

Ca+2 P-3

Ca+2 P

Ca

Ionic Bonding

Ca+2 P-3

Ca+2 P

Ca

Ionic Bonding

Ca+2 P-3

Ca+2P

-3

Ca+2

Ionic Bonding

Ca3P2

Formula Unit

Writing Ionic FormulasCriss Cross Method

Ca +2 P -323

Ca3 P2

Ca3P2

Properties of Ionic Compounds Crystalline structure. A regular repeating arrangement of ions

in the solid. Ions are strongly bonded. Structure is rigid. High melting points- because of strong

forces between ions.

Crystalline structure

Ionic solids are brittle

+ - + -+- +-

+ - + -+- +-

Ionic solids are brittle

+ - + -

+- +-+ - + -

+- +-

Strong Repulsion breaks crystal apart.

Reactions of Metals Lose electrons Become positive ions (Cations) Have smaller radii Acquire the noble gas configuration

Reactions of Non-Metals Gain electrons Become negative ions (Anions) Have larger radii Acquire the noble gas configuration

Do they Conduct? Conducting electricity is allowing charges to move. Solids:

– the ions are locked in place.

– (NaCls) so NO conductivity.

– Ionic solids are insulators. When melted,(NaCll ) the ions can move around. So

YES conductivity.– Ionic solids have high melting points. (800ºC) – Melted means molten

Dissolved in water(NaClaq) YES conductivity.

Metallic Bonds Metal bonded to more metal. (Ag, Au,

Sn, etc. all have metallic bonds.) How atoms are held together in the

metallic solid. Metals hold onto their valence electrons

very weakly. Think of them as positive ions floating in

a sea of electrons.

Sea of Electrons

+ + + ++ + + +

+ + + +

Electrons are free to move through the solid.

Metals conduct electricity and heat.

Metals are Malleable Hammered into shape (bend). Ductile - drawn into wires.

Malleable

+ + + ++ + + +

+ + + +

Malleable

+ + + +

+ + + ++ + + +

Electrons allow atoms to slide by.

Ductile

+ + + +

+ + + ++ + + +

Electrons can be drawn into a thin wire.

Energy Changes in Bond Formation Chemical Bonds are forces that hold

atoms together. Energy is required to overcome these

attractive forces and separate the atoms in a compound.

Breaking a bond Endothermic – Energy on left side of rxn AB + 100J A + B

Making a bond Exothermic– Energy on right side of rxn A + B AB + 100J

Energy and Stability The greater the amount of energy

released in forming the bond the greater its stability.

B + C BC + 100 joules K + L KL + 400 joules

(more stable)