CHEMICAL BONDS Ionic

Chapter 6

6.1 BONDING - journal

1.

Begin filling in the table on the top of the Bonding Basics – Ionic Bonding Worksheet.

6.1 BONDING

 Chemical PROPERTIES depend on the number of valence electrons.

6.1 BONDING

 Therefore, chemical bonding and reactivity depend on an element’s electron configuration.

6.1 BONDING

 STABLE ELECTRON CONFIGURATION: 

Which group does this describe?

6.1 BONDING

 What do elements with UNSTABLE ELECTRON CONFIGURATIONS do?

6.1 BONDING



They BOND and form compounds

 IONIC BONDING

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer 

Both Sodium and Chlorine are now STABLE in their highest energy levels

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer 

What types of elements are Sodium and Chlorine?

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal.

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal.



When an atom gains or loses electrons, what does it get?



A CHARGE.

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal 

ION: An atom with a positive or negative CHARGE from electron transfer.

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal 

In the bond, one becomes positive (loses electrons) and one becomes negative (gains electrons).

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal 

Positive Ion (loses electrons): Cation



Negative Ion (gains electrons): Anion

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal 

WHAT DO OPPOSITE CHARGES DO?

6.1 BONDING

 IONIC BONDING – the forming of a stable electron configuration through electron transfer between a metal and a nonmetal 

ATTRACT.



This is when the IONIC BOND forms.

6.1 BONDING



HOW can you predict which elements will make positive cations and which will make negative anions?

6.1 IONIC BONDING

 Ionization Energy: the ability to PULL ON ELECTRONS.

Look at “Data Analysis” at the top of page 160.



Which side has the MOST PULL?



Which side GIVES UP electrons more easily?

6.1 IONIC BONDING

 Ionization Energy: the ability to PULL ON ELECTRONS.

 

Take out your Periodic Table.

Predict the OXIDATION NUMBERS (charges) of the ions for A Groups

6.1 IONIC BONDING

4.

1.



PROPERTIES OF IONIC COMPOUNDS

Form between a metal and a nonmetal 3.

2.

Brittle/crystalline High melting/boiling points Dissolve (ions come apart) in water & conduct electricity

6.1 IONIC BONDING

 3.

1.

2.

NAMING IONIC COMPOUNDS

NaCl – Sodium Chloride HF – Hydrogen Fluoride MgI 2 – Magnesium Iodide 4.

KBr - ???

Potassium Bromide This is Binary Nomenclature Ionic Bonding Challenge

IONIC BONDING



POLYATOMIC IONS

Sometimes groups of atoms can have a positive or negative charge.

COMMON POLYATOMIC IONS 1.

3.

2.

NH 4 + – Ammonium NO 3 – Nitrate OH 1 - Hydroxide 4.

6.

5.

CO 3 2 – Carbonate SO 4 2 - Sulfate PO 4 2 - Phosphate

6.1 IONIC BONDING

1.

2.

3.

4.



NAMING COMPOUNDS WITH POLYATOMIC IONS

CaCO 3

1.

Calcium carbonate

HNO 3

1.

Hydrogen nitrate (nitric acid)

NH 4 Cl

1.

Ammonium chloride

NaOH

1.

Sodium hydroxide

6.1 IONIC BONDING

6.1 IONIC BONDING – Journal 2

 Ionization Energy: the ability to PULL ON ELECTRONS.



FOLLOW THE DIRECTIONS AT THE TOP OF THE BLANK PERIODIC TABLE FROM THE BACK OF THE ROOM.

6.1 BONDING – Journal 2

 Define ionic bond  Define ionization energy  Take out your Ionic Bonding basics worksheet and make sure you have a Lewis Dot for each element on the page, front and back  Begin filling out the Covalent Bonding Basics Table