DP SL CHEMISTRYSTANDARD C

• STANDARD C: (CHAPTER 4) TYPES OF BONDING: Comparing and contrasting ionic, covalent and metallic bonding. Identifying the properties associated with each type of bond.

• LG (a) Describe an ionic bond between atoms.• LG (b) Deduce which type of ions form when Groups 1,2,3 elements lose electrons• LG (c) Deduce which type of ions form when Groups 5,6,7 elements gain electrons• LG (d) State that transition metals can form more than one type of ion• LG (e) Describe the lattice structure of ionic compounds• LG (f) Predict whether a compound made up of two elements would be ionic based on the

location of the elements on the periodic table• LG (g) Describe a covalent bond between atoms• LG (h) Predict whether a compound made up of two elements would be covalent based on

the location of the elements on the periodic table.• LG (i) Describe and compare the structure and bonding in the three allotropes of carbon• LG (j) Describe the structure and bonding in silicon and silicon dioxide• LG (k) Describe a metallic bond• LG(l) Compare and explain the properties of substances resulting from the different types of

bonds

CHAPTER 4 BONDINGBOND- WHEN TWO OR MORE ATOMS CHEMICALLY COMBINE TO FORM A

COMPOUND. -ATOMS COMBINE IN ORDER TO BECOME MORE STABLE(ACHIEVE A

NOBLE GAS CONFIGURATION) AND LOWER THEIR POTENTIAL ENERGY.

TYPES OF BONDS:IONIC-ELECTROSTATIC ATTRACTION BETWEEN CATIONS AND ANIONS

-INVOLVES A TRANSFER OF ELECTRONSCOVALENT- USUALLY INVOLVES NONMETALS WITH NONMETALS OR NONMETALS WITH METALLOIDS

-INVOLVES A SHARING OF ELECTRONSMETALLIC- HOW METALS ATOMS ARE HELD TOGETHER.

-ELECTRONS BECOME DELOCALIZED AND ARE FREE TO MOVE THROUGHOUT THE ENTIRE METAL AS A “SEA OF ELECTRONS.”

LG: (a) Describe an ionic bond between atoms.

LG (e) Describe the lattice structure of ionic compounds

THE FORCE OF ELECTROSTATIC ATTRACTION BETWEEN IONS IN A COMPOUND CAUSES THEM TO SURROUND THEMSELVES WITH IONS OF THE OPPOSITE CHARGE CREATING A 3-DIMENSIONAL CRYSTALLINE STRUCTURE KNOWN AS AN IONIC LATTICE

IONIC BONDING INVOLVES A TRANSFER OF ELECTRONS TO CREATE CATIONS AND ANIONS. IT IS THE ELECTROSTATIC ATTRACTION BETWEEN CATIONS AND ANIONS THAT CREATES THE IONIC BOND

CATIONS ARE CREATED WHEN METALS GIVE UP ELECTRONS .

GROUP 1 METALS GIVE UP ONE ELECTRONGROUP 2 METALS GIVE UP TWO

ELECTRONSGROUP 3 METALS GIVE UP THREE

ELECTRON

ANIONS ARE CREATED WHEN NONMETALS RECEIVE ELECTRONS

GROUP 5 NONMETALS RECEIVE THREE ELECTRONS

GROUP 6 NONMETALS RECEIVE TWO ELECTRONS

GROUP 7 NONMETALS RECEIVE ONE ELECTRON

LG (b) Deduce which type of ions form when Groups 1,2,3 elements lose electrons

LG (c) Deduce which type of ions form when Groups 5,6,7 elements gain electronsLG (d) State that transition metals can form more than one type of ion

TRANSITION METALS (d & f BLOCKS) CAN FORM MORE THAN ONE ION DUE TO THE FACT THAT THE s & d ORBITALS ARE SO CLOSE IN ENERGY. WE CALL THESE TYPE OF METALS MULTIVALENT.

FOR EXAMPLE:

IRON CAN FORM Fe2+ & Fe3+ IONSCOPPER CAN FORM Cu+ & Cu2+ IONS

WE WILL LEARN MORE MULTIVALENT METALS IN STANDARD E

LG (g) Describe a covalent bond between atoms

EXAMPLES OF COVALENT/MOLECULAR COMPOUNDS

THE DIFFERENCE IN ELECTRONEGATIVITY VALUES BETWEEN TWO ELEMENTS IS OFTEN USED TO DETERMINE IF A BOND IS IONIC OR COVALENT. ( REFER TO CHART ABOVE)

THE FURTHER APART TWO ELEMENTS ARE ON THE PERIODIC TABLE THE LARGER THE DIFFERENCE IN ELECTRONEGATIVITY VALUES.

LG (f) Predict whether a compound made up of two elements would be ionic based on the location of the elements on the periodic table.

LG (h) Predict whether a compound made up of two elements would be covalent based on the location of the elements on the periodic table.

LG (k) Describe a metallic bond

LG(l) Compare and explain the properties of substances resulting from the different types of bonds

Covalent Network SolidsLG (j) Describe the structure and bonding in silicon and silicon dioxide

These are giant molecular lattice structures. This implies that strong covalent bonding holds their atoms together in a highly regular extended network. The bonding between the atoms goes on and on in three dimensions.

The elements carbon, silicon and boron form covalent networks instead of covalent molecules.

Silicon dioxide, SiO2, also exists as a covalent network and is known as quartz. Its structure is similar to diamond.

Carbon’s allotropes (diamond, graphite and fullerenes ) exists as covalent network solids

Melting requires the separation of the species comprising the solid state, and boiling the separation of the species comprising the liquid state. Because of the large amount of energy needed to break huge numbers of covalent bonds, all giant covalent network structures have high melting points and boiling points and are insoluble in water.

DIAMOND

EACH CARBON IS TETRAHEDRALLY

BONDEDTO 4 OTHER CARBON ATOMS

GRAPHITE

EACH CARBON IS BONDED TO 3 OTHER CARBONS FROMING

HEXAGONS IN PARALLEL LAYERS

FULLERENE

EACH CARBON ATOM IS A SPHERE OF 60 CARBON ATOMS

CONSISTING OF 12 PENTAGONS AND 20

HEXAGONS. THE SPHERE IS A CLOSED

CAGE IN WHICH EACH CARBON IS BONDED

TO 3 OTHER CARBONS

3 ALLOTROPES OF CARBONLG (i) Describe and compare the structure and bonding in the three allotropes of Carbon