DP SL CHEMISTRY STANDARD 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 BONDING BOND- 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 ELECTRONS COVALENT- USUALLY INVOLVES NONMETALS WITH NONMETALS OR NONMETALS WITH METALLOIDS -INVOLVES A SHARING OF ELECTRONS METALLIC- 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 ELECTRON GROUP 2 METALS GIVE UP TWO ELECTRONS GROUP 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 electrons LG (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 Fe 2+ & Fe 3+ IONS COPPER CAN FORM Cu + & Cu 2+ 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 Solids LG (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, SiO 2, 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 CARBON LG (i) Describe and compare the structure and bonding in the three allotropes of Carbon