DP SL CHEMISTRY
STANDARD C
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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
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
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
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+ IONS
COPPER 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
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.
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 (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, 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.
3 ALLOTROPES OF CARBON
LG (i) Describe and compare the structure and bonding in the three
allotropes of Carbon
FULLERENE
DIAMOND
GRAPHITE
EACH CARBON IS
TETRAHEDRALLY
BONDEDTO 4 OTHER
CARBON ATOMS
EACH CARBON IS
BONDED TO 3 OTHER
CARBONS FROMING
HEXAGONS IN
PARALLEL LAYERS
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