chapter 7: ionic and metallic bonding chapter 9: naming compounds and writing formulas
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Chapter 7: Ionic and Metallic BondingChapter 9: Naming Compounds and
Writing Formulas
Electron Configuration Exceptions P. 136
Cr – [Ar] 4s2 3d4 - does not occur
Cr – [Ar] 4s1 3d5 – occurs
Why? • Greater stability is achieved with half filled
3d5 orbitals.
Another example:
Cu – [Ar] 4s2 3d9 - does not occur
Cu – [Ar] 4s1 3d10 – occurs
Why? • Greater stability is achieved with
completely filled 3d10 orbitals.
Other Exceptions that follow this pattern:
Ag, Au
P. 208 - Q - 58 and 59
Valence Electrons Dictate Chemical Properties
• Representative Elements – look at the Group #
• Symbolically represented by Electron Dot Structures
P. 193 - #8
Remember Stability
• Octet Rule – atoms want to obtain a noble gas electron configuration
• ns2 np6
• Metals – lose electrons to gain the octet of the next lowest energy level– Cations
• Non-Metals – gain electrons to obtain a complete octet– Anions
Cation Formation
K 1s2 2s2 2p6 3s2 3p6 4s1 reactive
Metals – lose electrons to gain the octet of the next lowest energy level
K 1s2 2s2 2p6 3s2 3p6 unreactive
K K+1 + e-
Cations – lose electrons
Transition Metals: Pseudo Noble Gas Configurations
Ag - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 5s1
Options – lose 11 electrons or gain 7
Neither happens
Ag loses 1 electron to gain a pseudo noble gas configuration
Ag1+ - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10
Transition Metals – Why Multiple Charges?
Fe - 1s2 2s2 2p6 3s2 3p6 4s2 3d6
Can become Fe2+ or Fe3+
Fe2+ Fe3+
loses the 4s2 electron s loses the 4s2 electrons and one 3d electron
Creates 5 half filled 3d orbitals
Anion Formation
Cl 1s2 2s2 2p6 3s2 3p5 reactive
Non Metals – gain electrons to complete their octet
Cl1- 1s2 2s2 2p6 3s2 3p6 unreactive
Cl + e- Cl 1-
A Halide
Anions – end in -ide
• Gain electrons
Ionic Bonds form Ionic Compounds
• Electrostatic attraction of cations and anions
• Neutral compounds • Binary compounds – MgO, not CaSO4
Ionic Bonds
Ionic Bonds
P. 208 - Q - 66
Practice
• Show how the following form ionic compounds.– Electron configuration, orbital diagram and electron dot
diagrams
1. 3 Sodium atoms and one Nitrogen Atom2. 2 Lithium atoms and one Oxygen Atom3. 1 Strontium atom and 2 Fluorine Atoms
P. 196 - Q - 12 and 13
Ionic Compounds
• Chemical Formula – the type and number of atoms in smallest representative unit of a substance
• Formula unit – the lowest whole number ratio of ions in an “ionic compound”
Naming Ions
• Monatomic Ions – a single atom with a charge– Cations - K1+, Ca2+
– Anions – O2-, N3-
• Drop the ending and add –ide
• Polyatomic ions – charged ions containing more than one atom
Polyatomic Ions
• Most end in -ate or -ite• NO3
- Nitrate NO2- Nitrite
• SO42- Sulfate SO3
2- Sulfite
• more oxygen atoms - suffix –ate• fewer oxygen atoms - suffix -ite
Bonding Nomenclature – Naming Ionic Compounds and Binary Molecular Compounds
Are they a metal and a non-metal or a metal and a polyatomic ion?
Are they 2 non-metals?
Does the cation have one oxidation number?
Does the cation have multiple
oxidation numbers?
State the name of the cation.
State the name of the anion. Drop the ending and add –ide. Do not change if it is a
polyatomic ion.
State the name of the cation.
State the name of the anion. Drop the ending and add –ide. Do not change if it is a
polyatomic ion.
State the oxidation number of the cation in Roman
numerals. Use the anion to determine the charge.
State the name of the 1st element.
State the name of the 2nd element. Drop the ending and
add –ide.
Add prefixes to identify the number of each element
1 – mono* 6 – hexa2 – di 7- hepta3 – tri 8 - octa4 – tetra 9 - nona5- penta 10- deca
* used only on the 2nd element
Ionic Compound Binary Molecular Compound
Ex. Na1+ Ex. Fe2+ or Fe3+
Ex. Sodium Ex. Iron
Ex. Sodium Bromide Ex. Sulfate
Ex. Iron (III) Sulfate Ex. Dicarbon Hexafluoride
Fe ( ) SO42-
Fe ( ) SO42-
SO42-
Fe must be 3+ because there are 2 Fe ions and the sulfate ions have a 6- charge.
NaBr, Fe2(SO4)3, C2H6
Bonding Nomenclature – Writing Formulas for Ionic Compounds and Binary Molecular Compounds
Are they a metal and a non-metal or a metal and a polyatomic ion?
Are they 2 non-metals?
Write the symbol of the cation and the anion.
Assign charges to each. Remember that roman numerals apply to the cation.
Are they balanced? Rewrite the symbols without the charges.
Rewrite the symbols and symplify the crossed charges. Do not write
the crossed charge if it was a 1.
Write the symbol of each element.
Each prefix identifies the quantity of each element.
Write the number as a subscript for each
corresponding prefix.
1 – mono* 6 – hexa2 – di 7- hepta3 – tri 8 - octa4 – tetra 9 - nona5- penta 10- deca
* used only on the 2nd element
Ionic Compound Binary Molecular Compound
No
Cross the charges.
yes
Properties of Ionic Compounds
• Depend on attraction of bonded elements• Na and Cl
– + surrounded by –– - surrounded by +
• Forms a crystal lattice– Size and number of ions
determine the shape
Properties - continued
• Melting and boiling points and hardness– Depend on attraction of ions– Greater attraction = ↑MP, BP and hardness
Mg 2+ O2-
Greater attraction
Continued
• Non conductor of electricity– Ions are static
• Conduct electricity when in water or melted– Ions free to move– Called electrolytes when dissolved in water
Exothermic nature
• Ionic compounds release energy upon formation because they are becoming more stable
Does the size of the ion influence the lattice energy?
Does the charge of the ion influence the lattice energy?
Lattice Energy - energy needed to separate one mole of ions
Lattice energy
• energy needed to separate one mole of ions – Depends on size of ions– Smaller the ion the greater the attraction
– Proximity to the nucleus
– Depends on the charge of the ion• Greater the charge the greater the attraction
P. 199 Q - 22
Metallic Bonds
Electron Sea Model
• Atoms outer energy levels overlap
• Electrons move freely from atom to atom (delocalized electrons, s and d electrons)
• Cations are formed
• Metallic bond forms when delocalized electrons are attracted to the metallic cations
P. 203 - Q - 23
Aufbau Diagram
Equal energies – 2 p
Sublevels have different energy levels
Energy levels overlap
Properties of Metals Explained
Mobile cations and electrons
• Moderate melting pts. extreme boiling pts.
• malleable and ductile
Strong Attraction for each other• durabilityMobile electrons• good conductors of heat and electricity Interaction with photons of light• lusterAmount of delocalized electrons• ↑electrons ↑strength and hardness• s block weak, d block hard
P. 203 – 26, 27 - P. 207 - Q – 46, 47, 48, 51
Alloys – mixture of 2 or more elements that have metallic properties superior to their parent element
Types of Alloys – Tech and Society (Page 204-205)
• Substitutional – similar size elements are substituted with one another– Stainless steel, pewter, gold
• Interstitial – extremely small atoms fill in the holes between much larger atoms
• Properties become more desirable– Carbon-steel – much harder, stronger, less ductile
than iron alone, corrosion resistant
P. 203 - Q - 25