mastering chemistry
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Mastering Chemistry. Registration and Log In Course ID: MCWICKUN89304. Basic Concepts of Chemical Bonding. Chapter 8. What’s Ahead (p 297). Three types of bonds Lewis symbols Ionic bonding Octet rule Lattice energy in ionic compounds. Three Types of Chemical Bonds. Ionic bond - PowerPoint PPT PresentationTRANSCRIPT
Mastering ChemistryMastering Chemistry
• Registration and Log InRegistration and Log In
• Course ID:Course ID:
• MCWICKUN89304MCWICKUN89304
Basic Concepts Basic Concepts of Chemical of Chemical
BondingBonding
Chapter 8Chapter 8
What’s Ahead (p 297)What’s Ahead (p 297)
• Three types of bonds
• Lewis symbols
• Ionic bonding
• Octet rule
• Lattice energy in ionic compounds
Three Types of Chemical BondsThree Types of Chemical Bonds
• Ionic bondIonic bond– Transfer of electronsTransfer of electrons– Between metal and nonmetal ionsBetween metal and nonmetal ions
• Covalent bondCovalent bond– Sharing of pairs of electronsSharing of pairs of electrons– Between nonmetal atomsBetween nonmetal atoms
• Metallic bondMetallic bond– Bonding electrons relatively free Bonding electrons relatively free
to moveto move
Valence electrons: outer shell electrons of an atom; valence electrons participate in chemical bonding.
1A 1ns1
2A 2ns2
3A 3ns2np1
4A 4ns2np2
5A 5ns2np3
6A 6ns2np4
7A 7ns2np5
Group # of valence e-e- configuration
Table 8.1
Show only valence electrons!
Ionic Bonding
Na (s) + ½ Cl2 (g) → NaCl (s) ΔHfo = −410.9 kJ
The Crystal Structure of Sodium Chloride
Fig 8.3
Li + F Li+ F -The Ionic Bond
1s22s11s22s22p5 1s21s22s22p6[He][Ne]
Li Li+ + e-
e- + F F -
F -Li+ + Li+ F -LiF(s)
Octet Rule: Atoms tend togain, lose, or share electronsuntil surrounded by 8 valenceelectrons
Lattice energy (E):
• increases as Q increases and/or
• increases as d decreases
Electrostatic (Lattice) Energy
Eel = k Q+Q-d
Q+ is the charge on the cation
Q- is the charge on the aniond is the distance between the ions
Lattice energy (E): the energy required to completely separate one mole of a solid ionic compound into gaseous ions
Eqn. [8.4]
Metal atoms lose electrons so that cation has a noble-gas outer electron configuration
Nonmetal atoms gain electrons so that anion has a noble-gas outer electron configuration
Electron Configurations of Cations and Anions
of Representative Elements
+1 +2 +3 -1-2-3
Cations and Anions Of Representative Elements
Electron Configurations of Cations of Transition Metals
When a cation is formed from an atom of a transition metal, electrons are always removed first from the ns orbital and then from the (n – 1)d orbitals.
Fe: [Ar]4s23d6
Fe2+: [Ar]4s03d6 or [Ar]3d6
Fe3+: [Ar]4s03d5 or [Ar]3d5
Mn: [Ar]4s23d5
Mn2+: [Ar]4s03d5 or [Ar]3d5
“First in, first out”
Three Types of Chemical BondsThree Types of Chemical Bonds
• Ionic bondIonic bond– Transfer of electronsTransfer of electrons– Between metal and nonmetal ionsBetween metal and nonmetal ions
• Metallic bondMetallic bond
– Bonding electrons relatively free to Bonding electrons relatively free to movemove
• Covalent bondCovalent bond– Sharing of electronsSharing of electrons– Between nonmetal atomsBetween nonmetal atoms
Metallic Crystals• Lattice points occupied by metal atoms• Held together by metallic bonds• Soft to hard, low to high melting point• Good conductors of heat and electricity
Cross Section of a Metallic Crystal
nucleus &core e-
mobile “sea”of valence e-
Electron-Sea Model
Covalent BondingCovalent Bonding• Objectives:Objectives:
– Characteristic propertiesCharacteristic properties
– Lewis structuresLewis structures
– Multiple bondsMultiple bonds
– Bond polarity and electronegativityBond polarity and electronegativity
• Atoms share pairs of electrons
• Several electrostatic interactions in these bonds:
Attractions between electrons and nuclei
Repulsions between electrons
Repulsions between nuclei
Covalent Bonding
Change in electron density as two hydrogen
atoms approach each other
Covalent Bond
Why should two atoms share electrons?
F F+
7e- 7e-
F F
8e- 8e-
F F
F F
Lewis structure of F2
lone pairslone pairs
lone pairslone pairs
single covalent bond
single covalent bond
H HO+ + OH H O HHor
Lewis structure of water
Double bond – two atoms share two pairs of electrons
single covalent bonds
O C O or O C O
double bonds
Triple bond – two atoms share three pairs of electrons
N N N N
triple bond
or