The Ties That Bind
-
Upload
nicole-cochran -
Category
Documents
-
view
29 -
download
4
description
Transcript of The Ties That Bind
The Ties That Bind
Chemical Bonding and Interactions
Chemical Bonding and Interactions1. Stable Electron Configurations2. Electron-Dot (Lewis) Structures
1. Drawing, Rules for Drawing2. The Octet Rule3. Some Exceptions to the Rule
3. Ionic Bonding1. Naming ionic compounds2. Drawing
4. Covalent Bonding1. Naming covalent compounds2. Drawing3. Electronegativity and Polar Covalent Compounds
5. Molecular Shapes and the VSEPR Theory6. Intermolecular Forces of Attraction
1. H-bonds, Dipole-Dipole, Ion-Dipole, London Dispersion Forces
It’s all about stability…
1. Fact: Noble gases are inert (undergo few, if any, chemical reactions)
2. Theory: The inertness of these gases is a result of their electronic structure
3. If elements could alter their electron structures like those of the noble gases, they would be less reactive.
Electron Configurations of Cations and Anions
Na [Ne]3s1 Na+ [Ne]
Ca [Ar]4s2 Ca2+ [Ar]
Al [Ne]3s23p1 Al3+ [Ne]
Atoms lose electrons so that cation has a noble-gas outer electron configuration.
H 1s1 H- 1s2 or [He]
F 1s22s22p5 F- 1s22s22p6 or [Ne]
O 1s22s22p4 O2- 1s22s22p6 or [Ne]
N 1s22s22p3 N3- 1s22s22p6 or [Ne]
Atoms gain electrons so that anion has a noble-gas outer electron configuration.
Of Representative Elements
+1
+2
+3 -1-2-3
Cations and Anions Of Representative Elements
Na+: [Ne] Al3+: [Ne] F-: 1s22s22p6 or [Ne]
O2-: 1s22s22p6 or [Ne] N3-: 1s22s22p6 or [Ne]
Na+, Al3+, F-, O2-, and N3- are all isoelectronic with Ne
What neutral atom is isoelectronic with H- ?
H-: 1s2 same electron configuration as He
9.1
Valence electrons are the outer shell electrons of an atom. The valence electrons are the electrons thatparticipate in chemical bonding.
1A 1ns1
2A 2ns2
3A 3ns2np1
4A 4ns2np2
5A 5ns2np3
6A 6ns2np4
7A 7ns2np5
Group # of valence e-e- configuration
(Electron Dot Structures)
*We generally place the electrons one four sides of a square around the element symbol.*Octet rule: we know that s2p6 is a noble gas configuration. We assume that an atom is stable when surrounded by 8 electrons (4 electron pairs).
A violent bond: Sodium and Chlorine Sodium is a soft, reactive metal. Chlorine is a greenish-yellow gas which is
toxic (WWI poison) Sodium chloride is used for our food.
Ionic BondingIonic Bonding
Consider the reaction between sodium and chlorine:Na(s) + ½Cl2(g) NaCl(s)
Chemistry In Action:
Sodium Chloride
Mining Salt Solar Evaporation for Salt
9.2
Li + F Li+ F -
The Ionic Bond
1s22s11s22s22p5 1s21s22s22p6[He][Ne]
Li Li+ + e-
e- + F F -
F -Li+ + Li+ F -
IONIC BONDING-bonding due to
electrostatic attraction arising from an exchange of electrons.
ionic compounds consist of a combination of cations and an anions
• the formula is always the same as the empirical formula
• the sum of the charges on the cation(s) and anion(s) in each formula unit must equal zero
The ionic compound NaCl
2.6
Ionic BondingIonic Bonding
*NaCl forms a very regular structure in which each Na+ ion is surrounded by
6 Cl ions.
Similarly, each Cl ion is surrounded by six Na+ ions.
There is a regular arrangement of Na+ and Cl in 3D.
Note that the ions are packed as closely as possible.
Note that it is not easy to find a molecular formula to describe the ionic
lattice.
9.3
Lattice energy (E) increases as Q increases and/or
as r decreases.
cmpd lattice energyMgF2
MgO
LiF
LiCl
2957
3938
1036
853
Q= +2,-1
Q= +2,-2
r F < r Cl
SIDEBAR: Electrostatic (Lattice) Energy
E = kQ+Q-r
Q+ is the charge on the cation
Q- is the charge on the anionr is the distance between the ions
Lattice energy (E) is the energy required to completely separate one mole of a solid ionic compound into gaseous ions.
9.3
An ion is an atom, or group of atoms, that has a net positive or negative charge.
cation – ion with a positive chargeIf a neutral atom loses one or more electronsit becomes a cation.
anion – ion with a negative chargeIf a neutral atom gains one or more electronsit becomes an anion.
Na 11 protons11 electrons Na+ 11 protons
10 electrons
Cl 17 protons17 electrons Cl-
17 protons18 electrons
2.5
A monatomic ion contains only one atom
A polyatomic ion contains more than one atom
2.5
Na+, Cl-, Ca2+, O2-, Al3+, N3-
OH-, CN-, NH4+, NO3
-
Test Yourself:
1. MgO
2. MgBr2
3. The combination of the ion of magnesium and the ion of nitrogen
Formula of Ionic Compounds
Al2O3
2.6
2 x +3 = +6 3 x -2 = -6
Al3+ O2-
CaBr2
1 x +2 = +2 2 x -1 = -2
Ca2+ Br-
Na2CO3
1 x +2 = +2 1 x -2 = -2
Na+ CO32-
2.6
2.7
Chemical Nomenclature Ionic Compounds
often a metal + nonmetal anion (nonmetal), add “ide” to element name
BaCl2 barium chloride
K2O potassium oxide
Mg(OH)2 magnesium hydroxide
KNO3 potassium nitrate
2.7
Transition metal ionic compounds indicate charge on metal with Roman numerals
FeCl2 2 Cl- -2 so Fe is +2 iron(II) chloride
FeCl3 3 Cl- -3 so Fe is +3 iron(III) chloride
Cr2S3 3 S-2 -6 so Cr is +3 (6/2) chromium(III) sulfide
2.7
2.7
Covalent BondingCovalent Bonding
A covalent bond is a chemical bond in which two or more electrons are shared by two atoms.
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
9.4
8e-
H HO+ + OH H O HHor
2e- 2e-
Lewis structure of water
Double bond – two atoms share two pairs of electrons
single covalent bonds
O C O or O C O
8e- 8e-8e-double bonds double bonds
Triple bond – two atoms share three pairs of electrons
N N8e-8e-
N N
triple bondtriple bond
or
9.4
Bond Type
Bond Length
(pm)
C-C 154
CC 133
CC 120
C-N 143
CN 138
CN 116
Lengths of Covalent Bonds
Bond Lengths
Triple bond < Double Bond < Single Bond 9.4
9.4
H F FH
Polar covalent bond or polar bond is a covalent bond with greater electron density around one of the two atoms
electron richregion
electron poorregion e- riche- poor
+ -
9.5
Electronegativity is the ability of an atom to attract toward itself the electrons in a chemical bond.
Electron Affinity - measurable, Cl is highest
Electronegativity - relative, F is highest
X (g) + e- X-(g)
9.5
9.5
Bond Polarity and ElectronegativityBond Polarity and Electronegativity
ElectronegativityElectronegativity
Drawing Lewis StructuresDrawing Lewis Structures1. Add the valence electrons.2. Identify the central atom (usually the one with the highest molecular mass, lowest electronegativity, or closest to the center of the periodic table).3. Place the central atom in the center of the molecule and add all other atoms around it.4.Place one bond (two electrons) between each pair of atoms.5.Complete the octet for the central atom.6.Complete the octets for all other atoms. Use double bonds if necessary.7. Place remaining electrons on the central atom.
Write the Lewis structure of nitrogen trifluoride (NF3).
Step 1 – N is less electronegative than F, put N in center
F N F
F
Step 2 – Count valence electrons N - 5 (2s22p3) and F - 7 (2s22p5)
5 + (3 x 7) = 26 valence electrons
Step 3 – Draw single bonds between N and F atoms and complete octets on N and F atoms.
Step 4 - Check, are # of e- in structure equal to number of valence e- ?
3 single bonds (3x2) + 10 lone pairs (10x2) = 26 valence electrons
9.6
Trial
1. Write the Lewis stucture for1. H2O
2. CO2
3. NH3
4. CH4
5. N2
6. BH3
Exceptions to the Octet Rule
The Incomplete Octet
H HBeBe – 2e-
2H – 2x1e-
4e-
BeH2
BF3
B – 3e-
3F – 3x7e-
24e-
F B F
F
3 single bonds (3x2) = 69 lone pairs (9x2) = 18
Total = 24
9.9
Exceptions to the Octet Rule
Odd-Electron Molecules
N – 5e-
O – 6e-
11e-
NO N O
The Expanded Octet (central atom with principal quantum number n > 2)
SF6
S – 6e-
6F – 42e-
48e-
S
F
F
F
FF
F
6 single bonds (6x2) = 1218 lone pairs (18x2) = 36
Total = 48
9.9
Strengths of Covalent BondsStrengths of Covalent Bonds
Bond Enthalpies and Bond LengthBond Enthalpies and Bond Length
Covalent
share e-
Polar Covalent
partial transfer of e-
Ionic
transfer e-
Increasing difference in electronegativity
Classification of bonds by difference in electronegativity
Difference Bond Type
0 Covalent
2 Ionic
0 < and <2 Polar Covalent
9.5
Classify the following bonds as ionic, polar covalent, or covalent: The bond in CsCl; the bond in H2S; andthe NN bond in H2NNH2.
Cs – 0.7 Cl – 3.0 3.0 – 0.7 = 2.3 Ionic
H – 2.1 S – 2.5 2.5 – 2.1 = 0.4 Polar Covalent
N – 3.0 N – 3.0 3.0 – 3.0 = 0 Covalent
9.5
Test Yourself
1. Write the formula and draw the ionic structure1. Magnesium (II) bromide2. Iron (III) Oxide3. Sodium Azide4. Ammonium Chloride5. Magnesium Nitrate6. Ammonium Phosphate
2. Write the name1. FeO2. Fe2O3
3. LiBr4. KCrO4
5. K2Cr2O7