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PAP Chapter 6 PAP Chapter 6 CHEMICAL CHEMICAL BONDINGBONDING
PAP Chapter 6 PAP Chapter 6 CHEMICAL CHEMICAL BONDINGBONDING
Cocaine
Chemical BondingChemical BondingA chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
Metallic Bonding
Metallic – holds atoms of metals togetherA metallic bond is formed between all
metals. Examples include a piece of Copper, Zinc, Sodium, Iron. Any metal
Metallic bonds result from the attraction between metal atoms and the surrounding sea of delocalized electrons
valence electrons can move freely around the whole metal structure—they are not confined to any one atom
Characteristics of Metals
ODuctile- draw into thin wireOMalleable-ability to hammer into
O Thin sheetsOShiny (luster)OConducts heat and electricity OSolid at room temperature
Metallic BondingThis model explains many of the
properties of metals: the mobile electrons can enter/leave
the metal structure, so metals are good conductors of heat and electricity!
metal cations are not locked into any crystal structure, so they can slide past each other when stressed. That makes metal malleable and ductile.
The de-excitation ( The electron falling back down to a lower energy level) is responsible for the shiny (luster) appearance of metals.
Ionic BondsOcomplete transfer
of 1 or more electrons from one atom to another (one loses, the other gains) forming oppositely charged ions that attract one another
Remember Cations and Anions
An atom which loses an electron becomes positively charged and is called a cation.
Examples: Na+, K+, Ca2+, Al3+
Metals usually become cations
An atom which gains an electron becomes negatively charged and is called an anion.
Nonmetals usually become anions.
Examples: Cl-, S2-, N3-
Characteristics of Ionic Bonds
The electrons align themselves into an orderly arrangement that is known as crystal lattice. This makes the shape that you see into a crystal.
Characteristics of Ionic Compounds
Strong attraction between ionsSoluble in waterConduct electricity in solutionConduct electricity when
moltenHigh melting pointsHigh boiling pointsHard but brittleSolid at room temperature
What are electron dot formulas orLewis Dot Diagrams
Electron dot formulas are diagrams that show valence electrons in the atoms of an element as dots around the symbol of the element.
1.1. Make Generalizations Make Generalizations As illustrated by the electron dot formulas in the table, how are the elements in a group similar?
1.1. Make Generalizations Make Generalizations As illustrated by the electron dot formulas in the table, how are the elements in a group similar?
How are electron dot formulas for ionic bonds constructed?
Ionic bonds form as a result of electrostatic attractions between cations and anions.
Electron dot formulas show the valence electrons and charges of these ions and may be used to illustrate the ionic bonds.
Examples
ExamplesO Lithium and BromineO Magnesium and ChlorineO Sodium and SulfurO Aluminum and Oxygen
Day 2
Covalent BondsCovalent Bonds:Covalent —valence electrons are shared between nonmetal atoms
Covalent BondNonpolar Covalent bond- Covalent
bond in which the bonding electrons are shared equally by the bounded atoms, resulting in a balanced distribution of an electrical charge.
Polar Covalent bond- Covalent bond in which the bonded atoms have an unequal attraction for shared electrons. Each atom has a chargePartial positive- (+δ) Partial negative- (- δ)
Characteristics of Covalent Bonds
OTwo non-metals bonded together
ORelatively weak bondsOUsually a gas or liquid at room
temperatureODoes not conduct electricity in
solutionOLow melting pointOLow boiling pointOSoluble in alcohol and insoluble
in water
The type of bond can usually be calculated by finding the difference in electronegativity of the
two atoms that are going together.
ElectronegativityIncreases
ElectronegativityDecreases
OIf the difference in electronegativities is between:O 1.8 to 4.0: IonicO 0.4 to 1.7: Polar CovalentO 0.0 to 0.3: Non-Polar Covalent
Example: NaClNa = 0.9, Cl = 3.0Difference is 2.1, sothis is an ionic bond!
Electronegativity Difference
Example: H2OH = 2.1, O = 3.5Difference is 1.4, sothis is a polar covalent bond !
ODiatomic Molecules are nonpolar covalent compounds.
OA diatomic molecule is a molecule only containing two atoms
OThe seven diatomic molecules areOH2, N2, O2, F2, Cl2, Br2, I2OThese diatomic molecules are never by themselves.
Diatomic Molecules
Octet RuleOctet Rule
Chemical Compounds tend to form so that each atom, by gaining, losing or sharing electrons, has an octet of eight electrons in its highest occupied energy level
Electron dot formulas:covalent bonds O In a covalent bond, no ions form. Instead, nonmetallic
atoms share electrons, which results in each atom having a noble-gas configuration.
O Single Covalent Bonds -A single covalent bond results when two atoms share one pair of electrons, as in the case of hydrogen gas, which is a diatomic molecule.
OExamples: F2 , HBr, Cl4
(contd.)
ODouble Covalent Bonds- When atoms bond by sharing two pairs of electrons, the result is a double covalent bond, as in a molecule of carbon dioxide, CO2. The double bond is shown by four dots or two dashes.
Triple Covalent Bonds- When atoms bond by sharing three pairs of electrons, the result is a triple covalent bond, as in a molecule of nitrogen gas, N2. The triple bond is shown by six dots or three dashes.
Violations of the Octet RuleViolations of the Octet RuleUsually occurs with B and elements of Usually occurs with B and elements of
higher periods. Common exceptions are: higher periods. Common exceptions are:
Be, B, P, S, and Xe. Be, B, P, S, and Xe.
BF3BF3
SF4SF4
Be: 4
B: 6
P: 8 OR 10
S: 8, 10, OR 12
Xe: 8, 10, OR 12
Lewis Structures
HF
H2O
H F
or H - F
H O H
or H - O - H
NH3
CH4
H N HH
or H - N - H
H
H C HH
H
or H - C - H
H
H
Lewis Structures
Extra Slides
H2O is POLAR because it has a positive end and a negative end. (difference in electronegativity)
O has a greater share in bonding electrons than does H.
O has a greater share in bonding electrons than does H.
O has slight negative charge (-δ) and H has slight positive charge (+ δ)
Bond Polarity
This is why oil and water will not mix! Oil is nonpolar, and water is polar.
The two will repel each other, and so you can not dissolve one in the other
Bond PolarityBond Polarity
Bond PolarityBond Polarity
“Like Dissolves Like”Polar dissolves PolarNonpolar dissolves
NonpolarPolar also dissolved
IonicEx: water and salt