David Hudson UK Patent NonMetallic Monoatomic Forms of Transition Elements
Ionic Nomenclature: 1. Binary: made-up of one monoatomic cation ion and one monoatomic anion. Metal...
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Transcript of Ionic Nomenclature: 1. Binary: made-up of one monoatomic cation ion and one monoatomic anion. Metal...
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Ionic Nomenclature:1. Binary: made-up of one monoatomic cation ion and one monoatomic anion. Metal (+) bond to Non-Metal (-)2. For binary acids, the cation is ALWAYS H+ . HBr3. Writing ‘Formula Units’
-Write the symbol of the element.-Assign oxidation numbers.-Criss Cross- Simplify
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4. Naming Binary Ionic compounds- anion will end in –ide- first name is the name of the element.-second name is the name of the anion with the ending dropped
and –ide added. Calcium bromide- All cations other than Group 1A, 2A and Aluminum will have and Roman numeral to indicate the oxidation number of the that
metal. Iron (III) chloride
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5. Binary acids; Hydro-anion root-ic acid. Hydrochloric acid.
6. Ternary Compounds: ionic compound in which at least one of the ions is a polyatomic ion.
7. For a ternary acid, the cation ion is ALWAYS H+ . H2SO4 .
-Naming ternary acids follows –ate,-ic , -ite, -ous
Sulfuric acid
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8. Writing the ‘Formula Unit’ (Same 4 steps)-write the atom or polyatomic ion-assign the oxidation number-criss cross-simplify (more than one poly, put ( ) )
9. Naming ternary ionic compounds-first name is the name of the
element (or Ammonia if NH3).
-second name is the name of the polyatomic ion.
Cr(HSO4)3 Chromium bisulfate
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10. Bases: Ionic compounds in which the anion is hydroxide, OH- (except NH3)
Ba(OH)2 Barium hydroxide
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1. Cations are positive ions. Always written first.2. Anions are the negative ions. Written after the
cation3. Positive and negative ion pack in a regular pattern that balances the forces called an ionic crystal or crystal lattice.4. Lattice energy defines the strength of the ionic
bond. Large lattice energy = stronger bond5. Form 3-D compounds6. High melting and high boiling point.7. Compound defined by hardness and brittle.8. Almost always exothermic when bond is broken.
Energy-in to form the bond and energy-out when the bond is broken
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9. Further separation on the periodic table, the MORE ionic characteristics. 10. Conductive current dissolved and molted state. Greater solubility = more ionic11. Ionic compounds are electrolytes = they carry an electric current when dissolved.12. Ionic compounds are referred to as formula units (FU).13. Net charge of the compound must = zero14. Greater ∆EN = greater ionic characteristic
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UEQWhat are the unique characteristics of a
covalently bonded molecule?
LEQWhat is a covalent bond?
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The joining of two or more elements through the sharing of valance electrons to form a molecule
Purpose: To form a stable octet between the elements
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1. Covalent bonds are molecules (neutral) 2. Do not conduct electricity 3. Low melting and boiling points 4. Are less soluble in water and more soluble
in non-aqueous solvents.5. Can form multiple bonds. 6. Multiple bonds shorten bonding length and
increases bonding strength.7. Weak force of attraction between
molecules.
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8. Elements close on the periodic tables tend to form covalent bonds.9. Metallic bonds are a type of covalent bond10. Hydrates bond covalently.
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Atoms the share electrons form molecules. Molecules are expressed in ‘Molecular
Formulas’ Naming follows binary ionic naming trends
with prefixes to define the number of each atom in the molecule.
Hydrates follow binary naming with a prefix to identify the number of water molecules.◦ Molecular formulas are NOT simplified.
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Prefixes:mono- for one (used w/ the second name
usually)di- for 2 hexa- for 6tri- for 3 hepta- for 7tetra- for 4 octa- for 8penta- for 5 nano- for 9deca- for 10
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N2O5
Dinitrogen pentoxide
CCl4Carbon tetrachloride
Silicon dioxideSiO2
Diphosphorous hexaflourideP2F6
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CuO . 5H2O
Copper (II) oxide pentahydrateNiCl3 . 2H2O
Nickle (III) chloride dihydrateChromium (II) sulfate heptahydrate
CrSO4 . 7 H2O
Barium sulfide trihydrateBaS . 3H2O
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What is polarity and how is it applied to molecular bonding?
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Non-Polar: equal sharing of the valance electrons.
Polar: unequal sharing of the valance electrons.
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Polarity refers to the uneven sharing of valance electrons.
Electronegativity refers to the pull on another atoms valance electrons.
If the EN values are not the same then there is polarity (uneven pulling).
If the EN values are equal, then there is no polarity (even pulling) called non-polar
The closer the EN values the less polar.
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Shape of molecule is symmetrical.
Homonuclear molecules.◦Diatomic molecules:
N2, O2, F2, Cl2, Br2, I2, and H2
Makes the #7
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Shape of the molecules is asymmetrical due to unequal sharing of the electrons.
Heteronuclear: one nuclear charge is stronger than another.
Polarity is the function of the change in electronegativity (EN)◦ Increase EN, = more ionic chstc.
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Rank these in decreasing covalent characteristics:
H2O, N2, NO3- , NaBr2, CO2
Solution:
1. Identify the electronegativity for each element in the molecule.2. Less covalent > 1.7 > more covalent.
N2 > NO3- > CO2 > H2O > NaBr2
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Identify if the following is pure covalent, polar covalent or ionic: Use ∆EN
O3
N2O5
RbClN2
CCl4NH3
Cl2SO2
BaBr2
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Pictorial representation of valance electrons.
Dot structure Stick structure
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BCl3
CCl4
NF3
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Representative elements share electrons to take on a Noble gas electron configuration.
Each element in a molecule will follow the octet rule.
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Formula to determine the number of shared electrons:
N – A = S N = # of electrons needed to form a
Noble gas configuration. A = # of electrons available in the
valance. S = # of electrons shared
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CS2
C2H4
CO32-
CHCl3
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Sigma Bonds are the single electron overlap of the s orbital.
Forms single bonds, end-to-end. Pi Bonds are the overlap of the s and p
orbitals. Forms double and triple bonds w/ s end-
to-end and p side-to-side.
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The joining together of two or more elements by the sharing of the valence electrons.The Lewis Structure: representation of the electrons in the valance of an atom. * Group A elements = the Group number is
the number of valance electrons.For Example: N C P ClShow the Lewis structure for the following.
PH3 CCl4 H2S SiH4
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Covalent bonds are formed when valance electrons between two elements are share either by an end-to-end overlap relationship or an side-to-side overlap relationship.
1.Sigma bond (σ ): single covalent bond with a end-to-end relationship
BeCl2 CH4 AlF3 NH3
*sigma bonds are single bonds*bonding length is longer (Table 8.1)*bonding strength is less (Table 8.2)
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pi bonds ( π ) : A side-to-side overlap of valance electrons. Forms multiple bonds.
CO2 O2 N2
*one sigma + one pi = double bond*one sigma + two pi = triple bond *double bond shorter bond length*double bond stronger bond*triple bond shortest bond length*triple bond strongest bond
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CO2
N2
CS2
HNO3
NO31-
Which are polar? Which are non-polar? Which are non-polar with polar bonds?
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Equally acceptable formulas. HNO3
NO31-
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Most beryllium compounds Most Group IIIA elements Compound which require more than 8e-
in the valance. Compounds containing d or f transitional
elements ‘S’ with an odd number of electrons
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CCl4 CO2
N2O5
N2O S3O5
NF3
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Follows the rules as ionic compounds except prefixes are used to note ‘how many’.
Table 8-3, page 248.
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VB Theory : Valance Bond Theory, orbital overlaps
VSEPR Theory: Valance Shell Electron Pair Repulsion Theory◦ Electrons arrange to max the distance between
electrons◦ Bonding pairs v. Unshared pairs
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Linear (2) Trigonal Planar Tetrahedral Trigonal Pyramidal Angular (Bent) Trigonal Bipyramidal Octehedral
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Formula AB2 w/ no unshared pairs VSEPR: bonding angle of 180o
VB: sp overlap Forms a polar bond and a non-polar
molecule.
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Formula of AB3 and no unshared pairs. VSEPR: bonding angle of 120o
VB: SP2 overlap Polar bond w/ non-polar molecule
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Formula of AB4 w/ no unshared pairs. VSEPR: bonding angle of 109.5o
VB: sp3 overlap Forms polar bonds and non-polar molecule.
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Formula AB3 w/ one unshared pair on A. General: subtract 2.5o for each unshared
pair. VSEPR: bonding angle of 107o
VB: sp3 overlap w/ a polar bond and a polar molecule
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Formula AB2 w/ 2 unshared pairs on A VSEPR: bonding angle of 104.5o
VB: sp3 overlap w/ polar bonds and polar molecule.
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Formula AB w/ 3 unshared pairs VSEPR: bonding angle of 102o VB: sp3 overlap w/ polar bonds and polar
molecule.
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Formula AB5 w/ no unshared pairs VSEPR: bonding angles at 90o, 120o and
180o
VB: sp3d overlap w/ polar bonds and polar molecule.
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Formula AB6 w/ no unshared pairs VSEPR: bonding angles of 90o, 120o and
180o
VB: sp3d2 overlap w/ polar bonds and molecule
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Molecule VB VSEPR Shape NI3PH3
CH4
SF6
H2S
PF5
BeCl2