Flashcards for Ionic & Metallic Bonding
What particle is transferred in ionic
bonding?
Electron
How do you identify an ionic formula?
Metal + Nonmetal
How do you identify a covalent formula?
All Nonmetals
What do metals do?
Metals lose electrons & form
positive ions.
What do nonmetals do?
Nonmetals gain electrons & form
negative ions.
What are the properties of metals?
1) Luster2) Good conductors of heat &
electricity3) Malleable & ductile4) Low ionization energy & low
electronegativity5) High mp, high bp & low vapor
pressure
Why do atoms form bonds?
To get the same electron configuration as the nearest noble gas.
What is a chemical bond?
Force of attraction that holds 2 atoms together.
What are the properties of ionic compounds?
1) Hard, brittle2) High melting point, high boiling point3) Low vapor pressure4) Poor conductors of heat5) Solids do not conduct electricity at all6) Melts & solutions do conduct a current7) Ions in solution react quickly
What is the structure of ionic compounds?
Crystal lattice: lattice points are positive &
negative ions.
Subscripts in formulas
Tell how many atoms of that element are present.
No subscript means “1.”
Empirical Formula
Subscripts in chemical formula have smallest
whole number ratio
Empirical Formula
Ionic compounds only have empirical
formulas.
Crystal lattice
Regular, repeating pattern in 3 dimensions.
Compounds are electrically …
Neutral.
Writing formulas from the ions for binary compounds.
• Write the ions, positive 1st.• If the superscripts (charges)
do NOT add to zero, “criss-cross.”
• Na+1 S-2 becomes Na2S
Molecular Formula
Gives exact composition of molecule.
What is the structure of metals.
Crystal lattice: all lattice points are
positive ions.
Delocalized electrons
Valence electrons in metals are free to
roam throughout the metal.
Sea of mobile electrons
Phrase used to describe valence electrons in
metallic bonding.
Metallic Bonds
Formulas have metals only.
Subscripts in chemical formulas
Microscopic scale – give atomic ratios
Macroscopic scale – give mole ratios
Lewis Dot Structures for Ionic Compounds
Have square brackets and charges. Charges add up to 0. Positive ion has no dots. Negative ion has 8 dots.
Lewis Dot Structures for NaCl
[Na]+[:Cl:]-
::
Lewis Dot Structures for NaOH
[Na]+[:O:H]-
::
Group 1 metals form …
+1 ions
Group 2 metals form …
+2 ions
Group 16 nonmetals form …
-2 ions
Group 17 nonmetals form …
-1 ions
Group 18 nonmetals form …
They don’t form ions. There the
noble gases!
Binary Compounds
Composed of 2 elements! (2 uppercase letters)
Naming Binary Ionic Compounds: Stock
System
Name positive ion 1st (metal).Name negative ion 2nd (nonmetal).
Change ending to –ide.If metal has more than 1 oxidation
state, use Roman numeral to specify which.
NaCl
Binary Ionic Cmpd.Na has only 1 oxidation
state.Sodium Chloride
FeCl2
Binary Ionic Cmpd.Fe has 2 possible oxidation states.Iron (II) chloride
Fe(NO3)3
Contains a polyatomic.Fe has 2 possible oxidation states.Iron (III) Nitrate
Polyatomic Ion
• A group of covalently bonded atoms that carries a charge.
• Can form ionic bonds with other ions.
• Have names.
NaNO3
• NO3 = nitrate ion• Sodium nitrate
Cu(NO3)2
• NO3 = nitrate ion• Copper has more than one oxidation
state.• The copper here must have a +2
charge.• Copper (II) nitrate.
Cu2SO4
• SO4 = sulfate ion• Copper has more than one oxidation
state.• The copper here must have a +1
charge.• Copper (I) sulfate.
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