ionic and metallic bonding - Waterford · •all elements are ‘stable’ with an octet of eight valence electrons “Atoms of metals tend to lose their valence electrons, leaving
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ionic and metallic
bonding chapter 7
Chemical Nomenclature
The Skill of Writing and
Naming Chemical
Formulas
the b i g idea
• determine the number of valence electrons for an
element.
• determine which elements gain/lose electrons,
the charges their ions carry, and state how ions
are formed.
• differentiate between ionic bonding and covalent
bonding.
you will be able to:
valence electrons -
review • valence electron - outermost energy level electrons
• electrons involved in chemical bonding
• highest energy electrons in an atom / ion
• number of valence electrons - group number of the
element
• transition metals - 2 valence electrons
• atoms will lose, gain, or share electrons to achieve an
electronic structure identical to that of a noble gas
• all elements are ‘stable’ with an octet of eight valence
electrons
“Atoms of metals tend to lose their valence electrons,
leaving a complete octet in the next-lowest energy level.
Atoms of some nonmetals tend to gain electrons or to
share electrons with another nonmetal to achieve a
complete octet.”
the octet rule
Properties of Metals
• Shiny
• Conduct electricity
• Ductile
• Malleable
• Lose electrons
• All but gold and copper are grey in color
Properties of
Nonmetals
• Not shiny
• Most are colored
• Do not conduct electricity
• Not malleable
• Gain electrons
cation formation • element (metal) loses electrons
• K K+ + e-
K+
• element (nonmetal) gains electrons
• P + 3 e- P3-
P3-
anion formation
Ar 18
Oxidation Numbers • The overall charge of an ion after it loses or gains electrons
• Can be determined by looking at the periodic table
Formation of Ionic Compounds • Composed of a metal cation and a nonmetal anion
• METAL is always written FIRST
• Ionic compounds are electrically NEUTRAL
• Overall charge is ZERO
• The total positive charge equals the total negative
charge
chemical formula
• shows the type and number of elements in
the smallest representative unit of a
substance
Writing Formulas for Binary Ionic Compounds
Two simple steps:
• Write the symbol and charge of each ion
• Write the positive ion of metal first, and the negative ion Ba2+ Cl
Cl
• Balance the charges by writing the number of ions needed as subscripts
BaCl2
• SHORTCUT: Use the Crossover Rule
the crossover rule: binary ionic compounds
Mg Mg 2+ F 1- F
Mg 1 F 2
MgF2
Cs Cs + S 2- S
write the neutral chemical formula for the ionic compound formed
between Cs and S atoms
Cs 2 S 1
Cs2S
write the neutral chemical formula for the ionic compound formed
between Mg and F atoms
the crossover rule
Be Be 2+ O 2- O
Be 2 O 2
Be2O2
Ca Ca 2+ As 3- As
write the neutral chemical formula for the ionic compound formed
between Ca and As atoms
Ca 3 As 2
Ca3As2
reduce! BeO
write the neutral chemical formula for the ionic compound formed
between Be and O atoms
Learning Check
Write the correct formula for the compounds containing the
following ions.
A. Na+, S2-
B. Al3+, Cl-
C. Mg2+, N3-
Naming Binary Ionic
Compounds
Name the metal first, then the
nonmetal as -ide
Use name of a metal with a fixed
charge
Groups 1A, 2A, 3A
and Ag, Zn, and Cd
• Examples:
NaCl sodium chloride
ZnI2 zinc iodide
Al2O3 aluminum oxide
Learning Check
Complete the names of the following binary compounds:
Na3N sodium ________________
KBr potassium ________________
Al2O3 aluminum ________________
MgS _________________________
Transition Metals
• Most transition metals and Group 14 metals form 2 or more positive
ions
• Zn2+, Ag+, and Cd2+ form only one ion
Names of Variable Charge Metals
• Use a Roman Number after the name of a metal that forms two or more ions
• Transition metals and the metals in groups 14 and 15
Lead Pb2+ lead(II)
Pb4+ lead(IV)
Names of Variable Charge Metals
Learning Check
Complete the names of the following binary compounds with
variable metal ions:
FeBr2 iron (_____) bromide
Cu2O copper (_____) oxide
SnCl4 ___ ( _____ ) ______________
Fe2O3 ________________________
CuS ________________________
polyatomic ions: ternary
ionic compounds • cations and anions composed of two or more
atoms
• the entire ion ‘assumes’ the positive or negative
charge
• behave in the same manner as monatomic (single
atom) ions
Three Possible Types of
Ternary Ionic Compounds
• Ammonium cation + anion (nonmetal)
• Cation (metal) + polyatomic anion
• Ammonium cation + polyatomic
anion
the crossover rule - polyatomic ions
Li Li + NO3 -1
write the neutral chemical formula for the ionic compound formed
between lithium and nitrate
Li 1 NO 3
LiNO3
the crossover rule - polyatomic ions
NH4 +
write the neutral chemical formula for the ionic compound formed between
ammonium and oxygen
NH4 2 O 1
(NH4)2O
O 2- O
parenthesis for polyatomic ions when there is more than one in the formula
the crossover rule - polyatomic ions
Ba 2+
write the neutral chemical formula for the ionic compound formed between
barium and phosphate
Ba 3 PO 4 2
Ba3(PO4)2
PO4 3-
parenthesis for polyatomic ions when there is more than one in the formula
Learning Check
1. aluminum nitrate
a) AlNO3 b) Al(NO)3 c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH b) Fe3OH c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)
Mixed Practice
Binary and Ternary Ionic Compunds
Write the formula:
• Copper (II) chlorate
• Calcium nitride
• Aluminum carbonate
• Potassium bromide
• Barium fluoride
• Cesium hydroxide
Naming Ternary Compounds
• Contains at least 3 elements
• There MUST be at least one polyatomic ion
• It helps to circle the ions
• Examples:
NaNO3 Sodium nitrate
K2SO4 Potassium sulfate
Al(HCO3)3 Aluminum bicarbonate or Aluminum hydrogen
carbonate
Learning Check
Match each set with the correct name:
1. Na2CO3 a) magnesium sulfite
MgSO3 b) magnesium sulfate
MgSO4 c) sodium carbonate
2. Ca(HCO3)2 a) calcium carbonate
CaCO3 b) calcium phosphate
Ca3(PO4)2 c) calcium bicarbonate
Mixed Practice! Name the following:
• Na2O
• CaCO3
• PbS2
• Sn3N2
• Cu3PO4
• HgF2
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