Transcript – Ionic bonds Chemical bonds that result from the electrical

Ionic bonds – Chemical bonds
that result from the electrical
attraction between large
numbers of cations and anions
Cation – ?
Anion – ?
Ionic bonds most commonly form
between …?
Ionic bonds are made up of
charged pieces (ions) … Ions can
be made up of single atoms or
groups of atoms bonded together
(polyatomic ions)
Binary ionic compound – ionic
compound consisting of only 2
elements (monatomic ions)
Naming:
Name the cation and add an
ide ending to the anion
Examples:
sodium and chlorine form…
sodium chloride
magnesium and oxygen
form…
magnesium oxide
What’s a binary ionic
compound?
Binary ionic compound – ionic
compound consisting of only 2
elements (monatomic ions)
Bromine bonds with sodium
Sodium bromide
Cesium bonds with oxygen
Cesium oxide
Silver bonds with fluorine
Silver fluoride
What type of compounds have
we learned to name?
How do you identify this type
of compound?
chlorine bonds with lithium
Lithium bromide
magnesium bonds with sulfur
Magnesium sulfide
aluminum bonds with oxygen
Aluminum oxide
Problem… names do not
directly indicate ratio of ions…
Answer… empirical formula
Li2O
NaCl
MgF2
Determining formulas –
Crisscross method
Determining formulas – Crisscross
method
1. determine charges
2. Take away the +/- and
crisscross them to determine
subscripts
Determine the empirical formula for an
ionic compound containing…
potassium and fluorine
calcium and fluorine
cesium and sulfur
aluminum and oxygen
Name the compounds formed when the following
elements bond:
1. Calcium and fluorine
2. Chlorine and strontium
3. Silver and oxygen
Write the formulas for the following compounds:
1. Lithium bromide
2. Barium chloride
3. Sodium oxide
Throwing in the transition metals:
Use roman numerals if more
than one charge is possible
Roman numeral = charge, if
none use sheet, then same as
binary ionic compounds
The weird guys…
Throwing in the transition metals:
FeO
Au2S
CuF2
PbS
SbF3
Work
backwards
- the
overall
charge in
a
compound
must be 0
Throwing in the transition metals:
Lead II oxide
Silver bromide
Ferric Chloride
Throwing in the transition metals:
FeO
Au2S
CuF2
PbS
SbF3
Work
backwards
- the
overall
charge in
a
compound
must be 0
Throwing in the transition metals:
Lead II oxide
Silver bromide
Ferric Chloride
silver chloride
iron III oxide
copper II sulfide
NiF2
Au2O3
Cu2S
cadmium chloride
potassium oxide
Ni2O3
BaF2
Binary ionic compound –
ionic compound consisting of
only 2 elements (monatomic
ions)
Binary Compound – A compound
with 2 elements
more than 2 atoms = OK
(CaF2)
more than 2 elements NOT ok
(NaCrO4)
Throwing in polyatomic ions:
If formula has more than 2 eles.
Names do not change (no ide-ending)!
a non-ide ending should clue
you in (memorize hydroxide + CN-1)
more than one ion = parenthesis
Check:
Is the compound binary?
Does it contain a transition
metal?
If yes, use your ion sheet!!!
Throwing in polyatomic ions:
MgSO4
(NH4)2S
NaOH
CrSO3
Zn3(PO4)2
Throwing in polyatomic ions:
Calcium Sulfate
Lithium Cyanide
Magnesium Hydroxide
Potassium Clorate
potassium hydroxide
Iron III carbonate
SnO2
Co(NO3)2
Day 3
3-7
calcium nitrate
silver carbonate
Li2SO3
Cu(OH)2
sodium nitrite
nickel III oxide
magnesium chlorite
Pb(CO3)2
Iron III sulfite
Co2(CO3)3
Copper II nitrite
Zn3(PO3)2
Tin IV sulfite
CoPO4
1. Explain how you would
determine the name for Pb(CO3)2.
DETAILED EXPLANATION! What is
the name?
1. Is a compound of C bonded
to H an ionic compound? WHY
or WHY NOT?
2. Name me: +2 ion of Copper
and a bromine ion combine
3. Write the formula for the
ionic compound in # 2
1.Write the formulas for the following:
Cuprous Sulfide
Ferric Carbonate
Ammonium Nitrite
2.Write the names for the following:
K3BO3
Co(NO2)3
Ag3PO4
Using Lewis dots to represent
bonds (Lewis dots for
compounds):
Na
Cl
Na Cl
Shared electrons (bonds)
are represented with a line
Acid - Compound that yields H+ ions (always
starts with an H) – molecular compounds that
act like ionics
Naming:
Acids are named for their anions
Binary: hydro – anion base – ic
ending – the word “acid”
Naming:
Acids are named for their anions
Binary: hydro – anion base – ic
ending – the word “acid”
Non-binary: ate ending becomes ic,
ite ending becomes ous
HF
HBr
HNO3
HNO2
Naming:
Acids are named for their anions
Binary: hydro – anion base – ic
ending – the word “acid”
Non-binary: ate ending becomes ic,
ite ending becomes ous
Hydrochloric acid
Sulfurous acid
HCl = hydrochloric acid
HNO3 = nitric acid
HC2H3O2 = acetic acid
H2SO4 = sulfuric acid
H3PO4 = phosphoric acid
Binary Molecular Compounds
Based on Prefixes
1. Less electronegative first – prefix only if
more than one atom
2. Second element – prefix, root of name,
ending ide (if only two elements)
3. o or a @ the end of prefix is dropped if name
begins with a vowel (monooxide,
monoxide)
Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
1
2
3
4
5
6
7
8
9
10
Binary
Molecular
Compounds
– prefix
system
Binary Molecular Compounds
Write the Name:
N2O5
Dinitrogen pentoxide
SbF3
Antimony trifluoride
Write the Formula:
Germanium tetraiodide
GeI4
diphosphorous trioxide P2O3
Binary Molecular Compounds
Write the Name:
As2O5
diarsenic pentoxide
ICl3
iodine trichloride
Write the Formula:
carbon tetraiodide
CI4
dinitrogen trioxide
N2O3
Electrolyte – anything that conducts electricity
when melted or dissolved in water