Chemical Interactions Occur between the Valence Electrons Dots represent valence electrons When atoms combine to make molecules they form chemical bonds Valence electron interaction ID: 934800
Download Presentation The PPT/PDF document "Ionic Compounds Lewis Dot Diagrams" is the property of its rightful owner. Permission is granted to download and print the materials on this web site for personal, non-commercial use only, and to display it on your personal computer provided you do not modify the materials and that you retain all copyright notices contained in the materials. By downloading content from our website, you accept the terms of this agreement.
Slide1
Ionic Compounds
Slide2Lewis Dot Diagrams
Chemical Interactions Occur between the Valence Electrons
Dots
: represent
valence electrons
Slide3When atoms combine to make molecules, they form
chemical bonds.
Valence
electron
interaction
Slide4Forming Chemical Bonds
Octet Rule
Atoms will form bonds by:
SharingGiving or
Takingelectrons to complete
their octet
Higher energy farther away from nucleus
Slide5Atoms form ions to have stable electron configurations (similar to noble gases)
hh
Slide6Ionic Bonds
Ionic Bonds
form when one atom (nonmetal) gains electrons and the other atom (metal) loses electrons in order to gain stability.
Slide7Ionic Bonds form between a
metal (cation) and a nonmetal (anion).
Slide8To form an ion, lithium will most likely:
Gain 1 electron
Gain 2 electrons
Lose 1 electron
Lose 2 electrons
Slide9Forming Chemical Bonds
Lithium
Better
to lose
1 electron or to gain 7 electrons?
X
Slide10Therefore, as an ion lithium will have what charge?
1+
2+
1-
2-
Slide11Ionic Bonds
Atoms gain or lose its electrons
+
NaCl - salt
Slide12Chemical Interactions Occur between the
Valence Electrons
Lewis structures are simpler to do & see
Slide13Formation of MgCl2
Slide14Formation of Na2S
Slide15Slide16Write down the chemical formula for Aluminum
Flouride
Slide17Formation of AlF3
Slide18Today is a practice Day!
We need to be able to name ions given chemical formulaWe need to be able to determine the chemical formula given the name
Slide19Valence Electrons
Noble Gas Structure = Octet
1,2 3,4,5,6,7,8
Slide20IONIC BONDS / Cat
ions
and
An
ions
Cation – positive ions
Transition Metals use
Roman Numerals to tell you the ox #
Anion – negative ions
Slide21Oxidation Numbers
Oxidation Numbers
- indicated # of e’ lost, gained or shared.
Ex. Oxidation number of chlorine is -1
Slide22Halogens will have an oxidation number of:
+1
+2
-1
-2
Slide23Alkaline earth metals will have an oxidation number of:
+1
+2
-1
-2
Slide24We will name binary compounds together
Using pages 156- 158Describe how to name cations and anions when they are by themselves
Slide25Naming Binary Ionic Compounds
Write the name of the ionic compound, Ca2N3.
Write the name of the ionic compound, K
2
O.
Slide26What is the name of BeBr2?
Boron bromine
Beryllium bromine
Bromide
beryllide
Beryllium bromide
Beryllide bromide
Slide27Metals with Variable Charges
Many transition metals can form more than one type of cation.For this reason, you must show the oxidation number in the name using Roman Numerals
Slide28Slide29Naming Binary Ionic Compounds with Transition Metal Cations
Write the name of the ionic compound, Cu2
O.
.
Write the name of the ionic compound, NiS.
Slide30What is the name for SnBr2?
Bromide Tin
Tin Bromide
Tin (I) Bromide
Tin (II) Bromide
Tin (III) Bromide
Tin (IV) Bromide
Slide31What is the name for FeI3?
Iron iodide
Iron (I) iodide
Iron (II) iodide
Iron (III) iodide
Slide32What is the name for MnS?
Manganese sulfide
Manganese (I) sulfide
Manganese (II) sulfide
Manganese (III) sulfide
Slide33Exceptions:
Some of the transition metals have only one ionic charge:
Do not
need to use roman numerals for these:
Silver is always 1+ (Ag1+)Cadmium
and Zinc are always 2+ (Cd2+
and Zn2+)
Slide34Writing Formulas for Binary Ionic Compounds
Write the formula for barium iodide.Write the formula for sodium oxide.
Write the formula for aluminum nitride.
Write the formula for copper (I) sulfide.
Slide35Criss
-Cross Method for Writing Formulas
- You can write the oxidation
number and
criss
-cross
them as subscripts.
- Note – if not in lowest termsyou must reduce the subscripts
(ex. Magnesium oxide)
Al
3+
S
2-
2
3
= Al
2
S
3
Slide36What is the formula for aluminum bromide?
AlBr
AlBr
2
Al
3Br
Br3AlAlBr3
Slide37What is the formula for magnesium oxide?
MgO
Mg
2
O
2MgO2
Mg2OOMg
Slide38Write the formula for titanium (II) chloride.
TiCl
Ti
2
Cl
TiCl2
Ti2Cl2
Slide39Write the formula for tin (IV) oxide.
SnO
SnO
4
SnO
2Sn
4OSn2O
Slide40POLYATOMIC IONS
Not all compounds are made of only 2 types of atoms
poly – “many”
Memorize the polyatomic ions from p. 170.
Slide41Tricks for Polyatomic Naming
Perchlorate per+root+ate ClO4-1
chlorate root+ate ClO
3
-1 chlorite root+ite ClO2-1Hypochlorite hypo+root+ite ClO
-1Prefixes and suffixes designate number of oxygens
Slide42Naming Polyatomic Ionic Compounds
Polyatomic ionic compounds are named just like binary ionic compounds.Exception: be sure to enclose the polyatomic ion in parentheses before writing the subscript (only necessary if subscript is not 1).
Ex. Barium hydroxide =
Ba
(OH)2
Slide43Write the formula for Calcium Nitrate.
CaNO
2
Ca(NO
2
)2Ca2NO
3Ca2NO2Ca(NO3)2
Slide44Write the formula for Magnesium Phosphate.
MgPO
4
Mg
3
(PO4)2Mg
4(PO3)2MgPO3Mg(PO4)
2
Slide45Naming Ionic Compounds