1. Chemical Nomenclature

2. Nomenclature A System of Naming Compounds
Compounds are two or more atoms of different elements bonded together.

3. 10/25 Chemical Formulas & Naming Compounds Draw the table outline & leave room for us to write on it & at the top

4. -- 1+ 2+ 3+ -- 3- 2- 1-
Generally metals form cations and non-metals form anions.

5. Binary compounds Binary Compounds Compounds composed of two elements
Two types
Ionic
Covalent

6. Ions… (copy this slide)
Electrons are arranged on energy levels or “shells”. Atoms are most stable with 8 electrons on their outermost shell. This is often referred to as the octet rule.
Number of valence electrons on the outer energy level come from the elements in “TALL” Groups I-8
Elements in first 3 Tall groups will lose or give up their valence electrons to fall back on a previous full orbital with 8 valence electrons to satisfy the octet rule.
While elements in tall groups 5,6,7 will gain those valence electrons to fill up outer orbital with 8 valence electrons to satisfy the octet rule.

7. Example: Aluminum Chloride
Criss-Cross Rule
Example: Aluminum Chloride
Step 1:
Aluminum Chloride
write out name with space
Al Cl 3+ 1-
Step 2:
write symbols & charge of elements
Al Cl
Step 3: 1 3
criss-cross charges as subsrcipts
Step 4: AlCl 3
combine as formula unit
(“1” is never shown)

8. Example: Aluminum Sulfide
Criss-Cross Rule
Example: Aluminum Sulfide
Step 1: Aluminum Chloride
Step 2: Al3+ S2-
Step 3: Al S 2 3
Step 4: Al S 2 3

9. Example: Aluminum Oxide
Criss-Cross Rule
Example: Aluminum Oxide
Step 1: Aluminum Oxide
Step 2: Al3+ O2-
Step 3: Al O 2 3
Step 4: Al2O3

10. Example: Magnesium Oxide
Criss-Cross Rule
Example: Magnesium Oxide
Step 1: Magnesium Oxide
Step 2: Mg2+ O2-
Step 3: Mg O 2 2
Step 4: Mg2O2
If you end up with a common denominator then you must reduce!
Step 5: MgO

11. + Ions…explained..
Na Group electron on outer shell O will lose 1 e- to expose the complete inside shell.
Now #e- = 10 but #p+ = 11 so the sodium is an ion with the formula Na1+.
Mg Group electrons on outer shell
Mg will lose 2 e-
Now #e- = 10 but #p+ = 12 so the magnesium is an ion with the formula Mg2+

12. - Ions… explained…
To achieve the octet, atoms with more than 4 electrons on the outer shell will gain enough electrons to reach 8.
Cl Group electrons on outer shell
Cl will gain 1 e- .
Now #e- = 18 but #p+ = 17 so the chlorine is an ion with the formula Cl1-.

13. 10/26 Complete the following table using the periodic table:
Element
Ion formula
Valence e-
Gain or lose # of e-
Ion Name
1. Na
2. Ni
3. P
4. O
5. & 6. Make 2 compounds using the above elements, be sure to write the + one first combined with a - one

14. "GENEROUS"
NON-METALS
METALS
"GREEDY"
with their electrons

15. Naming Ionic Binary Compounds

16. Practice Binary Compounds:
Formula Name
barium oxide
BaO ____________________
________________ sodium bromide
MgI2 ____________________
KCl ____________________
________________ strontium fluoride
________________ cesium fluoride
NaBr
magnesium iodide
potassium chloride
SrF2
CsF

17. (Know this) Binary compounds simplified (when only 2 elements of a metal & a nonmetal) :
Use the following method to determine the formula of an ionic compound:
1. Write the two ions with their charges (metal first).
2. Ignoring the + or – charges, “crisscross” the numbers and make them subscripts.
3. Then, rewrite the formula, dropping the charges.
Then to name binary compounds:
Name the first element
Change the ending of the second element to -ide

18. “Perhaps one of you gentlemen would mind telling me just
what is outside the window that you find so attractive..?”
Image courtesy NearingZero.net

20. Naming binary ionic compounds
The name of the cation (+ charged ion) & write it first, followed by the anion (- charged ion).
The name of the cation is the same as the name of the metal.
The name of the anion (- charged ion) takes the root of the nonmetal name and adds the suffix -ide.
Calcium and oxygen  calcium oxide.
Aluminum and sulfur  aluminum sulfide.

21. Ionic Compounds Ionic Compounds often a metal + nonmetal
anion (nonmetal), change endging to “-ide”
Rules for naming Ionic Compounds
All compound must be neutral UNLESS indicated otherwise.
The cation is always named first and the anion second
The cation takes the name of the element
The anion is named by the root of the element name and changing the ending to “-ide”.
Ex. Chlorine becomes Chloride

22. Examples of Binary Ionic Compounds
Cations (positively charged ions) and anions (negatively charged ions) will associate with each other and form a neutral binary compound to reduce energy .
1 Na Cl NaCl
1 Ca O CaO
3 K N K3N
2 Al S Al2S3

23. Examples BaCl2 barium chloride K2O potassium oxide * Mg(OH)2
magnesium hydroxide
* KNO3
potassium nitrate
* Has more than 2 elements in it, so it has a polyatomic ion present

24. Common Monatomic Cations and Anions
We will start by naming inorganic Binary Compounds—Compounds composed of 2 elements. We will look at both ionic and covalent
Remember compounds want to have a neutral charge
Rules for binary ionic compounds (type I)
The cation is always written first
Monatomic ions (cation) take the name of the element
Monatomic ions (anions) take the root name of the element and add “ide”
Formulas from names
Calcium Hydroxide = Ca(OH)2

25. "GENEROUS"
NON-METALS
METALS
"GREEDY"
with their electrons

26. Keeping Track of Electrons
The electrons responsible for the chemical properties of atoms are those in the outer energy level.
Valence electrons - electrons in the outer energy level.
Core electrons -those in the energy levels below.

27. Keeping Track of Electrons
Atoms in the same column
Have the same outer electron configuration.
Have the same valence electrons.
Easily found by looking up the group number on the periodic table.
Group 2A - Be, Mg, Ca, etc.-
2 valence electrons

28. Lewis or Electron Dot Diagram:
1) Count up total number of valence electrons
2) Connect all atoms with single bonds
- “multiple” atoms usually on outside
- “single” atoms usually in center;
C always in center,
H always on outside.
3) Complete octets on exterior atoms
(not H, though)
4) Check
- all atoms (except H) have an octet;
if not, try multiple bonds
- any extra electrons?
Put on central atom

29. C Lewis Dot Diagram Write the element symbol.
Carbon is in the 4th group, so it has 4 valence electrons.
Starting at the top or the right, draw 4 electrons, or dots, counter-clockwise around the element symbol. C

30. C Lewis Dot Diagram Check your work.
Using your periodic table, check that Carbon is in the 4th group.
You should have 4 total electrons, or dots, drawn in for Carbon. C

31. 11/1 SOME Transition metal & metalloids may have different oxidation charge than just a +2 & require the use a Roman Numeral:
Reverse the subscripts to find the oxidation charge for a metal & write with Roman numerals in ( ) after the metal in the compound name. You can put the (II) even for the +2 ones but not really required to do so.
FeCl2
2 Cl so Fe is +2
Iron(II) chloride
FeCl3
3 Cl so Fe is +3
Iron(III) chloride
Cr2S3
3 S-2 -6 so Cr is +3 (6/2)
chromium(III) sulfide

32. Common Type II Cations Binary Ionic compounds (type II)
There are many metals that form more then one type of cation
So there are more then one type of ionic compound
The Charge on the metal ion must be specified of a metal
Iron (ii) or Iron (III)– the roman numeral indicates the charge of the cation
The cation with the higher charge end in “ic” = Iron (III) Ferric
The cation with the lower charge ends in “ous” = Iron (II) Ferrous
Example Ferric Chloride = Iron (III) Chloride
Ferrous Chloride = Iron (II) Chloride

33. Name the following & check to see if they need a Roman numeral in the name:
If it is a transition metal check the charge
Will it need a Roman Numeral? Do criss cross backward to see
Compound name
1) Fe2O3
2) MnO2
3) Cu3N2
4) V2O3
5) PbS
6)CrO3

34. Write the following compounds from the names:
Compound name
Criss cross method (ask yourself how does that Roman Numeral impact it?)
Formula
7) Iron(III) sulfide
8) Titanium(IV) selenide
9) Lead(IV) chloride
10) Silver (I) nitride
11) Tin (III) iodide

35. 11/1 Polyatomic Ion Compounds – means 3 or more elements present
Ternary compounds are those containing three different elements.
(NaNO3, NH4Cl, etc.). The naming of ternary compounds involves the
memorization of several positive and negative polyatomic ions, (two or
more atoms per ion), and adding these names to the element with which
they combine.
i.e., Sodium ion, Na1+ added to the nitrate ion, NO31-, to give the compound, NaNO3, sodium nitrate.
Binary rules for indicating the oxidation number of metals and for indicating
the numbers of atoms present are followed. The polyatomic ions are listed in
a separate handout.

36. Polyatomic Ions - Memorize
Eight “-ATE’s”
PO43- ……………
SO42- ……………
CO32- …………..
ClO31- …………..
NO31- ………..….
phosphate
sulfate
carbonate
chlorate
nitrate
phosphATE
sulfATE
carbonATE
chlorATE
nitrATE
Exceptions:
ammonium
hydroxide
cyanide
NH41+ ……………
OH1- ……………
CN1- …………..

37. Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion Name Ion Name
NH ammonium CO carbonate
NO nitrite HCO hydrogen carbonate
NO nitrate (“bicarbonate” is a widely
SO sulfite used common name)
SO sulfate ClO hypochlorite
HSO hydrogen sulfate ClO chlorite
(“bisulfate” is a widely ClO chlorate
used common name) ClO perchlorate
OH hydroxide C2H3O acetate
CN cyanide MnO permanganate
PO phosphate Cr2O dichromate
HPO hydrogen phosphate CrO chromate
H2PO dihydrogen phosphate O peroxide
Groups of atoms that bear a net electrical charge
Atoms that make up a polyatomic atom are held together by the same covalent bonds that hold atoms together in molecules
Many more kinds of polyatomic ions than monatomic ions and polyatomic anions are more numerous than polyatomic cations
Method used to predict empirical formula for ionic compounds that contain monatomic ions can be used for compounds containing polyatomic ions. Overall charge on the cations must balance the overall charge on the anions in the formula unit.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100
Print Version

38. Ternary Compounds NaNO2 KClO3 Ca3(PO4)2 Fe(OH)3 NaHCO3 sodium nitrite
potassium chlorate
calcium phosphate
iron (III) hydroxide
sodium bicarbonate
Or sodium hydrogen carbonate

39. Rules for Parentheses Parentheses are used only when the following
two condition are met:
There is a radical (polyatomic ion) present and…
There are two or more of that radical in the formula.
Examples:
NaNO3 NO31- is a radical, but there is only one of it.
Co(NO3)2 NO31- is a radical and there are two of them
(NH4)2SO4 NH41+ is a radical and there are two of them;
SO42- is a radical but there is only one of it.
Co(OH)2 OH1- is a radical and there are two of it.
Al2(CO3)3 CO32- is a radical and there are three of them.
NaOH OH1- is a radical but there is only one of it.

40. 11/2 Check for understanding…
Check all compounds starting with a transition metal or metalloid for the charge that it has & if the charge used in the compound is different than the PT then must add a Roman numeral in the name to clarify the charge used.
   
Write the correct name for each of these compounds:
Fe(OH)2
(NH4)3PO4
AlPO4
Cu(C2H3O2)2
CaCO3
NH4OH
Cr2(SO4)3
Mg(NO3)2

41. Lewis or Electron Dot Diagrams
1. Draw the Lewis dot diagrams for the following: H P Ca Ar Cl Al C

42. 11/4 Ionic or covalent?
IONIC compound: is the transfer of e- that contains a metal and a nonmetal in its formula
The metal will give up e- causing a + charge item to the nonmetal resulting in a – charge part of the compound
Na+1 Cl-1  NaCl
Covalent compound: is the sharing of valence e- that is made up of 2 nonmetal Uses a different set up rules for naming than ionic compounds Ex. CO carbon monoxide

43. 11/7 Identify if the following as ionic or a covalent compound:
1. Fe(OH)4 2. CO2 3. (NH4)3PO4 4. AlPO4 5. Cu(C2H3O2)3 6. I2P5 7. CO3 8. CaCO3 9. NH4OH 10. H20
11. Explain how you know if these are ionic or covalent compounds?

44. Covalent Bonding
Bonds between atoms are formed through the sharing of electrons
Covalent bonds form between two non-metal atoms through sharing of pairs of electrons
Atoms have a “desire” to have their outer energy levels filled (Octet Rule)
Covalent bonding can be represented with Lewis Dot Diagrams

45. Nonmetals hold onto their valence electrons.
11/7 Covalent Naming
Nonmetals hold onto their valence electrons.
They can’t give away electrons to bond.
Get it by sharing valence electrons with each other.
Different from an ionic bond because they actually form molecules.
Called a binary molecular compound
The first vowel is often dropped to avoid the combination of “ao” or “oo”.
CO = carbon monoxide (monooxide

46. Greek Prefixes for Two Nonmetals
YOU must know these:
Greek Prefixes for Two Nonmetals
Number Indicated Prefixes
1 mono-
2 di-
3 tri-
4 tetra-
5 penta-
6 hexa-
7 hepta-
8 octa-
9 nona-
10 deca-

47. Binary Molecular Compounds
N2O dinitrogen monoxide
N2O dinitrogen trioxide
N2O dinitrogen pentoxide
ICl iodine monochloride
ICl iodine trichloride
SO sulfur dioxide
SO sulfur trioxide
Technical Note: Iodine trichloride is actually a dimer with the formula I2Cl6

48. 11/7 Name the following covalent compounds:
1) NO _________________
2) N3O7 _________________
3) N2O3 __nitrogen _____oxide
4) I P _________________
5) ICl4 _________________
6) SO3 _________________
7) SO2 _________________ 2 5

49. Write the covalent formulas for the following:
1. diphosphorous pentoxide
2. Nitrogen trifluoride
3. Dinitrogen pentoxide
4. sulfur dioxide
5. carbon tetrachloride
6. carbon monoxide
7. phosphorous pentabromide

50. 11/9 Draw the Lewis electron dot diagram for the following, include the oxidation charge on each & name them:
1. MgI2
2. CaO
3. NaCl
4. AlF3

51. 11/9 Vocabulary for Chemical Bonding Unit: 1
11/9 Vocabulary for Chemical Bonding Unit: 1. Login to your techbook at
2. Select the unit titled Chemical Bonds
3. Make a vocabulary list from each section and write the definitions and provide an example with each definition or draw a picture
Vocab in each section of the unit:
Definition
Picture or example
Covalent bonding
Ion Formation
Ionic Bonding
Lewis Structures & Molecular Geometry
Metallic Bonding

52. NaCl CO2 Vocabulary CHEMICAL FORMULA IONIC COVALENT formula unit
molecular
formula
NaCl
CO2

53. NaCl NaNO3 Vocabulary COMPOUND more than 2 elements 2 elements binary
ternary
compound
NaCl
NaNO3

54. Na+ NO3- Vocabulary ION 1 atom 2 or more atoms monatomic Ion
polyatomic
Ion
Na+
NO3-
Courtesy Christy Johannesson

55. Naming Simple Chemical Compounds
Ionic (metal and nonmetal)
Covalent (2 nonmetals)
Metal
Nonmetal
First
nonmetal
Second
nonmetal
Forms
only one
positive
ion
Forms
more than
one positive
ion
Single
Negative
Ion
Polyatomic
Ion
Use the
name of
element
Use element
name followed
by a Roman
numeral to
show the charge
Use the name
of the
element, but
end with ide
Use the
name of
polyatomic
ion (ate or
Ite)
Before
element name
use a prefix
to match
subscript
Use a prefix
before
element name
and end
with ide

56. 11/14 Ionic vs. Covalent:
Explain the difference between an ionic compound and a covalent molecule.
Explain how to name ionic compounds when there is only 2 elements present.
Explain how to name ionic compounds when there are more than 2 elements present in the compound.
Explain how to name covalent molecules.
Explain which types of compounds use prefixes in the name and what the prefixes are for 1-10 values.
Explain how to draw a Lewis electron dot structure for an ionic compound.
Explain how to draw a Lewis electron dot structure for a covalent molecule.

57. 8. Name AuCl3 ___________________ 9
8. Name AuCl3 ___________________ 9. Draw the Lewis structure for AuCl3 10. Is AuCl3 ionic or covalent in bonding nature? 11. Draw the Lewis structure for CH2O 12. Is CH2O ionic or covalent? 13. What is CH2O structure name? 14. Explain how you determined the structure of CH2O.

58. 11/15 Lewis Dot Structures & Shape Names: Draw the molecular structures using valence e- & name the shape based on how many lone pair of e- are on the center element
Name & formula
Draw structure with valence e-
How many lone e- pairs are there on the center element?
Name the shape
1. Nitrogen trifluoride, NF3
2. Carbon dioxide, _____
3. _________, CH2O
4. Carbon tetrafluoride, ___
5. ____, NCl3