1. Naming Ionic Compounds

2. Chemical reactions occur when atoms gain, lose, or share electrons.
Metals
Nonmetals
Nonmetals _____________ electrons.
This gives them a ____ charge.
Negative ions are called ___________.
gain / accept _
anions
Metals ________________ electrons.
This gives them a ____ charge.
Positive ions are called ___________.
lose / donate +
cations

3. Look for the Roman Numeral!
Remember that the charge of an ion can be determined by its place on the Periodic Table. +1 +4 or -4 +2 +3 -3 -2 -1
Look for the Roman Numeral!

4. For each elements on your notes, predict the charge of its most common ion using the periodic table.-3 +2 +2 -1 +1 +2 -1 -2 +1 -1 -2 +1 -3 +1 -1

5. Na Na+ + e- Mg Mg+2 + 2e- Rules for Naming Ions
When metals lose electrons they become ions, but their name does not change. Na
Na+ + e-
electron
sodium
sodium Mg
Mg e-
2 electrons
magnesium
magnesium

6. F + e- F- S + 2e- S-2 Rules for Naming Ions
When nonmetals gain electrons they become ions, and their name does change.
F e- F-
fluoride
fluorine
electron
S e-
S-2
sulfur
2 electrons
sulfide

7. chlor- + -ide = chloride
Rules for Naming Ions
1. The names of metals do not change.
2. Changing the name of nonmetals:
root of element name ide = name of ion
Examples:
The name of chlorine’s ion:
chlor ide = chloride
The name of nitrogen’s ion:
nitr ide = nitride

8. Examples of naming ions:
The name of calcium’s ion:
calcium
(The names of metals don’t change!)
The name of oxygen’s ion:
ox ide = oxide
The name of aluminum’s ion:
aluminum
(The names of metals don’t change!)

9. Write the name of each of the ions on your notes.
sulfide
lithium
nitride
bromide
potassium
chloride
oxide
hydrogen (+), hydride (-)

10. There are also ions that form after elements have shared electrons
There are also ions that form after elements have shared electrons. These ions are known as polyatomic ions, and each polyatomic ion already has a name.

11. Write the name of each of the polyatomic ions on your notes using your reference sheet as a guide.
sulfate
carbonate
permanganate
sulfite
hydroxide
nitrate

12. Steps for Naming Ionic Compounds
CaBr2
calcium
bromide
Step 1: Write the name of the metal ion.
Step 2: Write the name of the nonmetal ion.
Step 3: YOU ARE DONE! It is that easy.

13. 1. NaF
2. MgO
sodium
fluoride
magnesium
oxide
3. SrCl2
4. Li2S
strontium
chloride
lithium
sulfide
5. CaO
6. KI
calcium
oxide
potassium
iodide

14. When polyatomic ions are used, simply use the name of the polyatomic ion in the compound.
1. NH4F
2. CaSO4
ammonium
fluoride
calcium
sulfate
3. Mg(NO3)2
4. NaOH
magnesium
nitrate
sodium
hydroxide

15. Name the ionic compounds that are found on your notes.
calcium chloride
potassium sulfide
potassium permanganate
barium oxide
ammonium chloride
cesium chloride
magnesium sulfate
sodium bromide
aluminum phosphide

16. Mg I +2 - MgI2 magnesium iodide
You can also determine the formula of an ionic compound from its name. To do this, you will need to use what you already know about the Periodic Table.
magnesium iodide Mg I +2 -
MgI2
Step 1: Write the symbol of the metal ion.
Step 2: Write the symbol of the nonmetal ion.
Step 3: Determine the charges using the periodic table.
Step 4: Determine the formula from the ions.

17. Sr NO3 +2 - Sr(NO3)2 strontium nitrate
This is just as easy to do with polyatomic ions. You just need to use the name of the polyatomic ion.
strontium nitrate Sr
NO3 +2 -
Sr(NO3)2
Step 1: Write the symbol of the metal ion.
Step 2: Write the formula of the polyatomic ion.
Step 3: Determine the charges using the periodic table and the table of polyatomic ions.
Step 4: Determine the formula from the ions.

18. N-3 NO3- S-2 SO3-2 P-3 PO4-3 nitrate nitride sulfide sulfite phosphate
Be very careful that you do not mix up the names of ions. This is very common for beginners to naming.
Decide which name goes with each ion.
nitrate
N-3
NO3-
nitride
sulfide
S-2
SO3-2
sulfite
phosphate
P-3
PO4-3
phosphide

19. We know they are positive because metals are always positive.
Remember that the names of transition metals include their charge because their charges are less predictable.
What are the charges of the transition metals below:
Iron (II) _______ Iron (III) _______
Copper (II) _______ Copper (I) _______
Tin (IV) _______ Tin (II) _______
Lead (II) _______ Lead (IV) _______ +2 +3 +2 +1 +4 +2 +2 +4
We know they are positive because metals are always positive.

20. Fe O +3 -2 Fe2O3 iron (III) oxide
The charges of the transition metals are important when you are determining the formula of an ionic compound.
iron (III) oxide Fe O +3 -2
Fe2O3
Step 1: Write the symbol of the cation.
Step 2: Write the symbol of the anion.
Step 3: Determine the charges using the periodic table and the roman numerals.
Step 4: Determine the formula from the ions.

21. SO4-2 S-2 SO3-2 N-3 NO2- NO3- Helpful Hint:
If the ion ends in –ide, it is probably from the periodic table. If the ion ends in –ate or –ite, it is a polyatomic ion.
Examples:
sulfate
sulfide
sulfite
SO4-2
S-2
SO3-2
nitride
nitrite
nitrate
N-3
NO2-
NO3-

22. Write the formula of each of the ionic compounds named on your notes.KI
SnCl4
BaSO4
NaCl
SrS
CuCO3
AlBr3
Li3N

23. Naming Binary Covalent Compounds23

24. Chemical reactions occur when atoms gain, lose, or share electrons.
shared electrons
Nonmetals
Chemical reactions occur when atoms gain, lose, or share electrons.
Sharing electrons creates a covalent bond
Nonmetals can _______ electrons to form a covalent bond.
This creates a ___________.
share
molecule 24

25. Determining if a compound is ionic or covalent is easy.
What elements do covalent compounds contain?
Covalent compounds contain only nonmetals.
What elements do ionic compounds contain?
Ionic compounds contain a metal and a nonmetal. 25

26. Decide whether the compounds on your notes are ionic or covalent.26

27. Important Facts: H+ H2 H-
Because hydrogen only has 1 proton and 1 electron, it behaves differently than any other element on the periodic table of elements.
Hydrogen can donate its 1 electron. H+ H2
Hydrogen can share electrons.
Hydrogen can gain 1 electron. H-
This means that hydrogen can act as either a metal or a nonmetal! 27

28. There are 7 elements that exist in nature as diatomic molecules.
What elements exist as diatomic molecules?
H2, N2, O2, F2, Cl2, Br2, I2 28

29. Binary Covalent Compounds
There are millions of covalent compounds. These can be classified into many different types of compounds. Each type of compound has a different set of rules for naming. You will be learning about the easiest type of covalent compound to name:
Binary Covalent Compounds
What does binary mean?
Binary means 2.
Binary covalent compounds are between 2 different nonmetals. 29

30. phosphorous and chlorine
Nonmetals can share electrons in many different ways. This means that two nonmetals can create multiple compounds together.
carbon and oxygen
phosphorous and chlorine CO
CO2
PCl3
PCl5
nitrogen and oxygen
N2O4
N2O3
Each of these contains a different ratio of elements. Because of this, we have to make sure that the name of the compound explains the correct ratio. 30

31. To show the correct ratio of elements, we use prefixes.31

32. Binary Covalent Compounds
Steps for Naming
Binary Covalent Compounds
N2O4
dinitrogen
nitrogen
tetroxide
oxide
Step 1: Write the name of the first nonmetal.
Step 2: Write the name of the second nonmetal changing its ending to -ide.
Step 3: Add prefixes to specify how many of each element are present. 32

33. Rules for Using Prefixes
Rule 1: Prefixes are only for BINARY COVALENT compounds.
Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1.
Example: CO2 is carbon dioxide, and not monocarbon dioxide.
Rule 3: Remove the -o or -a from a prefix before adding it to oxide.
Example: CO is carbon monoxide, and not carbon monooxide. 33

34. How would you write each of the prefixes in front of oxide?
Remember: Remove the -o or -a from a prefix before adding it to oxide. Leave -i alone.
mono- ____________ di- ____________
tri- ____________ tetra- ____________
penta- ____________ hexa- ____________
hepta- ____________ octa- ____________
nona- ____________ deca- ____________
monoxide
dioxide
trioxide
tetroxide
pentoxide
hexoxide
heptoxide
octoxide
nonoxide
decoxide 34

35. Name the binary covalent compounds that are found on your notes.
carbon dioxide
carbon disulfide
phosphorous tribromide
phosphorous pentabromide
diphosphorous pentasulfide
dinitrogen monosulfide
silicon disulfide
nitrogen tribromide
dinitrogen tetrachloride 35

36. dinitrogen tetrafluoride
Because of the prefixes, it is very easy to go from the name of a binary covalent compound to its formula.
dinitrogen tetrafluoride N2 F4
Step 1: Write the symbol of the first nonmetal and the subscript that matches the prefix.
Step 2: Write the symbol of the second nonmetal and the subscript that matches the prefix. 36

37. Write the formulas of the binary covalent compounds in your notes.
CCl4
IF7
PCl5
N2O4
N2O
PCl3 CS CO
BH3
ICl
S2Br6
S4N4
H2O
SiS2
PI3
ClF5
NCl3
NO2 37

38. Naming Ionic and Covalent Compounds Review38

39. Chemical reactions occur when atoms gain, lose, or share electrons.
This is what creates compounds!
Nonmetals _____________ electrons.
This gives them a ____ charge.
Negative ions are called ___________.
gain / accept _
anions
Metals ________________ electrons.
This gives them a ____ charge.
Positive ions are called ___________.
lose / donate +
cations 39

40. Ionic compounds contain a metal and a nonmetal.
What elements do ionic compounds contain?
Ionic compounds contain a metal and a nonmetal.
Nonmetals
Metals 40

41. MgCl2 Steps for Naming Ionic Compounds YOU ARE DONE! It is that easy.
magnesium
chloride
Step 1: Write the name of the metal ion.
Step 2: Write the name of the nonmetal ion.
Remember that we change the name of nonmetal ions to –ide.
YOU ARE DONE! It is that easy. 41

42. Chemical reactions occur when atoms gain, lose, or share electrons.
shared electrons
Nonmetals
Chemical reactions occur when atoms gain, lose, or share electrons.
Sharing electrons creates a covalent bond
Nonmetals can _______ electrons to form a covalent bond.
This creates a ___________.
share
molecule 42

43. What elements do covalent compounds contain?
Covalent compounds contain only nonmetals.
Nonmetals 43

44. Steps for Naming Covalent Compounds
diphosphorous
phosphorous
tetrasulfide
sulfide
Step 1: Write the name of the first nonmetal.
Step 2: Write the name of the second nonmetal changing its ending to -ide.
Step 3: Add prefixes to specify how many of each element are present. 44

45. Rules for Using Prefixes with
Covalent Compounds
Rule 1: Prefixes are only for COVALENT compounds.
Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1.
Example: PCl3 is phosphorous trichloride, and not monophosphorous trichloride.
Rule 3: Remove the -o or -a from a prefix before adding it to oxide.
Example: N2O4 is nitrogen tetroxide, and not nitrogen tetraoxide. 45

46. Determining if a compound is ionic or covalent is easy.
What elements do ionic compounds contain?
Ionic compounds contain a metal and a nonmetal.
What elements do covalent compounds contain?
Covalent compounds contain only nonmetals. 46

47. Decide whether the compounds on your notes are ionic or covalent.47

48. Only COVALENT COMPOUNDS use PREFIXES!
Once you decide if a compound is ionic or covalent you know whether or not to use prefixes.
Only COVALENT COMPOUNDS use PREFIXES!
Do NOT make the mistake of using prefixes with ionic compounds. You will be forced to decide between answer choices with and without prefixes on your exam. Know the difference! 48

49. Steps for Naming a Compound
Step 1: Decide if the compound is ionic or covalent.
Step 2: Write the name of the first element as it appears on the periodic table, change the name of the second element to end with -ide.
Ionic compounds are finished at this point.
Step 3: If, and only if, the compound is covalent, add prefixes. 49

50. Remember, if polyatomic ions appear in an ionic compound, simply use the name of the ion as it appears in the table of polyatomic ions.
1. NH4Cl
2. MgSO3
ammonium
chloride
magnesium
sulfite
3. Ca(NO2)2
4. KOH
calcium
nitrite
potassium
hydroxide 50

51. Write the names of the compounds that appear on your notes.
carbon tetrabromide
carbon monosulfide
sodium permanganate
strontium iodide
potassium sulfate
dinitrogen tetrasulfide
magnesium nitrate
silicon tetrachloride
diphosphorous pentoxide 51

52. Determining the Formula of an Ionic Compound from Its Name
potassium sulfide K S + -2
K2S
Step 1: Write the symbol of the metal ion.
Step 2: Write the symbol of the nonmetal ion.
Step 3: Determine the charges using the periodic table.
Step 4: Determine the formula from the ions. 52

53. The charges are the same, so they cancel!
This is just as easy to do with polyatomic ions. You just need to use the table of polyatomic ions found on the naming compounds reference sheet.
barium sulfate
The charges are the same, so they cancel! Ba
SO4 +2 -2
BaSO4
Step 1: Write the symbol of the metal ion.
Step 2: Write the formula of the polyatomic ion.
Step 3: Determine the charges using the periodic table and the table of polyatomic ions.
Step 4: Determine the formula from the ions. 53

54. S-2 SO4-2 P-3 PO4-3 N-3 NO2- sulfide sulfate phosphate phosphide
Be very careful that you do not mix up the names of ions. This is very common for beginners to naming.
Decide which name goes with each ion.
sulfide
S-2
SO4-2
sulfate
phosphate
P-3
PO4-3
phosphide
nitrite
N-3
NO2-
nitride 54

55. We know they are positive because metals are always positive.
Remember that the names of transition metals include their charge because their charges are less predictable.
What are the charges of the transition metals below:
d-block
Tin (IV) _______ Tin (II) _______
Lead (II) _______ Lead (IV) _______
Iron (II) _______ Iron (III) _______
Copper (II) _______ Copper (I) _______ +4 +2 +4 +2 +2 +3 +2 +1
We know they are positive because metals are always positive. 55

56. Cu NO3 +2 - Cu(NO3)2 copper (II) nitrate
The charges of the transition metals are important when you are determining the formula of an ionic compound.
copper (II) nitrate Cu
NO3 +2 -
Cu(NO3)2
Step 1: Write the symbol of the metal ion.
Step 2: Write the symbol of the polyatomic ion.
Step 3: Determine the charges using the periodic table, polyatomic ions table, or the roman numerals.
Step 4: Determine the formula from the ions. 56

57. Because of the prefixes, it is very easy to go from the name of a binary covalent compound to its formula.
dihydrogen monoxide H2 O
Step 1: Write the symbol of the first nonmetal and the subscript that matches the prefix.
Step 2: Write the symbol of the second nonmetal and the subscript that matches the prefix. 57

58. Example: carbon dioxide
Remember: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1.
Example: carbon dioxide
CO2 58

59. Write the formulas of the compounds that appear on your notes based on their names.
HCl
BaF2
SnS
N2O
CS2
S2Cl6
Na3PO4
PtCl2 59

60. Naming Acids

61. Binary Acids
Contain only two atoms, one is hydrogen, another is an anion
The names of these anions all end in –IDE
These acids become hydro _______ic acids
Fill in the blank with the root of the anion

62. Hydro ____ ic Acid HCl (hydrogen chloride) HBr (hydrogen bromide)
HF (hydrogen fluoride)
HI ( hydrogen iodide)
HCN (not a binary acid, but still ends in an –ide ending)-(hydrogen cyanide)

63. Hydro _______ ic Acids HCl (hydrogen chloride) HBr (hydrogen bromide)
Hydrochloric acid
HBr (hydrogen bromide)
Hydrobromic acid
HF (hydrogen fluoride)
Hydrofluoric acid
HI ( hydrogen iodide)
Hydroiodic acid
HCN (not a binary acid, but still ends in an –ide ending)-(hydrogen cyanide)
Hydrocyanic acid

64. Oxyacids
These acids contain a radical group that has oxygen as part of its formula
These radical group names end in both
-ate, and –ite
The more oxygen atoms the anion has in an acid the stronger the acid will be.
HNO3 and HNO2

65. Radical groups that end in -ATE
These acids are named by using the template _______ ic acid

66. _______ ic acid HNO3 H2SO4 H2CO3 Hydrogen nitrate Nitric acid
Hydrogren sulfate sulfuric acid
H2CO3
Hydrogen carbonate carbonic acid

67. Groups that end in -ITE
Acids that have traditional names that end in –ite will use the template ____ ous acid

68. ---------- ous acid HNO2 (hydrogen nitrite) H2SO3 (hydrogen sulfite)
H3PO3 (hydrogen phosphite)

69. More/less oxygens than ate or ite
HClO4 (hydrogen perchlorate)
HClO3 (hydrogen chlorate)**
HClO2 (hydrogen chlorite)**
HClO (hydrogen hypochlorite)

70. HClO4 (hydrogen perchlorate)
HClO3 (hydrogen chlorate)
HClO2 (hydrogen chlorite)
HClO (hydrogen hypochlorite)
Per _______ ic
_______ic
_______ous
Hypo______ous

71. HIO3 (hydrogen iodate)
HIO2 (hydrogen iodite)
HIO (hydgrogen hypoiodite)
_____ ic acid
_____ous acid
Hypo____ous acid