2. Summary on relationships among elements,
compounds, and other categories of matter

4. Compound - is a substance composed of two or
more elements chemically united in fixed
proportions. It has a constant composition that can
be broken down into elements by chemical
processes.

5. Metals Non Metals
Chemical reactions occur when atoms gain, lose, or share electrons.
Nonmetals _____________ electrons.
This gives them a ____ charge.
Negative ions are called ___________.
Metals ________________ electrons.
This gives them a ____ charge.
Positive ions are called ___________.
gain / accept
-
anion
Lose/donate
+
cation

6. Remember that the charge of an ion can be determined by its
place on the Periodic Table.
1+
2+ 3+
4+
or
4- 3- 2- 1-
0
Look for the roman numeral

7. Common monoatomic ions arranged according to their
positions in the periodic table
1+
2+ 3+
4+
or
4- 3- 2- 1-
0
Look for the roman numeral

8. Naming
Compounds

9. Binary compounds- compounds composed
of two elements.
Binary Ionic Compounds contain a positive ion (cation)
which is always written first in the formula and a negative ion
(anion).

10. NAMING BINARY IONIC
COMPOUNDS

11. Naming Binary Ionic Compounds

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

15. Try this!
1. NaF
2. SrCl2
3. MgO
4. CaO
Sodium fluoride
Strontium chloride
Magnesium oxide
Calcium oxide

16. WRITING FORMULA FROM NAME –
Binary Ionic Compound

17. WRITING FORMULAS FROM NAME
You can determine the formula of an ionic compound from its
name. To do this, REMEMBER THIS RULE:
The subscript of the cation is numerically equal to the charge
on the anion, and the subscript of the anion is numerically
equal to the charge on the cation.

18. magnesium iodide
Step 1: Write the symbol of the metal ion and its charge.
Step 2: Write the symbol of the nonmetal ion and its charge
Step 3: Crisscross the charges.
Step 4: Determine the formula from the ions.
Mg2+
I-
MgI2

19. TRY THIS!
1. Potassium Iodide KI
2. Gallium Bromide GaBr3
3. Calcium Oxide CaO

20. NAMING BINARY IONIC COMPOUNDS (TYPE II)

21. Stock system- the use
of Roman numeral to
indicate the charge of
the cation of the same
element.
Elements that form only one
cation do not need to be
identified by a Roman numeral.

23. 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.

24. a. CuCl
b. HgO
c. Fe2O3
Give the systematic name for each of the following compounds:
Copper(I) chloride
Mercury(II) oxide
Iron(III) oxide

25. WRITING FORMULA FROM
NAME –
type II

26. The charges of the transition metals are important when you are
determining the formula of an ionic compound.
iron (III) oxide
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.
Fe O
3+ -2
Fe2O3

27. TRY THIS!
1. Lead(II) chloride PbCl2
2. Manganese(IV) oxide MnO2

28. 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.

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

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

32. This is just as easy to do with polyatomic ions. You just
need to use the name of the polyatomic ion.
strontium nitrate
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.
Sr NO3
2+ -
Sr(NO3)2

33. Given the following systematic names, write the
formula for each compound:
a. potassium iodide
b. calcium oxide
c. gallium bromide
d. Cesium perchlorate
e. Potassium bromide
KI
CaO
GaBr3
CsClO4
KBr

34. Write the formula of each of the ionic compounds.
KI
SnCl4
BaSO4
NaCl
SrS
CuCO3
AlBr3
Li3N

35. NAMING BINARY COVALENT
COMPOUNDS

36. Non metal
shared
electrons
Chemical reactions occur when atoms gain, lose, or
share electrons.
Sharing electrons creates a covalent bond
Nonmetals can _______ electrons to form a
covalent bond.
share

37. Ionic vs. Covalent
Ionic compounds
contain a metal and
a nonmetal.
Covalent compounds
contain only nonmetals.
What elements do ionic compounds contain?
What elements do covalent compounds
contain?

38. Decide whether the compounds on
your notes are ionic or covalent.
I
C C
C
I
I

39. Important Facts:
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+
Hydrogen can
gain 1
electron.
H-
Hydrogen can
share
electrons.
This means that hydrogen can act as either a
metal or a nonmetal!
H2

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

41. Binary covalent compounds are between 2
different nonmetals.

42. Nonmetals can share electrons in many different ways. This means
that two nonmetals can create multiple compounds together.
CO2
CO
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.
carbon and oxygen
PCl5
PCl3
phosphorous and chlorine
N2O3
N2O4
nitrogen and oxygen

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

44. Steps for Naming
Binary Covalent Compounds
N2O4
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.
nitrogen oxide
dinitrogen tetroxide

45. Rules for Using Prefixes
Rule 1: Prefixes are only used 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.
Rule 3: Remove the -o or -a from a prefix before adding it to
oxide.
Example: CO2 is carbon dioxide, and not
monocarbon dioxide.
Example: CO is carbon monoxide, and not
carbon monooxide.

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

47. Try this!
carbon dioxide
carbon disulfide
phosphorous tribromide
phosphorous pentabromide
diphosphorous pentasulfide
dinitrogen monosulfide
silicon disulfide
nitrogen tribromide
dinitrogen tetrachloride

48. Ready to mix? Try this!
carbon tetrabromide
carbon monosulfide
sodium permanganate
strontium iodide
potassium sulfate
dinitrogen tetrasulfide
magnesium nitrate
silicon tetrachloride
diphosphorous pentoxide

49. Thank You!
Think like a cation and stay
positive!