BOHR DIAGRAMS FOR ATOMS

1
SCIENCE 1206 – UNIT 2 CHEMISTRY November 2012– January 2013
NAMING COMPOUNDS AND WRITING CHEMICAL FORMULAS
NAME:_________________________________________________
OUTLINE
BOHR DIAGRAMS FOR ATOMS
TYPES OF CHEMICAL BONDS
IUPAC
MOLECULAR COMPOUNDS
‣ TYPES
1. SIMPLE COVALENT
2. COMMON NAME
IONIC COMPOUNDS
‣ SIMPLE IONIC
‣ MULTIVALENT
‣ POLYATOMIC/COMPLEX
‣ HYDRATED IONIC
ACIDS
BOHR DIAGRAMS FOR ATOMS
AKA: ______________________________________________________________
_____________________ and _____________________ are found in the nucleus.
_____________________ are found in energy levels
o 1 st level – _____________________
o 2 nd level – _____________________
o 3 rd level – _____________________
atomic # = _____________________
= _____________________
# of n o = __________________________________________
eg. Sodium (Na)
o atomic # =
o mass # =
o # of p + =
_______
_______
_______
o # of e - = _______
o # of n o = ______________

2
VALENCE LEVEL
_________________________________________________________________
Electrons in this level are called _________________________________________
To become more stable, atoms _______________________________ electrons such
that their valence level has the maximum number of electrons.
(ie. they have the electron structure of the nearest inert noble gas.)
Example:
Draw a Bohr diagram for a Li atom:
Example:
Draw a Bohr diagram for a Ne atom:
Example:
Draw a Bohr diagram for a S atom:
Which Bohr diagram above is drawn incorrectly?

3
TYPES OF CHEMICAL BONDS
A CHEMICAL BOND is a ____________________________________________.
2 TYPES of Chemical bonds
o __________________________________
o __________________________________
COVALENT BOND
IONIC BOND
A COVALENT BOND _______________________________________________.
AKA: _______________________________
Occurs between ___________________________________________________.
Solutions of covalently bonded substances are ______________________________.
An IONIC BOND is _________________________________________________
_______________________________.
Usually between ____________________________________________________.
Solutions of ionic bonded substances are __________________________________.
______________________________ consist of atoms or ions of two or more
elements bonded together.
ELECTROLYTES
◦ A solution that _______________________________________________.
◦ General Examples: _____________________________________________
◦ Specific Examples: _____________________________________________
___________________________________________________________
NON-ELECTROLYTES
◦ A solution that _______________________________________________.
◦ General Examples: _____________________________________________
◦ Specific Examples: _____________________________________________

4
IUPAC
________________________________________________________________________
A global organization that _____________________________________________.
One job of the IUPAC is to give compounds _______________________________.
MOLECULAR ELEMENTS
There are 7 elements that are ___________________________, in their natural
state.
___________
___________
___________
___________
___________
___________
___________
Other molecular elements: ___________ ___________
Memory tool: _________________________________
MOLECULAR COMPOUNDS
Composed of ______________________________________________________.
2 TYPES:
o _______________________________________________
o _______________________________________________
BINARY MOLECULAR COMPOUNDS
AKA: ______________________________________________________.
Composed of two types of elements (binary)
Binary Molecular Compounds use IUPAC prefixes to indicate the number of each atom
present:
1 6
2 7
3 8
4 9
5 10

5
Writing the Name from the Molecular Formula
RULES:
1. ________________________________________________________________.
2. ________________________________________________________________.
3. ________________________________________________________________.
examples
o N2O4
o P2O5
o CCl4
o SO3
________________________
________________________
________________________
________________________
Writing the Molecular Formula from the Name
RULES:
1. ________________________________________________________________.
2. ________________________________________________________________.
examples
carbon monoxide
triphosphorus pentabromide
sulfur hexafluoride
dicarbon tetrasulfide
____________
____________
____________
____________

6
TRIVIAL NAME Molecular Compounds
AKA: ____________________________________________________________.
There are SOME molecular compounds that go by their COMMON NAMES, and we
must memorize these names.
Formula
Trivial / Common Name
O 3
H 2 O
H 2 O 2
NH 3
CH 4
CH 3 OH
C 2 H 5 OH
C 6 H 12 O 6
C 12 H 22 O 11
HOMEWORK ALERT!!!
Complete TABLES A, B, C and D in your booklet for HOMEWORK.
Refer to the following notes for help:
Table A
o Writing the Formula from the Name
Table B
o Writing the Name from the Formula
Table C & D
o Everything!
o Watch out for those common name molecular compounds!!!

7
TABLE A.
Writing the Formula from the Name – Molecular Compounds
Name Formula Name Formula
1. chlorine monoxide 11. sulfur dioxide
2. oxygen difluoride 12. carbon tetrafluoride
3. boron phosphide 13. disulfur dichloride
4. dinitrogen monoxide 14. triarsenic dibromide
5. nitrogen trifluoride 15. silicon tetrachloride
6. sulfur tetrachloride 16. xenon hexafluoride
7. xenon trioxide 17. krypton difluoride
8. carbon dioxide 18. dichlorine monoxide
9. diphosphorus pentoxide 19. selenium dioxide
10. phosphorus trichloride 20. dinitrogen pentasulfide
B. Writing the Name from the Formula – Molecular Compounds
Formula Name Formula Name
21. As 4 O 10 31. P 2 O 5
22. BrO 3 32. S 2 Cl 2
23. PH 3 33. ICl 2
24. N 2 O 3 34. SO 2
25. NI 3 35. P 4 S 10
26. SF 6 36. SiF 4
27. N 2 O 5 37. OF 2
28. PCl 3 38. Cl 2 O
29. CO 39. SiO 2
30. PBr 5 40. N 2 S 5

8
C. Write the formulas for the following compounds in the space
provided.
41. carbon dioxide 51. nitrogen monoxide
42. silicon dioxide 52. tetraphosphorus decoxide
43. water 53. silicon monocarbide
44. carbon disulfide 54. methanol
45. ammonia 55. diphosphorus pentabromide
46. carbon tetrachloride 56. arsenic tribromide
47. methane 57. carbon monoxide
48. ozone 58. sulfur dioxide
49. fluorine 59. neon
50. diphosphorus trioxide 60. dinitrogentetroxide
D. Write the names for the following compounds, in the space provided.
61. CBr 4 71. N 2 O
62. I 2 72. C 2 H 5 OH
63. PF 3 73. O 3
64. N 2 O 4 74. Ar
65. CO 75. P 4
66. NH 3 76. ClO 2
67. H 2 O 2 77. SiCl 2
68. SCl 6 78. BH 3
69. SO 3 79. C 2 S 4
70. P 4 O 6 80. OF 2

9
IONS
Atoms other than the ________________________ are ____________________,
and need to _____________________________________ to become more stable.
Sharing electrons results in a _________________________________.
If they ____________________________________, atoms become ___________
and form ______________________________ with other atoms.
WHAT IS AN ION?
Ions are ____________________________ that have lost or gained electrons to
achieve the valence configurations of a noble gas.
OCTET RULE
o ___________________________________________________________
___________________________________________________________.
o NOTE: _____________________________________________________
TWO TYPES OF IONS:
1. CATIONS
o _____________________ ions that form when an atom loses electrons.
o A cation has more __________________ than _____________________
and therefore has a net ___________________________ charge.
o ___________________________ form cations.
o MEMORY TOOL:
___________________________________________________
o EXAMPLE: lithium ion ________________________________
2. ANIONS:
o ______________________ ions that are formed when an atom
_____________ electrons.
o It has more ____________________ than _____________________ and
therefore has a net _____________________ charge.
o ____________________________ form anions.
o NOTE: Change the ending of the name of anions to ___________________.
o MEMORY TOOL: ___________________________________
o EXAMPLE: fluoride ion ______________________________

10
HOMEWORK!!!
Complete TABLE E in your booklet for homework!
Do a few examples in class so that when you go home, you know what you are doing!!!
TABLE E - SIMPLE ION FORMATION
• An ION forms when an atom gains or loses one or more valence electrons. Ions have a FILLED
VALENCE LEVEL resulting in the SAME # OF ELECTRONS AS THE NEAREST NOBLE GAS.
• Positive ions (CATIONS) form when atoms lose electrons.
• Negative ions (ANIONS) form when atoms gain electrons.
• Complete the following table. Remember that the name for an ANION or nonmetallic ion ends
in - ide while the full element name is used for CATIONS (metallic ions).
Ion Name
Ion
Symbol
Number
of p +
Number
of e - Number of e -
lost or gained
Same electrons as
which noble gas
e.g. fluoride F - 9 10 Gained one Ne
1. 53 54
2. 16 Gained two
3. potassium Lost one
4. Ca 2+
5.
35 36
6. Sr 2+
7. H + (none)
8. 8 Gained two
9. 12 Lost two
10. aluminum 10
11. 34 36
12. H -
13. lithium Lost one
14. Rb +
15. 17 18

11
IONIC COMPOUNDS
Composed of a ________________________ and an
______________________________.
Metals form cations when they _______________________ electrons.
Nonmetals form anions by ________________________ electrons.
An ionic bond is the _______________________________ between these
oppositely charged ions.
Ions stay together in _______________________________.
Example: NaCl (Draw on your sheet)
Example: NaCl

12
Ex. How does sodium fluoride form?
3 TYPES:
1. Binary Ionic Compounds
SIMPLE
MULTIVALENT
2. Polyatomic Ionic Compounds
3. Hydrated Ionic Compounds
BINARY IONIC COMPOUNDS
“Binary” means only 2 types of ions involved.
Simple Ionic Compounds
Simple ionic compounds are composed of _________________________________
___________________________.
Given formula, write name
o Rules:
1. ___________________________________________________________
___________________________________________________________
2. ___________________________________________________________
___________________________________________________________
3. ___________________________________________________________
___________________________________________________________
EXAMPLES:
MgBr2
KCl
Na2S
Mg3P2
Ba3N2
_________________________
_________________________
_________________________
_________________________
_________________________

13
EXAMPLES:
WHAT’S WRONG WITH THE FOLLOWING NAMES FOR BaS?
barium sulfur __________________________________________
Barium Sulfide __________________________________________
barium sulfuride __________________________________________
HOMEWORK!
Do TABLE F and G in the booklet for homework.
Follow rules for:
o “GIVEN FORMULA, WRITE NAME” for Ionic Compounds.
TABLE F.
Writing the Name from the Formula – Simple Ionic
Formula Name Formula Name
1. MgS 11. K 2 S
2. KBr 12. LiBr
3. Ba 3 N 2 13. Sr 3 P 2
4. Al 2 O 3 14. BaCl 2
5. NaI 15. NaBr
6. SrF 2 16. MgF 2
7. Li 2 S 17. Na 2 O
8. RaCl 2 18. SrS
9. CaO 19. BN
10. AlP 20. AlN

14
TABLE G
Give the correct chemical formula and name for the compounds possible between the following
ions.
Ion /
Cl - N 3- O 2- S 2- P 3-
name
Na +
Mg 2+
Al 3+
Ca 2+
K +
Zn 2+
Li +
Ba 2+
Ga 3+

15
Simple Ionic Compounds
GIVEN NAME, WRITE FORMULA
o RULES:
1. ______________________________________________________________.
2. ______________________________________________________________.
3. ______________________________________________________________
______________________________________________________________.
4. ______________________________________________________________.
5. ______________________________________________________________.
EXAMPLES:
sodium bromide
_____________________
barium iodide
_____________________
magnesium oxide
_____________________
aluminum oxide
_____________________
HOMEWORK!!!
Complete TABLES H and I for homework!
TABLE H:
o Given NAME, Write FORMULA
TABLE I:
o TOP HALF – Molecular Compound Naming
o BOTTOM HALF – Ionic Compound Naming

16
TABLE H. Writing the Formula from the Name – Simple Ionic
Name Formula Name Formula
1. magnesium oxide 11. cesium sulfide
2. lithium bromide 12. potassium chloride
3. calcium nitride 13. strontium phosphide
4. aluminum sulfide 14. barium iodide
5. potassium iodide 15. sodium fluoride
6. strontium chloride 16. calcium bromide
7. sodium sulfide 17. beryllium oxide
8. radium bromide 18. strontium sulfide
9. magnesium sulfide 19. barium fluoride
10. aluminum nitride 20. aluminum phosphide

Molecular Compounds
Binary Ionic Compounds – Simple Ions
17
TABLE I. Writing the Formula from the Name – Molecular & Simple Ionic
Name Formula Name Formula
1. P 4O 6 11. iodine trifluoride
2. S 2F 10 12. chlorine dioxide
3. N 2O 4 13. methane
4. ICl 5 14. boron trifluoride
5. SF 6 15 diboron hexahydride
6. CH 3OH 16. phosphorous trihydride
7. S 4N 2 17. ethanol
8. H 2O 2 18. carbon disulfide
9. N 2O 3 19. sulfur trioxide
10. NH 3 20. diarsenic trioxide
21. CaCl 2 31. potassium iodide
22. MgO 32. aluminum chloride
23. NaBr 33. lithium nitride
24. Al 2O 3 34. barium chloride
25. CaO 35. magnesium hydride
26. ZnO 36. magnesium chloride
27. Ag 2S 37. sodium sulfide
28. CaF 2 38. zinc sulfide
29. CaH 2 39. potassium chloride
30. K 2S 40. silver bromide

18
MULTIVALENT IONIC COMPOUNDS
Ions of some transition elements can have more than one possible charge.
Such elements are called ____________________________________________.
For example, what are the 2 possible charges for copper – Cu?
o _________________
o _________________
We use _____________________________ to indicate the type of charge on these
multivalent ions.
1+ I
2+ II
3+ III
4+ I V
5+ V
6+ VI
NOTE: ________________________________________________________________
GIVEN NAME, WRITE FORMULA
RULES
1. ___________________________________________________________________________
___________________________________________________________________________
2. ___________________________________________________________________________
___________________________________________________________________________
EXAMPLES:
copper (II) oxide _________________________
lead (IV) sulfide _________________________
tin sulfide _________________________
HOMEWORK!!!
Do Tables J and K on the following pages!
Remember to ONLY use the ROMAN NUMERAL with the MULTIVALENT IONS!!!

19
TABLE J.
Writing the Formula from the Name – Multivalent Ionic
Name Formula Name Formula
1. iron(II) chloride 11. iron(III) chloride
2. copper(I) sulfide 12. copper(II) sulfide
3. lead(IV) iodide 13. lead(II) bromide
4. tin(II) fluoride 14. tin(IV) iodide
5. mercury(I) bromide 15. mercury(II) fluoride
6. nickel(II) oxide 16. nickel(IV) oxide
7. chromium(III) oxide 17. manganese(III) chloride
8. gold(I) iodide 18. chromium(II) nitride
9. manganese(II) nitride 19. gold(III) oxide
10. cobalt(III) phosphide 20. cobalt(II) phosphide
TABLE K
Give the correct chemical formula and name for the compounds possible between the following
ions.
Sn 2+
Cl - N 3- O 2- S 2- B r-
Sn 4+
Ni 2+
Ni 3+
Au 1+
Au 3+
Cu 2+
Cu 1+

20
GIVEN FORMULA, WRITE NAME
RULES
1. ___________________________________________________________
2. ___________________________________________________________.
There are 2 METHODS:
a. METHOD 1
Charges must add up to zero.
b. METHOD 2
Charge of Anion X Subscript of Anion
Subscript of Cation
Examples:
PbI 2 _________________________
Fe 2 O 3 _________________________
CuCl _________________________
MnO 2 _________________________
HOMEWORK!!!
Do Tables L & M for homework!
Remember, doing some workings can help prevent any mistakes!!!

21
TABLE L.
Writing the Name from the Formula – Multivalent Ionic
Formula Name Formula Name
1. NiS 11. CuI 2
2. VBr 4 12. CuBr
3. Mn 3 N 2 13. PbSe
4. Fe 2 O 3 14. Fe 2 Se 3
5. FeI 2 15. NiCl 2
6. Mn 3 P 4 16. MnO 2
7. Cu 2 S 17. Cu 2 Se
8. CuCl 2 18. TiO 2
9. NiO 19. NiSe 2
10. CrF 2 20. CrO
TABLE M. Fill in the proper name or formula of the multivalent ionic
compounds below.
Formula Name Formula Name
eg. CuS
copper (I) sulfide
1. uranium (IV) oxide 11. lead (IV) oxide
2. lead (IV) sulfide 12. HgO
3. SnO 2
13. V 2O 5
4. manganese (IV) oxide 14. tin (II) fluoride
5. Sb 2 S 3
15. chromium (III) oxide
6. iron (III) oxide 16. TiO 2
7. HgS 17. AuF 3
8. PdS 2
18. uranium (VI) bromide
9. copper (II) sulfide 19. NiBr 2
10. FeS 20. cobalt chloride

22
POLYATOMIC IONIC COMPOUNDS
DEFINITION:
_________________________________________________________________
________________________________________________________________.
On the back of your periodic table, there is a POLYATOMIC ION TABLE.
Endings of polyatomic ions are easily recognizable as they are often _______________
or __________________, which provides a good clue.
EXAMPLES:
nitrate
nitrite
cyanide
hydroxide
bicarbonate
chlorate
________
________
________
________
________
________
carbonate
sulfate
phosphate
ammonium
acetate
________
________
________
________
________
GIVEN NAME, WRITE FORMULA
lithium sulfate _____________________
ammonium carbonate _____________________
hydrogen dichromate _____________________
sodium acetate _____________________
GIVEN FORMULA, WRITE NAME
HNO 3 _____________________
NaOH _____________________
KMnO 4 _____________________
Cu 2 SO 4 _____________________
SOME OTHER NAMES . . .
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________

23
HOMEWORK!!! ☻☺
Do Tables N & O for homework!!!
Remember to use the crossover method for charges.
You may find it helpful to use BRACKETS around ALL polyatomic ions when writing the
formulae.
TABLE N. Place the symbol for each ion in the space provided, then write the
correct chemical formula for the ionic compound. Be sure to balance the charges.
Remember complex ions end in -ite, and -ate, except for hydroxide and
ammonium.
Ex : potassium __ K + __ sulfate __ SO4 2- __ __ K 2 SO 4 ___
1. aluminum _________ chloride __________ _______________
2. calcium _________ sulfite __________ _______________
3. sodium _________ phosphate __________ _______________
4. copper(II) _________ nitrate __________ _______________
5. chromium(II) _________ nitride __________ _______________
6. silver _________ chromate __________ _______________
7. nickel(III) _________ iodide __________ _______________
8. barium _________ nitride __________ _______________
9. sodium _________ carbonate __________ _______________
10. zinc _________ acetate __________ _______________
11. magnesium _________ hydroxide __________ _______________
12. iron(III) _________ nitrite __________ _______________
13. mercury(I) _________ oxide __________ _______________
14. copper(II) _________ chlorate __________ _______________
15. potassium _________ tetraborate __________ _______________
16. aluminum _________ bicarbonate __________ _______________
17. lead(II) _________ bisulfate __________ _______________
18. beryllium _________ iodide __________ _______________
19. mercury(II) _________ nitride __________ _______________
20. ammonium _________ oxide __________ _______________
21. iron(II) _________ bromide __________ _______________
22. strontium _________ sulfite __________ _______________
23. nickel(II) _________ hydroxide __________ _______________
24. copper(II) _________ hydrogen sulfate__________ _______________
25. mercury(I) _________ chlorate __________ _______________
26. aluminum _________ carbonate __________ _______________
27. potassium _________ nitrate __________ _______________
28. calcium _________ phosphate __________ _______________

24
TABLE O. Provide the name of the compound or chemical formula.
Chemical
Formula
Compound Name
Chemical
Formula
Compound Name
1. Li2CO3 15. KH2PO4
2. K2SO4 16. potassium hydroxide
3. Al(OH)3 17. lithium phosphate
4. Fe(ClO)3 18. iron (III) hydroxide
5. H2SO4 19. sodium bicarbonate
6. Ca(HCO3)2 20. calcium chlorate
7. Pb3(PO4)2 21. hydrogen borate
8. Zn(CH3COO)2
22. ammonium nitrate
9. Cu(NO3)2
23. sodium hypochlorite
10. Cu(NO2)2
24. potassium nitrate
11. K2S2O3
12. CaCO3
25. calcium cyanide
26. chromium (III) nitrite
13. Na2Cr2O7
27. iron (II) chlorite
14. NaCN

25
HYDRATED IONIC COMPOUNDS
Hydrated ionic compounds have ___________________ attached to their crystal lattice
structure.
Solutions become hydrated when they are crystallized from a water solution.
They are often recognizable by eye because they are often ____________________ and
_____________________________.
Examples: _______________________________________________________________
BLUESTONE CuSO 4 • 5H 2 O
o _________________________________________________________________.
o _________________________________________________________________.
We indicate the presence of water with the word ______________________________
and we indicate the number of water molecules with our GREEK PREFIXES:
o __________________________________________________________________
__________________________________________________________________
ANHYDROUS: __________________________________________________________
GIVEN NAME, WRITE FORMULA
barium chloride dehydrate _____________________
potassium hydroxide hexahydrate _____________________
sodium carbonate octahydrate _____________________
cobalt (II) chloride decahydrate _____________________
GIVEN FORMULA, WRITE NAME
CaSO 4 • 2H 2 O ________________________________________
Na 3 PO 4 • 4H 2 O ________________________________________
HCN • 3H 2 O ________________________________________
HOMEWORK:
COMPLETE TABLE P ON THE NEXT PAGE OF YOUR HANDOUT.

26
TABLE P.
Provide the name or formula for each of the following.
Compound Name
Formula
1. copper (II) sulfate pentahydrate
MgSO 4 • 7 H 2 O
3. potassium carbonate octahydrate
MgCl 2 • 6 H 2 O
5. barium chloride dehydrate
Cd(NO 3 ) 2 • 4 H 2 O
7. lithium bromide trihydrate
Na 2 S 2 O 3 • 5 H 2 O
9. cobalt (II) chloride hexahydrate
AlCl 3 • 6 H 2 O
11.zinc sulfate nonahydrate
CaCl 2 • 2 H 2 O
13.barium hydroxide monohydrate
Na 2 SO 4 • 10 H 2 O
15.magnesium silicate pentahydrate