Chemical Names,
Formulas and Bonding
General Chem
Re: 10/11 JG
Covalent Naming
Nonmetal-nonmetal
Share electrons
No ions- nothing to balance
Name must tell elements and amounts
Rules:
Divide formula in half
Name first element
Name second element change the ending to -IDE
Use Greek prefixes to identify subscripts
(Mono is optional for first element, required with
Common Prefixes
1-mono
6-hexa
2-di
7-hepta
3-tri
8-octa
4-tetra
9-nona
5-penta
10-deca
second element)
Common “-Ide” Names
bromide
iodide
selenide
hydride
carbide
nitride
oxide
fluoride
phosphide
sulfide
chloride
Sample:
CO (mono)carbon monoxide
Name:
1. P4O10
tetraphosphorus decaoxide
5. SO3
2. N2H4
dinitrogen tetrahydride
6. N2O6
3. SF6
7. NO
4. C3H8
8. SO2
Write formulas for the following:
9. chlorine dioxide
10. dichlorine monoxide
ClO2
Cl2O
11. iodine tribromide
12. nitrogen trioxide
13. diphosphorus tetraoxide
14. carbon tetrafluoride
Covalent Formula Writing and Naming
Write the correct name or formula for each of the following:
1. dinitrogen trioxide __________________
21. P2O5 ________________________
2. sulfur trioxide ______________________
22. N2S3 _________________________
3. carbon dioxide _____________________
23. CCl4 _________________________
4. tetraphosphorus decasulfide __________
24. CO3 __________________________
5. sulfur hexafluoride __________________
25. PBr3 __________________________
6. oxygen difluoride ____________________
26. CO ___________________________
7. dinitrogen tetraoxide ___________________
27. SCl2 __________________________
8. sulfur dioxide _______________________
28. S2Cl2 _________________________
9. diarsenic trioxide ____________________
29. N2O4 _________________________
10. disulfur dichloride ___________________
30. ClF3 __________________________
11. dinitrogen pentoxide __________________
31. SiCl4 __________________________
12. sulfur diiodide ______________________
32. SO4 ___________________________
13. nitrogen dioxide ______________________
33. N2O5 __________________________
14. iodine monochloride ___________________
34. Cl2O ___________________________
15. silicon tetrabromide __________________
35. NO ___________________________
16. selenium difluoride __________________
36. NO2 __________________________
17. carbon disulfide _____________________
37. ClO6 __________________________
18. dinitrogen trisulfide __________________
38. N2Cl4 __________________________
19. silicon disulfide _____________________
39. N2O ___________________________
20. diarsenic trisulfide _________________
40. PCl5 ___________________________
NOTES:
NOTES:
ELECTRON DOT FORMULA WORKSHEET
Background: Covalent bonding is formed between nonmetals and nonmetals. A covalent bond is
a shared pair of electrons. Atoms share electrons to obtain an electron configuration of a noble
gas, this allows the atoms to become more stable. Molecules can be represented by means of
diagrams in which VALENCE electrons are shown as dots around the chemical symbols of the atoms
and bonds are represented as lines. (This is especially useful when diagramming covalent bonds.)
Historical Note:
The dot formulas are sometimes referred to as Lewis Dot Structures after the
chemist who first introduced them in 1916---G.N. Lewis.
Rules:
1. Determine the total number of valence electrons.
2. Draw a skeleton structure:
Aim for symmetry.
Be sure to include all elements in the formula!!
Do not string out oxygens. Do not make boxes.
3. Each bond - represents 2 electrons
4. Place electrons as dots around atoms to achieve stable octets (8) and
stable duets (2) for hydrogen. Exceptions: 4 for Be and 6 for B
6. Be sure the total number of electrons in the diagram equals the original
number of total valence electrons.
Examples:
1.
Nitrogen = N = group 5 (periodic table) = 5 valence electrons
Electron Dot Formula
2.
Cl2 = group 7(periodic table)
2 atoms Cl x 7 valence electrons = 14 total valence electrons
Electron Dot Formula
3.
H 2O
H = group 1 = 1 valence electron
O= group 6 = 6 valence electrons
H = 2 atoms H X 1 valence electron =
2 valence electrons
O = 1 atom O X 6 valence electron = + 6 valence electrons
8 total valence electrons
Electron Dot Formula
1. Draw the electron dot structures for the following atoms.
a)
F
b)
Cl
c)
P
d)
O
e)
C
f)
N
g)
H
h)
Br
2. 1. Name the compound
2.draw the electron dot structures
3.state the geometric shape for the following molecules.
a) Br2 name & shape
b) HCl name & shape
c)CH4 name & shape
d) NH3 name & shape
e) H2S name & shape
f) SiF4 name & shape
g) PF3 name & shape
h)C2H6 name & shape
i)C2Cl2H4
j) N2H4 name
k) C5H12 name
l) Cl2O name & shape
The Saga Continues
Single Bonds:
Cl2
one pair of electrons shared between bonding atoms
14 total valence electrons
Double Bonds: two pairs of electrons shared between bonding atoms
O2
12 total valence electrons
Triple Bonds: Three pairs of electrons shared between bonding atoms
N2
10 total valence electrons
All atoms still need to achieve a stable octet (or duet for H).
Follow all bonding rules.
Draw electron dot structures for the following compounds.
1. CO2 name
2. SiS2 name
3. C2H4 name
4. H2CO
5. H2C2O2
6. NH4+1 shape
7. N2O2 name
8. HCN name
9. C2H2 name
10. C2H5OH
11. C2H3OH
12. C2N2 name
13. OH-1
14. CN-1
More Dot Structures
1. CF4 shape, name
2. CH2Cl2 shape
3. PF3 shape, name
4. H2S shape, name
5. F2 shape , name
6. N2H4 name
7. CH3COOH
8. CH3NH2
9. C3H4 name
10. CCl2O
11. CH3CN
12. P2H2 name
13. CS2 name
14. N2O2 name
15. C2H3O
16. SI2 name, shape
Ionic Compounds
There are four places to find the charge of an ion:
1. The main block elements
2. The Roman numerals
3. The polyatomic ion sheet
4. Determine the charge from the other ions in the compound.
All compounds have a net charge of zero.
How to Write Ionic Formulas
Ex: Determine the chemical formula for magnesium oxide.
1. Always write the cation first then the anion. To find the ionic charge look at
your main block elements, the Roman numerals, and/or your polyatomic ion
sheet.
Mg+2 O -2
2.Write the compound using subscripts so that the net charge is equal to
ZERO
MgO
Ex : Determine the chemical formula for ammonium carbonate
1. Always write the cation first then the anion. To find the ionic charge look at
your mainblock elements, the Roman numerals, and/or your polyatomic ion
sheet.
(NH4)+1
(CO3)-2
2.NEVER CHANGE THE POLYATOMIC ION.For multiple polyatomic ions use ( ).
The net charge of the compound must equal zero.
(NH4)2CO3
How to Name Ionic Compounds.
Ex: Write the chemical name for CaCl2
1. Write the cation first
calcium
2. If the cation is a transition metal, tin(Sn), lead(Pb), animony(Sb), or
bismuth(Bi). Write the charge as a Roman numeral.
does not apply
3. Write the anion. If the ion is a nonmetal element change the ending to -ide.
calcium chloride
Ex: Write the chemical name for PbO
1. Write the cation first
lead
2.If the cation is a transition metal, tin(Sn), lead(Pb), animony(Sb), or
bismuth(Bi). Write the charge as a Roman numeral.
lead(II)
3. Write the anion. If the ion is a nonmetal element change the ending to -ide.
lead(II) oxide
Ex: Write the chemical name for (NH4)2SO4
1. Write the cation first(taken form the polyatomic ion sheet)
ammonium
2. If the cation is a transition metal, tin(Sn), or lead(Pb) Write the charge as a
Roman numeral.
does not apply
3. Write the anion. If the ion is a nonmetal element change the ending to -ide.
ammonium sulfate
ex:
MgO
Fe2(CO3)3
AuN
AgC2H3O2
magnesium oxide
iron(III) carbonate
gold(III)nitride
silver acetate
NOTES:
NOTES:
Ionic Formula Writing
1. Al
+3
Br _____________
-1
21. lead(II) chloride ____________
2. Al+3 (C2H3O2)-1 ___________
22. silver nitrate ____________
3. Ba+2 S-2 ______________
23. mercury(II) iodide ___________
4. (NH4)+1 (NO3)-1 ___________
24. strontium nitrite ___________
5. Ca+2
I-1 ______________
25. barium sulfate ____________
6. Cr+3
F-1 _________
26. tin(IV) sulfide ___________
7. (NH4)+1 (OH)-1 ________
27. copper(II) chlorate _________
8. Cu+1
28. iron(II) oxide ___________
Cl-1 _________
9. H+1
S-2__________
29. lead(II) bromide ____________
10. K+1
(OH)-1 __________
30. iron(III) phosphate __________
11. H+1 (CO3)-2 ____________
31. lead(II) chromate ___________
12. Hg+1 (C2H3O2)-1 ____________
32. magnesium fluoride __________
13. Cu+1
S-2 ______________
33. hydrogen bromide ___________
14. Al+3 O-2 _____________
34. magnesium sulfide __________
15. Sn+2 O-2 _______________
35. lithium iodide ______________
16. Ag+1 Cl-1 _________
36. silver carbonate __________
17. Ca+2 (PO4)-3 ____________
37. zinc sulfite _____________
18. Ba+2 (Cr2O7)-2 ____________
38. iron(II) chlorate ____________
19. Bi+3 (AsO4)-3 __________
39. barium oxide _____________
20. Na+1 (ClO)-1 ____________
40. ammonium phospate __________
Ionic Naming
1. CaCl2 ________________
21. PbCl2 ________________
2. Al2O3 ________________
22.Sr(NO3)2_______________
3. Na2S ________________
23. AuI3 ________________
4. FeS ________________
24. CuO ________________
5. NH4NO2 ________________
25. HgBr ________________
6. Ba3N2 ________________
26. BeSO4 ______________
7. AlF3 ________________
27. Co3N ________________
8. Ca3P2 ________________
28. AuI ________________
9. K2CO3 ________________
29. W2O3 ________________
10. KI ________________
30. Co(OH)2 ______________
11. Li2C2O4 ________________
31. SnF4 ________________
12. SrBr2 ________________
32. AgCl ________________
13. FeCl3 ________________
33. CuO ________________
14. AgNO3 ________________
34.Al2(CO3)3_______________
15. MgSO3 ________________
35. Cu2O ________________
16. CdI2 ________________
36. AlN ________________
17. BaSO4 ________________
37. Pb(CO3)2 ______________
18. Fe2S3 ________________
38. K3N ________________
19. SnO ________________
39. Au3PO4 ______________
20. Be(C2H3O2)2 ________________
40. NaCl ________________
Ionic Roman # & Polyatomics
Write the following compounds:
1. beryllium nitrate ___________________________________
2. manganese (II)iodide___________________________________
3. chromium (III) sulfide _________________________________
4. lithium chromate
________________________________
5. ammonium chloride
_____________________________
6. copper (I) phosphide _________________________________
7. sodium phosphate
_________________________________
8. iron (III) hydroxide___________________________________
9. zinc sulfite
_________________________________
10. gold (II) acetate
_________________________________
Name the following compounds:
1. FeCl2
____________________________________
2. CrO
____________________________________
3. Mg(OH)2 ____________________________________
4. Ca(NO2)2 ____________________________________
5. NiBr2
____________________________________
6. Cu2SO4
____________________________________
7. HgCO3
____________________________________
8. K2CO3
____________________________________
9. (NH4)2O ____________________________________
10. SnI4
____________________________________
Ionic Naming
Provide the formula for the following:
1. potassium phosphate ______________________
6. Ca3N2___________
2. iron (III) chloride
______________________
7. Li2SO4___________
3. mercury (I) oxide
______________________
8. Ni(CN)2___________
4. aluminum carbonate ______________________
9. SnF4 ___________
5. sodium chromate
10. Sr(NO3)2_________
______________________
Each of the following name-formula pairs is incorrect. Determine what is wrong
with the pair, write a sentence explaining what is wrong, and then provide the
correct name or formula as needed.
11. PbCl2 – lead chloride
12. CuO – copper (I) oxide
13. Co3(PO4)2 – carbonate phosphate
14. CdI2 – cadmium (II) iodide
15. NH4NO2 – nitrogen tetrahydride mono nitrogen dioxide
16. copper (II) chlorate – Cu2ClO3
17. lithium iodide – LiIO3
18. barium oxide – BaO2
19. lead (III) sulfide – Pb2(SO4)2
20. hydrogen bromide – H2Br
Mixed Practice
Ionic vs. Covalent Compounds
Is the compound ionic or covalent?
1. CO
_______________________
Name the following compounds:
_______________________
2. BaI2
_______________________
_______________________
3. CrF3
_______________________
_______________________
4. CaCrO4
_______________________
_______________________
5. Cu(OH)2 _______________________
_______________________
6. N2O3
_______________________
_______________________
7. SrO
_______________________
_______________________
8. NH4Br
_______________________
_______________________
9. PF3
_______________________
_______________________
10. CoCl3
_______________________
_______________________
11. Al2O3
_______________________
_______________________
12. Mg(NO3)2______________________
_______________________
13. NaCl
_______________________
_______________________
14. K2SO4
_______________________
_______________________
15. P2O3
_______________________
_______________________
Is the compound covalent or ionic?
Write the correct formula.
1. aluminum chloride ________________
_______________________
2. calcium oxide
_______________________
________________
3. lithium hydroxide ________________
_______________________
4. diphosphorous tetraoxide __________
_______________________
5. cobalt (II) sulfate ________________
_______________________
6. ammonium iodide ________________
_______________________
7. sodium phosphate ________________
_______________________
8. iron (III) oxide ________________
_______________________
9. sulfur trioxide ________________
_______________________
10. nickel (II) acetate ________________
_______________________
11. carbon tetrachloride ______________
_______________________
12. potassium sulfide ________________
_______________________
13. dinitrogen pentoxide ______________
_______________________
14. magnesium nitride ________________
_______________________
15. barium phosphate ________________
_______________________
Mixed practice
Mixed Practice Writing and Naming
Name the following compounds:
1. C2H6
______________________________
2. CaBr2
______________________________
Write the following formulas:
21. copper (II) nitrate ___________
22. dinitrogen trioxide __________
3. LiMnO4
__________________________
23. lead (IV) chloride ___________
4. H2O
_________________________
24. aluminum hydroxide ________
5. HF ____________________________________
25. ammonium acetate __________
6. P4O10
_____________________________
26. silicon disulfide _____________
7. Al2O3
__________________________
27. sulfur dioxide ______________
8. Na2SO3
_____________________________
28. copper (I) oxide _____________
9. BaO
_______________________________
29. diphosphorus pentasulfide _____
10. H3PO4
_______________________________
30. carbon tetrafluoride __________
11. Na2O
________________________________
31. zinc permanganate __________
12. Hg(OH)2
____________________________
32. tin (II) phosphate ___________
13. SO3
________________________________
33. iron (III) carbonate __________
14. NI3
______________________________
34. silver phosphide ____________
15. Cu2CO3
______________________________
35. silicon tetraiodide ___________
16. NO
___________________________
36. strontium fluoride __________
17. P2S5
____________________________
37. cadmium hydroxide _________
18. Co3PO4
__________________________
38. iron (III) chromate __________
19. CS2
___________________________
39. ammonium sulfide _________
20. SF2
____________________________
40. lithium oxide ___________
Electronegativity Values