Chemical Naming
(Nomenclature)
NAME:
PERIOD:
S154
LEWIS
Dot Diagrams for Atom, Ions, and
Atoms &
Ions Atoms
Ionic
Compounds
same number of protons as they have electrons.
Valence electrons are the electrons found in the outermost energy level. The number of valence electrons can
be determined from an atoms position on the periodic table. Ions are charged particles or atoms that have lost
(transferred away) or gained electrons in order to have a stable (full or empty) energy level like the noble gas
closest to it on the periodic table, When an atom loses electron(s) it becomes positively charged because it has
more protons than elecfrons. When an atom gains electrons it becomes negatively charged because it has more
are neutral, that is they have the
electrons than protons.
Elements in group 1 (alkali metals) have one valence electrom In a dot diagram of the atom, the electron is
shown by a single dot above the symbol. When an atom loses its electron the dot diagram is now just the
symbol of the element, with no dot (because they were lost), brackets are drawn around the symbol showing it
is an ion, and the charge of the atom is shown as a super script to the right of the brackets.
Ion of Lithium
Example: Lithium, Li Atom of lithium
Neutral atom ---->
Elements in group 2 (alkaline earth metals) have two valence electrons. In a dot diagram of the atom, the
elecfrons are shown by two dots above the symbol. When an atom loses its electrons the dot diagram is now
just the symbol of the element, with no dots (because they were lost), brackets are drawn around the symbol
showing it is an ion, and the charge of the atom is shown as a super script to the right of the brackets.
Example: Beryllium,
Be
Ion Be of Beryllium
Atom of Beryllium
Neutral atom ---->
Be
[Be]2+
Elements in group 13 have three valence electrons, In a dot diagram of the atom, the electrons
by a
two dots above the symbol alid one to the right of the symbol.. When an atom loses its electrons,
the dot diagram is now just the symbol of the element, with no dot (because they were lost), brackets are drawn
around the symbol showing it is an ion, and the charge of the atom is shown as a super script to the right of the
three dots,
brackets.
Example: Boron,
D Atom of Boron
Ion of Boron, B3+
Neutral atom ---->
Elements in group 14 have four valence electrons and tend not to form ions. In a dot diagram of the atom, the
electrons are shown by a four dots, two dots above the symbol, one to the right of the symbol, and one below,
Or one dot each
above, below, and one each side.
Exampl.e: Carbon,
C Atom of Carbon
or
Neutral atom ---->
Elements in group 15 have five valence electrons. In a dot diagram of the at0in, the electrons are shown by a
five dots, two dots above the symbol, one to the right of the symbol, one below, and one to the left.. When an
atom gains 3 electrons, the dot diagram is now the symbol of the element, with eight dots (showing a full
valence energy level), brackets are drawh around the symbol showing it is an ion, and the charge oftbe atom is
shown as a super script to the right of the brackets.
Example: Nitrogen,
N
Atom of Nitrogen, N
Ion of Nitrogen,
Neutral atom ---->
Page 1
Elements in group 16 have six valence electrons, In a dot diagram of the atom, the electrons are shown by six
dots, two dots above the symbol, two to the right of the symbol, one below, and one to the left.. When an atom
gains 2 electrons, the dot diagram is now the symbol of the element, with eight dots (showing a full valence
energy level), brackets are drawn around the symbol showing it is an ion, and the charge of the atom is shown
asa super script.to the right..of.the
Example: Oxygen,
O
brackets.
Atom of Oxygen; O
Ion of Oxygen, 02-
Neutral atom ---->
Elements in group 17 ( the halogens) have seven valence electrons. In a dot diagram of the atom, the elecfrons
are shown by a seven dots, two dots above the symbol, two to the right of the symbol; two below, and one to
the left,. When an atom gains one electron, the dot diagram is now the symbol of the element, with eight dots
(showing a full valence energy level), brackets are drawn around the symbol showing it is an ion, and the
charge of the atom is shown as a super script to the right of the brackets,
Atom of Fluorine, F
Ion of Nitrogen, FExample: Fluorine, F
Neutral atom ---->
Elements in group 18 (noble gases) have full set of 8 valence electons (2 in the case helium). In a dot
diagram of the atom, the electrons are shown by a eight dots, two dots above the symbol, two to the right of the
symbol, two below, and two to the left. Because the are full (stable) they do not form ions.
Examples: Helium, H (full with 2 electrons)
Neon, Ne
Page 2
Name
Drawing Dot Diagrams of Ionic Compounds
Draw the dot
made from the iven cation and anion.
Example:
Cation
Cation = Na
=
02
Anion
Anion
3.
2.
Cation
= Cal+
Anion
Anion
4.
5.
Cation.
A1
Cation
Cation — Mg2+
=K
Anion
Anion
6.
7.
Cation = Ga3+
Cation= Rb
Anion
Anion
-02
= N3v
9.
8,
Cation
Cation
B
Anion = p3
Anion
AS3
101
11.
Cation = sr2+
Cation
= Cs
Anion = 02
Anion
13.
Cation=
Anion
MO
2+
Ca
Cation
Anion
14.
Cation
Anion =
Cation =
An.ioti
K
— 82
Page 3
tonic (Metal
Naming binary
ionic
compounds: Rules
+
Nonmetal)
to follow:
write iän with positive charge
2. the
second word
is
first.
formed by changing
the ending to "ide'.
examples: NaaO
Sodium Oxido
:
MgCh: Magnesium
Chloride
Practice Problems:
Use the rules above te complete the fol}owing:
1.
Circle
Magnesium Oxide
Myo
which of the following below are
cations (positively charged)
Barium Sulfide
2.
c
3.
K3P
3.
Se
Mn
4.
N03N
4.
H
o
S.
BaF2
5.
Write the chemical formulas for the following compounds:
I.
Calcium Bromide
2. Lithium
3.
1.
Oxide
Aluminum
5.
Water
More
:
2.
Potassium Fluoride
4.
example
Sulfide
Sr
As
Ca
symbol of positive and negative ions
1. write
2. criss
No
N
—
cross charges,
if
charge
isn'f
Calcium Oxide Ca
-2
0b
Cao
Sodium Nitride Na
p
NO'P
3.
ZERO
3.
4.
5.
Practice (You can do
it,
yes you can!)
l.
NaH
1.
2.
calcium*nitride
2.
7.
Beryllium Fluoride
3.
AIN
3.
8.
K20
4.
Strontium oxide
4.
9. HCI
5.
Rb3P
5.
10.
6.
8.
9.
Sodium chloride
10.
Questions
1.
What
2.
What are a
3.
What
is
is
the difference between a binary and tertiary
cation
compound?
and an anion?
the difference between a superscript and a subscripl?
Page
1:
Naming Compounds
Soldan revised 02/03
Page 4
Transitional Metals (groups 3
is
used
Roman Numerals:
12 on your Periodical Table)
more than one, positive
Transitional Metals have
Roman Numeral
—
ionic charit. In order to determine the charge, o
to indicate the charge.
3
1
8 VI"
VII
Ill
9 IX
lox
To determine the charge, look at the periodical table for the choices.
If
the chemical formula is written, un criss
Remember
*toss
to figure the
charge and indicate by a
Roman Num.
change the second ion's ending to "ide'
to
Examples: Iron
(Ill)
iodide
Fe 13
SnC14 Tin (IV) chloride
Practice Problems:
copper
(II)
2.
Tin (IV)
3.
Gold
oxide
bromide
(Ill)
fluoride
Manganese
5.
Nickel
6.
TiN
7.
CoF3
8.
W20s
9.
OsBr6
10.
PbCi4
(II)
(VI!) nitride
chloride
Questions
1.
Where are
2.
How do you
transitional metals located on your periodical table?
figure out the eharge once the transitional element
is in
a
compound?
Page 4 Transitional Metal Compounds
Soldon revised 02/03
Page 5
Writinq
Formulas
for
Binary
Ionic
Compounds
Lithium suifiae
2.
Aluminum
3.
Magnesium oxide
4.
Zinc phosphide
5.
Rubidium chloride
6.
Calcium telfunide
7.
Strontium nitride
8.
Barium fluoride
9.
Silver chloride
10.
Cadmium bromide
iodide
11. Lithium chloride
12. Cesium hydride
13. Radium arsenide
14.
Aluminum oxide
15. Potassium bromide
Make
5 of
your own!
And.
iustup
for
a review:
16. Sulfur dichloride
17. Tetraiodine nonoxide
18. Sulfur hexafluoride
19. Carbon disulfide
20. Phosphorous pentafluoride
Page 6
Formulas
Writinq
1.
Copper
2.
Iron
3.
Copper
4.
Tin
5.
Nickel
6.
Manganese
7.
Titanium (IV) nitride
8.
Cobalt
9.
Lead
10.
Chromium
Iron
(II)
Binarv
Ionic
Compounds (with
transition
metals)
sulfide
oxide
(II)
oxide
(l)
bromide
(II)
phosphide
(Ill)
(Ill)
(II)
12. Titanium
iodide
bromide
(Ill)
hydride
(Ill)
13. Antimony
(II)
15. Polonium
(IV) fluoride
selenide
(Ill)
14. Cobalt
for
(Ill)
iodide
sulfide
hydride
(II)
selenide
Make
upfor
5 ofa your
own!
just
review:
And.
16. carbon rmnoxide
17. calcium chloride
18. potassium oxide
19. water
20. strontium bromide
Page 7
Naming
Ionic (metal + nonmetal) Compounds
Naming Chemical Compounds Worksheet
Name the following
1)
NaBr
2)
Cao
3)
Li2S
4)
MgBr2
ionic
compounds:
5)
Write the formulas for the following ionic compounds:
6)
potassium iodide
7)
magnesium oxide
8)
aluminum
9)
sodium
10)
calcium carbonate
11)
lithium sulfate
12)
beryllium phosphide
13)
magnesium hydroxide
14)
sodium phosphate
15)
aluminum carbonate
16)
calcium chloride
17)
sodium cyanide
18)
aluminum oxide
19)
magnesium acetate
20)
ammonium
chloride
nitrate
chloride
Page 8
Name.
Naminq
1.
Csi
2.
CaBr2
3.
Mgs
4.
Bao
5.
NaH
6.
K20
Binary
Ionic
Compounds:
7.
8.
NaCi
9.
Ag2S
10. RaSe
11. AlBr3
12.
RbF
13.
Cd3P2
14. znC12
15. BeO
And. just for a review:
Ca 3 P 2
16. BC13
BaCl2
17. so-3
18.
Cs N
3
NH3
19. Potassium Bromide
HO
22
20. Strontium Selenide
Page 9
Naming & Writing Formulas
Name
(There are no roman numerals or polyatomic ions on this page)
Fill in
the table with the missin
Cation
Anion
ions, formula or
Formula
names from the given ions, formula, or name.
Name
Be
5.
6.
Cao
Ga2S3
sr3P2
Mg12
10.
ZnO
11.
Aluminum Nitride
12.
Calcium Chloride
Magnesium
Sulfide
14
Gallium Chloride
15
Cadmium Bromide
Page 10
Naming & Writing Formulas for Elements
With more than one Oxidation Numbers
Fill in the table
Cation
1.
with the missing
Anion
ions,
Name
fonnula or names from the
•ven ions, formul
or name.
Name
Formula
cu
2.
3.
6.
Cuo
7.
8.
Ni3P2
9.
Pb12
10.
ZnO
Nickel
12.
13.
14
15.
Tin
(111)
(II)
Cobalt
Chloride
(11)
Chromium
Nitride
Sulfide
(Ill)
Chloride
Cadmium Bromide
Page 11
Naming & Writing Formulas for Ionic
Compounds with Polyatomic ions #3
Fill in the table
Cation
Name
with the missing ions, formula or names from the
Anion
iv.en•
ions, formula, or name.
Name
Formula
cu
Oil
2.
C03
Cr
6.
cuS03
8,
10.
11,
12.
13.
14
15
NiS04
Tin
(11)
Copper
Phosphate
(II)
Chromium
Manganese
Chlorate
(Ill)
(II)
Sulfate
hydroxide
Lead (I V) Nitrate
Page 12
Covalent naming rule reminders:
1) Change the ending of the second element to -ide.
3.) Never use 'mono' on the first element.
2) Add a prefix to each element to indicate how many of it there is.
Name
Naming Covalent
Compounds
Naming
Covalent (nonmetal+nonmetal)
Compounds
mono
Prefixes:
penta
1-10.
one
=
5
hexa
octa
=
8
hepta = 7 tetra = 4
nona = 9 deca = 10
Write the correct formula from the even name.
Name
Formula
1.
Chorine monoxide
2.
Oxygen difluoride
Dinitrogen monoxide
Nitrogen trichloride
Sulfur tetrabromide
6.
Carbon dioxide
Diphosphorous pentoxide
Bromine pentafluoride
Disulfur dichloride
10,
Tetraarsenic decoxide
11-20. Write the correct
name from the
Name
11.
Dinitrogen Pentasulfide
"ven formula.
Formula
N2S5
12.
co
13.
S03
N203
N20
16.
xeF6
PC15
18.
SiC14
19.
C102
20.
ICl
Page 13
Dot Diagrams of some Covalent Compounds
Name
Draw dot diagrams for the following covalent compounds.
02 (Oxygen gas)
2.
HI
3,
H2Se (Hydrogen selenide)
4.
NH3
5.
CF4 (Carbon tegafluoride)
6.
C2H6
1.
iodide)
(ammonia)
4.
(ethane)
.9
7.
HFO
9.
Nz
(hypoffiorous acid)
(nitrogen gas)
8.
10.
OBr2 (oxygen dibromide)
CHC13
(friChlor.omethane)
Page 14
nonmetal + nonmetal
Covalent
Compound Naming
Practice
Name the following covalent compounds:
1)
seF6
2)
Te03
3)
H20
4)
scu
5)
PC12
6)
NC13
7)
Bra
9)
S04
10)
IF7
Write the formulas of the following covalent
compounds:
monoxide
11)
sulfur
12)
tellurium tetrachloride
13)
dinitrogen trioxide
14)
tetrasulfur dinitride
15)
carbon tetraiodide
16)
dicarbon tetrabromide
17)
hydrogen chloride
18)
carbon diselenide
19)
triboron silicide
20)
tellurium dichloride
mono
mono
Page 15
This wotk is licensed under a Creative Commons Attribution - NonCommercial 4.0 International License
and is copyrighted (c) 2015 by Ian Guch. For more practice sheets and tutorials, visit www.chemfiestacom
Naming Chemical Compounds
This
a mixture of naming and formula writing.
is
ionic or covalent.
Make sure you determine
Covalent compounds have 2 non-metals.
LOOK at the
if
this
is
periodic
table. Ionic salts are metals + non-metals.
Ionic or Covalent
1.
Name this
a
ro riatel
NaBr
2.
4.
5.
FeP04
7.
so
8.
CuOH
For each of the following questions, determine whether the compound
covalent and write the appropriate formula for
Ionic or Covalent
is
ionic or
it.
Write thea
ro riate formula
10. Silicon dioxide
11.
Nickel (111) sulfide
12. Nickel sulfate
13. Silver
acetate
14.
biboron tetrabromide
15.
Carbon tetrachloride
16.
Potassium carbonate
17.
Iron (II) carbonate
18. Tin (IV) selenide
19. Chlorine
as
Page 16
Naming Chemical Compounds 2
This
a mixture of naming and formula writing.
is
ionic or covalent.
Make sure you determine
Covalent compounds have 2 non-metals.
if
this
is
LOOK at the periodic
table. Ionic salts are metals + non-metals.
Ionic or Covalent
1.
NazC03
3.
NH
5.
FeS04
Si02
6.
Gact3
7.
coBrz
9.
co
4.
Name this
a
ro riatel
For each of the following questions, determine whether the compound
covalent and write the appropriate formula for
Ionic or Covalent
10. Dinitro
11.
is ionic
or
it.
Write thea
ro riate formula
en trioxide
Diatomic nitro en
12. Lithium
acetate
13.
Phos horous trifluoride
14.
Vanadium(V) oxide
15.
Phos horus trifluoride
16.
Aluminum h droxide
17.
Zinc Sulfide
18. Silicon tetrafluoride
19. Silver
hos hate
Page 17