Academic
Chemistry UNIT 6
MENCLATURE
. N
"I
Nilrogÿn
Name:
Class Period:
Test Date:
-I
Chemistry Calendar
9
Bill Nye: Atoms and
Molecules pg 3
Intro: Element or
Compound?Page 4
16
quiz!!
Mixed Practice PG 15
10
11
Notes #2: Valence
Electrons, Lewis
Notes #3: Binary Ioni(
Chemical Names and
Dot structures
Formulas Pg. 8-9
and Ions
13
Notes #3: Binary
Ionic Compounds
with Transition
Metals Pg. 11
Notes #4: Ionic
Compounds
with Polyatomic
Ions Pg 13
HW: pg 12
HW: pg 14
P. 5-6
HW: pg 7
HW: pg 10
17
18
Notes #5: Covalent
Molecules
Ionic and Covalent
Bonding Activity
19
Pg 16
Guide pg 18-19
HW: pg 17 AND
Study Guide
DUETHURSDAY!
Page 18-19
HW: Study
12
DLA!
REVIEW
Check Study Guide
HW: Study
Guide Page 18-19
25
24
2O
26
27
Dimensional
Nomenclat2ÿ")Analysis
Test
Poster
NO SCHC OL THANKSGIVING l IREAK!
Activity
It
Nomenclature Test: Monday ÿ/27
Bill Nye- Atolns
Name:
The middJe of the atom is called the
.
The two particles in the nucleus are
andVÿ ÿ/ÿ'ÿfÿ 6
3ÿ
The heaviest part of the atom is the
4ÿ
The particles which have a positive charge are
5ÿ
The particleswhich have no charge are Hÿ4ÿ"ÿ'ÿ
6ÿ
The particles which have a negative charge are (ÿ}ÿVlÿ
7.
Atoms are mostly
8ÿ
The basic building blocks of aH matter are
9.
Atoms are like letters and molecules are like
i0.
All matter is made of ÿlÿqÿ/ÿlÿ
1.1.
Atoms combine to form C,OÿOOIVÿ4,ÿ / Vvll#t e,04)ÿ-ÿ2ÿ
12.
Water can be broken down by passing an electric, current through it.
and ÿZÿ Vÿq DDL)ÿ
What two gasses are
produced by the break diown of water?
13,
What does the atomic number tell you?
p fGv
14.
What is the chemical name for:
HzO -->
1S.
16.
NaCI -->
CÿHsNsOÿ -->
oms are tOÿ small to be seen, How do scientist study atoms and the particles which make up
atoms?
Everything in the un, iverse is either
or
NOTES 1: Compounds and Their Formulas
Compounds have been defined as matter formed by two or more different elements joined by a
chemical bond.
Formulas allow scientists to identify the composition of compounds. Every formula contains the symbols
of elements that make up the compound. One example is NaCI, also known as table salt, is formed when
sodium (Na) and chlorine (CI) combine in a chemical reaction.
Baking soda, or sodium bicarbonate, has a more complicated formulaÿNaHCOÿ Baking soda is formed when
sodium (Na), hydrogen (H), carbon (C), and oxygen (O) combine in a cÿeaction. The small number 3
in the formula is called a subscript.
A subscript shows the number of atoms of an element in a compound. The subscript always refers to
the symbol just before it in the formula. If there is no subscript following a symbol, it means there is
only one of that kind of atom in the molecule.
Example: Baking soda thus conÿins,
1 atom of sodium,__l atom of hydrogen,
____ll atom of carbon, and ÿ atoms of oxygen in each molecule.
A molecule iS the term used for any bonded elements.
Identify the following substances:
NaHCO3
Complete ÿ,e chart by first idenI:ifÿ,ing each of ffhe substaaÿc.ea by name. 'Then desÿibe each.
substance by placfÿg a check in the appropriate box.
Name
Element Compound
Symbol:
Atom
Molecule
J
,/
d
Oÿ
H
/
Hÿ
/
C
,/
CO
AI
/
ALl
,/
/
/
G o14
COÿ
,1
4
NOTES 2: VALENCE ELECTRONS, LEWIS DOT DIAGRAMS, AND
OXIDATION NUMBERS
Review:
1. How many total electrons are in a neutral atom of Sulfur? Iÿ-"
2. How many electrons are in sulfur'ÿ]ÿghest energy leveJj(it's most
outer shell) (HINT: use the picture to the right)?
---ÿ
3. How many electrons does sulfur need to gain or lose in order to have 8
valence electrons (electrons in the outermost shell)?
RECAP: BOHR'S ATOMIC MODEL
Bohfÿ.ÿDed an atomic model in which the electrons are arranged in specific ÿ-'i/ÿtFÿ /
The 10ÿ ÿ _0,ÿ/ÿ. 7 ÿ;ÿ/i (n=l) is located closest to the nucleus. The highest
level is located farther away from the nucleus.
* The electrons in the highest (outer most) energy level for any element are known as
tl Ol t ce,,
electrons.*
*Valence electrons are electrons are involved in chemical bonding.
VALENCE ELECTRONS can be easily found by looking at the Iÿ FUÿ/
[ÿ i#iÿ bÿf
the periodic table.
Examples:
or"A" number located above the column ÿhere the element is located on
[ Group #
If)
Ai-- Group # and
Asoit has ÿ valence
electrons.
f Asoit has Lÿ valence
Pb= Group #ÿand __
The number next to
electrons.
the A is the valence
Practice:
Determine the number of valence electrons for:
1. Phosphoÿs:
2. Argon: _ÿ
3. Lead:
4. Barium: _ÿ
PerlodlQ TaMÿ o! Ille [htmentl
**This only works for GROUP A Elements.
/3
Another exception is Helium. Who only has o/ÿ valence electrons.
I!
Practice: Label the Valence Electrons for each Group A column on
the periodic table to the right.
' "1 '1"1'1'1 '1' I I'!'"1 1'"1
IIII
LEWIS DOT DIAGRAMS:
is a diagram in which the chemical symbol of an element represents
the nucleus and the inner energy level and "dots" represent the valence electrons.
There can only be up to 8 valence electrons and thus only 8 dots around a symbol. The first 4 dots are
single and then they pair up as more are added. Octet rule states that all atoms wish to be like the
Nobel gases (group 18) with a full valence of 8 electrons.
How are the dots arranged? Treat the symbol as if it were a square, with 1 dot on each of the 4 sides
before pairing up.
element symbol
00ÿIj ......... one dot for each valence electron
I
OXIDATION NUMBERS: is the number oj: electrons an atom gains, loses, or shares when it forms a
chemical bond and achieves the octet rule. This will also be the charge of the ION.
Metals as a rule lose electrons and will have a (+) charge.
Nonmetals will gain electrons and have a (-) charge
It- Metals and Nonmetals
0
Nobel gases in group 18 will not lose or gain and have a 0
charge
ÿ/ÿlfÿ ÿ ÿ-vÿ
Label the periodic table at right for the ion charge created as
atoms achieve the Octet rule (full valence of 8):
, a IMETALS
\
Examples:
Name
#Valence
Lewis Dot
How many electrons are
Electrons
Diagram
needed to have a complete
outer shell?
Helium
2
°
O
0
(Ion charge)
0
Carbon
Fluorine
Needs to gain 1
o
#
Neon
F°
o
u#
0
0
6
Homework:
How many
electrons must be
Element
# of
Lewis Dot Diagram
Valence
Name
Electrons
added (- ion)
Oxidation
cation
Or
removed(+ ion)
Number
or
to have a
(Ion charge)
anion
complete outer
.#,
shell?
Lithium
I
"CI.
Q,
Xenon
0
Phosphorus
0
t
Sodium
I
Oxygen
lqCb°
o
b
J
Add 2 electrons
0°0
00
Hydrogen
+1
,
Name 2 elements that have the same Lewis dot structure as oxygen:
,
How many valence electrons do elements in group 2A have?
3.
¢ÿL
Besides hydrogen, which other element is an exception to the Octet rule?
7
NOTES #3: Binary Ionic Chemical Names and Formulas
Quick Review
• ÿ-ÿ ÿ
- atoms that have lost or gained one or more electrons•
•
Cÿ!)ÿ ÿVÿv
•
ÿ
- positively charged ion
1'
V%ÿ
' charged •
- negat,vely
non ÿ
•
• Thÿakrÿe on the ion is known as the 0ÿ !ÿ/ÿ'ÿ/ÿ [/ÿjÿ/ÿlÿ/ÿ
•
ÿ* !ÿ'ÿ'ÿIGÿ lgJÿ'ÿ - ion consisting of two or more atoms
Practice - write the ion with the charge for the following elements
I"ONI"C COMPOUNb$
• Ioÿc CQmpÿunds are made up, of a ,,
Metals and Nonmetals
or
"ÿ1
8
in
+ ÿlÿaÿ
W
• The boÿ/ÿvÿ
of electrons.
o The electron is transferred from the
')1ÿ f/ÿ to the ÿ Vÿ (ÿ
so that both atoms have a complete valence
shell (usually 8 electrons in valance).
• The overall charge of ionic compounds must equal
i
:
(o).
Naming Ionic Compounds (ÿ'ÿt/
(-VÿC/Vÿ 'Vÿ ÿ'ÿ I
• First namethe ÿÿ and then th.e ÿlÿVÿ
• Change the ending of the anion to ,4 14 ÿ
• (metal followed by nonmetal)
Na
Example:
• •
• MgCI2
• Li2S
Practice:
• MgO
• KÿP
• CsCI
•
Ba3N2
magnesium chloride
LH'hlÿfÿ ÿ'ÿ1ÿÿ
DRAWING Lewis Dot Structures for Ionic Compounds
• The overall charge on the compound must equal zero, that is, the number of electrons lost by one atom
must equal the number of electrons gained by the other atom.
• The Lewis Structure (electron dot diagram) of each ion is used to construct the Lewis Structure (electron
dot diagram) for the ionic compound.
The Lewis Dot structures show the location of the valence electrons after the
electrons have been transferred.
Examples: Lithium fluoride
• Lithium atom loses one electron to form the cation Li+
[bi] +
• Fluorine atom gains one electron to form the anion F-
• Lithium fluoride compound can be represented as
Draw the Lewis structure of Lithium oxide.
r:ÿ':]- i
...................................... .......
What would be the chemical formula for this compound?
Writing Chemical Formulas
• When given two ions, /ÿt1ÿ/'1ÿ/ÿ the charges and make them the \ÿÿ/ÿ?ÿ2.
• DQNOÿkeeRthe+/-siÿns
• gÿ) ÿ./ subscripts if possible
This means we must reduce the subscripts if they have a common denominator.
Example: Ca4Fs--)
A. Using Balanced charges Method:
B. Using the Crisÿross method:
Example: Li÷1 02
• **Sum ofcharges must equal zero.
Ex:
a. Na+1 + C1-1 -) NaCI (+1+-1= O)
b. Mg+2+ 0-2-)MgO* (+2+-2=0)
* Don't write this Mg202 because it must be reduced.
Now, let's use the name to write the chemical formula
Name
cation
anion
•
Lithium oxide
Magnesium sulfide
LJ_ÿ
formula
Lewis Dot Structure
Li,o gij,+Ei :,
Chÿ
Your turn: HOMEWORK:
Write the chemical formulas from the ions.
=ÿ
N%ÿ 0
2/ Ca÷2 F-1
31 A'÷3
/ÿ, #ÿ
Se-2
,,(ÿ, .4- Z.
ÿ1ÿ ÿ
0
Write the chemical formulas from the name:
6) Sodium iodide cation: ÿJÿLÿÿ'ÿ anion: .ÿ
Formula:
7) Strontium bromide
cation: ÿ=ÿ
anion:__ÿ
Formula:
.ÿa nion:ÿ__ÿI.
Formula:
8) Aluminum
oxide cation:
9) Barium sulfide cation: ÿ ?'ÿanion: .Sÿ'ÿ
Formula:
Write the name from the formula:
10) NaCl
50ÿiI Iljm Cÿ'ÿ ! 0 ifÿ 4-1ÿ
=ÿ =a==
,,!o!IIÿ 5vll&
Draw the Lewis Dot structure for numbers 1, 2 & 3 above:
#1)
#2)
ÿ
'ÿ -77
oo
L-0 0
ÿJ
10
NOTES #4: Binary Ionic Compounds with Transition Metals(Cations)
Multivalent Cations are found in the group ÿ elements (the middle of the periodic table).
k
Roman
Charge
Numeral
t.
@l@ l [ @@[@@@@ÿlo4g]ÿJÿjÿ
I
+1
II
4-7-
III
IV
# q-
V
VI
These elements are also known as the %ÿ Iÿihil'ÿ
metals.
If your cation is a transition metal, then you mÿst speciE/the charge with a
.ÿ0ÿqL4ÿq
mum ÿ4/_ÿ
VII
VIII
.
4q
+f¢
Example: Iron (110 Sulfide
Just like the compounds we looked at yeÿ_fÿaÿ_;ÿhe sum of charges must equaland still the /xJlfÿ ÿ'ÿ
we can use
formula.
ÿ-zÿ, I <,"
method when writing the chemical
PRACTICE:
Chemical NAME
Cation
Anion
1. Copperl sulfide
Cu 5
0ÿ
2. Manganese II oxide
3. Tin IV fluoride
Chemical FORMULA
gn 4+
Pblÿ
Fe203
PbOÿ
6.
CoP
.
• To figure out the charge of the transition metal, just "uncross the charges .
EXCEPTIONS!I! These metals do NOT need a roman numeral.
0 Zn+2
0 Cd+2
o Ag+ÿ
11
HOMEWORK: Binary Ionic Compounds with Transition Metal Cations
Name the compound from just the formula.
• To figure out the charge of the transition metal, just "uncross the charges".
Chemical Formula
FIuoÿ'IHÿ
2. SnF4 ÿ'Iÿfÿ (ÿ) -"'ÿlÿOÿJ['/&
Write the chemical formula for the following compounds.
Chemical Name
8. copper Ilchloride
9. zinc sulfide
10. tin IV bromide
11. mercury II iodide
cation
anion
ÿ ÿ
ÿiÿf Sÿÿ/ÿ ÿt-ÿ- lÿr I-
2
12. copper II sulfide
ÿ2ÿf Sÿ.-
13. nickel III sulfide
ÿI ÿ'ÿ" g ÿ-
14. iron III oxide
Chemical Formula
kJ
"
rÿ* 0ÿ-
.ÿ .itanium.,,..o..hi.e 7ÿ 3ÿ P 3-
I,P
12
NOTES #5: Ionic Compounds with Polyatomic Ions
Polyatomic ions are groups of atoms that behave as one unit.
Hydrogen carbonate HCOÿ"
Acetate
c##2, %coo ....
Ammonium
NHÿ"
Carbonate
CO23-
Chlorate
aoÿ
Chlorite
aoÿ
CrO2-
Cyanide
CN"
OH-
Hypochlorite
CIO-
Nitrate
NO7
Nitrite
NO2
Perch Iorate
7
7
CI 04
Permanganate
7
Chromate
Hydroxide
ÿi
MnOÿ
Phosphate
POÿ-
Su Ifate
SO2-
ii
Dichromate
%oÿ,- i',
Sulfite
SO21
• They are treated like single ions in formulas, butuse Pÿlllf'ÿ/il'+ÿiÿl-ÿ ( )
when more than one is used in a formula.
• NEVER change name or look of polyatomic. If you change the subscripts for any part of the polyatomic,
then it is no longer that same polyatomic ion.
• Otherwise....Use all the same rules for naming and writing compounds as with any other ionic
compound.
PRACTICE:
Practice
Formula
Name
AI+3
Ca+2
K+I
CIO3'
ÿ' ÿiIt0 ÿ
Po-l-4#lUÿ CA Io<f6
Name the following compÿfl L)
• Ba(OH,2
ÿ "t"ÿOI Iÿ14-g
• CaS04 ÿlclum <..CO I,.P--4P6
• (NH4).P tÿ'ÿFilf'lq0V!!0ÿ(Vÿ Phoÿ-pÿi4&,
Write the formula for the following compounds:
cation
anion
Strontium phosphate
• Lithium acetate
• Sodium sulfate
Li*
&&4-
+ <7ou. z-
rd z,5oq13
Homework: Ionic Compounds with Polyatomic Ions
Identif the polyatomic ion and its charge
Polyatomic Ion
Acetate
Hydroxide
Formula of polyatomic ion
Ion charge
[4
OI
Ammonium
+
Sulfate
?/
Sulfite
SOÿ
Zÿ
Carbonate
Phosphate
v
poi
5-
Name the following compounds (Use Roman numerals and parenthesis as needed)
1. Cr(CIOÿ)3
2. ZnC03
3. NH40H
6. LiNO2
.ÿÿ.o.ÿ @c4ÿxÿ4ÿ 7. Na2SO4
4. Pb(NOÿ)2
8. Cu(NO3)2
Write the chemical formula
9. Silver hydroxide .
10. Copper (II) nitrate _
Or uÿ ,,704ÿ
11. Chromium (IV) sulfate
Mixed-Up Practice ( Give the name or formula)
12. K2C03
13. AI2(SO4) 3
14. FeP
ra ÿ (qTiT)
oÿbll
nitraTEÿ
Nÿ P'TI
ÿx]Oÿ
0-
15. Ammonium
<'JlsT,'
16. titanium IV sulfide
17.
Co pCÿe rÿ(lÿl)hydrÿgxide
]4
MIXED PRACTICE
DIRECTIONS: For each of the following write the correct formula/name and state the type of bond that
holds the elements together.
NAME
,
calcium carbonate
2.
nickel II chlorate
3.
zinc hydroxide
4.
barium sulfate
5.
mercury II chloride
6.
silver carbonate
7.
copper I sulfate
8.
ammonium chloride
9.
Zn(N03)2
i0.
NaC2H302
11. FeCI3
12.
CuCI
13.
N H4CI
14.
AgBr
15.
Sn(OH)4
15
NOTES #6: Naminq & Forming Covalent (Molecular) Compounds
COVALENT (MOLECULAR) COMPOUNDS
i
i
• Covalent compounds are made up of all ÿ0ÿ1ÿ ('ÿ (also called molecular compounds).
• To name a covalent compound, name the first element, then name the second one and change its ending
toÿ. Use ÿ-[1'ÿ ÿ,ÿo ÿ ,ÿ ÿo slÿow how many atoms of each element you have.
• M olecularcompoundscontain (ÿ(ÿ,;ÿ ÿ'ÿt"
• ÿ-ÿ/ÿ ÿI ÿI'ÿ
bonds and are formed when elements .
valence electrons.
The rules for naming and writing covalent molecules are different than those for ionic compounds.
• NO crisscross
• NO reducing
• Prefixes are used in naming to show the number of each element
Prefixes (Memorize theseH !)
Pre&x
133.OI10-
A
.ÿetals
except
Nobel
gases
nÿbeÿ
(group 18)
indicated
g
1
di-
2
tri-
3
tetra-
4
penta-
5
hexa-
6
hepta-
7
oc, ta-
8
I1Onÿ-
9
deca-
t 0
P20s
CCIÿ
Examples:
diphosphorus pentoxide
carbon tetrachloride
SÿOÿ
NOÿ
CO
s omitted if on the first element
To write the formula of a covalent compound, simply translate the prefixes and element names.
• dinitrogen dioxide
• diphosphorus heptoxide
• tetrasulfur tetranitride
16
HOMEWORK: Naming & Forming Covalent / Molecular Compounds
Covalent compounds using Prefixes:
**Do NOT reduce subscripts for covalent compounds
**Be careful that you do NOT use prefixes for ionic compounds.
Nitrogen trihydride
Sulfur hexafluoride
Dinitrogen pentoxide
Nitrogen monoxide
carbon tetrachloride
nitrogen monoxide
disphosphorus pentoxide
NBr3
OH8
OF2
P205
PFs
SiCl4
17
Academic Chemistry Nomenclature Study Guide
Nomenclature TEST on
1. Define the following:
a. Octet Rule
c. Valence electron -- ÿ ÿ ÿ) Cÿ/ÿ/ÿ/ÿ ÿ/ÿ ,ÿ ÿ ÿ L)ÿ'ÿ,,Y WVÿ ÿ,Cf ÿv'ÿ'ÿ ÿ,/
i v?d
d. Lewis Dot Structure ÿ-ÿ'ÿVÿiiÿ, A/,}ÿ -ÿ ÿ/ÿt,/ÿ'ÿ'x7ÿ/ÿL" ÿJltÿ/'ÿ'//gÿ C'ÿIÿÿQÿ
e. What's a poIÿomtc ion
,
When Group 1A elements form ions, when they ÿshare) electrons.
3. Where are metals found on the periodic table?
4. Where are nonmeÿms Touncl on the perioaic ÿable.
5. Do Nobel gases in group 18 form compounds? ÿ ÿ Why or why not? (Hint: octet rule)
6. How many valence electrons are in an atom of nitrogen? ÿ How many are in calcium?
7. How does magnesium obey the octet rule when reacting to form compounds?
(lose or gain or share electrons)
8. Covalent bonds ÿtransfer> electrons between ÿ!ÿ/ÿmÿiand m[ÿ'ÿQÿV3,ÿIÿI
9. Ionic bonds (shaÿ electrons between Vÿ ÿ-ÿ, \
and ÿ ÿ)ÿ 'I/ÿ #ÿ.f-ÿ i
10. Cations haven ÿ/negative)charge because they haveÿosÿ#ÿained)electrons.
----'ÿ they
have (Iost/6electrons.
11. Anions have a (positive/ÿeÿcharge because
18
12. Fill in the following chart with the correct information:
CHEMICAL NAME
CHEMICAL
FORMULA
Ions
(If applicable)
Lithium fluoride
Lead II oxide
Li 'ÿ Fiÿ
Ionic/Covalent
Li F
pbÿ Oz-
IF IONIC, DRAW LEWIS
STRUCTURE
L"+ÿ,ÿ}-II f2ÿ,ÿ
;ÿql c
CÿvaiD'ÿ
o1ÿ0,7 Oowatÿq-
Sulfur hexafluoride
Trichlorine heptaoxide
Silveÿrr ca rboÿnnatÿe in/]
<ÿr rF'l Zo
17641u
Mercury I oxide
L!L) zt
HOH
Cÿv'41ÿf
Li %r;I i
LiBr
A.I ÿiO ÿ---
..So4ÿ 0m R ÿYÿ.t-6
7ÿot,,l t cÿ
NAN02
Faroÿ°
FeO
SnBr4
Pl
30ÿ
5u
TYPE OF BOND
( I ÿ;t,s2,' I/II
m4oÿÿ ulff,//////
0
7>'mtc,
oÿfliu
%ÿt0
N20s
NaOH
SCI2
0 ,
70 r:-o/
L €,o __1
19
i .............
1ÿ
ÿ ÿ ÿ "t:ÿ
"
........ 'ÿ ........ ÿ ÿii ...........................
Z
.:t
E
Z
ÿ
ÿ
,
ÿ.iÿ-'
ÿ
.n
g
kÿ
U
o
,,0
o
Z
E
rÿ
oa
,ÿ'
ca
_
2 ..... .,,÷,
w
,-I
-
,,,,,i,. •
ÿ
o
,,,,,,,, , ,,, , ,
IN
,iÿ ÿ_ ÿo.
........ ,,.,,,, ....
20
x" h'.¸ .i
o,oooÿou,
!
EEEÿ
N ÿ N N N
'
ÿ
.g g .r
ggNÿ
8u8ÿ
uÿ
U
.J
I
o i: 8
i
U
uÿ
21