10/23 Happy Mole Day! Bring your book tomorrow Test Thursday We will finish up notes today on Polyatomic Ions

1
10/23 Happy Mole Day!Bring your book
tomorrowTest ThursdayWe will finish up notes
today on Polyatomic Ions

• Answer the following in your notes
• A Na ion has a 1 charge because it _____ (lost
  or gained) electrons.
• The electron dot structure for Phosphorous is
• The total charges of any compound must add to
  ____.
• The oxidation number for Sulfur is _____.
• Choose the binary compound.
• NaCl b) MgSO4 c) AuNO3

2
Tue 10/24Get out all WS for this unit

• When e- are transferred a ___bond is made.
• Write the formula for Lithium Sulfide, for
  Lithium Sulfate.
• Write the formula for Barium Phosphate.
• Name one element that will not form a compound.
  Why?
• What is the electrical charge of a compound?
• What is the name of HI
• How many valence e- does Nitrogen have? Will it
  gain or lose e-? Is it a metal or nonmetal?
• If an element gains electrons, the oxidation
  is___.

3
10/25

• Pick Up Review Sheet. Start working on it.
• Quiz today
• Test tomorrow BRING A PENCIL
• Chapter 24 Vocab due on Friday (See pg 761 17
  words)

4
Metals vs Nonmetals

• Complete Metals, Nonmetals, and Metalloids
  Worksheet
• Chapter 20 is a self study unit

5

• The smallest particle of an element is an
• atom
• If the outer energy level is completely filled
  with electrons then the atom is chemically
• stable
• If the outer energy level is incomplete, valences
  of 1 to 7 then these atoms will gain, lose, or
  share electrons with other atoms and form

6
Compounds
7
1. Atoms combine to become chemically stable.
Stability is achieved if an atomsouter energy
level is completely filled with electrons.

• Stability in Bonding
• A. Chemical Stability

10p 10n
NEON
8

1. Atoms combine by gaining, losing, or sharing
   electrons. When atoms combine with other atoms
   they form compounds.

9

1. A chemical bond is a force that hold the atoms
   together in a substance.

10
(No Transcript)
11
4. Atoms of all the elements have from 1 to
7 electrons in their outer energy level except
the noble gases (VIIIA). Therefore all elements
combine except noble gases.
3p 4n
9p 10n
12
THE MAGIC NUMBER IS
The Octet Rule
13
B. A compound is a pure substance made up of two
or more elements that are chemically joined in
definite proportions.Ex. Carbon dioxide is
CO2 Carbon monoxide (the poison) is CO .
14
Compounds do not look or act like the elements
that form them.

• Sodium is a silvery metal that reacts
  violently with water

Chlorine is a poisonous, green gas.
Does salt share any of those properties?
15
C. Chemical Formulas 1. a chemical formula
shows the elements that a compound contains and
the number of atoms of each element.
Na2SO4
Ba3(PO4)2
16
2. Subscript - a small lowered number that
shows number of atoms of each element in the
compound.
Ba3P2
Ba
Ba
Ba
P
P
17

• Valence electrons are the electrons in the outer
  energy level of an atom. An elements number of
  valence electrons is the same as the group
  number.
• ex. All elements in group IVA have 4 valence
  electrons

18
E. An electron dot diagram

• Shows the number of valence electrons
• Ex.

19
II. Types of Chemical Bonds
20
II. Types of Chemical Bonds A. Covalent Bonds

• 1. A covalent bond is the force of attraction
  that forms when atoms share electrons. They form
  between NONMETALS.
• ex. H20, CO2
• 2. A molecule is a group of atoms that combine
  by sharing electrons

21
B. Ionic Bonds

• Ion an atom that has a positive or a negative
  charge resulting from the gain or loss of
  electrons indicated with a superscript.
• ex. O-2 has gained 2 e-
• Na1 has lost 1 e-

22
Ionic Bond

• The force of attraction between opposite charges
  of the ions in an ionic compound
• ex.
• a) In ionic bonds, the atoms transfer electrons

Na1
Cl-1
23

• b.) Ionic compounds always form between
  metals nonmetals. Metals lose e- and nonmetals
  gain e-.
• Li1 F-1
• Positive ion metal lost e-
• Negative ion nonmetal gained e-

9p 10n0
3p 4n0
F-1
Li1
24
Na1 Cl-1
NaCl
ex. NaCl is an ionic compound Which is the
metal? Which is the nonmetal?
25
(No Transcript)
26
When atoms lose or gain Electrons they become
ions. What type depends on its oxidation
number. III. Oxidation Numbers
Mg2
Cl-1
O-2
P-3
Na1
Al3
27
A. Oxidation number - the charge of an atom,
indicating whether the atom has lost () or
gained (-) electrons and how many electrons it
lost or gained.
Superscript
3
Al
28

• Gaining electrons results in negative oxidation
  number (charge). The atom has gained negative
  charge from additional electrons!
• Ex Sulfur 2electrons S-2

29

• Losing electrons results in a positive oxidation
  number (charge)
• Ex.
• Calcium -2 electrons Ca2
• HINT LEFT LOSE e- positively charged ions

30
Determine Oxidation with group
Group Lose or gain electrons How many Oxidation Number
1A lose 1 1
2A lose 2 2
3A lose 3 3
4A Lose or gain 4 4 or -4
5A gain 3 -3
6A gain 2 -2
7A gain 1 -1
8A none none 0
31
In Review
The means that this Lithium has lost
electrons. The 1 means that this Lithium has lost
1 electron.
Li1
HINT LEFT LOSE e- positively charged ions
32
Lithium is in group 1A so it gives away or
donates one electron.
-
-
NEGATIVE CHARGES -

-
-
-






POSITIVE CHARGES -

-
Add the number of positive charges and negative
charges together.
3
-2
1
33
How do you find the oxidation number for
O
Al
N
P
S
34
Its Friday!!!! 10/20

• Pick up worksheet by Brinclhof
• Work on Oxidation side
• Write a word with the prefix bi on the board.
  What does this prefix mean?
• How many different elements are in the following
  compound
• Ca(C2H3O2)2

35

IV. Binary Compounds
Binary compounds are composed of only two
elements. (Look for 2 capital letters!)Ex. NaCl
sodium chloride Mg3N2 magnesium
nitride

36

• Writing Formulas
• Formulas consist of a positive ion and a negative
  ion. USE SYMBOLS

The positive ion always comes 1st
MgO
AlP
NaCl
P-3
O-2
Cl-1
Na1
Al3
Mg2
37
Hydrogen is a ion even though its a nonmetal
and it is written first.
38
A subscript of (1) is NEVER written.
NO!!!
Na1Cl1
39
2. The total oxidation numbers or charge on a
compound must add up to ZERO. IF NOT use the
criss cross method.
CaO
O-2
Ca2
2 -2 0
40
Criss CrossFinding formulas

• Determine the charge of each ion in the compound.
• Aluminum oxide Al3 O-2
• Potassium Chloride K1 Cl-1
• Calcium nitrate Ca 2 NO3-1
• 2. Add the oxidation numbers together.
• 3-2 1 1-1 0 2-1 1

41
Aluminum Oxide
3. If the total zero the formula is balanced
with one ion each. ex KCl 4. If the total does
not equal zero use the crisscross method
to determine the number of ions needed for each
side of the formula.
Potassium Chloride
3
2
Al3 O-2 Al O
42
B. Naming Binary Non-variableCompounds

• Write name the positive ion
• Write name the negative ion
• changing the ending to IDE.
• AlBr3

bromide
Aluminum
43
-ides
N - O F - P - S - Cl - Br - I -
Nitrogen Oxygen Flourine Phosphorous Sulfur Chl
orine Bromine Iodine
Nitride Oxide Flouride Phosphide Sulfide Chlori
de Bromide Iodide
44
IV. Polyatomic Ions
45
A. Polyatomic ions - groups of 2 or more atoms
covalently bonded that have a charge.
NH41
SO3-2
PO4-3
ClO3-1
SO4-2
NO3-1
C2H3O2-1
NO4-1
CO3-2
46
B. Writing Formulas using Polyatomic Ions

1. Follow rules to write formulas for Binary
   Compounds
2. If a subscript needs to be added to a polyatomic
   ion, write parenthesis around the polyatomic ion
   first. Then write the subscript outside after
   the parenthesis.
3. Never break up the atoms of a polyatomic ion or
   change its subscripts.

47
Aluminum Sulfate
3
2
Al3 SO4 -2 Al SO4
(
)
48
Naming Polyatomic Compounds

• Name the positive ion
• Name the negative ion
• AlPO4

phosphate
Aluminum