Download 2202 Chapter 1 - Eric G. Lambert School

Review of 1206
Physical or chemical?
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Page 9 #4
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Qualitative or quantitative?
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6 #2, 3
The atom
Subatomic
particle
Charge
Symbol
Mass (in g)
Radius (in m)
electron
1-
e-
9.02x10-28
Smaller than
10-18
proton
1+
p+
1.67x10-24
10-15
neutron
0
n0
1.67x10-24
10-15
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The nucleus of an atom
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Atomic number (Z): # protons
Mass number (A): # protons + neutrons
Atomic symbol (X): element symbol
A
X
Z
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The nucleus of an atom
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Page 14 # 5
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The periodic table
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Page 16 fig 1.10
Page 17 #6
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The periodic table
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Energy levels – orbits
Valence electrons
Periodic trends
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The periodic table
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Page 20, #7
Page 20-21 review #1-4, 6
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Types of Compounds
A. Molecular compounds
B. Ionic Compounds
C. Acids
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Types of Compounds
A. Molecular Compounds
- composed of two or more nonmetals
eg. CF4
C6H12O6
P4
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Types of Compounds
B. Ionic Compounds
- composed of a cation and an anion
(usually metal and nonmetal)
eg. NaCl
Mg3N2
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Cations
+
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anions
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re
eg
a
t
i
v
e
Types of Compounds
C. Acids
- acids are hydrogen compounds
that are dissolved in water
eg. HF(aq) H2SO4(aq)
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aqueous
Naming & Formulas
A. Molecular Compounds

Diatomic:
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Help Our Needy Class Find Brains
Immediately.
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Left on PT first
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last element ends in - ide
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prefixes indicate the number of each
atom in binary molecular compounds
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Naming & Formulas
Prefixes for binary compounds
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Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
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Naming & Formulas
eg. N3H5
disulfur octahydride
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Naming & Formulas
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Page 24 #9-10
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Naming & Formulas
B. Ionic Compounds
1. simple ions
2. multivalent metals
3. polyatomic ions
4. hydrates
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Naming & Formulas
1. Simple Ions (only one possible charge)
- Cross Over Method
- Reduce to lowest terms
eg. calcium chloride
sodium nitride
magnesium sulfide
K2O
BeF2
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‘CrossOver’ Method
magnesium ion
Mg
3-
2+
N
Mg3N2
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nitride ion
Cancel Charges (LCM)
Mg
2+
3-
N
x3
x2
6+
6-
Mg3N2
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Naming & Formulas
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Page 26 #13-16
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Naming & Formulas
2. Multivalent Ions
- Stock system (Roman numerals)
- Classical system
-ic indicates bigger charge
-ous indicates smaller charge
- reduce to lowest terms
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Naming & Formulas
eg.
lead (II) chloride
NiCl3
lead (IV) chloride
CuO
lead (IV) nitride
lead (IV) sulfide
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Cu2O
Naming & Formulas
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Page 28 #17-20
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Naming & Formulas
3. Polyatomic Ions
- a group of atoms with a charge
- cross over method / lowest terms
- BRACKETS
eg. calcium hydroxide
ammonium sulfate
PbSO4
Sn3(PO4)4
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Naming & Formulas
Common Polyatomic Ions
-Ammonium NH4+
-Hydroxide OH-Carbonate CO32-Nitrate NO3-Sulfate SO42-Hydrogen Carbonate HCO3-Hydrogen Sulfate HSO4-Phosphate PO438:12 PM
Naming & Formulas
4. Hydrates
- water mixed in with the ions
- heating removes the water to make an
anhydrous (dry) compound
- use prefixes to indicate ratio of water to ions
eg. CuSO4• 5 H2O
copper (II) sulfate pentahydrate
lithium chloride dihydrate
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Naming & Formulas
C. Acids
- acids form when hydrogen compounds
are dissolved in water
- the subscript (aq) is used to indicate
aqueous or dissolved in water
- 3 rules for naming acids
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Naming & Formulas
Ionic name
hydrogen ___ide
hydrogen ___ate
hydrogen ___ite
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
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Acid name
hydro___ic acid
______ic acid
______ous acid
Naming & Formulas
Writing Acid Names
- write the ionic name for the hydrogen
compound
- apply the correct rule for the acid name
eg. HCl(aq)
hydrogen chloride  hydrochloric acid
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Naming & Formulas
eg. HCl(aq)
hydrogen chloride  hydrochloric
acid
eg. HClO3(aq)
hydrogen chlorate  chloric acid
eg. HClO2(aq)
hydrogen chlorite  chlorous acid
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Naming & Formulas
Writing Acid Formulas
- use the correct rule to write the ionic name
- use ion charges to write the formula
eg. bromic acid
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 hydrogen bromate
 H+
BrO3
HBrO3(aq)
Naming & Formulas
hydrobromic acid  hydrogen bromide
 H+
Br 
HBr(aq)
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Practice:
Write the formulas for:
calcium phosphide
magnesium sulfide
aluminum phosphide
potassium oxide
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Write names for:
Li3N
MgO
BeF2
Al2S3
CF4
MultiValent Compounds
FeO
iron oxide
iron (III)oxide
iron (II) oxide
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Reaction Types
1. Simple Composition (Synthesis)
Element + Element  Compound
eg.
H2 + O2  H2O
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Reaction Types
2. Simple Decomposition
Compound  Element + Element
eg.
K2O  K + O2
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Reaction Types
3. Single Displacement
Compound + Element  Compound + Element
eg.
Cu +
Cl2
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AgNO3  Cu(NO3)2 +
+
NaF

F2 +
NaCl
Ag
copper wire is immersed in a silver
nitrate solution
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Solutions of potassium iodide and
lead(II) nitrate are mixed.
Potassium + lead(II) →
iodide
nitrate
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Reaction Types
4. Double Displacement
Compound + Compound  Compound + Compound
eg.
Pb(NO3)2 +
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KBr  KNO3
+ PbBr2
Reaction Types
5. Hydrocarbon Combustion
CxHy + O2(g)  CO2(g) + H2O(g)
eg.
C3H8(g) +
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O2(g) 
CO2(g) +
H2O(g)
Predicting Products
Write the name for the products in each of
the following.
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Predicting Products
Write the formula(s) for the products in each
of the following.
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Mg + O2
→ MgO
AlCl3 + CaI2 → AlI3 + CaCl2
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