Title: CHEMISTRY 161
1CHEMISTRY 161 Chapter 3
21. Structure of an Atom
subatomic particles
electrons (cloud)
neutrons (nucleus)
protons (nucleus)
m(n) / m(e) 2000
m(n) gt m(p)
32. Atomic Mass Number
mass number (number of protons plus neutrons)
atomic number (number of protons) (number of
electrons)
4Compounds Chemical Reactions
- Compounds
- 2. The Chemical Formula
- 3. The Chemical Equation
- 4. The Name of Chemicals
51. Compounds
molecular compounds
ionic compounds
EXPI
6Molecular Compounds
1. consist of electrically neutral particles
called molecules
2. each molecule consists of atoms
3. atoms are connected via electrons
4. connections are called bonds (springs)
EXPII
7Molecular Compounds
Group
Period IVA VA
VIA VIIA Noble Gas 2
CH4 NH3 H2O HF
Ne 3 SiH4 PH3 H2S
HCl Ar 4 GeH4 AsH3
H2Se HBr Kr 5
SbH3 H2Te HI Xe
lots of molecules contain hydrogen
EXPIII
8Jupiter
H2, He
CH4
PH3
EXPIV
9Saturn
H2O (s)
H2, He
CH4
NH3/PH3
10Ionic Compounds I
1. consist of charged particles
2. charged particles are called ions
3. ions are formed by electron transfers from
atoms
atom (neutral)
take electron(s) (oxidation)
add electron(s) (reduction)
cation(Na) (positive charge) (metal)
anion(Cl-) (negative charge) (non-metal)
11Ionic Compounds II
4. ionic compounds are held together by
electrostatic forces
non-metal
metal
NaCl
MgO
EXPV
12Compounds Chemical Reactions
1. Compounds 2. The Chemical Formula 3. The
Chemical Equation 4. The Name of Chemicals
132. The Chemical Formula
collection of chemical symbols used to describe
the composition of elements and compounds
NaCl
H2O
Fe2O3
CaSO4 ? 2 H2O
142. The Chemical Formula
collection of chemical symbols used to describe
the composition of elements and compounds
EXPVI
15F2
EXPVII
16O2
17S8
18N2
19P4
20H2
21Compounds Chemical Reactions
1. Compounds 2. The Chemical Formula 3. The
Chemical Equation 4. The Name of Chemicals
223. The Chemical Equation
chemical equation describes what happens in a
chemical reaction
chemical reaction is combination of elements
and/or compounds
?
H2 O2 H2O
2
2
balancing mass conservation
233. The Chemical Equation
2 H2 O2 ? 2 H2O
s solid l liquid g gas aq
aqueous solution
2 H2(g) O2 (g) ? 2 H2O (l)
24Examples
- phosphor with oxygen
2. sulfur with oxygen
3. methane with oxygen
25Compounds Chemical Reactions
1. Compounds 2. The Chemical Formula 3. The
Chemical Equation 4. The Name of Chemicals
26Organic Compounds
compounds containing mostly hydrogen and
carbon minor amount other elements (N, O, S, P)
hydrocarbons
H
C
alkanes
CnH2n2
27Organic Compounds?
CO2
H2CO
C4H10
CO
H2O
C4H10 combustion
EXPVIII
28Titan Saturns Largest Moon
29Cassini-Huygens Mission
30Cassini-Huygens Mission
31Inorganic Compounds
binary compounds
compounds consisting of ONLY TWO different
elements
NaCl
CO2
CaSO4
naming compounds
nomenclature
nomen (Latin) name
32Metal (Main Group) Non-Metal
part one (metal)
part two
English name of element
stem ide
NaCl
MgO
BeS
symbol stem first element
second element O ox-
oxygen oxide S
sulf- sulfur sulfide
N nitr- nitrogen
nitride P phosph- phosphorus
phosphide F fluor-
fluorine fluoride Cl
chlor- chlorine chloride
Br brom- bromine
bromide I iod- iodine
iodide
33Nomenclature Inorganic Compounds
main group metal
stem ide
element
ionic compounds (metal non-metal)
34Nomenclature Inorganic Compounds
main group metal
stem ide
element
ionic compounds (metal non-metal)
molecular compounds
prefix stem ide
prefix element
35Molecular Compounds
PF3
PF5
CO
CO2
HCl
N2O5
NO
NO2
Greek Prefixes
mono- 1 (often omitted) hexa- 6
di- 2
hepta- 7 tri- 3
octa- 8 tetra-
4 nona- 9
penta- 5 deca-
10
36Nomenclature Inorganic Compounds
main group metal
stem ide
element
ionic compounds (metal non-metal)
trans. group metal
oxstate
stem ide
element
FeO
Fe2O3
molecular compounds
stem ide
prefix element prefix
37ionic compounds
cations anions
compounds must be electrically neutral
Mn
Em-
nonmetals
metals transition metals
charge state of ions
38-/ 3/5
-/ 2/4
-2
-1
0
1
2
3
CaCl2
K2S
main group metals always start with cation
39oxidation states
NiCl2
CuO
CuCl
Mn2O3
B2O3
transition metals always start with anions
40molecular compounds
ionic compounds
polyatomic ionic compounds
ammonium chloride
sodium dichromate
magnesium carbonate
rubidium sulfate
calcium phosphate
41Nomenclature Inorganic Compounds
main group metal
stem ide
element
ionic compounds (metal non-metal)
trans. group metal
oxstate
stem ide
element
molecular compounds
stem ide
prefix element prefix
42Mass Percentage Composition
P4O10
X 100
X 100
43- Example
- A sample was analyzed and contains 0.1417 g of
nitrogen and 0.4045 g of oxygen. - Calculate the percentage composition.
X 100
1. mass of whole sample
2. percentages of elements
44MOLECULAR FORMULA
H2O
EMPIRICAL FORMULA
H2O2
HO
H2O
H2O
P2O5
P4O10
P22O25
45- Example
- A sample contains 0.522 g of nitrogen and 1.490
g of oxygen. Calculate its empirical formula.
N2O5
46COMBUSTION
CxHy
CO2
H2O
EXPIX
47COMBUSTION
C3H8
H2O
O2
CO2
0.013068 g
How many grams of oxygen are consumed?
- balance equation
- convert to moles
48- The combustion of a 5.217 g sample of a compound
of C, H, and O gave 7.406 g CO2 and 4.512 g of
H2O. - Calculate the empirical formula of the compound.
How many grams of Al2O3 are produced when 41.5 g
Al react? 2Al(s) Fe2O3(s) Al2O3(s) 2
Fe(s)
49Compounds Chemical Reactions
- Compounds
- 2. The Chemical Formula
- 3. The Chemical Equation
- 4. The Name of Chemicals
50Nomenclature Inorganic Compounds
main group metal
stem ide
element
ionic compounds (metal non-metal)
trans. group metal
oxstate
stem ide
element
molecular compounds
stem ide
prefix element prefix