Download Ionic bonding

Happy Birthday Gertrude B. Elion (1918)
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Read for Wednesday:
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HOMEWORK – DUE Wednesday 1/25/17
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BW 3a (Bookwork): CH 3 #'s 3, 4, 11-24 all, 26, 27
WS 3 (Worksheet): (from course website)
HOMEWORK – DUE Wednesday 2/1/17
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BW 2 (Bookwork): CH 2 #'s 1-7 all, 21, 23, 36, 47-50 all, 57, 59-66 all, 81, 82, 113, 114, 116, 127, 132
WS 2 (Worksheet): (from course website)
HOMEWORK – DUE Monday 1/30/17
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Chapter 3: Sections 3-4
BW 3b (Bookwork): CH 3 #'s 41, 45, 48, 56-61 all, 68, 70, 72, 73, 78, 79, 85, 88, 95, 96, 104, 119, 124
WS 4 (Worksheet): (from course website)
Lab Wednesday/Thursday
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EXP 2
Prelab includes making flashcards!!!!
Announcements
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Course Website
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Chem 311 – Strategies for Problem Solving in Chemistry
Fridays from 12:00 – 2:25 PM in room 401
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Before There Were Atoms…
Three laws that lead to the atomic view of the atom:
1) Law of Conservation of Mass
Total mass must be same before and after a reaction
2) Law of Definite Proportions
No matter the source, a compound is always made of the same elements
in the same mass ratio
3) Law of Multiple Proportions
If two elements combine to form more than one type of compound with
each other, the masses of one element that combined with a fixed
mass of the other element are in ratios of small whole numbers
Before There Were Atoms…
Three laws that lead to the atomic view of the atom:
1) Law of Conservation of Mass
Total mass must be same before and after a reaction
I am BBQing and start with 20 pounds of charcoal. When I am done, there is only 4
pounds of ash left. How can we explain the apparent failure of the Law of Mass
Conservation?
48.0 g of carbon react with 128 g of oxygen, how much CO2 should be formed?
176 g CO2(g)
48.0 g of carbon react with 148 g of oxygen. After the reaction is complete, there
is still only 176 g of CO2 formed. Has the Law of Conservation of Mass failed?
20.0 g O2(g) left over
Before There Were Atoms…
Three laws that lead to the atomic view of the atom:
1) Law of Conservation of Mass
Total mass must be same before and after a reaction
14.71 g of CrCl3 is added to 23.41 g of Pb(NO3)2. If all of the Pb(NO3)2 is used up and
11.22 g of Cr(NO3)3 and 19.66 g of PbCl2 are produced, what mass of CrCl3 remains?
CrCl3(aq) + Pb(NO3)2(aq)  Cr(NO3)3(aq) + PbCl2(s)
total mass
start
14.71 g
23.41 g
0g
0g
38.12 g
end
?g
0g
11.22 g
19.66 g
? + 30.88 g
7.24 g
Before There Were Atoms…
Three laws that lead to the atomic view of the atom:
2) Law of Definite Proportions
No matter the source, a compound is always made of the same elements
in the same mass ratio
48.0 g of carbon react with 128 g of oxygen, forming 176 g CO2, how much CO2
should be formed from 72.0 g of carbon?
176 g CO 2 X g CO 2
=
48.0 g C
72.0 g C
72.0 g C 
X = 264 g CO2(g)
176 g CO 2
=X g CO 2
48.0 g C
Before There Were Atoms…
Three laws that lead to the atomic view of the atom:
2) Law of Definite Proportions
No matter the source, a compound is always made of the same elements
in the same mass ratio
48.0 g of carbon react with 128 g of oxygen, forming 176 g CO2, how much O2
should be react with 72.0 g of carbon?
128 g O 2 X g O 2
=
48.0 g C 72.0 g C
72.0 g C 
X = 192 g O2(g)
128 g O 2
=X g O 2
48.0 g C
Before There Were Atoms…
Three laws that lead to the atomic view of the atom:
2) Law of Definite Proportions
No matter the source, a compound is always made of the same elements
in the same mass ratio
A 219.6 kg sample of NaCl from The Great Salt Lake contains 86.4 kg of sodium, what
mass of chloride would be present in a 76.8 kg sample of NaCl from the Dead Sea?
219.6 kg NaCl – 86.4 kg Na = 133.2 kg Cl
133.2 kg Cl
X g Cl
=
219.6 kg NaCl 76.8 kg NaCl
76.8 kg NaCl 
X = 46.8 kg Cl
133.2 kg Cl
=X g Cl
219.6 kg NaCl
The Atom
 REALLY
early atomic theory…
 Democritus
~350 BC
 Atomos - Greek meaning indivisible
 Modern
Definition:
 Smallest
piece that matter can be broken up into and still maintain
the properties of an element
My Atom Broke
 Subatomic
Particles
 Nucleus
Protons
 Carry
– p+
a single positive charge
 Number of p+ = ATOMIC NUMBER
 1.673x10–24 g
VIIIA
18
IA
1
1
H
1.01
IIIA
13
IIA
2
IVA
14
VA
15
VIA
16
VIIA
17
2
He
4.00
3
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
6.94
9.01
10.81
12.01
14.01
16.00
19.00
20.18
11
12
13
14
15
16
17
18
Na
Mg
22.99
24.31
19
20
IIIB
3
IVB
4
VB
5
VIB
6
VIIB
7
VIII
8
VIII
9
VIII
10
IB
11
IIB
12
21
22
23
24
25
26
27
28
29
30
Al
Si
P
S
Cl
Ar
26.98
28.09
30.97
32.07
35.45
39.95
31
32
33
34
35
36
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
39.10
40.08
44.96
47.88
50.94
52.00
54.94
55.85
58.93
58.69
63.55
65.39
69.72
72.61
74.92
78.96
79.90
83.80
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
85.47
87.62
88.91
91.22
92.91
95.94
(99)
101.07
102.91
106.42
107.87
112.41
114.82
118.71
121.75
127.60
126.90
131.29
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.91
137.33
138.91
178.49
180.95
183.85
186.21
190.2
192.22
195.08
196.97
200.59
204.38
207.2
208.98
(209)
(210)
(222)
87
88
89
104
105
106
107
108
109
110
111
112
116
114
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
--
--
--
(223)
(226)
(227)
(261)
(262)
(263)
(262)
(265)
(266)
(271)
(272)
(277)
(285)
(289)
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
140.12
140.91
144.24
(147)
150.36
151.97
157.25
158.93
162.50
164.93
167.26
168.93
173.04
174.97
90
91
92
93
94
95
96
97
98
99
100
101
102
103
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
(232)
(231)
(238)
(237)
(244)
(243)
(247)
(247)
(251)
(252)
(257)
(258)
(259)
(260)
My Atom Broke
 Subatomic
Particles
 Nucleus
Neutrons
– no
 No
charge
 # can vary from atom to atom
1.675x10–24 g
(roughly the same mass as p+)
My Atom Broke
 Subatomic
Particles
 Outside
the nucleus
Electrons – e–
 Carry
a single negative charge
 ~1830 e – = mass of p+ or no
 9.11x10 –28 g
 Responsible for most of the chemistry that ever happens because of
their involvement in bonding
Types of Bonding : Ionic Compounds
Ionic bonding involves the complete TRANSFER of electrons
from one atom to another.
Usually observed when a metal bonds to a nonmetal.
-
-
-
+
+ + +
+ + + +
+ + +
-
-
-
-
-
+ + +
+ + +
+ + +
-
-
-
Types of Bonding : Ionic Compounds
Ionic bonding involves the complete TRANSFER of electrons
from one atom to another.
Usually observed when a metal bonds to a nonmetal.
Metals have low ionization energy, making it relatively easy to
remove electrons from them
Nonmetals have high electron affinities, making it advantageous to
add electrons to these atoms
The oppositely charged ions are then attracted to each other, resulting
in an ionic bond
Types of Bonding: Ionic Compounds

Ionic compounds tend to be hard, rigid, and brittle, with high melting points.
Types of Bonding: Ionic Compounds


Ionic compounds tend to be hard, rigid, and brittle, with high melting points.
Ionic compounds do not conduct electricity in the solid state.

In the solid state, the ions are fixed in place in the lattice and do not move.
Types of Bonding: Ionic Compounds


Ionic compounds tend to be hard, rigid, and brittle, with high melting points.
Ionic compounds do not conduct electricity in the solid state.


In the solid state, the ions are fixed in place in the lattice and do not move.
Ionic compounds conduct electricity when melted or dissolved.

In the liquid state or in solution, the ions are free to move and carry a current.
Types of Bonding: Covalent Compounds
Covalent bonding involves the SHARING of electrons
Usually observed when a nonmetal bonds to a nonmetal.
+
+
-
-
-
-
-
6p+
+
-
+
Types of Bonding: Covalent Compounds
Covalent bonding involves the SHARING of electrons
Usually observed when a nonmetal bonds to a nonmetal.
Nonmetal atoms have relatively high ionization energies, so it is difficult to
remove electrons from them
When nonmetals bond together, it is better in terms of potential energy for
the atoms to share valence electrons
Potential energy lowest when the electron is between the nuclei, holding the
atoms together by attracting nuclei of both atoms
Atoms vs. Ions

Atoms are NEUTRAL!!!!!
This means that they have zero charge
 #p+ = #e–

Charge!!!
1 p+
1 e–
–
0
47 p+
47 e–
–
0
When #p+ = #e-, the atom has no charge and is neutral
Atoms vs. Ions

Atoms can gain or lose e- to form IONS
ANY charged particle is called an ion
 Losing e- gives POSITIVELY charge

Charge!!!
11 p+ =11 p+
10 e- = 10 e–
11
When an atom
LOSES electrons
–
+1
Before
Na
After

Na+ + e-
Atoms vs. Ions

Atoms can gain or lose e- to form IONS
ANY charged particle is called an ion
 Losing e- gives POSITIVELY charge

 Called
cations
 Usually formed from metals

Gaining e- gives a NEGATIVELY charged ion
Charge!!!
16 p+ =16 p+
16 e- = 18 e–
18
When an atom
GAINS electrons
–
–2
Before
S
S + 2e-
After

S2- + 2e
S2-
WRONG!!
Atoms vs. Ions

Atoms can gain or lose e- to form IONS
ANY charged particle is called an ion
 Losing e- gives POSITIVELY charge

 Called
cations
 Usually formed from metals

Gaining e- gives a NEGATIVELY charged ion
 Called
anions
 Usually formed from non-metals
My Atom Broke
 Subatomic
Particles
 Nucleus
Neutrons
No
– no
charge
# can vary from atom to atom
+
+
16p
16no
16p
o
17n
16p+
o
18n
16p+
20no
+
+
16p
16no
16p
o
17n
16p+
o
18n
16p+
20no
Mass of no about equal to mass of p+
16p+
16no
16p+
17no
16p+
18no
16p+
20no
Do each of these atoms have the same mass?
Isotopes: Atoms having the
same atomic number,
but different atomic
masses
+
Atomic symbols
16p
16no
Mass number = # p+ + # no
16p+
17no
A
E
S
16
Z
16p+
18no
Atomic number
16p+
20no
Symbol of
element
16p+
16no
32
S
16
16p+
17no
33
S
16
16p+
18no
34
S
16
16p+
20no
36
S
16
A
E
Z
32
S
16
Shorthand: Sulfur-33
S-36
36S