Chemical Bonds

1
Chemical Bonds
nucleus
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
2
Chemical Bonds

proton
neutron
-
electron
nucleus
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
3
Chemical Bonds
Name
Atomic Number
Be
Symbol
Atomic Mass

proton
neutron
-
electron
nucleus
electron cloud
Be
Orbital Notation
Be
Electron Configuration
Be
Electron-Dot (Lewis-Dot) Structure
4
Chemical Bonds
Name
Atomic Number
O
Symbol
Atomic Mass

proton
neutron
-
electron
nucleus
electron cloud
O
Orbital Notation
O
Electron Configuration
O
Electron-Dot (Lewis-Dot) Structure
5
Draw orbital notations for the following
Draw electron configurations for the following
Draw electron-dot (Lewis-Dot) structures for the
following
C
C
C
Ne
Ne
Ne
Mg
Mg
Mg
P
P
P
Ca
Ca
Ca
6
Forming an Ionic Bond
Na
Na
3s
Cl
Cl
Cl
1s
2s
3s
2p
3p
7
Forming an Ionic Bond
Na
Na
Cl
Cl
Cl
1s
2s
3s
2p
3p
Be
Be
Be
1s
O
O
O
1s
2s
2p
8
Chemical Bond
A. Ionic Bond
9
A. Ionic Bond
10
Properties of Ionic Compounds
-when ionic compounds form, they form a
_____________, a ________________ _________
arrangement of _______ and ________ ions
-the energy required to separate _______ (6.02 x
1023) of ions from each other is called the
________________, the more ________ the lattice
energy, the ______ the attraction between ions
-the strength of the attraction between ions
affects the compounds __________ _________
11
Properties of Ionic Compounds
A. Lattice Energy
12
Properties of Ionic Compounds
A. Lattice Energy
0
-200
-400
F
Cl
-600
Br
-800
I
-1000
-1200
Li
Na
K
13
Properties of Ionic Compounds
A. Lattice Energy
-the lattice energy is more negative in ionic
compounds that have ____________________,
because the ions are ___________________ to each
other
B. Melting and Boiling Points
14
Properties of Ionic Compounds
B. Melting and Boiling Points
-ionic compounds with higher lattice energies
have _________melting and boiling points temps.
-smaller ions are more ________ attracted to
each other, because the _______ is closer to the
_______ _________, while ions with larger
positive and negative charges are more ________
attracted to each other
C. Electrical Conductivity
-to conduct electricity, charged particles must
be _________________, so ionic compounds
generally do not conduct electricity as a _____,
but generally do as a ______ or when
______________ _______________
15
Properties of Ionic Compounds
D. Hardness
-the ions in ionic compounds with
_______________ lattice energies are more
_________ attracted to each other, so they tend
to be ________
For Review
1. Rank the following ionic compounds, in order,
from most negative to least negative lattice
energy RbCl, RbF, RbBr, RbI
2. Rank the following ionic compounds, in order,
from highest to lowest melting point
temperature NaCl, MgCl2, MgO
3. Rank the following ionic compounds, in order,
from softest to hardest Li2O, Li2S, Li2Te,
Li2Se
4. Rank the following ionic compounds, in order,
from ions most strongly to ions least
strongly attracted to each other MgF2, RbCl,
CaF2, CaCl2, MgO
16
Naming Ionic Compounds
1. MgF2 ___________________
2. Rb2S ___________________
3. Ba(NO3)2 ___________________
4. (NH4)2Te ___________________
5. (NH4)3PO4 ___________________
6. Na2SO4 ___________________
7. Cu3P ___________________________________
8. Fe(OH)3 ________________________________
9. Cr2(CO3)3 _____________________________________
__
10. Sn(HCO3)4 ____________________________________
______
17
Metallic Bonds
-like ionic compounds, metals in their ______
state form ________ structures
-each metal atom contributes its _______
_________ to a ___________ _____ of electrons,
which move freely throughout the solid
-without its ________ _________, each metal atom
forms a _________ _______
-the attraction between the ________ _________
and the _____________ ___________ is called a
_________ _____
Properties of Metals
-influenced strongly by the strength of
attraction between the _______ ________ and the
number of ____________ ___________
18
Properties of Metals
A. Melting Point
-since it doesnt matter where the _________
_______ are within the _______ __________ of the
metal, the cations _______ _________ easily,
while still remaining in ______ _______ with
each other, so ________ _______ temperatures
are relatively ____
-the _________ the attraction between ________
________ and the ____ of ______________
__________, the ________ the melting point
temperature, so ________ atoms tend to have
_______ melting point temperatures.
19
Properties of Metals
A. Melting Point
20
Properties of Metals
A. Melting Point
-________ _______ temperatures are _________ by
increasing the number of ________ ________
contributed to the _____ of ______________
__________. ___________ __________ like _______
and _________ contribute their ______ ________
electrons as well as their __________ __________
to the ____ of ________________ __________,
__________ the melting point temperature
dramatically.
21
Properties of Metals
B. Malleability Ductility
-because particles in a metal can easily change
position, they are __________, or can be
__________ _____ _______ or other shapes easily
-because particles in a metal can easily change
position, they are __________, or can be
__________ _____ _______
C. Durability Boiling Point
-even though particles in a metal can easily
change position, they are __________
____________, to the ____ of __________
surrounding them, and are __________ to _______
from the metal, giving them a high ___________
and a high ________ ______ temperature as well
22
Properties of Metals
D. Conductivity
-because __________ __________ in a metal are
_____ ___ _____ while keeping _________ ______
intact, the __________ move _____ from place to
place easily, so metal are _____ ___________ of
_____
-because __________ __________ in a metal are
_____ ___ _____, they move easily as a part of
an ________ ________ when an __________
__________ or ________ is applied to the metal,
and the ________ ________ structure of the
__________ ________ allows the __________ to
flow without _________ with the ________, which
allows for little __________
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Properties of Metals
E. Luster
-because ____________ ___________ are free to
move, they can interact with ______, __________
and __________ ________ of _______, giving
metals their _______ ________
F. Hardness Strength
-as the number of ___________ __________
contributed to the ____ of _________ increases,
the strength of the _________ _____ increases,
so metals such as _______, which contribute ____
________, are relatively _____ and _____, while
metals that contribute their outer __ electrons
plus their inner __ electrons such as _________,
_____, or _______ are relatively _____ and
_______
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Metal Alloys
-because it doesnt matter what _________ the
_________ ________ are in in a metal, it is easy
to introduce other _________ __________ into the
________ structure of a metal, creating an
______, or ________ of metals
-in ______________ _______, atoms of one kind of
metal, like _______, are replaced with atoms of
another kind of metal, like _______, to form an
______ like ________ _______, which has the
properties of both metals. Pure _____ is
beautiful, rare, and almost completely
_________, and so is highly valuable, but it is
too _____ to be of much use by itself, so it is
________ with ________ and ______ to make
_________ or _________ _____, which is still
beautiful, but much _______ and _________
-in ______________ _______, atoms of another kind
of element, like _______, are inserted into the
spaces in between the cations of a metal like
_____ to form _______ ______, which is _______,
________, and less ________ than _____