Post on 12-Nov-2014
description
Muddiest Point – Bonding Defini1on Video
Bonding Visual Glossary!"#$%!&"'- High electrical conductivity due to half full or overlapping band gap. Metals are generally the best conductors due to their delocalized electrons.
!"()*+#&,-"#$- Sharing of electrons between two or more atoms. (Primary bond)
!"#$%&'%(%)*$+$,-')#$.,/'
!"#$%&'%(%)*$+$,-'"0&$,1%#*,-!
2
2
2
2
3
32 4
!"%*".-/!,0"'!+- An attractive or repulsive bonding force between two partially charged particles
$/1"*+,21+'.)#+#&3- Slightly stronger attraction or repulsion force than temporary dipole between two polar molecules
$/1"*+,2&+.1"')'43-Momentary attraction or repulsion between two polar molecules
+*+!&'"#+5)&/(+- An atom that is likely to accept valance electrons
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# +*+!&'"1"6/&/(+- An atom that is likely to donate a Valance electron
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# ."$%*%6,"0,+*)6&/!/&4,2738 The stiffness of the material when the material is undergoing deformation. The stronger the bond, the stiffer the material.
94$'"5+#,-"#$- Bonding of hydrogen atoms to the most electronegative atom in the molecule
/#6%*)&"'8 Low electrical conductivity due to a large band gap.
/"#/!,-"#$- Transfer of electrons from two oppositely charged ions
/6"&"1+- Atoms of the same element but have different numbers of neutrons and therefore different atomic mass
Attractive Force = opposite charged particle
Repulsive Force= same charged particle !"#$%$& "' (%)&*+,+*-
.%"/0 1.*20&&3 .*2)+45 "'*60 %+40)2 0%)&*+, 207+"4
Bonding Visual Glossary!"#$%!&"'- High electrical conductivity due to half full or overlapping band gap. Metals are generally the best conductors due to their delocalized electrons.
!"()*+#&,-"#$- Sharing of electrons between two or more atoms. (Primary bond)
!"#$%&'%(%)*$+$,-')#$.,/'
!"#$%&'%(%)*$+$,-'"0&$,1%#*,-!
2
2
2
2
3
32 4
!"%*".-/!,0"'!+- An attractive or repulsive bonding force between two partially charged particles
$/1"*+,21+'.)#+#&3- Slightly stronger attraction or repulsion force than temporary dipole between two polar molecules
$/1"*+,2&+.1"')'43-Momentary attraction or repulsion between two polar molecules
+*+!&'"#+5)&/(+- An atom that is likely to accept valance electrons
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# +*+!&'"1"6/&/(+- An atom that is likely to donate a Valance electron
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# ."$%*%6,"0,+*)6&/!/&4,2738 The stiffness of the material when the material is undergoing deformation. The stronger the bond, the stiffer the material.
94$'"5+#,-"#$- Bonding of hydrogen atoms to the most electronegative atom in the molecule
/#6%*)&"'8 Low electrical conductivity due to a large band gap.
/"#/!,-"#$- Transfer of electrons from two oppositely charged ions
/6"&"1+- Atoms of the same element but have different numbers of neutrons and therefore different atomic mass
Attractive Force = opposite charged particle
Repulsive Force= same charged particle !"#$%$& "' (%)&*+,+*-
.%"/0 1.*20&&3 .*2)+45 "'*60 %+40)2 0%)&*+, 207+"4
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Primary Bonding
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Bonding Visual Glossary!"#$%!&"'- High electrical conductivity due to half full or overlapping band gap. Metals are generally the best conductors due to their delocalized electrons.
!"()*+#&,-"#$- Sharing of electrons between two or more atoms. (Primary bond)
!"#$%&'%(%)*$+$,-')#$.,/'
!"#$%&'%(%)*$+$,-'"0&$,1%#*,-!
2
2
2
2
3
32 4
!"%*".-/!,0"'!+- An attractive or repulsive bonding force between two partially charged particles
$/1"*+,21+'.)#+#&3- Slightly stronger attraction or repulsion force than temporary dipole between two polar molecules
$/1"*+,2&+.1"')'43-Momentary attraction or repulsion between two polar molecules
+*+!&'"#+5)&/(+- An atom that is likely to accept valance electrons
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# +*+!&'"1"6/&/(+- An atom that is likely to donate a Valance electron
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# ."$%*%6,"0,+*)6&/!/&4,2738 The stiffness of the material when the material is undergoing deformation. The stronger the bond, the stiffer the material.
94$'"5+#,-"#$- Bonding of hydrogen atoms to the most electronegative atom in the molecule
/#6%*)&"'8 Low electrical conductivity due to a large band gap.
/"#/!,-"#$- Transfer of electrons from two oppositely charged ions
/6"&"1+- Atoms of the same element but have different numbers of neutrons and therefore different atomic mass
Attractive Force = opposite charged particle
Repulsive Force= same charged particle !"#$%$& "' (%)&*+,+*-
.%"/0 1.*20&&3 .*2)+45 "'*60 %+40)2 0%)&*+, 207+"4
Bonding Visual Glossary!"#$%!&"'- High electrical conductivity due to half full or overlapping band gap. Metals are generally the best conductors due to their delocalized electrons.
!"()*+#&,-"#$- Sharing of electrons between two or more atoms. (Primary bond)
!"#$%&'%(%)*$+$,-')#$.,/'
!"#$%&'%(%)*$+$,-'"0&$,1%#*,-!
2
2
2
2
3
32 4
!"%*".-/!,0"'!+- An attractive or repulsive bonding force between two partially charged particles
$/1"*+,21+'.)#+#&3- Slightly stronger attraction or repulsion force than temporary dipole between two polar molecules
$/1"*+,2&+.1"')'43-Momentary attraction or repulsion between two polar molecules
+*+!&'"#+5)&/(+- An atom that is likely to accept valance electrons
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# +*+!&'"1"6/&/(+- An atom that is likely to donate a Valance electron
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# ."$%*%6,"0,+*)6&/!/&4,2738 The stiffness of the material when the material is undergoing deformation. The stronger the bond, the stiffer the material.
94$'"5+#,-"#$- Bonding of hydrogen atoms to the most electronegative atom in the molecule
/#6%*)&"'8 Low electrical conductivity due to a large band gap.
/"#/!,-"#$- Transfer of electrons from two oppositely charged ions
/6"&"1+- Atoms of the same element but have different numbers of neutrons and therefore different atomic mass
Attractive Force = opposite charged particle
Repulsive Force= same charged particle !"#$%$& "' (%)&*+,+*-
.%"/0 1.*20&&3 .*2)+45 "'*60 %+40)2 0%)&*+, 207+"4
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Dipoles and Polar Molecules Dipole: A separa1on of posi1ve and nega1ve charges. Caused by unbalanced electron clouds.
Bonding Visual Glossary!"#$%!&"'- High electrical conductivity due to half full or overlapping band gap. Metals are generally the best conductors due to their delocalized electrons.
!"()*+#&,-"#$- Sharing of electrons between two or more atoms. (Primary bond)
!"#$%&'%(%)*$+$,-')#$.,/'
!"#$%&'%(%)*$+$,-'"0&$,1%#*,-!
2
2
2
2
3
32 4
!"%*".-/!,0"'!+- An attractive or repulsive bonding force between two partially charged particles
$/1"*+,21+'.)#+#&3- Slightly stronger attraction or repulsion force than temporary dipole between two polar molecules
$/1"*+,2&+.1"')'43-Momentary attraction or repulsion between two polar molecules
+*+!&'"#+5)&/(+- An atom that is likely to accept valance electrons
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# +*+!&'"1"6/&/(+- An atom that is likely to donate a Valance electron
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# ."$%*%6,"0,+*)6&/!/&4,2738 The stiffness of the material when the material is undergoing deformation. The stronger the bond, the stiffer the material.
94$'"5+#,-"#$- Bonding of hydrogen atoms to the most electronegative atom in the molecule
/#6%*)&"'8 Low electrical conductivity due to a large band gap.
/"#/!,-"#$- Transfer of electrons from two oppositely charged ions
/6"&"1+- Atoms of the same element but have different numbers of neutrons and therefore different atomic mass
Attractive Force = opposite charged particle
Repulsive Force= same charged particle !"#$%$& "' (%)&*+,+*-
.%"/0 1.*20&&3 .*2)+45 "'*60 %+40)2 0%)&*+, 207+"4
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Secondary Bonding
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Van der Waals
Proper1es Related to Bonding
Bonding Visual Glossary!"#$%!&"'- High electrical conductivity due to half full or overlapping band gap. Metals are generally the best conductors due to their delocalized electrons.
!"()*+#&,-"#$- Sharing of electrons between two or more atoms. (Primary bond)
!"#$%&'%(%)*$+$,-')#$.,/'
!"#$%&'%(%)*$+$,-'"0&$,1%#*,-!
2
2
2
2
3
32 4
!"%*".-/!,0"'!+- An attractive or repulsive bonding force between two partially charged particles
$/1"*+,21+'.)#+#&3- Slightly stronger attraction or repulsion force than temporary dipole between two polar molecules
$/1"*+,2&+.1"')'43-Momentary attraction or repulsion between two polar molecules
+*+!&'"#+5)&/(+- An atom that is likely to accept valance electrons
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# +*+!&'"1"6/&/(+- An atom that is likely to donate a Valance electron
2% '
5 % '
6$ '
7$ '
8% '
9/ '
:/%$*'1#!%
!'
#))%;*'<%'
#))%;*'=%'
1:>%'?;'<%'
1:>%'?;'=%'
1:>%'?;'@%'
A 'B: ' C% '
D%*#( '
5,/-%*#( '
E/*%$-%&:#*% '
2 '
5# ' 3( '
C$ '
E '
6* '
F '
G 'D1 '
3# '
G$ '
C# '
9# '
7 '
9. '
3! '
A$ '
G) '
H '
G% '
I% '
J, '
!"#$%&'(')*%*+# !"#$%&',#-.%*+# ."$%*%6,"0,+*)6&/!/&4,2738 The stiffness of the material when the material is undergoing deformation. The stronger the bond, the stiffer the material.
94$'"5+#,-"#$- Bonding of hydrogen atoms to the most electronegative atom in the molecule
/#6%*)&"'8 Low electrical conductivity due to a large band gap.
/"#/!,-"#$- Transfer of electrons from two oppositely charged ions
/6"&"1+- Atoms of the same element but have different numbers of neutrons and therefore different atomic mass
Attractive Force = opposite charged particle
Repulsive Force= same charged particle !"#$%$& "' (%)&*+,+*-
.%"/0 1.*20&&3 .*2)+45 "'*60 %+40)2 0%)&*+, 207+"4
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Bonding Visual Glossary!"#$%&'()*%&$(+,!- - Temperature at which the material changes physical states from solid to liquid. General trend is that when the bonding strength of a pure metal is stronger, the melting point is at a higher temperature.
!"$.##%/(0*&1- Mutually shared delocalized valence electrons (“sea of electrons”) by all the atoms in a metal
!*#"- The quantity of a substance corresponding to 6.023x1023 atoms or molecules 2.3#%(45/#36%*&(27%&/%)#"- Either one or two electrons with different spins can occupy an electron state at one time
)*#.7(!*#"/3#"- A molecule that has a nonzero permanent or temporary dipole moment
)7%!.78(0*&1%&'- Ionic, covalent, and metallic bonds whose bonding energies are large and have strong interatomic bonds
Metallic Ionic Covalent 6"/*&1.78(0*&1%&'- Van de waals and hydrogen bonding whose bonding energies and interatomic strength are smaller and weaker than the primary bonds 6"!%/*&13/$*76- Good electrical conductivity for a nonmetallic material due to the filled valence band and small energy band gap.
$9"7!.#("5).&6%*&(+ -- Change in length as thermal energy is either added or released to a material. The material with the stronger bonding will not expand as much as a material with weaker bonding when the same amount of thermal energy is applied. Tungsten Rod Aluminum rod
:.&(1"7(;..#6(0*&1- A secondary interatomic bond between neighboring atomic or molecular dipoles (permanent or temporary)
;.:"<!"/9.&%/.#(!*1"#- An atomic model where the electrons are thought to be wave-like
!"#$%&'# ()*+,'#&
!"#$%&'# -./ 0+% &0' 0)$0'%&,'*&)#$ 12)#& 2( 345627 28 95:62;
Tungsten Rod
Aluminum rod
Chapter 2 - 23
• Coefficient of thermal expansion,
What is Coefficient of Thermal Expansion
!" (T2-T1)LLo
coeff. thermal expansion
L
length, Lo
unheated, T1
heated, T2
It is the rate of change of length of a material with temperature change.
For a given T, lower L/Lo means lower and higher bond strength
!" L /Lo
TChapter 2 - 23
• Coefficient of thermal expansion,
What is Coefficient of Thermal Expansion
!" (T2-T1)LLo
coeff. thermal expansion
L
length, Lo
unheated, T1
heated, T2
It is the rate of change of length of a material with temperature change.
For a given T, lower L/Lo means lower and higher bond strength
!" L /Lo
T
Coefficient of Thermal Expansion It is the rate of change of length of a material with temperature change.
For a given ΔT, lower ΔL/Lo means lower α and higher bond strength
Δ L
length, L o The image cannot be displayed. Your computer may not have enough me
unheated, T 1
heated, T 2