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