Aim: How Do Metal Atoms Bond in a Metal? Do
Description: Aim: How Do Metal Atoms Bond in a Metal? Do Now: take out homework and compare responses What type of bonding occurs in metal? All metal elements have metallic bonding between each atom of that metal. Q:Which substance contains particles
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slide1. Aim: How Do Metal Atoms Bond in a Metal? Do Now: take out homework and compare responses<br>
slide2. What type of bonding occurs in metal? All metal elements have metallic bonding between each atom of that metal.
Q:Which substance contains particles held together by metallic bonds?
A) Ni(s)
B) Ne(s)
C) N2(s)
D) I2(s) Reason: Nickel is the only metal listed. Metal elements have metallic bonds between the metal atoms.<br>
slide3. Metallic Bonding Metallic bonding consists of the attraction of the free-floating valence electrons from the positively charged metal ions
Positive metal ions in a sea of electrons.
Electrons are shared amongst every metal ion. (sea of mobile electrons)<br>
slide4. Structure of Metals The metal ions are in a fixed position of a crystal lattice and the electrons are free to move throughout the lattice.
A crystal lattice describes the periodic arrays of a solid.
The bond results from the attraction between the free moving electrons and the positive ions.<br>
slide9. Questions Which type of bonding involves positive ions immersed in a sea of mobile electrons?
A) ionic
B) nonpolar covalent
C) polar covalent
D) metallic
Which factor distinguishes a metallic bond from an ionic bond or a covalent bond?
A) the mobility of electrons
B) the mobility of protons
C) the equal sharing of electrons
D) the unequal sharing of electrons Reason: The key term is sea of mobile electrons. This always refers to metallic bonds.<br>
slide10. http://cd1.edb.hkedcity.net/cd/science/chemistry/resource/animations/metallic_bond/metallic.html<br>
slide11. Conductivity of Metals Good conductors of heat
Metals conduct electricity because of the free moving electrons
Electricity is energy due to the flow of electrons<br>
slide13. Malleability of Metals Metals are malleable
When a force is applies the metal kernels move to a new location, changing the shape of a metal.<br>
slide15. Crystalline structures Metals are arranged in very compact and orderly patterns.
Metal atoms crystallize in characteristic patterns.<br>
slide16. Questions The ability to conduct electricity in the solid state is a characteristic of metallic bonding. This characteristic is best explained by the presence of
A) high ionization energies
B) high electronegativities
C) mobile electrons
D) mobile protons Reason: In an sample of metal, all the metal atoms are sharing each other’s electrons, allowing the electrons to be mobile.<br>
slide17. High melting points and boiling points Good conductor of electricity (solid and liquid) Good conductor of electricity (in solution and when melted) Ionic Compounds are brittle. Metals are malleable<br>
slide18. Alloys Alloys are mixtures composed of two or more elements, at least of which is a metal.
Alloys are usually stronger than their individual components
Steel: iron and carbon, boron, chromium, manganese, molybdenum, nickel, tungsten, vanadium.<br>
slide20. http://www.drkstreet.com/resources/metallic-bonding-animation.swf
http://www.ausetute.com.au/metallic.html
http://www.bbc.co.uk/schools/gcsebitesize/science/add_gateway_pre_2011/periodictable/metalsrev1.shtml
http://www.educationscotland.gov.uk/highersciences/chemistry/animations/bondingstructure.asp<br>
slide21. The ability to conduct electricity in a solid state is a characteristic of metallic bonding. This characteristic is best explained by A. high ionization energies
B. high electronegativities
C. mobile electrons
D. mobile protons<br>
slide22. Which element consists of positive ions immersed in a “sea” of mobile electrons? A. sulfur
B. nitrogen
C. calcium
D. chlorine<br>
slide2. What type of bonding occurs in metal? All metal elements have metallic bonding between each atom of that metal.
Q:Which substance contains particles held together by metallic bonds?
A) Ni(s)
B) Ne(s)
C) N2(s)
D) I2(s) Reason: Nickel is the only metal listed. Metal elements have metallic bonds between the metal atoms.<br>
slide3. Metallic Bonding Metallic bonding consists of the attraction of the free-floating valence electrons from the positively charged metal ions
Positive metal ions in a sea of electrons.
Electrons are shared amongst every metal ion. (sea of mobile electrons)<br>
slide4. Structure of Metals The metal ions are in a fixed position of a crystal lattice and the electrons are free to move throughout the lattice.
A crystal lattice describes the periodic arrays of a solid.
The bond results from the attraction between the free moving electrons and the positive ions.<br>
slide9. Questions Which type of bonding involves positive ions immersed in a sea of mobile electrons?
A) ionic
B) nonpolar covalent
C) polar covalent
D) metallic
Which factor distinguishes a metallic bond from an ionic bond or a covalent bond?
A) the mobility of electrons
B) the mobility of protons
C) the equal sharing of electrons
D) the unequal sharing of electrons Reason: The key term is sea of mobile electrons. This always refers to metallic bonds.<br>
slide10. http://cd1.edb.hkedcity.net/cd/science/chemistry/resource/animations/metallic_bond/metallic.html<br>
slide11. Conductivity of Metals Good conductors of heat
Metals conduct electricity because of the free moving electrons
Electricity is energy due to the flow of electrons<br>
slide13. Malleability of Metals Metals are malleable
When a force is applies the metal kernels move to a new location, changing the shape of a metal.<br>
slide15. Crystalline structures Metals are arranged in very compact and orderly patterns.
Metal atoms crystallize in characteristic patterns.<br>
slide16. Questions The ability to conduct electricity in the solid state is a characteristic of metallic bonding. This characteristic is best explained by the presence of
A) high ionization energies
B) high electronegativities
C) mobile electrons
D) mobile protons Reason: In an sample of metal, all the metal atoms are sharing each other’s electrons, allowing the electrons to be mobile.<br>
slide17. High melting points and boiling points Good conductor of electricity (solid and liquid) Good conductor of electricity (in solution and when melted) Ionic Compounds are brittle. Metals are malleable<br>
slide18. Alloys Alloys are mixtures composed of two or more elements, at least of which is a metal.
Alloys are usually stronger than their individual components
Steel: iron and carbon, boron, chromium, manganese, molybdenum, nickel, tungsten, vanadium.<br>
slide20. http://www.drkstreet.com/resources/metallic-bonding-animation.swf
http://www.ausetute.com.au/metallic.html
http://www.bbc.co.uk/schools/gcsebitesize/science/add_gateway_pre_2011/periodictable/metalsrev1.shtml
http://www.educationscotland.gov.uk/highersciences/chemistry/animations/bondingstructure.asp<br>
slide21. The ability to conduct electricity in a solid state is a characteristic of metallic bonding. This characteristic is best explained by A. high ionization energies
B. high electronegativities
C. mobile electrons
D. mobile protons<br>
slide22. Which element consists of positive ions immersed in a “sea” of mobile electrons? A. sulfur
B. nitrogen
C. calcium
D. chlorine<br>