Monoatomic has one atom, polyatomic has many atoms.
Work Cited:
http://wiki.answers.com/Q/Difference_between_monoatomic_ions_and_polyatomic_ions
Showing posts with label kelsey. Show all posts
Showing posts with label kelsey. Show all posts
Saturday, January 1, 2011
A class mate insists that sodium gains a postive charge when it becomes an ion because it gains a proton. Explain the students error.
The students error is you would lose an electron, not gain a proton. It's always the opposite, if there's a positive charge, you lose an electron, negative charge, gain a proton.
Why are most metals found in nature as ores that need refining and not as pure metals?
Metals are reactive and can have a more stable configuration by forming compounds.
Work Cited:
http://answers.yahoo.com/question/index?qid=20071024115125AAbVerr
Work Cited:
http://answers.yahoo.com/question/index?qid=20071024115125AAbVerr
Under the right conditions ionic substances can conduct electricity very well. Describe these conditions and explain why an ionic substance would be a poor choice as a conductor for a computer circuit board.
They are absorbed in water. They'd be a bad choice for a circuit board because they don't work in water.
Work Cited:
http://wiki.answers.com/Q/In_what_conditions_do_ionic_compounds_conduct_the_best_electricity
Work Cited:
http://wiki.answers.com/Q/In_what_conditions_do_ionic_compounds_conduct_the_best_electricity
Name two properties of metals and explain each in terms of the bonding model for metals.
High melting points
High densities
These would effect the bonding because they both have high melting points so if they bonded by melting, it would take longer. Their densities would also effect their overall product.
Work Cited:
http://chemistry.about.com/od/elementgroups/a/metals.htm
High densities
These would effect the bonding because they both have high melting points so if they bonded by melting, it would take longer. Their densities would also effect their overall product.
Work Cited:
http://chemistry.about.com/od/elementgroups/a/metals.htm
Thursday, December 30, 2010
What role does lattice energy play in forming an ionic compound?
Lattice energy plays a very important role in forming an ionic compound. Lattice energy is what gives electrons energy to move across and bond with other electrons to form a compound.
What are bond energies and how do they relate to stability of bonds?
A bond energy is the ammount of bond strength in a chemical compound. It's also the required heat to break Avogardo's number of molecules to be an individual number.
Stability of Bonds is simply the strength of a bond a compound has.
They relate because they both have to do with a chemical compound and their strength of bonding.
Work Cited:
http://en.wikipedia.org/wiki/Bond_energy
Stability of Bonds is simply the strength of a bond a compound has.
They relate because they both have to do with a chemical compound and their strength of bonding.
Work Cited:
http://en.wikipedia.org/wiki/Bond_energy
High Bond Energies of Salts are Used as an Argument by Some Scientists to Support Plans to Bury Toxic Waste in Salt Domes
Scientists believe salt domes would be a good place to store toxic wastes because they're stable enough to not let the waste come out and contaminate human resources. Also, salt isn't a very reactive compound so it would take a long time for toxic waste to react with salt.
Work Cited:
http://www.newton.dep.anl.gov/askasci/chem99/chem99023.htm
Wednesday, December 29, 2010
Energy and Stability when an Atom Chemically Bonds.
An atom becomes more stable when it forms a chemical bond. Energy can't be determined unless we know if it will gain or lose electrons.
Octet Rule
The Octet Rule is quite simple. It basically means that in order for an element to be full, it has to have a full octet. A full octet consists of eight atoms in an element. Exceptions to the rule of eight are Hydrogen and Helium which only need two.Beryllium, Alluminum, and Lithium also do not follow the Octet Rule. The Octet Rule relates to the formation of a bond because it states how many electrons is needs to correctly bond to another element.
Explain Why Atoms of the Noble Gases do not Easily Form Bonds, Unlike Other Atoms.
Noble gases don't easily form bonds like other atoms because their outter most electron shell is filled. When other atoms react, it's because they try to fill their outter most shell, but because noble gases already have theirs filled, they don't need to react. It is possible for a noble gas to reach, though.
Work Cited:
http://wiki.answers.com/Q/Why_do_the_noble_gases_not_usually_form_compounds
Work Cited:
http://wiki.answers.com/Q/Why_do_the_noble_gases_not_usually_form_compounds
Examples of Compounds Representing Ionic, Covalent, and Metallic Bonding
Ionic Bonding:
MgO
Magnesium Oxide
FeS
Iron (II) Sulfide
LiH
Lithium Hydride
Covalent Bonding:
NF3
Nitrogen Trifluoride
N2O4
Dinitrogen Tetroxide
OF2
Oxygen Diflouride
Metallic Bonding:
CuZn
Copper Zinc
Ti6O
Titanium Oxide.
You can tell the difference between Ionic, Covalent and Metallic bonding easily. Ionic bonding will always have the second element ending in -ide. With Covalent bonding, there will always be a prefix in either one or both of the elements (example: mono-one. di- two. etc). With Metallic Bonding, there will always be a number of different elements.
Work Cited:
http://www.chemistry.wustl.edu/~courses/genchem/Tutorials/Naming/covalent.htm
http://www.ausetute.com.au/namiform.html
MgO
Magnesium Oxide
FeS
Iron (II) Sulfide
LiH
Lithium Hydride
Covalent Bonding:
NF3
Nitrogen Trifluoride
N2O4
Dinitrogen Tetroxide
OF2
Oxygen Diflouride
Metallic Bonding:
CuZn
Copper Zinc
Ti6O
Titanium Oxide.
You can tell the difference between Ionic, Covalent and Metallic bonding easily. Ionic bonding will always have the second element ending in -ide. With Covalent bonding, there will always be a prefix in either one or both of the elements (example: mono-one. di- two. etc). With Metallic Bonding, there will always be a number of different elements.
Work Cited:
http://www.chemistry.wustl.edu/~courses/genchem/Tutorials/Naming/covalent.htm
http://www.ausetute.com.au/namiform.html
Three Types of Bonding: Ionic, Covalent and Metallic
Ionic Bonding:
Ionic Bonding is a chemical bond that combines a metal and nonmetal ion. The bond happens between a negatively charged ion and a positively charged ion. In an ionic bond, the metal gives at least one of its electrons to the nonmetal which makes a cation. Once the electron is transferred over to the nonmetal, an anion (negatively charged electron) is formed. When an electron is removed, more energy is created. When metals and nonmetals attract, less energy is created. When bonded atoms have more energy than the free atoms, it's called being favorable. Ionic bonding will only happen when the atoms are favorable.
Covalent Bonding:
Covalent bonding is a chemical bond that combines metals with other metals. In covalent bonding, the bonding doesn't necessarily have to happen between the same elements as long as they have comparable electronegativities. In order for a Lewis Structure with a covalent bond to be complete, there must be a full octet. A full octet mean that each element has eight electrons. When drawing a Lewis Structure, there are many things to consider. There are double bonds which is four electrons connecting an element as well as triple bonds which has six electrons connecting an element. Another thing to consider is that Hydrogen (H) has a full octet with two electrons. There can also be more than four elements connected to the central one.
Metallic Bonding:
Metallic Bonding occurs bewteen delocalised electrons and the metal nuclei. These bonds happen between solid metals and liquid metals. When metals reach their boiling point and melt, they combine. The delocalised move in a solid lattice. Mobile electrons act as charge carriers or energy carriers.
Work Cited:
http://en.wikipedia.org/wiki/Ionic_bond
http://www.chem1.com/acad/webtext/chembond/cb03.html
http://www.ausetute.com.au/metallic.html
Ionic Bonding is a chemical bond that combines a metal and nonmetal ion. The bond happens between a negatively charged ion and a positively charged ion. In an ionic bond, the metal gives at least one of its electrons to the nonmetal which makes a cation. Once the electron is transferred over to the nonmetal, an anion (negatively charged electron) is formed. When an electron is removed, more energy is created. When metals and nonmetals attract, less energy is created. When bonded atoms have more energy than the free atoms, it's called being favorable. Ionic bonding will only happen when the atoms are favorable.
Covalent Bonding:
Covalent bonding is a chemical bond that combines metals with other metals. In covalent bonding, the bonding doesn't necessarily have to happen between the same elements as long as they have comparable electronegativities. In order for a Lewis Structure with a covalent bond to be complete, there must be a full octet. A full octet mean that each element has eight electrons. When drawing a Lewis Structure, there are many things to consider. There are double bonds which is four electrons connecting an element as well as triple bonds which has six electrons connecting an element. Another thing to consider is that Hydrogen (H) has a full octet with two electrons. There can also be more than four elements connected to the central one.
Metallic Bonding:
Metallic Bonding occurs bewteen delocalised electrons and the metal nuclei. These bonds happen between solid metals and liquid metals. When metals reach their boiling point and melt, they combine. The delocalised move in a solid lattice. Mobile electrons act as charge carriers or energy carriers.
Work Cited:
http://en.wikipedia.org/wiki/Ionic_bond
http://www.chem1.com/acad/webtext/chembond/cb03.html
http://www.ausetute.com.au/metallic.html
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