Term
| Do ionic compounds usually have low or high melting points? |
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Definition
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Term
| What makes up a piece of metal? |
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Definition
| closely packed cations surrounded by mobile valence electrons that are not closely attached to a particular nucleus |
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Term
| Where is a sigma bond? Where is a pi bond? Which is stronger? |
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Definition
| in between; up and below; sigma |
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Term
| What is a oordinate covalent bond? |
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Definition
| one atom contributes two electrons |
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Term
| What is bond dissociation energy? |
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Definition
| the energy required to break a single covalent bond |
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Term
| A bond formed between two chlorine atoms would be a ______. |
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Definition
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Term
| Silver forms a cation by attaining a _________electron configuration with 18 outer elctrons including d electrons. |
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Definition
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Term
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Definition
| a mixture of elements; at least one is a metal |
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Term
| What are the two types of alloys? What is the difference between the two? |
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Definition
| subsitutional and interstitional; substitutional is when atoms of a different substance replaces the atom in the crystal; interstitial is when the atom fills in the spaces |
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Term
| What are intermolecular forces? |
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Definition
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Term
| What are the three types of intermolecular forces? |
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Definition
| dispersion, dipole, hydrogen bonds |
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Term
| Dispersion is caused by the ______. The bigger the atom the stronger the_____. |
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Definition
| the motion of electrons; force |
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Term
| What is the weakest of all the intermolecular forces? |
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Definition
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Term
| A dipole molecule has a _____and a______. |
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Definition
| positive end and a negative end |
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Term
| A special type of dipole is known as a ______. |
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Definition
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Term
| What is the strongest of all intermolecular forces? |
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Definition
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Term
| Why are hydrogen bonds the strongest of all the intermolecular forces? |
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Definition
| because it only has one proton and electron |
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Term
| During covalent bonding, atoms _____electrons. |
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Definition
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Term
| What are two names for equal electron sharing? |
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Definition
| pure covalent bonding or nonpolar covalent bonding |
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Term
| How do you determine whether an atom will have a double, triple, or single bond? |
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Definition
| look at the its number of valence electrons and count the number it needs to gain a full shell-that is the number for the bond |
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Term
| When does carbon form an sp three hybrid orbital? |
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Definition
| when it forms four bonds because it involves an s and three p orbitals |
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Term
| What does an atom have to form a network solid? What is an example of this? |
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Definition
| one atom has four covalent bonds to itself; diamond |
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Term
| In antibonding orbitals, _____is greater than attraction therefore bonding is unneccessary. |
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Definition
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Term
| Bonded pairs or unshared pairs of electrons are always trying to______. |
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Definition
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Term
| NH three has a______shape. |
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Definition
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Term
| Water is a _____molecule. |
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Definition
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Term
| When there are no unshared pairs of electrons, the shape is a _____. |
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Definition
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Term
| What are the three types of crystal structures that a metal can be? |
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Definition
| body centered cubic, face centered cubic, and hexagonal pac shape |
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Term
| What gives metals special properties? |
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Definition
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Term
| When do ionic bonds conduct electricity? |
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Definition
| when they're melted or dissolved in water |
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Term
| What is the coordination number? |
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Definition
| number of ions of opposite charge surrounding each ion in a crystal |
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Term
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Definition
| because of the electrostatic attraction between positive and negative ions |
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Term
| What does it mean when an inonic compound is electrically neutral? |
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Definition
| total positive charge is balanced by an equal negative charge |
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Term
| What do metals consist of? |
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Definition
| closely packed cations surrounded by mobile valence electrons |
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Term
| Why do ionic compounds shatter unlike metallic compounds? |
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Definition
| because pressure causes the like ions to contact and repel |
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Term
| Metal atoms arrange in closely packed orderly patterns called ______. |
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Definition
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Term
| What are the three common types of crystal structures in metals? |
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Definition
| body centered cubic, face centered cubic, and heaxagonal close packed |
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Term
| In a body centered cubic crystal structure, every atoms has_____. |
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Definition
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Term
| IN a face centered cubic crystal, every atom has ____neighbors. |
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Definition
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Term
| Hexagonal close packed crystal structures have ___neighbors but the shape is different from face centered cubic. |
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Definition
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Term
| Brass is an alloy of ____and_____. |
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Definition
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Term
| What is the most important type of alloy? |
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Definition
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Term
| What is a substitutional alloy? |
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Definition
| when an atoms is about the same size it can replace the other in the crystal |
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Term
| What is an intersitial alloy? |
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Definition
| If there is a big difference in atom sizes smaller atoms can fit into spaces (interstices )between larger atoms |
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Term
| Dipole interactions occur when _____. |
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Definition
| polar molecules are attracted to one another |
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Term
| When atoms combine, their atomic orbitals overlap producing_____. |
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Definition
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Term
| The number of overlapping atomic orbitals is equal to the number of______. |
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Definition
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Term
| Most _____contain coordinate covalent bonds. |
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Definition
| polyatomic cations and anions |
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