Term
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Definition
| electron in the highest occupied energy level of an atom |
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Term
| The number of valence electron largely determines... |
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Definition
| the chemical properties of an element |
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Term
| what subatomic particle is used in chemical bonds |
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Definition
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Term
| How do you find the number of valence electrons an element has |
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Definition
| look at it's group number |
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Term
| How many VEs does helium have? |
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Definition
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Term
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Definition
| a notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus |
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Term
| what is shown in a electron dot structure? |
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Definition
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Term
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Definition
| - atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons |
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Term
| Who came up with the octet rule? |
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Definition
| 1916, Chemist Gilbert Lewis |
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Term
| sublevels in the octet rule |
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Definition
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Term
| By following the octet rule what VE structure do the elements form |
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Definition
| The noble gas VE structure |
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Term
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Definition
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Term
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Definition
| gain electrons from other nonmetals |
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Term
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Definition
| lose electron; metals; positive |
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Term
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Definition
| gain electron; mostly nonmetals; negative |
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Term
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Definition
| negative ion formed when a halogen atom gains an electron |
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Term
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Definition
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Term
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Definition
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Term
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Definition
| compounds composed of positive and negative ions |
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Term
| ionic compounds usually contain |
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Definition
| metal cations and nonmetal anions |
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Term
| charge of ionic compounds |
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Definition
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Term
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Definition
| the electrostatic attraction that binds oppositely charged ions together |
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Term
| what happens in an ionic bond between sodium and chlorine |
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Definition
| Sodium gives an electron to chlorine so that they both contend to the octet rule |
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Term
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Definition
| an expression that indicates the number and type of atoms present in the smallest representative unit of a substance |
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Term
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Definition
| the lowest whole number ratio of ions in an ionic compound |
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Term
| what are most ionic compounds at room temperature? |
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Definition
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Term
| What at ionic compound melting points like? |
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Definition
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Term
| why ionic compounds have high melting points |
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Definition
| they are a stable structure and are tightly packed |
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Term
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Definition
| the number of ions of opposite charge that surround each ion in a crystal |
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Term
| what can ionic compounds conduct in water |
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Definition
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Term
| when in an electrical current what happens to cations |
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Definition
| move freely to one electrode |
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Term
| anions move towards what in an electric current |
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Definition
| The electrode opposite the elctrode the cations migrated towards |
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Term
| VEs on atoms can be modeled as what? |
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Definition
| a sea of electrons- they are mobile |
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Term
| Why are metals good conductors of electricity |
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Definition
| their electrons move freely |
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Term
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Definition
| the force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions |
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Term
| metal cations move freely past each other so... |
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Definition
| metals are ductile and malleable |
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Term
| why do metal cations (+ and +) movely free past each other? |
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Definition
| drifting VEs insulate them |
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Term
| Metal atoms are arrnaged how? |
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Definition
| compact and orderly patterns |
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Term
| body centered cube has how many atom neighbors? |
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Definition
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Term
| face centered cubic has how many atom neighbors? |
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Definition
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Term
| hexagonal closed packed has how many atom neighbors? |
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Definition
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Term
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Definition
| a mixture composed of two or more elements, at least one of which is a metal |
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Term
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Definition
| they have more useful properties than metals alone |
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Term
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Definition
| components in alloy are about the same size and can replace each other in the crystal |
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Term
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Definition
| components’ atomic sizes are very different; smaller atoms fit into larger spaces |
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