click below
click below
Normal Size Small Size show me how
Unit 6 Chemistry
Question | Answer |
---|---|
Chemical Bond | Force that holds two atoms together |
Atoms try to form an octet (stable arrangement of eight valence electrons in the outer energy level) | Gaining or losing valence electrons |
Ionic Bond | Elecrostatic force that holds oppositley charged particles together |
Characteristic of ionic bonding in ionic solids | The charge of the compund is neutral and is highly organized |
Crystal Lattice | A three dimensional geometric arrangement of particles that is highly orgaized. Each ion is surrounded by opposite charged ions which results in strong attraction |
1+ charge of ion | Group 1 |
2+ charge of ion | Group 2 |
3- charge of ion | Group 15 |
2- charge of ion | Group 16 |
3- charge of ion | Group 17 |
Cations | loses one valence electron. Ex) 2p6 3S1 = 2p6 |
Anions | gains one valence electron. Ex) 2p6 = 2p6 3S1 |
positive ions | formed from the loss of elecrons to form an octet |
negative ions | formed from gaining electrons to form an ctet |
Transition metals achieve ion formation | Typically lose their s electrons to form a 2+ charge and somtimes lose electrons from the d sublevel. Ex) 4S2 3D6 = 3D6 |
explanation of Cations, Anions, and electron configurations | Cations are positive, so they must lose electrons to become neutral. Anions are negative, so they must gain electrons to become neutral. |
Example of a Cation and electron configurations | Na : 1s2 2s2 2p6 3s1, Na+: 1s2 2s2 2p6 |
Ionic Compund | Compund that contains an ionic bond. Ex) NaCl |
General properties of ionic compunds | Repeating patter of Cations and Anions surrounding each other. Ex) crystal lattice |
strength and examples of ionic bonds | very strong. Ex) high melting point, high boiling point, strong brittle solids |
lattice energy size | compounds with higher charges on the ions have more lattice energy |
general properties and lattice energy | the more lattice energy an ionic bond has, the stronger the general properties are |
four rules for writing a formula unit for an ionic compound | 1. cations symbol then anions symbol. 2. subscripts = number of atoms in each elements. 3. charge must equal zero. 4. must have parenthesis if more than one (polyatomic ions) in compound |
five rules for nameing an ionic compound | 1. cation then anion. 2. use element name (monatomic). 3. use suffix ide (monatomic). 4. use roman numerals. 5. name cation then polyatomic |
metallic bond | bond between the positive metal cations and the delocalized valence electrons. the electron sea model describes how the valence electrons in a metal lattice are shared among all the cations. they can move freely |
five direct properties of metals that are a result of metallic bonding | very strong, high melting and boiling points, malleable and ductile, good conductivity. |
alloys | homogeneous mixture of elements with metallic properties. substitutional (brass and bronze) or interstital (steel and cast iron) |
compare ionic and metallic bonds | both bond in a crystal lattice structure. both have cations but ionic has anions and metallic has delocalized electrons |