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19 Cards in this Set
- Front
- Back
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what are properties of ionic, covalent, and metallic bonds
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ionic: high melting & boiling points, form crystals, dissolve in water, conduct electricity in water, very hard and brittle
covalent: lower melting and boiling points, generally softer than ionic compounds, usually more flammable, do not conduct electricity in any form, do not dissolve in water, often produce an odor metallic: very high melting and boiling points, not easily torn apart (ductile and malleable), conduct electricity as solids |
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draw lewis structures
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k
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what is a cation
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j
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what is an anion
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k
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how do cations and anions form
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atoms form ions by gaining (anions) or losing (cations) electrons to obtain a full valence level of electrons
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practice all that stuff of naming
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j
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acid
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k
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anion
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k
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binary acid
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k
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binary compound
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k
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cation
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k
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covalent bond
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in lewis structures, they share electrons
non metal to non metal |
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ionic bond
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electrons are gained or lost, happens between a metal and a non metal; the metal loses and the non metal gains the electron
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lewis dot diagram
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a method for depicting valence electrons and interactions of atoms
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metallic bond
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the elements create an electron pool; happens between 2 metals
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monatomic ion
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ion consisting of a single atom
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oxyacid
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k
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oxyanion
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k
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polyatomic ion
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ion consisting of more than one atom
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