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18 Cards in this Set
- Front
- Back
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Chemical Bond |
-a force that holds 2 atoms together -Ionic Bonds -Covalent Bond |
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Ionic Bond |
-a force between metals(cations) and non-metals(anions) by transferring electrons |
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Covalent Bond |
-a force between 2 non-metals that share electrons -covalently bonded compound = molecule |
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Octet Rule |
-atoms always want 8 valance electrons (to make a full outer shell) -*except Hydrogen(H) only wants 2 |
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Electronegativity |
-how likely an atom is to attract an electron in a chemical bond -electronegativity= 1.7 or higher = ionic bond -electronegativity = 1.6 or lower = covalent bond |
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Naming Ionic Compounds |
1) Name of the metal 2) Name of the non-metal with suffix -ide Ex. Calcium + Nitrogen = calcium nitride |
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Chemical Formula |
-overall charge for a compound is zero - neutral -everything must end up with a full octet (valance shell) |
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Criss Cross |
-the charge of the opposite ion becomes the subscript in the chemical formula Ex. K 1+ S 2- ---> K2S |
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Monatomic Ions |
-ions made up of ONE type of element Ex. K 1+ , Mg 2+ , N 3- Ex. Mg3N2 = an ionic compound made of two different monatomic ions |
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Polyatomic Ions |
-ions made up to 2 OR MORE types of elements Ex. NO3 1- = nitrate *subscripts DO NOT indicate charge |
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Transition Metals |
-always located on the d-block -always cations +1, +2, +3, +4 -no rules on what the charge can be (random) -use roman numerals - copper 2+ = copper (II) |
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Covalent Prefixes |
-prefixes are used to indicate the number of atoms of each element in the bond 1- mono 2 - di 3 - tri 4 - tetra 5 - penta 6 - hexa 7 - hepta 8 - octa 9 - nona 10 - deca *don't use the prefix 'mono'(1) on the first atom when naming the bond |
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Naming System |
1) use a prefix to indicate the number of the 1st element unless it's 1 (mono) 2) name the 1st element 3) use a prefix to indicate the number of the 2nd element 4) use suffix -ide at the end of the name |
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Diatomic Elements |
-2 atoms of the same element bonded together (all non-metal/all covalent) Ex. O bonded to O = O2 |
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Electron Pairs & Lone Electrons |
-electron pairs - electrons that are paired with another electron of the same atom - these electrons can't form bonds with other electrons -lone electrons - electrons that aren't paired with another electron - these electrons always from bonds with electrons of another atom |
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Central Atom |
-the central atom is the element that comes 1st in the chemical formula *except when the 1st one is hydrogen *can have more than 1 central atom |
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Steps to Making Lewis Dot Structures for Covalent Bonds |
1)identify the central atom and draw the chemical symbol with valance electrons 2)identify the bonding electrons of the central atom *only build off of bonding electrons 3) fill in the 2nd element where the bonding electrons are 4)fill in the valance electrons for the other atoms |
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Bonds of Covalent Bonds |
-solid line(s) used to represent the types of bonds between atoms 1 bond - 1 shared electron - 1 line *weakest 2 bonds - 2 shared electrons - 2 lines 3 bonds - 3 shared electrons - 3 lines *strongest |
