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
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Term
| Characteristics Ionic Bond |
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Definition
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Term
| Characteristics Covalent Bond |
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Definition
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Term
| Characteristics Metallic bond |
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Definition
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Term
| When forming covalent bonds, atoms want to… |
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Definition
| …share electrons to complete their valence |
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Term
| Hydrogen has 1 valence electron |
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Definition
| Hydrogen needs 2 e- to complete valence |
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Term
| Why isn't fluorine stable? |
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Definition
| Fluorine only has 7 valence electrons. |
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Term
| Definition: Electronegativity |
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Definition
| Attraction of an atom for valence e- in a chemical bond |
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Term
| Completely covalent bonds are between which type of atoms? |
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Definition
| Atoms of the same element |
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Term
| Range for non-polar covalent bonds |
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Definition
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Term
| Range for polar covalent bonds |
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Definition
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Term
| Determining electronegativity of bonds |
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Definition
| Take the absolute value of the difference in electronegativity of two atoms |
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Term
| Electrons in covalent bond are localized closer to which atom? |
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Definition
| The atom with the greater electronegativity |
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Term
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Definition
| Partially negative charged |
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Term
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Definition
| Partially positive charged |
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Term
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Definition
| Symbol for direction of dipole movement |
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Term
| Step 1 for building molecules |
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Definition
| Determine total number of valence electrons (all atoms) |
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Term
| Hint for Step 1 of building molecules |
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Definition
| If - charge, add 1 electron for every - charge. For + charge, subtract 1 electron. |
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Term
| Step 2 for building molecules |
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Definition
| Determine number of electrons needed to FILL valence |
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Term
| Step 3 for building molecules |
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Definition
| Take half the number of bonding electrons |
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Term
| Step 4 for building molecules |
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Definition
| Calculate # non-bonding electrons. Subtract bonding (step 1) from valence (step 2). |
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Term
| Step 5 for building molecules |
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Definition
| Build molecule, remembering to complete valence and add lone pair electrons if necessary. |
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Term
| Definition: Formal Charge |
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Definition
| The charge an atom would have it all bonding electrons were shared equally between bonded atoms |
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Term
| Formula for formal charge |
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Definition
| # valence electrons - # non-bonding electrons - # bonds gives the charge. |
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Term
| What kinds of atoms have formal charge? |
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Definition
| Only atoms that do not have the typical number of bonds have a formal charge. |
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Term
| What's the pattern for electronegativity on the periodic table? |
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Definition
| Electronegativity increases towards fluorine (up and right) |
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Term
| Step 1 for building molecules with expanded octets |
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Definition
| Work with the number of valence electrons |
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Term
| Step 2 for building molecules with expanded octets |
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Definition
| Place the less electronegative atom in the central location |
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Term
| Step 3 for building molecules with expanded octets |
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Definition
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Term
| Step 4 for building molecules with expanded octets |
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Definition
| Use the remaining valance electrons to first complete the octets for terminal atoms |
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Term
| Step 5 for building molecules with expanded octets |
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Definition
| Remaining valence electrons are placed on the central atom. |
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