Chapter 6
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Octet Rule | Atoms will gain, lose or share electrons in order to achieve a noble gas electron configuration
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| Lone pair | Pair of valence electrons that are not involved in covalent bond formation
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| Single Bond | A par of electrons shared by two atoms
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| Multiple bond | A chemical bond in which two atoms share two or more pair of electrons
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| Double bond | A multiple bond in which the atoms share two pair of electrons
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| Triple bond | A multiple bond in which the atoms share three pairs of electrons
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| Enthalpy | A thermodynamic quantity closely related to energy
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| Central atom | An atom that is bonded to more than one atom
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| Polar | Electrons are shared but not shared equally
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| Polar covalent bonds | Bonds in which electrons are unequally shared
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| Electronegativity | The ability of an atom to attract an electron pair in a covalent bond to itself (increases across a period, decreases down a group)*similar to atomic radius trend
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| Low electronegativity | Formation of cations
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| High electronegativity | Formation of anions
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| Nonpolar | Having a uniform distribution of electron density. Bonds between atoms whose electronegativities differ by less than 0.5 =purely covalent/nonpolar
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| Polar covalent | Bonds between atoms whose electronegativities range of 0.5-2.0
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| Ionic bonds | Bonds between atoms whose electronegativity differ by 2.0 or more
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| Dipole moment (μ) | Quantitative measurement of the polarity of a bond. μ= charge (Q) x distance (r) between charges
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| Formal charge | Method of electron "bookkeeping" in which shared electrons are divided equally between that atoms that share them
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| Resonance structure | Two or more equally valid Lewis structures for a single molecule that differ only in electron positions
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| Incomplete octet | Atoms with less than 4 valence electrons
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| Octet expansion | When more than eight electrons can be accommodated around the central atom. For 3rd period elements and above. (D orbitals)
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| Coordinate covalent bond/Dative bond | Bond in which one of the atoms donates both electrons
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| Molecules with ODD number of electrons | When total number of electrons is odd, not all the atoms will have complete octets, and there must be an UNPAIRED electron in the molecule
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| Free radicals | Molecules (species) with an odd number of electrons. Very reactive
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| Bond length | Distance between the nuclei of two atoms joined by a covalent bond
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| Atomic size | As atomic size increases bond length increases
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| Bond strength | The shorter the bond length the the stronger the bond strength
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Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
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Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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