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covalent bonding

QuestionAnswer
Covalent Bonding Bonding between a non-metal and a non-metal where electrons are shared between 2 atoms , often resulting in the formation of molecules.
Properties of Covalent (Molecular) Compounds Soft materials with low melting points/boiling points that generally cannot conduct electricity. Polar molecules dissolve well in water, but non-polar molecules do not.
Binary Covalent Compound A covalent compound containing exactly 2 elements that are both non-metals.
Covalent Naming Prefixes mono – one, di – two, tri – three, tetra – four, penta – five, hexa – six, hepta - seven, octa – eight, nona - nine, deca - ten.
Naming a Binary Covalent Compound Use prefixes to show the atom count, omit "mono" on the first element but use it on the second, change the second element's ending to –ide, and drop the "a" or "o" from a prefix if the element begins with a soft vowel.
Writing the Formula of a Binary Covalent Compound Convert the prefixes from the compound's name into numerical subscripts in the chemical formula, and do not write a subscript of “1”.
Common Covalent Names to Memorize H2O is water, CH4 is methane, and NH3 is ammonia.
Polar Covalent Bond A bond between 2 atoms of different non-metal elements where electrons are shared unequally, meaning the more electronegative atom hogs the electrons and becomes partially negative.
Nonpolar Covalent Bond A bond between 2 atoms of the same element where electrons are shared equally, meaning neither atom hogs electrons and no partial charges form.
Coordinate Covalent Bond A special covalent bond in which both of the shared bonding electrons come from the same single atom.
VSEPR Theory The valence shell electron pair repulsion theory, which states that bonding and non-bonding electronpairs around a central atom repel one another and move as far apart as possible in three dimensions to determine molecular shape.
Nonpolar Molecules Symmetrical molecules with an equal distribution of charge where any partial charges cancel each other out.
Polar Molecules Asymmetrical molecules with an unequal distribution of partial charge where partial charges do not cancel out.
Intermolecular Forces of Attraction (IMFs) Relatively weak attractions between multiple molecules, where stronger IMFs result in higher melting points and boiling points.
Three Types of IMFs London Dispersion Forces, Dipole – Dipole Attractions, and Hydrogen Bonding.
Molecule – Ion Attraction An attraction in water where ionic substances break apart, causing positive ions to be attracted to partial negative oxygen ends and negative ions to be attracted to partial positive hydrogen ends.
Network Solids Structures consisting of continuous covalent bonding throughout an entire solid, such as diamond, silica, and silicon carbide.
Properties of Network Solids Very hard materials with very high melting points that are poor conductors of heat/electricity and are completely insoluble in water.
Created by: markoii
 

 



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