bonding unit 3 chemistry review

linear

180 degrees, 2 bonds, 0 lone pairs (2 electron domains)

trigonal planar

120 degrees, 3 bonds, 0 lone pairs (3 electron domains)

bent (v-shape) #1

117 degrees, 2 bonds, 1 lone pair (3 electron domains)

tetrahedral

109.5 degrees, 4 bonds, 0 lone pairs (4 electron domains)

trigonal pyramidal

107.8 degrees, 3 bonds, 1 lonw pair (4 electron domains)

bent (v-shaped) #2

104.5 degrees, 2 bonds, 2 lone pairs (4 electron domains)

strongest IMF in nonpolar molecule

london dispersion forces

strongest IMF in polar molecule

dipole-dipole forces

hydrogen bonding

when H is bonded to N, O, or F in a molecule (strongest IMF)

properties of ionic compounds

mostly solids, high melting points (hard to melt), mostly highly soluble in water, conduct electricity well when melted or dissolved in water

properties of covalent compounds (molecules)

mostly gases, low melting points (easy to melt), mostly insoluble, mostly bad conductors

charge of Zn (zinc)

2+ (cation)

charge of Cd (cadmium)

2+ (cation)

charge of Ag (silver)

1+ (cation)

difference in electronegativity for nonpolar covalent bonds

0 - 0.4

difference in electronegativity for polar covalent bonds

0.5 - 1.7

difference in electronegativity for ionic bonds

1.8 and above

why do elements bond?

to achieve an octet

octet

when there are 8 valence electrons in outer shell

another name for covalent bonds

molecules

another name for ionic bonds

formula units

what makes a molecule polar/nonpolar?

when the dipoles don’t cancel out. this can happen when a) the shape of the object don’t cancel out the forces (e.g. bent molecules) or b) the IMF makes the molecule unevenly distributed (e.g. this can make a tetrahedral molecule polar)

dipole

uneven sharing of electrons because of high difference in electronegativity between 2 atoms in a bond

prefixes for naming molecules (covalent bonds)

mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-

resonance

when there are delocalized electrons in a molecule or polyatomic ion that result in there being many lewis dot diagrams to describe that one molecule