Shapes of molecules and polarity

name for electrons in outermost energy level

valence

number of valence electrons of a group 14 element

4

number of valence electrons of a group 16 element

6

bond angle for tetrahedral shape

109.5⁰

bond angle for trigonal planar shape

120⁰

bond angle for linear shape

180⁰

another name for non-bonding pair

lone pair

most electronegative element

fluorine

second most electronegative element

oxygen

electron arrangement for Cl, atomic # 17

2,8,7

valence electrons Cl has, atomic # 17

7

dipole

unsymmetrical charge distribution / "a separation of charge"

polar bond

covalent bond in which electrons are shared unequally

polar molecule

molecule with an unsymmetrical charge distribution, a dipole

examples of polar molecules

H₂O and HF and CH₃Cl

examples of non polar molecules

CO₂ and CCl₄ and BF₃

octet

8 electrons in an atom's outermost energy level

covalent bond

chemical bond formed by the sharing of electrons

electronegativity

ability of an element to attract electrons in a bond

δ+

symbol meaning a slight + charge

δ-

symbol meaning a slight - charge

shape of molecule with 3 bonding and 1 non-bonding regions

trigonal pyramidal, bond angle based on 109.5⁰

shape of molecule with 2 bonding and 2 non-bonding regions

v-shaped or bent or angular, bond angle based on 109.5⁰

shape of molecule with 2 bonding and 1 non-bonding regions

v-shaped or bent or angular, bond angle based on 120⁰

shape of molecule with 4 bonding and 0 non-bonding regions

tetrahedral, bond angle of 109.5⁰