Regarding Electrons
the only element which cannot have 8 valence electrons
hydrogen
ionic bonds are held together by
oppositely charged ions are attracted to each other
bond formed by atoms sharing 1 pair of electrons
single bond
covalent bonds are formed by:
atoms sharing 1 or more pairs of electrons to achieve a full octet
the family of polyatomic ions that have 1 or more oxygen atoms
oxyanions
the rule which explains how atoms are most stable
the octet rule
another term for an ionic compound
crystal
bond formed by atoms sharing 2 pairs of electrons
double bond
these groups of elements are involved in covalent bonding
nonmetals
molecules that give up hydrogen ions when dissolved in water
acids
in a lewis structure, the electron pairs that are not involved in bonding
lone pairs
ionic bonds are formed between these elements:
metal and nonmetal
bond formed by atoms sharing 3 pairs of electrons
low melting point
low boiling point
poor electrical conductivity
usually liquid or gas at room temp
reactions that release heat
exothermic reactions
in a lewis structure, the electron pairs that are involved in bonding
bonding pairs
the energy in the bonds of an ionic compound
lattice energy
a molecule with a positive or negative charge
polyatomic ion
covalent bonds where electrons are shared equally
non-polar bonds
reactions that absorb heat (or require heat to run)
endothermic reactions
the diagrams which show how electrons are shared between atoms
lewis structures
ionic crystals with water molecules integrated in the crystal
hydrates
compound formed when atoms are covalently bonded
molecule
covalent bonds where electrons are not shared equally (one atom hogs the electrons)
polar bonds
a number that represents the number of electrons lost or gained in an ion
oxidation number/oxidation state