concept 2.3: the formation and function of molecules and ionic compounds depend on chemical bonding between atoms

what is the strongest type of bond

covalent bond

what is a covalent bond

between atoms of the same element or atoms of different elements, the sharing of a pair of valence electrons by two atoms

what is an atoms Valence

an atoms bonding capacity usually equal to the number of unpaired electrons required to complete the atoms outermost (valence) shell NOT THE NUMBER OF VALENCE ELECTRONS

difference between a single bond and a double bond

a single bond is with one pair of valence electrons and a double bond is with two pairs of valence electrons

ionic bonds

anion and cation attracted to eachother, atoms strip electrons from their bonding partners

what are traits of ionic bonds

a compound that typically dissociates easily in aqueous solution

hydrogen bond

H2O to H2O interactions, forms when a hydrogen atom is covalently bonded to one electronegative atom is also attracted to another electronegative atom (typically oxygen or nitrogen)

Van Der Waals interactions

attractions between molecules that are close together

an example of Van Der Waals interactions

between a geckos toe hairs and a wall surface

electronegativity

an atoms attraction for the electrons in a covalent bond

relationship of electronegativity and example of electronegative molecules

oxygen and nitrogen, the more electronegative an atom is the stronger it will pull electrons towards itself

polar covalent bond

not symmetrical, one atom is more electronegative and pulls unequally

non polar covalent bond

symmetrical, the atoms share the electrons equally

what bonds often hold together a biological molecule

weak bonds hold them in their functional form

what does molecular shape do

molecular shape determines how biological molecules recognize and respond to one another

chemical equilibrium

reached when the forward and reverse reaction occur at the same time and the relative concentrations of reactant and products do not change

what effects the direction of a reaction

more reactant molecules

different equilibrium points

reduced concentrations