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Alkali Metals
Li, Na, K, Rb, Cs, Fr
appearance of alkali metals
soft silvery metals that give basic solutions
Bonding in alkali metals
M-M bonding is weak; gives delocalization of electrons which can surround a sea of cations
Isolation of Sodium
electrolysis of molten NaCl by the Down’s Process
the Down’s Process
Cl gas is given off at a graphite anode and molten sodium collects at a steel cathode; CaCl2 is added to NaCl to lower its melting point from 800 to about 630 degrees C
Isolation of Potassium metal
Melt Reaction, reaction of KCl with sodium metal to give NaCl and K
uses of alkali metals
form M+ ions which act as good reducing agents, alloys of Na and K are used in nuclear reactants as coolants, francium is used in reactive tracer experiments, Na+/K+ have physiological importance, Li+ used in treatment of bipolar disorder and in batteries
Chemical Properties of Alkali Metals
all reduce alcohols and water, reactivity increasing down the group due to greater ease of ionization
Na in ammonia
Na (and other alkalki metals) are soluble and will lose an electron in this liquid
Alkali metals and Oxygen
heating these metals in oxygen gas produces different products depending on the size of the cation
Li + O2
Oxide, Li2O
Na + O2
Na2O2, peroxide
K + O2 (and above)
superoxide, KO2
NaCl
vast deposits in oceans and deserts, starting material for sodium hydroxide
K+
less soluble than Na+ and less easily leached from minerals, selectively filtered out by plants
NaOH
soft waxy, corrosive solid, commonly used as a base, produces by electrolysis of brine
Na2SO4
used in paper making and detergents, formed by reaction of H2SO4 (bronsted acid) and NaCl
NaHCO3
baking soda, washing power, released CO2 on reaction with acid
reaction of M with H2
forms MH for all M
reaction of M with O2
forms Li2O
forms Na2O2
forms KO2
reaction of M with N2
forms Li3N, only works for Li
reaction of M with X2, a halogen
forms MX for all M
Reaction of M with H20
forms MOH and Hydrogen Gas for all M