The document discusses the properties of Group 1 elements (alkali metals) on the periodic table. Some key points: 1) The alkali metals have a general electronic configuration of ns1 and include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), and cesium (Cs). 2) Their physical properties, such as atomic radius and ionization energy, decrease down the group as nuclear charge decreases due to the lanthanide contraction. 3) Their chemical properties include reacting vigorously with water to form alkaline hydroxides and oxygen to form oxides/peroxides/superoxides. They are highly reactive metals.

1. Group I Elements
By Anushka Venkatesh

2. 1. Group 1 elements called alkali
metals as their hydroxides are
strongly alkaline.
2. General electronic
configuration-ns1
3. Francium is highly radioactive.
4. Na,K abundant.Li,Rb,Cs less
abundant

3. Physical Properties
Periodic trends
depend on-
1.nuclear charge
2. Screening effect
Why does reactivity
increase down the
group?
1. Atomic radii- largest in respective period.
Increases down the group i.e Li<Na<K<Rb<Cs
2. Ionization Enthalpy- M(g) M+(g) + e- HIE
lowest in respective period
Decreases down the group.
3. Hydration Enthalpy- M+(S) M+(AQ)
Proportional to charge/radius ratio.
The magnitude of hydration enthalpy decreases down a group. Li salts are always
hydrated as it has maximum degree of hydration enthalpy.

4. Reason behind
flame tests-
Heat excites electron
to higher energy
level,electron emits
radiation while
returning to ground
state.
How would E
value change
across a period?
4. Melting and boiling points- decrease down the group.
5. Density- Li<Na>K<Rb<Cs
6.Appearance- the alkali metals are silvery white,soft and light metals.
7.Flame test- Alkali metals and their salts impart characteristic colour to an oxidizing flame
and can be detected by their respective flame tests.
8. Standard Electrode Potential- measure of reducing power of element.
Magnitude decreases down the group .

5. Chemical Properties
1. Reaction with air-
Metal + dioxygen(from air) Metal Oxide [ Li reacts with N2 to form Li3N as well. Alkali metals are
Stored in kerosene because of their high reactivity towards
air and water.]
Metal Oxide + vapour(from air) Metal Hydroxide
Li-oxide Characteristics of alkali metal oxides-
Na-peroxide 1.superoxide(O2-) and peroxide are larger anions than oxide ion.Hence larger
Cations form peroxides and superoxides as they are more stable.[ fajans law]
K,Rb,Cs-superoxides 2.oxide,peroxide=colourless.superoxide=yellow/orange.

6. 2. Reaction with water-
2M +2 H2O 2 M+ + 2 OH- + H2
Aqueous metal hydroxide [here M is reducing H2O]
Despite having the highest E value, Li reacts less vigorously with water due to-
1. Its small size high ionization enthalpy
2. High hydration energy.
Characteristics of alkali metal hydroxides-
1.They are strongest of all bases.
2.They are white crystalline solids.

7. 3. Reaction with Dihydrogen
2M + H2 2(M+)(H-)
METAL HYDRIDE
T=673K except for Li which reacts at 1073K
Reason: Lithium’s small size makes it less reactive than the other alkali metals.

8. 4. Reaction with Halogens
2M + X2 2(M+)(X-)
METAL HALIDE
1.Li halides are somewhat covalent due to Li’s polarising power.
[ polarisation=Distortion of electron cloud of anion by the cation]
2. As Iodine is the largest halogen, LiI is the most covalent metal halide
Characteristics of metal halides-
1.Enthalpy of formation decreases down the group for chlorides,bromides and iodides but increases down the group for
fluorides.
2.Enthalpy of formation for fluorides>chlorides>bromides>iodides due to increase in size down the group.
3.Solubility of (M+)(X-) decreases down a group as hydration energy decreases and lattice energy increases(except
flourides)..
4.LiF has low solubility due to high lattice energy and CsI has low solubility due to low hydration enthalpy.

9. 5. Reducing Nature
M(s) M(g) sublimation energy H1
M(g) M+(g) ionization enthalpy H2
M +(g) M+(aq) hydration enthalpy H3
Lesser the value of [ H1+H2+H3] better the reducing agent.
High degree of hydration enthalpy makes lithium a strong reducing agent.

10. 6.Solutions in Liquid Ammonia
1. M + NH3 (M(NH3))+ + (e(NH3))-
Ammoniated ion - imparts blue colour to solution
2. M + NH3 MNH2 + ½ H2 [M is reducing NH3]
3. In concentrated solution ( excess of M) , the blue colour changes to bronze colour.

11. 7. Alkali metal salts of oxoacids
Oxoacids - acidic proton is on a hydroxyl group with an oxo group attached to the same atom i.e the (OH) and (O) is attached
to the same atom. Eg:H2SO4,H2CO3,HNO3,H3PO4 etc.
1. M + H2CO3 M2CO3 + 2 H+ [ M REDUCES H2C03]
2. M + H2CO3 MHCO3 + H+
1.These salts are soluble in water and are thermally stable.
2. Stability of the metal carbonates and bicarbonates increase down a the group .
Reason: increase in electropositivity down the group.
3. Boiling point and melting point is directly proportional to the ionic character of the salt.
Hence, LiHCO3 does not exist as solid under normal conditions. Li2CO3 is not stable to heat, it polarises (CO3)2-
ion as follows-
Li2CO3 Li2O + CO2

12. Anomalous properties of Lithium
Difference between Li and alkali metals-
1. It’s high B.P and M.P makes it harder than other metals.
2. It’s least reactive, strongest reducing agent and its forms monoxide and reacts with atmospheric nitrogen.
3. It’s deliquescent [ all these properties are due to its small size and high polarising
4. LiHCO3 isn't formed in solid state. ability]
5. Does not form ethynide when reacted with ethyne.
Similarity between Li and Mg-
1. Equal charge/radius ratio and ionic size. [ Li has a charge of 1 and Mg of 2 and their radii are similar,
2. They react slowly with water and react with nitrogen. Then how is charge/ radius ratio same?]
3. Their chlorides are soluble in organic solvents.
4. Both are deliquescent.