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CHEMISTRY (GROUP 1 (Rubidium, Rb (Chemical Properties (Equation: 2 Rb (s)…

- - - - Has lower boiling/melting point than Sodium
      - Easily to be tarnished within minutes
      - More reactive than Sodium
      - A soft metal
    - - Reacts more vigorously with water to form an alkaline solution, Potassium Hydroxide, KOH
        
        Equation: 4K (s) + 2H₂O (l) --> 4KOH (aq)
        
        Observation: There is tiny explosion with white smoke produced
      - Reacts with Oxygen to form Potassium Oxides
        
        Equation: 4K (s) + O₂ (g) --> 2K₂O (s)
        
        Observation: Burns in oxygen with lilac fame
  - - - Give a different characteristic of color with lilac of potassium and orange in sodium
    - - Equation: 2 Rb (s) + 2 H2O (l) → 2 RbOH (aq) + H2 (g)
      - obesevation: The colourless solution of rubidium hydroxide and hydrogen gas produce and the solution is acidic because it turn the phenolphthalein into pink colour
      - React with water to produce form a colourless solution of rubidium hydroxide (RbOH) and hydrogen gas.
  - - - More reactive than Lithium
      - Has lower boiling/melting point than Lithium
      - A soft metal
      - Easily tarnished when exposed to air
    - - Reacts with oxygen to form Sodium Oxides
        
        Equation: 4Na (s) + O₂ (g) --> 2Na₂O (s)
        
        Observation: Burns in oxygen with yellow-orange flame
      - Reacts vigorously with water to form an alkaline solution, Sodium Hydroxide, NaOH
        
        Equation: 4Na (s) + 2H₂O (l) --> 4NaOH (aq)
        
        Observation: There is red flame, the metal moves speedy on the water surface
  - - - White (on the cut - light yellow
      - extremely reactive
      - Colors the flame of a gas burner in the blue.
    - - React with water rapidly with water and form caesium hydroxide
        
        Equation: 2Cs (s) + 2H2O (l) → 2CsOH (aq) + H2 (g)
        
        Observation : A colourless solution of caesium hydroxide form,with the presence of hydrogen gas. :
      - Does not react with Nitrogen.
  - - - React with water rapidly to form an alkaline solution, Lithium Hydroxide, LiOH
        
        Equation: 4Li (s) + 2H₂O (l) --> 4LiOH (aq)
        
        Observation: Float on water and moves on the water surface
      - React with nitrogen in the air to produce Lithium Nitride, Li₃N
        
        Equation: 6Li (s) + N₂ (g) --> 2Li₃N (s)
        
        Observation: very dark (black) coloured metal
    - - Very dark in colour
      - The least reactive in the group
      - Lightest in the group
      - Highest melting/boiling point in the group
  - - - React with water rand produce francium hydroxide and hydrogen gas,but it rare done because francium is is very scarce and expensive.
    - - The least electronegative of all the known elements.
- - - - The boiling point decreases down the group
    - - The melting point decreases down the group
    - - The reactivity increases down the group.
        
        Why?
        
        1 electron is in the outermost sub-shell, s
        
        Down the group, the electron is further away from the nucleus due to the increase in atomic radius; proton is positively charged - the attraction of electrons towards the nucleus decreases
        
        There is the occurrence of electron shielding - down the group, the energy levels increase, the number of inner-shell electrons increase; reduction in effective nuclear charge between valence electrons and proton - electrons have higher tendency to be removed and reacted
        
        Electropositivity
        
        Definition
        
        Measure of tendency to donate electrons to form positive ions
        
        Trends
        
        Increases down the group
    - - Definition
        
        amount of energy required to remove the valence electron, of a gaseous atom, to form a cation (positively charged ion).
      - Trend
        
        Decreases down the group
    - - except Francium (density=unknown), the density of elements increases down the group
  - - - The melting point increases down the group
    - - The boiling point increases down the group
    - - The reactivity decreases down the group
        
        Why?
        
        Trends
        
        Decreases down the group
        
        Electronegativity
        
        Definition
        
        Measure of tendency to attract electrons to form negative ions
        
        Down the group, the electron is nearer to the nucleus due to the decrease in atomic radius - the attraction of electrons towards protons increases
    - - Definition
        
        amount of energy released when electron is added
      - Trend
        
        Decreases down the group
    - - except Astatine & Tennessine (density=unknown), the density of elements increases down the group
- - - - dark yellow when in liquid state, colourless/palen yellow when in gas state
      - most reactive elements - react with all elements in periodic table except Hydrogen, H and Neon, Ne
      - lowest melting and boiling point in the group
    - - React with metal wool producing Iron flouride
        
        Observation : rusty colour on the wool
      - React with carbon producing Carbon monoflouride
        
        Observation : big, yellow flame
      - React with sulphur producing Sulphur tetraflouride, SF4 / Sulphur hexaflouride, SF6
        
        Observation : light blue flame
        
        Equation
        
        sulphur hexaflouride : S (s) + 3F2 (g) --> SF6 (g)
  - - - low melting and boiling point
      - greenish yellow gas
      - heavier than air
      - highly reactive, corrosive and poisonous
    - - Reacts with water to form hydrochloric acid, HCl
      - Reacts with aluminium to form aluminium trichloride, AlCl3
        
        Observation : white fume of gas was present at first, then turns into a bright yellow flame
      - Treating wood : Reacts with iron to form iron chloride
        
        Observation : bright orange flame and brown gas is formed
    - - making PVC
      - used as a weapon in World War 1
  - - - low melting and boiling point
      - unpleasant smell
      - red liquid
      - volatile
    - - used as additives in plastic to make them less flammable
    - - Reacts with aluminium to produce aluminium tribromide
        
        Observation : bright yellow flame
  - - - Solid at room temperature
      - Very pungent in odour
      - density of iodine is 4.94 g/mL
        
        Sink in water
    - - Reaction of iodine with air
        
        Does not react with oxygen, O₂ and nitrogen, N₂
        
        React with ozone, O3
        
        iodine does react with ozone, O3, the second allotrope of oxygen, to form the unstable yellow I4O9, the nature of which is perhaps I(IO3)3.
      - Reaction of iodine with the halogens
        
        React with flourine
        
        At room temperature
        
        Equation : I2(s) + 5F2(g) → 2IF5(l) [colourless]
        
        At 250°C
        
        Equation : I2(g) + 7F2(g) → 2IF7(g) [colourless]
        
        At reaction conditions, (-45°C, suspension in CFCl3),
        
        Equation : I2(s) + 3F2(g) → 2IF3(s) [yellow]
        
        React with bromine
        
        Equation : I2(s) + Br2(l) → 2IBr(s)
        
        React with chloride
        
        At -80°C with excess liquid chlorine
        
        Equation : I2(s) + 3Cl2(l) + I2Cl6(s) [yellow
        
        presence of water
        
        Equation : I2(s) + 6H2O(l) + 5Cl2(g) → 2HIO3(s) + 10HCl(g)
      - Reaction of iodine with acids
        
        Reaction of iodine with hot concentrated nitric acid
        
        Equation : 3I2(s) + 10HNO3(aq) → 6HIO3(s) + 10NO(g) + 2H2O(l)
      - Reaction of iodine with bases
        
        reacts with hot aqueous alkali to produce iodate, IO3-
        
        Equation : 3I2(g) + 6OH-(aq) → IO3-(aq) + 5I-(aq) + 3H2O
  - - - Solid at room temperature
      - Black in colour
      - Astatine sublimes less readily than does iodine, having a lower vapor pressure
    - - Reaction of astatine with the halogens
        (dissolve in carbon tetrachloride, CCl4).
        
        reacts with bromine, Br2
        
        Equation : At2 + Br2 → 2AtBr
        
        React with iodine, I2
        
        Equation: At2 + I2 → 2At
      - Reaction of astatine with acids
        
        Astatine dissolves in dilute nitric acid, HNO3, or dilute hydrochloric acid, HCl.
  - - - artificially produced transuranium element of atomic number 117
      - Tennessine is harmful due to its radioactivity.
      - Tennessine is a synthetic radioactive metal and has only been produced in minute amounts.
    - - Reaction of tennessine with air
        
        As only a few atoms of tennessine have ever been made, its reactivity with air is unknown
      - Reaction of tennessine with water
        
        As only a few atoms of tennessine have ever been made, its reactivity with water is unknown
      - Reaction of tennessine with the halogens
        
        As only a few atoms of tennessine have ever been made, its reactivity with the halogens is unknown
      - Reaction of tennessine with acids
        
        As only a few atoms of tennessine have ever been made, its reactivity with acids is unknown
      - Reaction of tennessine with bases
        
        As only a few atoms of tennessine have ever been made, its reactivity with bases is unknown