{CBSE} hydrogen class 11 notes chapter 9[updated based on 2023]

{CBSE} hydrogen class 11 notes chapter 9[updated on 2023] | Hydride of Hydrogen electron(atom) with water {CBSE} hydrogen class 11 notes chapter 9[updated on 2023] || What are the Properties of Hydrogen || What are Physical properties of hydrogen || What are Chemical Properties of hydrogen || What is Hydride || What are the Applications of hydrogen || What are the Compounds of hydrogen || What are the basic properties of water

We provided In this article hydrogen class 11 notes chapter 9[updated 2022]{CBSE} and Hydride of Hydrogen electron(atom) with water for use in English medium(language).

What are the Properties of Hydrogen?

Hydrogen is the lightest element in the Periodic table. In a standard situation, hydrogen is a gas of diatomic molecule with H2.  Hydrogen is colourless, odourless, tasteless, non-toxic, and highly combustible. 

Instructions:-

• If you are not Read previous Topics of this article 👉Why the position of hydrogen is not fixed in elements periodic table👈 to read 
• If you are a student you can write an article in your copy as a note 👉Why the position of hydrogen is not fixed in elements periodic table👈 to write notes from starting.

What are the Physical properties of hydrogen?

• Hydrogen is s colourless or odourless gas.

• It is not soluble in water.

What are the Chemical Properties of hydrogen?

• Hydrogen exists as a diatomic molecule.

• Its bond length is very small due to the small size of the hydrogen atom. So, at room temperature, it is less reactive. At high temperatures above 2000k, only 0.081% of hydrogen molecules change into hydrogen atoms. But at 5000k 95.5% of hydrogen molecules change into hydrogen atoms.

In the chemical reaction: H-atom take part

H2 exist: HH {0.081% at 2000K and 95.5% at 5000K)

Bond energy inversely proportional to bond length

H - H= bond length small

Cause: H-atom Small

The reaction of hydrogen at high temperature.

Hydrogen undergoes the following type of chemical reaction

1. It loses an electron and convert them into an H+ ion and react with non-metal.

• N2 + 3H2  2NH3  (H - e=H+)

• Cl2 + H2  (sunlight) 2HCl  (H - e=H+)

• H2 + O2   heat  H2O

2. Reaction with metal

Hydrogen reacts with metal and gain one electron and convert into H- ion.

Na + H2    Na+H-  {H+e=H-}

Ca + H2    CaH2  ( H + e=H-)

Al + H2      AlH3

Hydrogen react with unsaturated hydrocarbon undergoes hydrogenation and make it saturated and the process is hydrogenation. This reaction is very useful. By this reaction vegetable oil converts into dalda.

V.G oil + H2 (Ni)  Dalda saturated

H: loss electron=H+: non-metal

H: gain electron= H-: metal

H: share electron make covalent bond: unsaturated hydrocarbon

1. What is Hydride?

Hydrogen reacts with elements and forms a compound this compound is called hydride.

This hydride is following types

• Ionic hydride or saline hydride

When hydrogen reacts with S block elements except for lithium, beryllium, boron and magnesium. Then hydride is called silent hydride.

CaH2 ionic hydride

Ca(20)= last 4S2: S-Block

2. Molecular hydride

When hydrogen is attached with p-block members (13 to 17 group) (18 group does not make any hydride). These are called molecular hydrides. This hydride is further classified into the following parts:-

1. Electron deficient hydride

2. Electron precise hydride

3. Electron reach hydride

1. Electron deficient hydride:-when hydrogen is combined with the 13th group member this compound has a deficiency of electrons and it is called electron-deficient hydride. It acts as a Lewis acid.

Al(13): p-Block, group=13(group=12 + electron in p)

AlH3 = electron-deficient hydride

2. Electron precise hydride

When hydrogen combines with the 14th group elements it does not lose or Gain electrons so it is called electron precise hydride. It neither act as Lewis acid nor Lewis base.

CH4 = electron precise

Acid= Na+, mg+2, Al+3

Base= Cl-, OH-, SO4

AlCl3 =electron deficient: Lewis acid

Acidic strength is Directly proportional to the Oxidation number.

• Those who have a deficiency of electrons act as Lewis acid.

• All positive charge radical is Lewis acid.

• Those which has an efficiency of electron act as Lewis base.

• All negative charge radical is Lewis base.

3.  Electron reach hydride

15 16 and 17th group elements combine with hydrogen and form an electron reach hydride. This hydride is Lewis base because it donates loan pair electron.

3. Metallic hydride(Non-stoichiometrical     hydride, Interstitial hydride)

When hydrogen reacts with the d and f block elements. Then hydride which is form interstitial hydride or metallic hydride.

Group 7, 8, 9 do not react with hydrogen. This is called hydride gas. In the 6 groups, only chromium make a hydride.

What are the Applications of hydrogen?

1. Making data from vegetable oil.

2. A hydrogen-oxygen fuel shell is used in the rocket.

3. Oxyhydrogen torch when hydrogen atom combined and formed molecule it has temperature approximately 4000k. It is used for cutting and Belding.

4. Making Ammonia (by Haber process)

N2 + 3H2 2NH3(Haber process)

5. Making HCl gas.

6. Making standard electrode potential.

7. In metallurgy process.

8. As a rocket fuel.

What are the Compounds of hydrogen?

1. Water (H2O)

Hybrid orbital= Sigma + loan pair=2+2=4 sp3

Bond angle=109.5 - 2×2.5=109.5 - 5=104.5

1. it has a high specific heat capacity.

• 4200 Kj/mole/k: radiation of automobile

• Cold area : H2O: ice, ice is a bad conductor of heat.

So, Aquatic animals survive - H2O(liquid).

• 3.08 litre O2 in 100 litre H2O (at room temperature). This oxygen is taken by aquatic animals for respiration.

High-temperature O2 decreases so life is in danger.

Low-temperature O2 increases so life is better.

• Body temperature maintenance (H2O)

In ice water molecule associated with hydrogen bonds 1 water molecule associated with 4 other water molecules with hydrogen bonds make it contain a large number of voids (empty). So volume increase and density decrease. Due to this property ice float on the surface of the water. 

1/9 part of the iceberg above the water.

Since ice is void in internal but volume increase. So the density of the iceberg-decrease de. So, it floats on the surface of the water.

What are the basic properties of water?

• Water dissolves organic as well as an inorganic compounds. So it is known as the universal solvent.

• Water has a dielectric constant (80). So it increases the conductivity.

• Dielectric property weakens ionic force.

If you did not read the previous article Read here 👇

Why the position of hydrogen is not fixed in the elements' periodic table

Next part we read about types of water

Hard water and soft water and many more…..