Chemical Bonding by hema jaggernauth https://padlet.com/hjnaparima/ICTnaps ICT in the classroom en-us 2017-11-02 17:18:45 UTC 2017-11-22 07:39:49 UTC hello@padlet.com https://padlet-assets.s3.amazonaws.com/icons/Planets.png Group 1 hjnaparima https://padlet.com/hjnaparima/ICTnaps/wish/203030717 Members:
Ms. H. Jaggernauth
What is a chemical bond?
a chemical bond is the electrostatic forces of attraction between two adjacent atoms.

Name the two  types of chemical bonds?
1. Intermolecular bonds - between molecules 
2. Intramolecular bonds - any force that holds together atoms which make up the molecule

List  types of intramolecular bonds?
1. Ionic bonds
2. Covalent bonds
3. Metallic bonds

List types of intermolecular bonds?
1. Hydrogen Bonding
2. Van der Waal's forces










]]> 2017-11-02 17:28:22 UTC https://padlet.com/hjnaparima/ICTnaps/wish/203030717 Group 3/COVALENT BOND hjnaparima https://padlet.com/hjnaparima/ICTnaps/wish/203032119 Members:
1)- Rondelle Ali
2)- Aadam Hosein
3)- Stephon Rajkumaringh

What is a covalent bond?
A covalent bond - involves the sharing of valency electrons between adjacent non-metal atoms. Covalent bonding results in the formation of molecules

List examples of covalent substances?
1) Carbon Dioxide
2) Ammonia Molecules
3) Chlorine Molecules.

List and explain properties of a covalent substance?
1) Composition- molecules with strong covalent bonds between atoms, but weak forces between molecules
2)State at room temperature - most are liquids or gasses owing to weak forces between molecules
3) Melting and boiling points-low mp and bp. The weak inter-molecular forces require little energy to break.
4) Solubility- most are soluble in organic solvents, e.g ethanol, but insoluble in water
5)Electrical conductivity- does not conduct electricity in any state. This is because there are no free ions or electrons are present.

Structure of a covlent substance?
There are two types of covalent structures:
1. Simple molecular
2. Giant covalent


SIMPLE MOLECULAR STRUCTURE
Structure of Iodine

GIANT COVALENT STRUCTURE
 
Structure of diamond and graphite]]> 2017-11-02 17:30:56 UTC https://padlet.com/hjnaparima/ICTnaps/wish/203032119 Group 4 / Metallic Bond hjnaparima https://padlet.com/hjnaparima/ICTnaps/wish/205898573 Members:
1) Hu-Gareth Foon
2) Andrew Larrah
3) Dhaarinesh Balkissoon
4) Adam Rahman
5) Jassiah Roberts
What is a metallic bond?
A metallic bond is a force of attraction between the valency electrons and the nuclei of adjacent ions. This bond involves the sharing of electrons between many positive ions.
Examples of metals?
1) Sodium
2) Magnesium
3)Aluminium
4)Iron
List & explain properties of metals?
1)Good conductors of electricity because of the free flowing electrons.
2)High tensile strength(resistance to bending) because of strong metallic bonds and cause of the structure of most metals.
3)Heat conductivity-  this is because of the delocalised electrons which carry the kinetic energy through the lattice.
4)High density in comparison to size of the object due to  compactness of the atoms.
General Structure of Metal
 5) High Melting and Boiling points- due to the presence of strong metallic bonds which require a lot of energy to break.
 ]]> 2017-11-11 16:10:19 UTC https://padlet.com/hjnaparima/ICTnaps/wish/205898573 Group5 / Allotrophs hjnaparima https://padlet.com/hjnaparima/ICTnaps/wish/206004906 Members:
1)Khaleel Mohammed
2)Chavez Kamal
3)Yuri Gopaul
:(4 Steven Motilal
5)Jakob John

What is an allotrophe?
one of two or more existing physical forms of an element . Example graphite and charcoal

Physical & chemical properties of allotrophs?
 Allotropes generally differ in physical properties such as color and hardness; they may also differ in molecular structure or chemical activity, but are usually alike in most chemical properties


Structure of Diamond:
 
 



Properties of diamond:
  •  toughness
    • Thermal conductivitity
    •  crystal structure




Structure of Graphite:
 
 


Properties of graphite:
• has a high melting point 
• has a soft slippery feel
• insoluble in water and organic solvents 
•used as a dry lubricant 

Uses of diamond:
•Diamond is the hardest naturally occurring substance. Due to its extreme hardness, it is used for making tools for cutting and grinding other hard materials and also used in oil-well drills for drilling holes
•Diamond is transparent and has very high refractive index. It possesses extraordinary brilliance. Because of these properties it is used for making jewellery.
•It is used in protective windows for space probes as it can keep out harmful radiations.

Uses of graphite:
•Since it is good conductor of electricity and is inert, it is used for making carbon electrodes in electrolytic cells and in dry cells.
•Because of its high melting point it is used for making graphite crucibles. Crucibles made of graphite are not attacked by dilute acids or fused  alkalies.
•It is a component of printers’ ink.
•It is used as moderator in nuclear reactor.








]]> 2017-11-12 17:16:48 UTC https://padlet.com/hjnaparima/ICTnaps/wish/206004906 Group 2- Ionic Bonding hjnaparima https://padlet.com/hjnaparima/ICTnaps/wish/206397444 Members:



What is an ionic bond?
An ionic bond is an electrostatic force between a metal[cations] and a non metal[anions] to form a new substance

List examples of ionic bonds
 
  • LiF - Lithium Fluoride.
  • LiCl - Lithium Chloride.
  • LiBr - Lithium Bromide.
  • LiI - Lithium Iodide.
  • NaF - Sodium Fluoride.
  • NaCl - Sodium Chloride.
  • NaBr - Sodium Bromide.
  • NaI - Sodium Iodide. 


list and explain properties of an ionic substance?

1. Ionic substances have high melting points and boiling points due to very strong ionic bonding. A lot of energy is required to break them.

2. Ionic substances are soluble in water rather than organic liquids because "like dissolves like." This is so because water is a polar molecule.The positive end of the water molecule is attracted to the anions on the surface of the solid ionic compound while the negative end  is attracted towards the cations, forming bonds with the anions and cations respectively. Bond formation results in the release of energy. This energy is transferred to the cations and anions making them vibrate faster eventually breaking the ionic bonds between the cations and anions causing them to break free from the ionic lattice and enter the solution.

3. Ionic substances are conductive when liquid - Ions are charged particles, but ionic compounds can only conduct electricity if their ions are free to move. Ionic compounds do not conduct electricity when they are solid,only when dissolved in water or melted. They are electrolytes. Ionic compounds also conduct electricity when molten.

4. Ionic crystals are brittle because the ions are locked into place in their lattice. They cannot be drawn into wires or hammered into shape,as metals can.




Structure of an ionic substance
NaCl
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