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1.6 Bonding (Polarity (Describe polar covalent, non-polar covalent, ionic…
1.6 Bonding
Polarity
Describe polar covalent, non-polar covalent, ionic and dative covalent bonds
Non-polar covalent bond- is a bond where two atoms share one or more pairs of electrons with each other.
Polar covalent bond- is a bond where two or more atoms share one or more pairs of electrons unequally (one atom has a greater pull)
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Ionic bond- is a bond formed between two oppositely charged ions, involves a complete transfer of ions.
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Predict whether a compound of two or more elements would be covalent from the position of the elements in their periodic table or from their electronegativity values.
Electronegativity increases as we move along and up the periodic table (Fr-F). A metal and nonmetal will give you a ionic bond ( metal gives away its electrons). A nonmetal and a nonmetal gives you a covalent bond (sharing electrons)
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Born-Haber Cycles
Describe quantitatively the energetic factors and characteristics involved in the formation of an ionic bond.
There are 3 factors that affect the formation of an ionic bond. 1. radius size. 2. charge of ion. 3. electromagnetically.
The smaller the radius size and the greater the charge the easier it is to form a ionic bond.
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List the properties of ionic crystals, and relate them to the lattice energy.
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Define electron affinity, atomisation and ionization energy.
The enthalpy of atomisation is the enthalpy change that accompanies the total separation of all atoms in a chemical substance .
Ionization energy is the quantity of energy that an isolated, gaseous atom in the ground electronic state must absorb to discharge an electron, resulting in a cation. This energy is usually expressed in kJ/mol, or the amount of energy it takes for all the atoms in a mole to lose one electron each
the electron affinity of an atom or molecule is defined as the amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion.
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