Pearson Baccalaureate Chemistry Higher Level 2nd Edition Print and Online Edition for the IB Diploma
Everything you need to help you with Chemistry chapter 4. These notes are perfectly summarized and organized in subtopic. Includes a compilation of information from the textbook, study guides, class notes and other IB resources. Super easy to read and a great amount of information to help you ace ...
Band 7 SL Chemistry Notes from a 44/45 Novemeber 2022 Graduate
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BONDING
● Positive ion = Cation
● Negative ion = Anion
Ionic bonding
● The electrostatic forces of attraction between oppositely charged ions
● Formed via the transfer of electrons between metals and nonmetals
● Ionic compounds form salts
● Transition metals have complex electron arrangement so they can
form more than one type of ion
- An electronegativity difference of 1.7 and up means the bond is ionic
Ionic compounds structure
● Forces of electrostatic attraction between ions cause ions to surround
themselves with ions of opposite charge, forming a three-dimensional
crystalline
Ionic compounds properties
Melting + Boiling point
● Electrostatic force of attraction between ions is very strong hence
large amounts of energy is required to break the ionic bond = high
melting + boiling point
● Solid at room temperature
● Melting point + Boiling point increase with charge due to greater
attraction between the ions
Volatility: Tendency for a substance to vaporize
● Low volatility/non-volatile
Conductivity
● Non conductive in solid state because there are no moveable ions or
delocalized electrons
● Conductive in aqueous + liquid state
, Metallic bonding
● The electrostatic force of attraction between the positive metal ions
and their delocalized electrons
● Strength of metallic bond depends on the charge of the ions and the
ionic radius
● Strength of metallic bond decreases down a group
Metallic structures
● Giant lattice structure (3D of cations, sea of delocalized electrons)
Metal alloys
● Alloys: Solution of solid metals
● Produce by adding one metal to another in the molten state
● Alloys are typically harder than the original metal because there are
different sized atoms that restrict amount of pressure that can be
applied
● Bonds are directional = layers cannot slide
● Alloys have delocalized electrons
Covalent bonding
● The electrostatic force of attraction between the positive nuclei and
the shared pair of electrons
● Formation of covalent bond stabilizes the atom as energy is released
● An electronegativity difference between 0-0.4 means the bond is
nonpolar covalent, 0.4-1.7 means the bond is polar covalent
- coordinate bond/dative covalent bond: An electron pair covalent bond
that is donated from one of the atoms (Ligands)
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