reviewer ni sir

• Intramolecular forces are forces between atoms within a molecule.
• types of intramolecular force: ionic, metallic, covalent
• Ionic bonding is the electrostatic attraction between oppositely charged ions. Formed by the transfer of electrons (metal and nonmetal). Has formal charge (+,-)
• Metallic bonding is the electrostatic attraction between delocalized electrons and the positive metal ions. Formed by sharing electrons of two or more metals. Has partial charge (Cation (+) with delocalized/free electron (-)).
• delocalized electrons are electrons in a molecule, ion or solid metal that are not associated with a single atom or a covalent bond.
• Nonpolar Covalent Bonding is when there is equal distribution of electrons because both atoms have similar electronegativities. There is no polarity present.
• Covalent bonding is the sharing of electrons between two or more nonmetals in a chemical reaction.
• types of polarity in covalent: polar and non-polar
• polar: unequal sharing of electronegativity eg H20
• non-polar: equal sharing of electronegativity eg. O2, Cl2
• intermolecular forces are forces between molecules
• fill in the blanks in the table below

  A) ionic

  B) ionic

  C) polar covalent

  D) polar covalent

  E) hydrogen bond

  F) non-polar covalent

  G) polar covalent

  H) non-polar covalent

  
• Surface Tension is the force that causes the surface of a liquid to contract. Water, in particular, has high surface tension because of hydrogen bonds. Temperature affects surface tension
• Viscosity is the ability of the liquid to flow and/or the liquid’s resistance to flow between the molecules of a liquid when they pass each other.

  • High resistance, high viscosity
  • High temperature, low viscosity
• Vaporization is the change of state from liquid to gas while the opposite is condensation.

  • Includes evaporation and boiling
  • Gas and vapor are similar but not the same
  • Volatile liquids tend to evaporate faster than water.
  • Boiling point of water is 100 degree C
• Molar heat of vaporization is the formation of liquid to gas with the addition of heat as a form of energy.

  • Heat of vaporization is the amount of heat needed to vaporize a given amount of liquid at its boiling point
• the unit of crystalline solids is called unit cell
• the structure of solids can be subdivided into simple and closed-packed.

  • In close-packed structure, the gap between the particles is called the void.
• Amorphous Solids’ atom arrangement is not organized as definite pattern.

  • Pseudo-solids/supercooled liquids
  • Ranged melting point
  • Isotropic – same response in any directions/same physical properties in different directions.
• Crystalline Solids’ atom arrangement is definite and organized.

  • True solids
  • Sharp melting point
  • Anisotropic – different response in any directions/different physical properties in different directions.
  • Has repeated unit that form Hexagon shape.
• types of crystalline solids: ionic solids, covalent solid, molecular solid, metallic crystals
• Ionic Solids have + and – ions held together by electrostatic attractions (ionic bond e.g. NaCl).

  • High melting points
  • Brittle
  • Insulator (solid form)
  • Conductor (molten form)
• Covalent Solids contains a three dimentional network of covalently bonded atoms.

  • Diamond
  • Very hard
  • High melting point
  • Poor conductors
  • Graphite (exception)
  • Soft
  • Electrically conductive
• Molecular Solids are formed through covalent bond.

  • Soft
  • Low to moderately high melting point
  • Poor thermal and electrical conductivity
  • Ice, table sugar
• Metallic Crystals are a uniform distribution of atomic nuclei within a sea of delocalized electrons.

  • High melting points
  • Malleable and ductile
  • Good conductors
• fill in the blanks

  A) evaporation

  B) exothermic

  C) endothermic

  D) freezing

  E) melting

  F) sublimation

  G) deposition

  H) triple point

  I) matter

  J) critical point

  K) liquid

  
• solution: also known as homogenous mixture, characterized by having uniform composition
• solute is the component that is dissolved by solvent
• solvent is the component that dissolves in solute
• aqueous solution: contains water as the solvent
• non-aqueous solution: does not contain water as the solvent
• types of bases on concentration of solution in two areas: hypotonic, isotonic, hypertonic
• hypotonic: inside is more concentrated that outside of the cell
• isotonic: inside and outside the cell has equal concentration
• hypertonic: outside is more concentrated that inside of the cell
• electrolyte is a substance that forms ions when dissolved in water, which enable conductivity of the current
• dissociation is the physical change that occurs when the ions in the solid separate and disperse uniformly throughout the solution
• strong electrolyte is considered to be completely ionized in water
• weak electrolyte are ionic compounds that are not completely ionized or dissociated in water
• nonelectrolyte is a compound that does not ionize in solution at all