Negative Charges

• Azimuthal Quantum Number (l)


  Tells the energy sublevel or the type of orbital the electron is in
• Core Electrons


  The inner electrons of an atom
• Electron Configuration


  The notation showing how electrons are arranged in the orbitals
• Group


  The vertical arrangement (18 groups) in the periodic table
• Heisenberg Uncertainty Principle


  States that no one can exactly measure everything about electron's movement and location
• Magnetic Quantum Number (ml)


  Denotes the orientation of the orbital in space
• Orbit


  A definite path traveled by an electron around the nucleus as described by Planetary Model
• Orbital


  A region, space, or cloud outside the nucleus where electrons can be found
• Period


  The horizontal arrangement (7 periods) of elements in the periodic table
• Principal Quantum Number (n)


  Gives the energy level an electron belongs to
• Spin Quantum Number (ms)


  Determines the way an electron spins (either clockwise (+1/2) or counterclockwise (-1/2))
• Valence Electrons


  Electrons found at the outermost energy level of an atom
• Ionic bond


  Happens between a nonmetal and a metal
• Covalent bonds


  Characterized by the sharing of electrons between two or more nonmetallic elements
• Ionic compound


  Forms when metallic and nonmetallic elements bond
• Covalent compound


  Forms when two or more nonmetallic elements bond
• Chemical formula

  Shows the kind and number of atoms present in a molecule
• Chemical name


  Shows the names of each element in a compound
• Physical property


  A characteristic that can be observed or measured
• ‘carbon’ is the Latin word ‘carbo’ which means charcoal.
• organic chemistry is the study of carbon compounds.
• Hydrocarbons


  The simplest organic compounds that contain only the elements carbon and hydrogen
• Hydrocarbons


  • Classified either as aliphatic or aromatic
• Aliphatic hydrocarbons


  Carbon atoms are linked with each other in open chains, either straight or branched
• Types of aliphatic hydrocarbons

  • Alkanes
  • Cycloalkanes
  • Alkenes
  • Alkynes
• Aromatic compounds


  Compounds that contain benzene rings as part of their structure
• Alkanes


  Saturated hydrocarbons with single carbon-to-carbon covalent bonds
• Alkenes


  Unsaturated hydrocarbons with at least one double carbon-to-carbon covalent bonds
• Alkynes


  Unsaturated hydrocarbons with at least one triple carbon-to-carbon covalent bonds
• Functional Group


  Responsible for the reactivity of the organic compound, these group of atoms affect the behavior of the parent organic molecule
• Types of Functional Groups

  • Alcohol
  • Ether
  • Aldehyde
  • Ketone
  • Carboxylic acid
  • Ester
  • Amine
  • Amide
  • Halide
• Alcohol


  Due the presence of OH group, it can form hydrogen bond that will results to higher boiling pt. compare to its parent molecule
• Ether


  Have low boiling point compare to alcohol due to its inability to form hydrogen bond, but it is more reactive than alkanes
• Aldehyde and Ketone


  Both contain carbonyl group which is carbon double bonded to an oxygen, the difference is in aldehyde the carbonyl group is at the end of the organic compound while in ketone the carbonyl group is inside the organic compound
• Carboxylic Acid


  Organic acid that contains both hydroxyl group and carbonyl group on the same carbon
• Ester


  Derived from its parent molecule which is carboxylic acid and alcohol, known for its fragrant smell
• Amine


  Characterized by the presence of nitrogen atom a lone pair of electrons and three substituents, neurotransmitters are amine-based molecule
• Amide


  Derived from carboxylic acid and amine, the simplest amides are derivatives of ammonia, amides are very weak bases
• Halide


  Binary compound wherein one part is a halogen, halides are used as solder paste
• Formula mass


  The sum of atomic masses of the ions present in the formula unit of an ionic compound