CHEMIO MIDTERM

• Nomenclature


  Other term for the word "naming"
• Binary compounds


  Compounds made of two different elements bonded together
• Monoatomic ion


  An ion composed of single atom
• Polyatomic ion


  An ion composed of more than one atom
• Cations


  Positively-charged ions due to losing of electrons (metals)
• Anions


  Negatively-charged ions due to gaining of electrons (non-metals)
• Nomenclature of cations


  • Name of metal atom
  • Use Roman Numerals to denote the charge of the atom
• Nomenclature of anions


  • Name of non-metal with "ide" ending
• Transition metals


  • Elements with partially filled d-orbitals
  • Also known as "transition elements"
• Nomenclature of transition metals

  • Use Roman Numerals to denote the charge of the atom
  • Ferrous (lower)
  • Ferric (higher)
  • Cuprous (lower)
  • Cupric (higher)
  • Aurous (lower)
  • Auric (higher)
  • Manganese (II)
  • Manganese (III)
  • Tin (II)
  • Tin (IV)
  • Lead (II)
  • Lead (IV)
• Polyatomic ions


  An ion composed of more than one atom
• Examples of polyatomic ions

  • Hydroxide
  • Sulfate
  • Nitrate
• Binary compounds - Type I


  Compounds between cations and anions
• Binary compounds - Type II


  Compounds between transition metals and nonmetals
• Nomenclature of binary compounds - Type I


  • Cation name + Anion name with "-ide" ending
• Nomenclature of binary compounds - Type II


  • Transition metal name with Roman Numerals + Anion name with "ide" ending
• Ternary compounds


  Formed from a metal cation and a polyatomic anion, contain 3 or more different elements in the formula
• Ternary compounds - Special rule


  When the formula unit contains two or more of the same polyatomic ion, that ion is written in parentheses with the subscript written outside the parentheses
• Covalent bond occurs between two or more non-metals by sharing of electrons, covalently bonded compounds consist of molecules
• Molecular formula


  Shows the kinds and numbers of atoms present in a molecule of a compound
• Periodic Table


  An arrangement of all the elements known to man in accordance with their increasing atomic number and recurring chemical properties

  
• Structural formula


  An ion composed of single atom
• Periodic Table


  • Elements are organized on the table according to their atomic number
  • Flows from LEFT to RIGHT

  
• Atomic Number


  The number of protons an atom of that element has
• Prefixes for molecular compounds

  • Mono (1)
  • Di (2)
  • Tri (3)
  • Tetra (4)
  • Penta (5)
  • Hexa (6)
  • Hepta (7)
  • Octa (8)
  • Nona (9)
  • Deca (10)
• Atomic Mass


  The "weight" of the atom (No of protons + no of neutrons)
• If there is only one of the first element in a molecular compound, do not use the prefix "mono"
• Valence electrons


  • The electrons in the outer energy level of an atom
  • The electrons that are transferred or shared when atoms bond together
• If the nonmetal starts with a vowel, drop the vowel ending from all prefixes except "di" and "tri"
• Dimitri Mendeleev


  The "Father of the Periodic table" who put forth the first iteration of the periodic table like the one we use now

  
• Mendeleev modeled his periodic table (initially 63 elements) based on increasing atomic mass, whereas the modern periodic law is based on the increasing order of atomic numbers

  
• Periods


  • The Rows on the Periodic table (left to right)
  • Elements in a row have the same number of electron shells
  • As Periods increase, "n" also increases (orbit size increases)
• Groups


  • Elements in a group have the same number of valence electrons
  • Elements in the same family share similar characteristics
• Groups


  • Group 1: 1 valence electron
  • Group 2: 2 valence electrons
  • Group 13: 3 valence electrons
  • Group 14: 4 valence electrons
  • Group 15: 5 valence electrons
  • Group 16: 6 valence electrons
  • Group 17: 7 valence electrons
  • Group 18: 8 valence electrons (most stable, except He who has 2)
• 1. P-D-F Blocks


  • Regions in the periodic table that have their corresponding blocks
• Electronegativity


  • A chemical property that describes the tendency of an atom or a functional group to attract electrons toward itself
  • Increases left to right across a period
  • Decreases top to bottom of groups
• Chemical bonding


  Formation of bonds between atoms, molecules, or ions
• Ionization Energy


  The energy required to remove the most loosely bound (Valence electron) electron from an isolated atom in a gaseous state
• Chemical bonds


  Attractive forces which holds the atoms, molecules, or ions together in the resulting compound
• Categories of the Periodic Table

  • Non-metals
  • Metals
  • Metalloids