chemistry

• amount of a substance

  Mole
• is a unit of measure of matter

  moles
• the relationship between the amounts of reactants in a chemical reaction

  stoichiometry
• Avogrado's Number

  6.02x10^23
• steps to solving stoichiometry

  1. balance equation first 2. Identify knowns and unknowns 3. convert mass to moles 4. use stoichiometric factor or ratio to determine amount of unknown in moles 5. convert back to mass if needed
• represents the smallest ratio of atoms in a compound

  empirical formula
• gives the total number of atoms of each present in one molecule or compound

  molecular formula
• steps to finding the molecular formula

  1. find empirical formula 2. calculate the atomic mass of e.f 3. divide final (M of m.f) by e.f 4. multiply coefficient by e.f
• empirical formula steps

  1. convert percentage to grams 2. calculate moles of each element 3. divide each mole by smallest
• stp

  standard temperature pressure
• rtp

  room temperature and pressure
• equal volume of gases at contrast P and T have same number of moles and gas

  Avogrado's Law
• is the reactant present in the smallest stoichiometric amount. it determines how much product can br form

  Limiting reactants
• forces that exist within

  molecules or fundamental/formula units

  (forces that hold atoms or ions in a

  compound)

  intramolecular
• forces of attraction that

  exist between the molecules in a

  compound

  intermolecular
• three types of chemical bond

  ionic, covalent, metallic
• Electrostatic attraction

  between ions

  ionic
• Sharing of

  electrons

  covalent
• Metal atoms

  bonded to

  several other

  atoms

  metallic
• 22.4 L or dm^3

  stp- standard room pressure
• 24 L or dm^3

  rtp- room temperature and pressure
• is a chemical bond

  formed by the electrostatic attraction

  between positive and negative ions.

  An ionic bond
• is a

  symbol in which the electrons in the

  valence shell of an atom or ion are

  represented by dots placed around the

  letter symbol of the element.

  A Lewis electron-dot symbol
• When two nonmetals bond, they often

  share electrons since they have similar

  attractions for them. This sharing of

  valence electrons is called the

  covalent

  bond.
• forces are attractive forces between molecules.

  intermolecular
• forces hold atoms together within in a molecule.

  intramolecular
• the nucleus ejects two protons and two neutrons.

  alpha decay,
• occurs when a neutron in the nucleus splits into a

  proton and an electron.

  Beta decay
• is not truly a decay reaction in the sense that the

  nucleus doesn’t become something different.

  Gamma decay
• Nuclide


  is a nucleus with a specified number of protons

  and neutrons.
• Radionuclide


  nuclide that are radioactive.
• Radioisotopes


  atoms containing a radionuclide
• IS THE “FATHER OF ATOMIC THEORY”

  john dalton
• DEMOCRITUS 


  THE FIRST PERSON TO COME UP WITH THE IDEA OF ATOM.
• Intermolecular forces


  The attractive forces that exist between molecules in a compound. Weaker than covalent bonds.
• Dipole-dipole forces


  Occur when two polar molecules are close to each other and the positive end of one molecule is attracted to the negative end of the other.
• Hydrogen bonding


  A special type of dipole-dipole force that occurs when a hydrogen atom is bonded to a highly electronegative atom, such as nitrogen, oxygen, or fluorine. The resulting bond is stronger than a regular dipole-dipole force.
• London dispersion forces


  The weakest type of intermolecular force that occurs in all molecules, regardless of their polarity. Result from the temporary movement of electrons in a molecule.