exam 2 chem

• Hypochlorite

  ClO-
• Hydroxide

  OH-
• Carbonate


  CO3(2-)
• Dihydrogen Phosphate: H2PO4-
• Cyanide

  CN-
• Ionic Radius Size

  smaller Zeff = larger ion

  larger Zeff = smaller ion
• Zeff

  Increases across PT

  Decreases down PT
• Electron Affinity

  Increases left to right
• Atomic Radius


  decreases left to right

  Increases going down
• Ammonium: NH+(4)
• Acetate: C2H3O2
• Azide: N3-
• Thiocyanate: SCN-
• Perchlorate: ClO-3
• Chlorate: ClO3-
• Chlorite: ClO2-
• Chromate: CrO4 2-
• dichromate: Cr2O7 2-
• Phosphite: PO3 3-
• Phosphate: PO4 3-
• Nitrate: NO3-
• Nitrite: NO2-
• Oxalate: C2O42-
• Permanganate: MnO4-
• Hydrogen Sulfate (Bisulfate): HSO4-
• Sulfate: SO4 2-
• Sulfite: SO3 2-
• Hydrogen Phosphate: HPO4 2- .
• Hydrogen Carbonate (bicarbonate): HCO3-
• How do you determine the mass of a sample given the number of moles and molar mass? Mass = Number of moles x Molar mass
• Define wavelength, frequency, and energy of light. Wavelength is the distance between two adjacent points on a wave. Frequency is the number of waves passing a point per second. Energy is the amount of energy transferred per second.
• Visible light has a wavelength range of approximately: 400nm to 700nm
• The Bohr model of the hydrogen atom explains: The electron shells around the nucleus.
• In an energy level diagram, a positive ΔE represents an absorption or emission: Absorption
• Define valence electrons and explain their importance in chemical bonding. Valence electrons are the outermost electrons in an atom. They are important in chemical bonding because they are involved in the formation of covalent bonds.
• Define effective nuclear charge and its symbol. The charge of an electron in an atom is equal to the sum of the charges of the protons and neutrons in the nucleus.
• How does effective nuclear charge influence atomic radius and ionization energy?

  Atomic radius: Decreases

  Ionization energy: Increases
• mono


  one
• di


  two
• tri


  three