CHEM 1030 Exam 2- Forbes AU
Questions and Answers
Atomic size trend
increases right to left
increases downward
(He smallest)
Principle Quantum Number
indicates the main energy level occupied by the electron
-increases downward
ex. bottom group atomic radius & nuclear charge > top group radius & nuclear
charge
valance electrons charge
weak
ionization energy trend
,increase left to right
increase upward
cations size
smaller (lose valance)
anions size
larger (gain valance)
Zeff
effective nuclear charge
Zeff= Z-S
Z= atomic number
S=inner shell electrons
valence electrons
atom's outermost electrons
,ionization energy (IE)
the energy required to remove one electron from a neutral atom of an element
electron affinity (EA)
adding an electron
-increases upward and left to right
types of bonds
ionic, covalent, metallic
ionic bond
metal + nonmetal
-held together by electrostatic attractions
ex. NaCl, MgO
electrostatic potential energy (Ee1)
strength of ionic attraction
Ee1=2.31 x 10^-19 j x nm (Q1 x Q2/d)
Q1=charge of ion
, Q2=charge of ion
d= addition of two distances
Lattice energy (U)
the energy required to completely separate one mole of a solid ionic compound
into gaseous ions
covalent bond
nonmetal + nonmetal
ex. H2 CO2 H2SO4
metallic bond
metal + metal
naming binary compounds of main group
1. first word is cation
2. second word is anion
-ide
ex. Al2O3 aluminum oxide
Questions and Answers
Atomic size trend
increases right to left
increases downward
(He smallest)
Principle Quantum Number
indicates the main energy level occupied by the electron
-increases downward
ex. bottom group atomic radius & nuclear charge > top group radius & nuclear
charge
valance electrons charge
weak
ionization energy trend
,increase left to right
increase upward
cations size
smaller (lose valance)
anions size
larger (gain valance)
Zeff
effective nuclear charge
Zeff= Z-S
Z= atomic number
S=inner shell electrons
valence electrons
atom's outermost electrons
,ionization energy (IE)
the energy required to remove one electron from a neutral atom of an element
electron affinity (EA)
adding an electron
-increases upward and left to right
types of bonds
ionic, covalent, metallic
ionic bond
metal + nonmetal
-held together by electrostatic attractions
ex. NaCl, MgO
electrostatic potential energy (Ee1)
strength of ionic attraction
Ee1=2.31 x 10^-19 j x nm (Q1 x Q2/d)
Q1=charge of ion
, Q2=charge of ion
d= addition of two distances
Lattice energy (U)
the energy required to completely separate one mole of a solid ionic compound
into gaseous ions
covalent bond
nonmetal + nonmetal
ex. H2 CO2 H2SO4
metallic bond
metal + metal
naming binary compounds of main group
1. first word is cation
2. second word is anion
-ide
ex. Al2O3 aluminum oxide
