AP chemistry 100% guaranteed well
elaborated questions and answers 2025
GRADED A+
to find empirical formula
1. Get mass of each element by dividing % given by grams in periodic table
2. Convert the mass of each element to moles
3. divide each by the lowest number of moles
If F in coulumbs law is + or -
+ means repulsion, - means attraction
electron levels
electron shells; the period numbers
electron sublevels/orbitals
s,p,d, & f. Number of electrons in each sub level: (s= 2) (p= 6) (d=10) (f=14)
electron configuration chart
groups & periods
GROUPS: columns
PERIODS: rows
ionization energy
amount of energy required to remove an electron
electronegativity
ability of atom to attract electrons
why is electronegativity inverse to atomic radius
larger radius = larger distance between nucleus of one atom and the outer shell of another
electron affinity
amount of energy released when atom gains electron. the more negative, the higher & more
exothermic (favorable)
electron affinity trend
, RIGHT AND UP, bc more energy is released when electronegative, nonmetals gain electrons. it
is exothermic
charges for each group
amount of valence for each group
polarity
a measure of how unequal electron distribution is in chemical bond, due to difference in
electronegativity
dipole arrow
points towards more electronegative atom in a bond
potential energy curve
x is distance, y is potential energy
to draw a lewis diagram
1. Count total valence electrons of all atoms; adjust based on ions
2. Determine central atom (least electronegative or written first) & draw atoms around with
single bonds
3. Subtract electrons used for bonding
4. Add remaining valences around atoms, trying to give each an octet.
if an atom can't have an octet in a lewis diagram?
Double/triple bonding required. If atom is in 3rd period or below, it is large enough to have more
than 8 electrons
formal charge
valence electrons - assigned electrons
dominant structure in the resonance
the one with the least amt of nonzero charges
if there is a nonzero formal charge in a structure
nonzero charge must go to the most electronegative atom
VSEPR Theory
Valence-shell electron-pair repulsion theory; bonds & electrons equally space themselves apart
to minimize repulsion
electron domains
elaborated questions and answers 2025
GRADED A+
to find empirical formula
1. Get mass of each element by dividing % given by grams in periodic table
2. Convert the mass of each element to moles
3. divide each by the lowest number of moles
If F in coulumbs law is + or -
+ means repulsion, - means attraction
electron levels
electron shells; the period numbers
electron sublevels/orbitals
s,p,d, & f. Number of electrons in each sub level: (s= 2) (p= 6) (d=10) (f=14)
electron configuration chart
groups & periods
GROUPS: columns
PERIODS: rows
ionization energy
amount of energy required to remove an electron
electronegativity
ability of atom to attract electrons
why is electronegativity inverse to atomic radius
larger radius = larger distance between nucleus of one atom and the outer shell of another
electron affinity
amount of energy released when atom gains electron. the more negative, the higher & more
exothermic (favorable)
electron affinity trend
, RIGHT AND UP, bc more energy is released when electronegative, nonmetals gain electrons. it
is exothermic
charges for each group
amount of valence for each group
polarity
a measure of how unequal electron distribution is in chemical bond, due to difference in
electronegativity
dipole arrow
points towards more electronegative atom in a bond
potential energy curve
x is distance, y is potential energy
to draw a lewis diagram
1. Count total valence electrons of all atoms; adjust based on ions
2. Determine central atom (least electronegative or written first) & draw atoms around with
single bonds
3. Subtract electrons used for bonding
4. Add remaining valences around atoms, trying to give each an octet.
if an atom can't have an octet in a lewis diagram?
Double/triple bonding required. If atom is in 3rd period or below, it is large enough to have more
than 8 electrons
formal charge
valence electrons - assigned electrons
dominant structure in the resonance
the one with the least amt of nonzero charges
if there is a nonzero formal charge in a structure
nonzero charge must go to the most electronegative atom
VSEPR Theory
Valence-shell electron-pair repulsion theory; bonds & electrons equally space themselves apart
to minimize repulsion
electron domains
