ACS General Chemistry 1 With
Questions And Answers||Latest Exam
2026-2027||Already Graded A+
Mass Number -ANSWER Proton+ Neutrons
Atomic Number -ANSWER # of protons/electrons (equal in elemental form)
- superscript -ANSWER Add e-
+ superscript -ANSWER subtract e-
Isotope -ANSWER Diff number of neutrons
Isomer -ANSWER two or more compounds with the same # of elements but dif structural
shape and properties
Allotrope -ANSWER Dif physical form an element can exist
(example carbon = graphite- charcoal- diamond
Beta Particle -ANSWER Electron from radioactive decay (one negative charge)
Alpha Particle -ANSWER two protons and two neutrons bonded together (two units with
positive charge)
Gold Foil Experience -ANSWER Rutherford discovered that some alpha particles were
scattered at large angles. Conclusion was that most mass of the mass and all of the
positive charge had to be concentrated in a tiny fraction of volume of atom. the rest of
the atom had to be mostly empty space.
Name Labe of Electron configuration
1s^1 -ANSWER 1= energy level
s= type of orbital
^1= # of E in orbital
Transition Elements Orbital letter -ANSWER d (five boxes and 10e-)
Alkaline Earth Metal -ANSWER S^2 (1 box and 2e-)
Lanthanides/ anthanitdes -ANSWER f (7 boxes and 14 Electrons)
Alkali Metals -ANSWER s^1
, group 13-18 -ANSWER p
Valance Shell -ANSWER outer most shell with electrons responsible for bonding
Photon -ANSWER is a packet of energy, the quantity of which is related to the frequency
of the electromagnetic radiation
how do photons interact with covalent bonds? -ANSWER high energy photons such as
ultraviolet parts of the electromagnetic spectrum have enough energy to disrupt
covalent bonds
n -ANSWER Principle quantum number (Shell, size)
l -ANSWER Angular quantum number (Subshell, s,p,d,f, shape)
Formula n-1
ml -ANSWER Magnetic quantum number (orbital, orientation)
-l to +l
Each electron in an orbital has its own set of how many quantum numbers -ANSWER
three
ms -ANSWER Electron spin
+1/2 or -1/2
l=0 -ANSWER s
l=1 -ANSWER p
l= 2 -ANSWER d
l=3 -ANSWER f
Formula for # of subshells -ANSWER 2l+1
S
0 nodal -ANSWER orbital and how many nodals
p
1 nodal -ANSWER Orbital and how many nodals
d
2 nodal -ANSWER orbital and how many nodals
Hund's Rule -ANSWER every orbital in sub-shell must be singly occupied before it can
be double occupied
Questions And Answers||Latest Exam
2026-2027||Already Graded A+
Mass Number -ANSWER Proton+ Neutrons
Atomic Number -ANSWER # of protons/electrons (equal in elemental form)
- superscript -ANSWER Add e-
+ superscript -ANSWER subtract e-
Isotope -ANSWER Diff number of neutrons
Isomer -ANSWER two or more compounds with the same # of elements but dif structural
shape and properties
Allotrope -ANSWER Dif physical form an element can exist
(example carbon = graphite- charcoal- diamond
Beta Particle -ANSWER Electron from radioactive decay (one negative charge)
Alpha Particle -ANSWER two protons and two neutrons bonded together (two units with
positive charge)
Gold Foil Experience -ANSWER Rutherford discovered that some alpha particles were
scattered at large angles. Conclusion was that most mass of the mass and all of the
positive charge had to be concentrated in a tiny fraction of volume of atom. the rest of
the atom had to be mostly empty space.
Name Labe of Electron configuration
1s^1 -ANSWER 1= energy level
s= type of orbital
^1= # of E in orbital
Transition Elements Orbital letter -ANSWER d (five boxes and 10e-)
Alkaline Earth Metal -ANSWER S^2 (1 box and 2e-)
Lanthanides/ anthanitdes -ANSWER f (7 boxes and 14 Electrons)
Alkali Metals -ANSWER s^1
, group 13-18 -ANSWER p
Valance Shell -ANSWER outer most shell with electrons responsible for bonding
Photon -ANSWER is a packet of energy, the quantity of which is related to the frequency
of the electromagnetic radiation
how do photons interact with covalent bonds? -ANSWER high energy photons such as
ultraviolet parts of the electromagnetic spectrum have enough energy to disrupt
covalent bonds
n -ANSWER Principle quantum number (Shell, size)
l -ANSWER Angular quantum number (Subshell, s,p,d,f, shape)
Formula n-1
ml -ANSWER Magnetic quantum number (orbital, orientation)
-l to +l
Each electron in an orbital has its own set of how many quantum numbers -ANSWER
three
ms -ANSWER Electron spin
+1/2 or -1/2
l=0 -ANSWER s
l=1 -ANSWER p
l= 2 -ANSWER d
l=3 -ANSWER f
Formula for # of subshells -ANSWER 2l+1
S
0 nodal -ANSWER orbital and how many nodals
p
1 nodal -ANSWER Orbital and how many nodals
d
2 nodal -ANSWER orbital and how many nodals
Hund's Rule -ANSWER every orbital in sub-shell must be singly occupied before it can
be double occupied
