Aleks Placement Test: Chemistry ACTUAL EXAM 2026
\NEWEST UPDATE WITH COMPLETE QUESTIONS AND
CORRECT DETAILED ANSWERS \VERIFIED 100%
GRADEDC A+
E = h•f
E is energy
Energy using Planck's
h is Planck's
Constant
constant f is
frequency in
hertz
Planck's Constant 6.626•10^-34 Joules/hertz
Wave-Particle Duality of Light Light sometimes acts like a particle and sometimes like a wave
Wave-Mechanical Model of A model of the atom in which the orbitals are nothing like orbits
the Atom
It is impossible to know the exact position and
Heisenberg Uncertainty
Principle momentum of an electron at the same time
The probability of finding electrons in certain regions of
Quantum Theory for an Atom
an atom is described by orbitals
A region around the nucleus of an atom where an
Atomic Orbital
electron with a given energy may be found 90% of the
time; 4 types: s, p, d, and f
, The principal quantum number; tells us which energy
N level an electron is found in, the maximum number of
electrons that can be found in one energy level, and
the size of an electron cloud
L The orbital quantum number; tells us the shape of the orbital
(s,p,d,f)
M Quantum number that tells us the orientation of the orbital in
space
S Quantum number that tells how an electron spins in an orbital
A rule that states that each electron has its own unique
Pauli Exclusion Principle set of quantum numbers and that two electrons with the
same spin cannot occupy the same orbital and that an
orbital can only hold two electrons
S Orbital The orbital with the lowest energy; it has one orbital and can
hold two electrons
The orbital with the second lowest energy; it has three
P Orbital
orbitals and can hold six electrons
The orbital with the second highest energy; it has five
D Orbital
orbitals and can hold ten electrons
F Orbital The orbital with the highest energy; it has seven orbitals and can
hold 14 electrons
Hund's Rule Each suborbital will fill with one electron before accepting a
second electron
Electron configuration shorthand
1. Find the noble gas that comes before the element
Kernel Structure 2. Write the gas in brackets
3. Determine energy level and orbital you are starting on
4.Follow the energy pyramid
Valence Electrons Electrons on outer most orbital; always the highest energy 's' and
'p' orbital
Oxidation State The electrons an element will gain or lose in order to become
stable (8 electrons)
Acids Always start with hydrogen; donate a proton in a solution
Oxyacid Acid that has an oxygen
Organic Acid Acid that contains a carbon atom
Diprotic Acid Acid that has 2 hydrogens to donate
Triprotic Acid Acid that has 3 hydrogens to give
_ ate _ _ ic acid
_ _ ite _ _ ous acid
Methane 1 carbon
, Ethane 2 carbon
Propane 3 carbon
Butane 4 carbon
Pentane 5 carbon
Hexane 6 carbon
Heptane 7 carbon
Octane 8 carbon
Nonatne 9 carbon
Decane 10 carbon
Alcohols Subtract a hydrogen and add a -OH group; add ol to end of
name
\NEWEST UPDATE WITH COMPLETE QUESTIONS AND
CORRECT DETAILED ANSWERS \VERIFIED 100%
GRADEDC A+
E = h•f
E is energy
Energy using Planck's
h is Planck's
Constant
constant f is
frequency in
hertz
Planck's Constant 6.626•10^-34 Joules/hertz
Wave-Particle Duality of Light Light sometimes acts like a particle and sometimes like a wave
Wave-Mechanical Model of A model of the atom in which the orbitals are nothing like orbits
the Atom
It is impossible to know the exact position and
Heisenberg Uncertainty
Principle momentum of an electron at the same time
The probability of finding electrons in certain regions of
Quantum Theory for an Atom
an atom is described by orbitals
A region around the nucleus of an atom where an
Atomic Orbital
electron with a given energy may be found 90% of the
time; 4 types: s, p, d, and f
, The principal quantum number; tells us which energy
N level an electron is found in, the maximum number of
electrons that can be found in one energy level, and
the size of an electron cloud
L The orbital quantum number; tells us the shape of the orbital
(s,p,d,f)
M Quantum number that tells us the orientation of the orbital in
space
S Quantum number that tells how an electron spins in an orbital
A rule that states that each electron has its own unique
Pauli Exclusion Principle set of quantum numbers and that two electrons with the
same spin cannot occupy the same orbital and that an
orbital can only hold two electrons
S Orbital The orbital with the lowest energy; it has one orbital and can
hold two electrons
The orbital with the second lowest energy; it has three
P Orbital
orbitals and can hold six electrons
The orbital with the second highest energy; it has five
D Orbital
orbitals and can hold ten electrons
F Orbital The orbital with the highest energy; it has seven orbitals and can
hold 14 electrons
Hund's Rule Each suborbital will fill with one electron before accepting a
second electron
Electron configuration shorthand
1. Find the noble gas that comes before the element
Kernel Structure 2. Write the gas in brackets
3. Determine energy level and orbital you are starting on
4.Follow the energy pyramid
Valence Electrons Electrons on outer most orbital; always the highest energy 's' and
'p' orbital
Oxidation State The electrons an element will gain or lose in order to become
stable (8 electrons)
Acids Always start with hydrogen; donate a proton in a solution
Oxyacid Acid that has an oxygen
Organic Acid Acid that contains a carbon atom
Diprotic Acid Acid that has 2 hydrogens to donate
Triprotic Acid Acid that has 3 hydrogens to give
_ ate _ _ ic acid
_ _ ite _ _ ous acid
Methane 1 carbon
, Ethane 2 carbon
Propane 3 carbon
Butane 4 carbon
Pentane 5 carbon
Hexane 6 carbon
Heptane 7 carbon
Octane 8 carbon
Nonatne 9 carbon
Decane 10 carbon
Alcohols Subtract a hydrogen and add a -OH group; add ol to end of
name
