clep chemistry exam latest questions and correct d
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CLEP Chemistry EXAM LATEST
QUESTIONS AND CORRECT DETAILED
ANSWERS | AGRADE
John Dalton - ANSWER>> Proposed that matter is composed of atoms; these atoms have different
identities called elements, which combine to form compounds; measured masses of reactants and
products.
J.J. Thompson - ANSWER>> Observed deflection of particles in a cathode ray tube; proposed that atoms
are composed of positive and negative charges; developed the plum pudding model of the atom
Robert Millikan - ANSWER>> Calculated the charge-to-mass ratio of electrons using oil drops falling in an
electric field; surmised the charge of a single electron
Ernest Rutherford - ANSWER>> Used the deflection of alpha particles in a cathode ray tube to discover
that most of the atom is empty space, with protons and neutrons centered in the nucleus.
Niels Bohr - ANSWER>> Determined that electrons exist around the nucleus at a fixed radius; electrons
with higher energy exist farther from the nucleus. Electrons give off electromagnetic radiation when
moving between energy levels.
Max Planck - ANSWER>> Determined that energy is quantized, or composed of discrete bundles.
6.63 x 10^-34 J*sec - ANSWER>> Planck's Constant (h)
3.00 x 10^8 m/sec - ANSWER>> Speed of Light (c)
E = hv - ANSWER>> Energy of a Photon Formula (1)
E = hc / wavelength - ANSWER>> Energy of a Photon Formula (2)
Louis DeBroglie - ANSWER>> Combined Einstein's relationship between mass and energy and the
relationship between velocity and the wavelength of light. All particles with momentum have a
corresponding wave nature.
Wavelength = h / mv - ANSWER>> Wavelength of Particles Formula
Heisenberg's Uncertainty Principle - ANSWER>> It is impossible to simultaneously know the position and
momentum of an electron.
Erwin Schrodinger - ANSWER>> Attributed a wave function to electrons, describing the probability of
where an electron might exist.
Orbitals - ANSWER>> Regions of high probability where electrons might exist; broken into four levels: s,
p, d, or f
Atomic Mass - ANSWER>> The cumulative mass of all the particles in the atom; found by adding the
masses of the protons and neutrons.
, Units: Atomic Mass Units (AMU)
Example:
helium = 2 protons + 2 neutrons
= 4 AMU
Atomic Number - ANSWER>> The number of protons in the nucleus of an atom, or the total nuclear
charge. Also the number of electrons surrounding the nucleus.
Isotopes - ANSWER>> Atoms with the same number of protons but different numbers of neutrons.
Example: carbon-12 (6 neutrons) vs carbon-14 (8 neutrons)
Atomic Weight - ANSWER>> Molar mass of the element, or the mass in grams of one mole of atoms
Pauli Exclusion Principle - ANSWER>> No two electrons can occupy the exact same energy level or have
the same set of four quantum numbers
Quantum numbers - ANSWER>> 1. Principal (n)
2. Angular Momentum (l)
3. Magnetic (ml)
4. Magnetic Spin (ms)
Principal Quantum Number - ANSWER>> The shell or energy level an electron occupies; values from 1-7.
Electrons with higher values are farther from the nucleus.
Angular Momentum Quantum Number - ANSWER>> The subshell the electron occupies; describes the
shape of an electron's orbital.
n = 1: l = 0 (s)
n = 2: l = 0 (s), 1 (p)
n = 3: l = 0 (s), 1 (p), 2 (d)
n = 4: l = 0 (s), 1 (p), 2 (d), 3 (f)
Magnetic Quantum Number - ANSWER>> Represents the orbital position.
l = 0: ml = 0 (1 possible s orbital)
l = 1: ml = -1, 0, 1 (3 possible p orbitals)
l = 2: ml = -2, -1, 0, 1, 2 (5 possible d orbitals)
l = 3: ml = -3, -2, -1, 0, 1, 2, 3 (7 possible f orbitals)
Magnetic Spin Quantum Number - ANSWER>> Each orbital contains at most 2 electrons: one with a
positive spin (+1/2) and one with a negative spin (-1/2)
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