Download Preparation Vocab Quiz

Chemistry U3 Vocabulary Quiz
Period: ____
Name: ______________________
Use the Word bank to identify each item described below.
1. Who discovered the nucleus and proposed the Nuclear Model of the atom?
2. “When determining the electron configuration of nitrogen, one electron is placed
in each of the three 2p orbitals” is an example of what?
3. The horizontal rows of the periodic table are called this.
4. What experiment was used to determine the charge of the electron?
5. An integer number that represents the number of protons and neutrons in an atom.
6. Who developed the first atomic theory based on experimental results?
7. What subatomic particle was discovered through the use of a Cathode Ray Tube?
8. Another name for the first vertical column of the periodic table.
9. It states that no two electrons can have the same four quantum numbers.
10. He is credited with developing the first periodic table by predicting a new element.
11. Electrons are only able to move in allowable orbits with specific energy.
12. When determining the electron configuration of aluminum, electrons must be
placed in the 2s orbital before the 2p orbital.
13. The ability of an atom to attract electrons to itself within a chemical bond.
14. A region of space that can hold two electrons and is shaped like a dumb bell.
15. The amount of energy needed to remove an electron from a neutral atom.
16. The quantum number that indicates the shape of an orbital and the type of subshell.
17. All orbitals of equal energy are occupied by one electron before a second electron
is added to any of them.
18. When excited electrons fall from a higher orbit back to the ground state they
emit specific frequencies of light referred to as emission spectra.
19. A concentrated collection of protons and neutrons in the center of an atom.
20. Atoms of one element cannot be converted into atoms of another element.
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proton
neutron
electron
nucleus
atom
atomic mass
mass number
atomic number
isotope
ion
charge
element
periodic table
period
group
alkali metal
alkaline earth metal
transition metal
representative metal
nonmetal
halogen
noble gas
atomic radii
ionic radii
isoelectronic series
ionization energy
electronegativity
s orbital
p orbital
d orbital
f orbital
s block
p block
d block
f block
quantum numbers
principle quantum number
angular momentum quantum number
magnetic quantum number
spin quantum number
orbital energy
Aufbau Principle
Hund’s rule
Pauli Exclusion Principle
Electron configuration
Democritis
Boyle
Lavoisier
Dalton
Thomson
Millikan
Rutherford
Bohr
Chadwick
Schrӧdinger
Heisenberg
deBroglie
Mendeleev
Atomic theory
Plum Pudding model
Nuclear atom
Bohr model
Quantum mechanics
Cathode Ray Tube
Oil Drop Experiment
Gold Foil Experiment
Optical Spectr