Atomic Theory Flashcards
State Bohr’s Theory
-Electrons exist in energy levels (orbits)
-You can get an electron to move up to a higher energy level by giving it energy. When it falls back down to its original energy level it gives off visible light.
Explain the relationship between energy, frequency, and wavelength.
Larger energy = higher frequency and slower wavelength.
Distinguish between a continuous, emission, and absorption spectrum. Describe how each is produced and provide examples.
List the electromagnetic series in order of increasing energy.
Radio waves, microwaves, infrared, visible light, UV, X-Rays, gamma rays.
What is a photon?
A packet of energy.
Why do emission line spectra prove that the energy of the atom is quantized?
Match Paschen, Balmer, and Lyman with appropriate energy frequencies and rings.
IR; Paschen, n=3
Visible; Balmer, n=2
UV; Lyman, n=1
State 3 methods of exiciting an electron.
Heat, light, electricity
The orbits in an atom are concentric. What does this mean?
They all share the same nucleus, and two or more rings around the nucleus would produce concentric repeating circles.
What is light of the highest energy? Lowest energy?
Blue, red
Define the term isotope. What do isotopes share and differ?
The same element with the same number of protons but differing the the number of neutrons, leading to different mass.
How does one isotope of carbon differ from another isotope of carbon?
One isotope of carbon has an atomic number of 6, a mass of 12 and another has an atomic number of 6, a mass of 13. The number of neutrons differs.
Complete a relative atomic mass practice question.
How does atomic notation work? (A, Z, X?)
What is the difference between ionic and covalent bonds?
Ionic - Non-Metal + Metal, Transfer of electrons to achieve a stable octet, electrostatic attraction, produces ions.
Covalent - 2 non-metals, share electrons in order to achieve a stable octet, and stay as atoms.
