Show:
Atomic Structure
Electron Arrangement
Bohring Experiments
Waves
Quantum Mechanics
100
What subatomic particles are in the nucleus and what is their charge?
Protons = positive and neutrons = neutral
100
Where are electrons located in the atom?
On energy levels, sublevels, in orbitals (answers will vary.)
100
Describe the Bohr model of the atom. Include subatomic particles and a description of their location.
Bohr placed the electrons in rings orbiting the nucleus, which held only protons at the time.
100
Define wavelength (can draw a picture.)
distance from crest to crest on consecutive waves
100
What happens to the electrons in atoms (in gaseous state) when electricity is passed through them?
They jump up to higher energy levels
200
What is the difference between an orbit and an orbital?
Orbit = 2D - rings (old idea) Orbital = 3D - e-clouds
200
Which neutral element is represented by the electron configuration: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d2 ?
Titanium (Ti)
200
When Rutherford conducted his gold foil experiment, he was trying to prove which model of the atom to be correct?
Plum pudding model (Thompson.)
200
How are wavelength and frequency related?
Inverse
200
What happens to the electrons in atoms of elements (in gaseous state) after electricity is passed through them and they have "jumped up" to a higher energy level? (Be specific)
They fall back down and emit Energy, Energy corresponds directly to frequency, different colors of light have different frequencies, so a pattern of colors is detected.
300
Thallium has 2 isotopes, Th-203 and Th-204. Its atomic number is 81 and atomic mass is 204.38 amu. Compare the two isotopes in terms of number of protons, neutrons, and electrons.
Both isotopes have 81 protons and 81 electrons. Th-203 has 122 neutrons and Th-204 has 123 neutrons.
300
Name the principle violated in Ag's electron configuration: (Kr)5s1, 4d9.
The Aufbau Principle (that says electrons occupy the orbitals of lowest energy first.)
300
Describe Rutherford's gold foil experiment and how it changed the model of the atom.
Rutherford shot alpha particles (+ charge) at a thin piece of gold foil (containing gold atoms.) Most particles went straight through, 1 in 8000 were deflected, signifying something + in the atom (nucleus) with lots of empty space and the electrons on the outside.
300
How are energy and wavelength related?
Inversely
300
What is an atomic emission spectrum called the "atomic fingerprint" for an element?
Each one is unique to the element (remember the glowing light boxes you looked at? Also the flame test lab!)
400
Compare the mass and volume of the nucleus to the mass and volume of the rest of the atom.
The nucleus has a large mass (dense core) and smaller volume compared to the rest of the atom.
400
Which rule states that electrons occupy equal energy orbitals separately before pairing up (maximum number of UNPAIRED electrons)?
Hund's Rule
400
Define "quantum" in terms of energy levels.
A quantum is the amount of energy required to move an electron from one energy level to another.
400
Compare the speed of UV rays to the speed of microwaves.
The same (speed of light: 3.0 x 10^8 m/s)
400
What is the Heisenberg Uncertainty Principle? (remember the fan)
It is impossible to know exactly both the velocity and the position of a particle (electron) at the same time. (by finding one, you change the other.)
500
Who discovered the neutron (and when)?
James Chadwick, 1932
500
What would be the ending of the e- configuration for Pu and how many valence electrons does it have?
5f5 is ending e-configuration, and it has 2 valence electrons
500
What is the photoelectric effect?
When a piece of metal is heated, electrons can be ejected from its surface. (they acquire enough energy to "escape")
500
Why did we talk about waves in this chapter?
Because electrons act like waves (and like particles.) They have properties of both (just like light.)
500
I am a spectroscopist. What do I do?
A spectroscopist observe various emission lines from sample, record and study them in order to calculate the relative concentrations of substances in the sample. With an advanced degree in chemistry, you, too, could be a spectroscopist!