Download 30-2 Ch 3 Test Review Atomic Theory DEBRIEF KEY

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Review for Atomic Theory Test (Ch.3)
Learning Targets/Key Ideas for Chemistry Part 1 Test
*Know the general rules of charges: all matter has charges, opposite charges attract, like charges repel.
*History and contributions of Scientists involved in the Atomic Theory (know the models)
*How to use the Periodic Table! Ex: Atomic Number, # of electrons, protons, neutrons, Valence Electrons,
*Understand different light spectra and how they are produced (think about the emitting the truth activity
we did)
1.
How do electrons influence the structure/shape and size/scale of atoms? Think about the charge of
the electron cloud.
THE NUCLEUS (PROTONS & NEUTRONS) MAKE UP 99% OF THE MASS/WEIGHT
OF AN ATOM HOWEVER IT IS 100,000x SMALLER (THINK OF A PEA IN THE MIDDLE OF
A FOOTBALL FIELD). ELECTRONS OCCUPY MOST OF THE SPACE OF AN ATOM.
2.
Why are elements (atoms) normally neutral? (Draw it, hint protons and electrons)
ATOMS IN THEIR “NORMAL” STATE HAVE EQUAL NUMBER
OF PROTONS (+) AND ELECTRONS (-).
3. How did the atomic theory (model) change over time? (Dalton, Thompson, Rutherford, Bohr, Chadwick
and Schrodinger):
Dalton
Thompson
Rutherford
Bohr
Chadwick
Schrodinger
4. Briefly explain how and why the atomic model has changed:
THROUGH ADVANCES IN TECHNOLOGY AND CONTINUED EXPERIMENTATION
SCIENTISTS HAVE BEEN ABLE TO IMPROVE THE ATOMIC MODEL.
5. Was the evidence that these scientists used to come up with their atom theories Direct Evidence or
Indirect Evidence? Explain: SCIENTIST INFERED WHAT THE ATOM LOOKS LIKE BASED
ON INDIRECT EVIDENCE (I.E. ALPHA PARTICLES BOUNCING BACK).
6. Draw a simplified version of Ernest Rutherford’s experiment and briefly explain how it worked:
6b: What were the 3 big findings/conclusions that Rutherford inferred from his experiments?
1) ATOMS ARE MOSTLY EMPTY SPACE
2) THE NUCLEOUS IS POSITIVELY CHARGED
3) NOT MUCH MASS TO THE ELECTRONS
7. Niels Bohr studied light spectrum, what did he infer about the following?
a) What produced the bright lines of the spectrum?
MOVING (JUMPING UP AND FALLING BACK TO ORIGINAL ORBITS) ELECTRONS (e-).
b) What produced the black lines of the spectrum?
SPACE WITHOUT ELECTRON MOVEMENT.
c)
What part of the atom is responsible for creating color? ELECTRON(s)
d) Which color (end) of the spectrum has the lowest energy?
RED
e)
Which color (end) of the spectrum has the highest energy?
VIOLET/PURPLE
8. Electron transitions between which 2 levels will produce the spectral line associated with the least
energy?
a. 2 and 1
5
b. 3 and 2
4
c. 5 and 3
d. 5 and 1
3
e. 4 and 2
2
1
9. Draw the Bohr Model of carbon, sodium, and chlorine. Show how each of them would become stable
(happy).
Carbon
Sodium
Chlorine
Share e-
Lose 1 e-
Gain 1 e-
10. Draw the Lewis Model of carbon, sodium, and chlorine. Show how each of them would become
stable (happy).
Carbon
Sodium
Chlorine
Unstable/Unhappy
Unstable/Unhappy
Unstable/Unhappy
Use your periodic table to determine the following:
11. The number of protons in a Helium atom is… 2 p+
12.
The number of neutrons in a Sulfur atom is….
16 n
13.
The number of electrons in a Potassium atom is…. 19 e-
14. The number of valence electrons in a Fluorine atom is…
15. The number of neutrons in a Strontium atom is….
16.
7 e-
50 n
The number of valence electrons in an Argon atom is….
8 e-