Transcript POGIL Answer Keys Grab a Marker and Trade Papers

POGIL Answer Keys
Grab a Marker and Trade Papers
2/x
Average Atomic Mass
1. 12
2. 24, 25, and 26
3. No, some have more mass that the
others
4. Mass 24 – 16
Mass 25 – 2
Mass 26 – 2
5. 24Mg
6.
Mass 24 – 8
Mass 25 – 1
Mass 26 – 1
2/x
7a. Mass 24 – 16
Mass 25 – 2
Mass 26 – 2
7b. It matches the model in Model 1
8. 24 amu – as that has the greatest
abundance
9a. 24.306
9b. No
10a. It would be too much to squeeze into
one box
10b. As the physical and chemical
properties of isotopes are the same it is
not usually important to scientists.
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11. Mary’s method = 24.305 amu
Jack’s method = 24.305 amu
Alan’s method = 24.984 amu
12a. Mary and Jack
12b. Alan’s method incorrectly weights all
the isotopes the same
13. 15.999 amu
14a. 24Mg
14b. As 24Mg is the most abundant the
weighted average will be closest to
24Mg
15. As the average mass is 10.81 boron-11
must be most abundant.
2/x
16a. Yes
16b. No, as the composition is identical
16c. The bonding between the atoms
makes the difference.
17. Allotrope – same composition, but
different characteristics because of
different bonding
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Coulombic Attraction
1. + = proton, - = electron
2. Attraction
3. As distance increases the force of
attraction decreases.
4. Less than
5. Greater than
6a. The force of attraction
6b. The strength
7a. It increases
7b. In decreases
8. More protons make for a larger force
9. 11.5 x 10-8 N
10. It should decrease
2/x
11. Row
12.
13. Chlorine
14a. No
14b. No
14c. Na = 11, Al = 13, Cl = 17
14d. Yes – more protons means more
attraction
15a. Ca
15b. Cu
15c. Ar
16a. Li = 3, Na = 11, K = 19
16b. Distance as the force of attraction
decreases while also having more protons
17a. Inverse
17b. Direct
2/x
2/x
Electron Energy and Light
1. Shades of the color
2. Yes
3. Violet = highest
4. red = lowest
5a. Red
5b. Violet
5c. Wavelength is inversely related to
frequency
6. There are lines that are different
7. Attract
8. Attraction, stonger
9. Gain
10.Lose
11. Absorbed to travel farther from
the nucleus
12a. Picture B
12b. Releases
12c. Higher,
lower
12d. Released
13.
2/x
2/x
14a. n = 6 to n = 2
14b. The greater change in distance
means the greater change in energy.
15. It only has 1 electron
16. Many, many H atoms each with their
electrons making different transitions.
17a. n = 7, 6, 5, 4, 3, or 2 to n=1
17b. n = 7, 6, 5, or 4 to n = 3
18a. Li and Na are not present
18b. H and He are present
19. Emission and absorption spectrum
would have lines at the same energies
(wavelengths) but one is emitted lines
(bright lines of color) and one absorbed
lines (lines of black within the rainbow)
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Periodic Trends
1a. The first number
1b. pm
1c. The size of the atom (from center of
nucleus to valence energy level)
2. Atomic radius increases
3. The atomic radius increases as the
number of energy levels increases
4. Atomic radius decreases
5. The effective nuclear charge increases
and pulls the electrons closer
6a. It takes energy to pull apart attracted
particles
6b. Tight = more energy
2/x
7. Ionization energy decreases
8. The farther distance between the
nucleus and the electrons means less
energy needed to remove the electron.
9. Ionization energy increases
10. The greater effective nuclear charge
requires more energy to remove
electrons
11. Metals should have low ionization
energy, so the electrons are easy to move
allowing for high conductivity, malleability,
and ductillity.
12. Diagram B
2/x
13a. Electronegativity decreases
13b. The increased distance means the
nucleus of one atom is farther from
the electrons of the other atom, so it
has a weaker attraction.
13c. It increases
13d. The greater effective nuclear charge
allows the nucleus to pull with
greater attraction.
14. (on the left)= Electronegativity and I.E.
(on the right)= atomic radius
2/x
15a. Skip
(IE of O is less than N)
15b. Skip
(Oxygen’s last electron is in an orbital
already containing an electron, so the
increase of electron-electron
repulsion between the electrons
make it easier to remove, even with
more effective nuclear charge)
16. Ba, Fe, Br