hand out answers:
using the periodic table:
1.
a. 8 or 0
b. 1
c. 3
d. 2
e. 6
f. 7
g. 5
h. 4
2.
a. 4
b.2
c. 7
d. 1
e. 3
f. 5
3.
a.[he]2s1
b.[he]2s22p5
c.[ar]4s23d104p3
d.[kr]5s2
e.[xe]6s25d106p3
4.
a. group 2A period 1 block S
b. group 3B period 3 block P
c. group 1A period 4 block S
d. group 3B period 4 block D
e. group 6A period 6 block P
Electrons In Atoms
Section 5.1 light and quantized energy
1. Energy
2. Wave
3. Light
4. Speed
5. Wave length
6. Amplitude
7. Frequency
8. Hertz
9. A and C
10. B
11. 2 waves/s or 2 hertz
12. C
13. B
14. D
15. B
16. F
17. T
18. T
19. T
20. F
21. F
22. T
Section 5.2 Quantum theory and the atom
1. Ground state
2. Frequencies
3. Lower
4. Higher
5. Electron
6. Energy levels
7. Atomic emission spectrum
8 and 9 doesn’t need to be answered
10. C
11. A
12. D
13. B
14. bohrs model treats electrons as particles traveling in specific circular orbits while the quantum mechanical model treats electrons as waves and doesn’t describe the path of an electron around the nucleus
15. do not
16. two
17. spherically shaped
18. n
19. electrons
20. three
21. 2s and 2p
22. nine
5.3 Electron configuration
1. electron configuration
2. lowest
3. stable
4. ground state electron configuration
5. aufbau principle
6. pauli exclusion principle
7. spins
8. hunds rule
Element | Atomic number | Orbitals | Electron configuration |
| 9. helium | 2 |
| 1s2 |
| 10. nitrogen | 7 |      | 1s22s22p3 |
| 11. neon | 10 |
| 1 |
12. atomic number :32 electrons :32
13. noble gas notation uses the bracketed symbol of the nearest preceding noble gas atom in the periodic table. Using noble gas notation allows you to represent the complete electron configuration of an atom with many electrons in a short hand form <
14. [Ar] 4s23d104p2
15. C
16. B
17. D
18. B
19. A
20. A
page 36 in the booklet
periodic trends assignment
1. O, C, Sn, Sr
Because there is a decrease in atomic radii as it moves from left to right across the periodic table and there is an increase in atomic radii as you move it moves down a group
2. Ar, Al, Cs ,Na
Because there is a decrease in ionization as it moves from left to right across the periodic table and there is an increase in ionization as it moves down a group
3. Mo, Te, I
Because Mo is a metal which is a good conductor of heat while Te and I are non metal
4. Additional orbitals between the nucleus and the outer electrons are occupied which causes the shielding of the outer electrons from the pull of the nucleus which increases the distance off sets the greater pull of the increased nuclear charge
Back page
3. largest: antimony smallest: nitrogen
4.
a. Fluorine
b. bromine
c. bromine
d. fluorine
5. group 6A period 3 block P
8. right, because non metals gain electrons
9. >1.7 ionic
< 1.7 covalent
10.
a. covalent
b. covalent
c. ionic
d. covalent
the next scriber is janine D.
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