Kinetics

Today, we started the 3rd unit which is "CHEMICAL KINETICS". Ms. K explained the important terms through pages 3-9. She also did a lab experiment which a Magnesium ribbon was individually dropped to 3 test tubes each containing 1M of HCL, 6M of HCL and 12M of HCL. When a Mg ribbon was dropped into 1M of HCL, it took 4 mins for it to dissolve completely. In 6M and 12M of HCl, it took 7 secs for it to dissolve. After the lab experiment, we were assigned to do page 10 questions 1-4.

Have a nice SPRING BREAK!!!!!!!!

The next scribe will be jen2x

march 23 - Anna B's scribe

for today’s class, we just corrected the answers from yesterday and answered some of the questions from the booklet

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.