Chapter 2 (pt 2)

Question 1

schrodinger equation

Answer 1

• different for every element due to different # in protons
• relates to energy
• Equation=E=-2.18x10^-18(1/n^2) where n=principle quantum number and is the shell #
• used when describing an energy relationship of e- as a result from the equation above

Question 2

electrons closest to the nucleus have the ____ coulombic attraction

Answer 2

greatest

Question 3

energy levels of electrons

Answer 3

-the energy increases (gets more positive) with shells while the coulombic attaraction decreases (n=1,2,3,4,…)

Question 4

color and electronic transition

Answer 4

consists of an electron getting excited (excitation) and then relaxing (relaxation) resulting in a photon. When the electron relaxes and creates a photon is when the color appears.

Question 5

excitation

Answer 5

electron goes from lower energy n-level to a higher energy n-level

Question 6

relaxation

Answer 6

electron goes from higher energy n-level to a lower energy n-level

Question 7

atoms like to be at the ____energy possible

Answer 7

lowest

Question 8

exothermic

Answer 8

when energy is flowing out of something, it is negative

Question 9

endothermic

Answer 9

when energy is flowing into somehting, it is positive

Question 10

quantum numbers

Answer 10

describe an e-‘s emergy, shape of orbit, probability of being found, and spin

Question 11

n

Answer 11

n=the principle quantum number (energy)

Question 12

l

Answer 12

• angular momentum quantum number (shape of orbit)
• describes how the orbits are distributed/what they look like
• has a range of values from 0 to n-1

Question 13

l=0

Answer 13

s-orbital (sphere shaped)

Question 14

l=1

Answer 14

p-orbital (dumbell shape)

Question 15

l=2

Answer 15

d-orbital (clover leaf shape)

Question 16

l=3

Answer 16

f-orbital (complex)

Question 17

ml

Answer 17

magnetic quantum number (how many of each orbital you actually have)

• a range of values from -l to 0 to +l (-1 0 +1)
• depending on the magnetic field there are different orientations of l that result

Question 18

when l=0 ml=?

Answer 18

ml=0

• 1 orbital ever in a l=0 or s-orbital
• means there is only ever one s-orbital per principle quantum level

Question 19

when l=1 ml=?

Answer 19

ml=-1, 0, +1
-3 orbitals ever in a l=1 or p-orbital set
means that there is always three p-orbitals per principle quantum level

Question 20

when l=2 ml=?

Answer 20

ml=-2, -1, 0, +1, +2
-5 orbitals ever in a l=2 or d-orbital set
means there are always 5 d-orbitals per principle quantum level

Question 21

when l=3 ml=?

Answer 21

ml=-3, -2, -1, 0, +1, +2, +3

• 7-orbitals for l=3 or f-orbital set
• means there are always seven f-orbitals per principle quantum level