hollywood high school school for advanced studies ap chemistry mr. brombach
TRANSCRIPT
![Page 1: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/1.jpg)
Hollywood High School
School for Advanced Studies
AP Chemistry
Mr. Brombach
![Page 2: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/2.jpg)
Unit I
Structure of an Atom
![Page 3: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/3.jpg)
Unit I. Schedule____________________________________________________
Lesson 1.1. Introduction
Lesson 1.2. Composition of an Atom. Isotopes
Lesson 1.3. The Nature of Light. Electromagnetic Spectrum
Lesson 1.4. Bohr’s Model of an Atom. Wave- Particle Nature of an Electron
Lesson 1.5. Orbitals. Quantum Numbers.
Lesson 1.6. Practice Quantum Numbers
Lesson 1.7. Unit Review
Lesson 1.8. Test # 1
![Page 4: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/4.jpg)
Lesson 1.1. Introduction ____________________________________________________________________________________
• Go to Hollywood HS website
• Open Mr. Brombach’s web log:• Go to AP-Chemistry• Find the following:
– Syllabus– Unit schedule– HW assignments– Handouts– Lecture notes– Lab Assignments
![Page 5: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/5.jpg)
HW Format____________________________________________
Name_____________________Period____ Date_________ #_____
HW 1.1.# 2.42, p.80
Question………………………………………………………
Answer………………………………………………………..
_______________________________________________
# 2.46, p.80
Question………………………………………………………
Answer……………………………………………………….. _____________________________________________
![Page 6: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/6.jpg)
Lesson 1.2. Composition of an Atom. Isotopes
_____________________________________________________________________________________________
Microworld Atoms Molecules
Elements Compounds
Macroworld Pure Substances Mixtures
Matter
![Page 7: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/7.jpg)
Lesson 1.2. Composition of an Atom. Isotopes
_____________________________________________________________________________________________
• Physical and chemical properties of a substance depend on its chemical structure
• That includes the arrangement of the atoms in a molecule and types of bonding between them
![Page 8: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/8.jpg)
Lesson 1.2. Composition of an Atom _____________________________________________________________________________________________
• Each atom is represented by the notation
mass number A
X symbol atomic number Z
• Atomic number (Z) equals the number of protons in the nucleus
Z = # p+
![Page 9: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/9.jpg)
Lesson 1.2. Composition of an Atom_____________________________________________________________________________________________
• An atom is neutral (the number of protons equals the number of electrons)
# p+ = # e-
• Mass number (A) is the total number of protons and neutrons
A = # p+ + # no
• Number on neutrons can be found from the formula:
# no = A - Z
![Page 10: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/10.jpg)
Lesson 1.2. Composition of an Atom_____________________________________________________________________________________________
• Since the mass of an atom is so small, to measure atomic mass we use a group called “Dalton (D)” (the old name amu)
1 D = 1.66 x 10-24 g• Atomic mass in the Periodic Table is done in
Daltons• For example, the mass of carbon atom
12
C is exactly mc = 12 D 6
or (12)(1.66 x 10-24 g) = 1.99 x 10-23 g
![Page 11: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/11.jpg)
Lesson 1.2. Isotopes _________________________________________________________________________________
• Not all atoms of a particular element have the same mass
• The difference in their mass number (A) is due to the presence of different number of neutrons (no)
• For ex.: There are two types of Boron (B) atom:– 10B or Boron – 10 (5 p+ + 5 no)– 11B or Boron – 11 (5 p+ + 6 no)
![Page 12: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/12.jpg)
Lesson 1.2. Isotopes _________________________________________________________________________________
• Isotopes of an element are atoms that have different number of neutrons and, therefore, different mass numbers
• An element occurs as a mixture of isotopes
• The atomic mass of an element is the average of its isotopic masses according to their natural abundances
![Page 13: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/13.jpg)
Lesson 1.2. Isotopes _________________________________________________________________________________
Isotopic form
Mass (D) Abundance,%
Fraction
24Mg 23.9850 78.99 0.7899
25Mg 24.9858 10.00 0.1000
26Mg 25.9826 11.01 0.1101
![Page 14: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/14.jpg)
Lesson 1.2. Isotopes _________________________________________________________________________________
• Find average atomic mass of Mg
• Atomic mass portion:24Mg = 23.9850 x 0.7899 = 18.945825Mg = 24.9858 x 0.1000 = 2.498626Mg = 25.9826 x 0.1101 = 2.8607
24.3024 D
![Page 15: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/15.jpg)
Lesson 1.3. Nature of Light _________________________________________________________________________________
• How do we know about atoms, as we cannot see them?
• To learn about atomic structure, scientists treat matter with different kind of energy (heat, electricity, ionization, magnetic field…)
Energy An Element EMR• As a result, the matter gives away electromagnetic
radiation (EMR)• By studying EMR, the scientists are able to
develop models of the atom
![Page 16: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/16.jpg)
Lesson 1.3. Nature of Light _________________________________________________________________________________
• EMR (light) travels as a wave• It is described by two independent variables:
wavelength and frequency• Wavelength (λ – lambda) is the distance (nm)
the wave travels during one cycle
• Frequency (√ - nu) is the number of cycles the wave undergoes per second (1/s or Hz)
• Speed of light in vacuum is constant and equals 3.00 x 108 m/s
![Page 17: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/17.jpg)
Lesson 1.3. Nature of Light _______________________________________________________________________
400 nm 750 nm
![Page 18: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/18.jpg)
Lesson 1.3. Nature of Light _______________________________________________________________________
• The wavelength is inversely proportional to the frequency
C λ = ----- (1) √
C – speed of light, m/s
λ – wavelength, nm
√ - frequency, 1/s or Hz
![Page 19: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/19.jpg)
Lesson 1.3. Nature of Light _______________________________________________________________________
• At the beginning of 20th century, the three phenomena involving matter and light could not be explained based on the wave nature of light:– The pattern of intensity and wavelength of light
emitted from hot, dense objects (blackbody radiation)
– The electric current generated when light shines on a metal plate (photoelectric effect)
– The individual colors emitted from electrically (or
thermally) excited gases (atomic spectra)
![Page 20: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/20.jpg)
Lesson 1.3. Nature of Light _______________________________________________________________________
• Explaining these phenomena required a radically new view of energy (light):– Plank’s quantum hypothesis (1900)
• A beam of light is not a continuous stream of energy; instead the beam consists of zillions of small, discrete packets of energy, each called quantum
– Einstein’s particulate nature of light (1905)• The quanta of light behave much like tiny particles of
matter, each quantum of light was called a photon
![Page 21: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/21.jpg)
Lesson 1.3. Nature of Light _______________________________________________________________________
• Thus, the light has properties of both, a wave and a particle
• To represent this duality, the photon is illustrated as a burst of light with a wave drawn inside the burst
• The scientists are free to choose which of these two modes fits their needs the best
![Page 22: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/22.jpg)
Lesson 1.3. Nature of Light _______________________________________________________________________
• The energy carried by the wave is directly proportional to the frequency
E = h√ (2)
E – energy, J
h – Plank’s constant (6.626 x 10-34 J•s)√ - frequency, 1/s or Hz
• The most powerful type of EMR are gamma rays that have the highest frequency
2.756 x 1022.756 x 102
![Page 23: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/23.jpg)
Lesson 1.4. Bohr’s Model of an Atom_______________________________________________________________________
Energy is absorbed Energy is released
•
ground state excited
state • Ground state or stationary state is the most stable (the
lowest level of energy)• To move to the higher level an object absorbs energy
and turns to excited state (less stable)• To go back to stable state, the object gives away (emits)
energy
•
![Page 24: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/24.jpg)
Lesson 1.4. Bohr’s Model of an Atom _______________________________________________________________________
• Accepting Plank’s and Einstein’s idea about quantized energy, Bohr proposed that the hydrogen atom had only certain energy levels
• If gaseous hydrogen is turned from ground state to excited state by electric discharge, it goes back to ground state by emitting EMR
![Page 25: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/25.jpg)
Lesson 1.4. Bohr’s Model of an Atom _______________________________________________________________________
See p.264 fig. 7.9
![Page 26: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/26.jpg)
Lesson 1.4. Bohr’s Model of an Atom _____________________________________________________
![Page 27: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/27.jpg)
Lesson 1.4. Atomic Spectra _______________________________________________________________________
• As emitted EMR passes through a slit and a prism, the EMR will be divided into individual wavelength
• The EMR does not create a continuous spectrum, or rainbow, as sunlight does
• Rather, it produces a line spectrum – a series of fine lines of individual colors separated by colorless spaces
![Page 28: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/28.jpg)
Lesson 1.4. Atomic Spectra___________________________________________________________
• The pattern of wavelength (frequencies) formed by a given element is referred to as element’s atomic spectrum• The wavelength at which the colored lines occur is individual characteristic of the element, its “fingerprint” that allows to identify an element
![Page 29: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/29.jpg)
Lesson 1.4. Atomic Spectra _______________________________________________________________________
• To find the position and wavelength of any line in a given series, use the Rydberg equation
1 1 1 ------ = R (------ - ------) (3) λ n1
2 n22
λ – wavelength of a particular spectral line
n1, n2 – integers representing energy levels (n2 >n1)
R – Rydberg constant = 1.097 x 107 1/m
![Page 30: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/30.jpg)
Lesson 1.3. Bohr’s Model of an Atom_______________________________________________________________________
Lesson 1.4. Bohr’s Model of an Atom______________________________________
∆
In an atom, an electron can move from one energy level to another only by absorbing or emitting a photon of energy
![Page 31: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/31.jpg)
Lesson 1.4. Bohr’s Model of an Atom _______________________________________________________________________
• The amount of energy an atom emits is the difference between energy of final and initial state
∆ Ephoton = Efin – Ein = = Eexcited state – Eground state (4)
• The greater the energy level, the greater the energy n E
• The energy of any excited state equals:
E = -2.18 x 10-18(1/n2), J (5)• The energy emitted of absorbed by H atom
∆ E = -2.18 x 10-18(1/nfin2 – 1/nin
2) (6)
![Page 32: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/32.jpg)
Lesson 1.5. The Wave-particle Nature of an Electron
_______________________________________________________________________
• Does photon have a mass?• The famous Einstein’s equation states the
relationship between energy and mass
E = mc2 (7)
E – energy, J
m – mass, g
c – speed of light, m/s
![Page 33: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/33.jpg)
Lesson 1.5. The Wave-particle Nature of an Electron
_______________________________________________________________________
• As light exists as a wave and as a particle, each model has the equation of energy:
E = mc2 (mass represents a particle)
E = h√ (frequency represents a wave)
mc2 = h√ √ = c/λ mc2 = hc/λ
h m = ----- (8)
λcm – mass of photon (EMR or particle)
![Page 34: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/34.jpg)
Lesson 1.5. The Wave-particle Nature of an Electron
_______________________________________________________________________
• De Broglie proposed the equation, which connects wave and particle properties of any object such as planet, baseball, or electron
h λ = ----- (9)
m v v – velocity (speed), m/s
• Since electron moves with a speed close to the speed of light, it also exists as a wave and as a particle (duality)
![Page 35: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/35.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________________
• If an electron has the properties of both a particle and a wave, what can we determine about its position in the atom?
• The Heisenberg’s Uncertainty Principle states that it is impossible to know simultaneously the exact position and velocity of a particle
• That means that we cannot prescribe exact paths
for electrons, such as the circular orbits of Bohr’s model
![Page 36: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/36.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________________
• The wave motion of objects on the atomic scale is examined in the field of quantum mechanics
• In 1926, Schrodinger formulated an equation from which the probability of finding the electron in hydrogen atom could be determined
• If we could plot the positions of an electron of a given energy over time as a series of tiny dots, the resulting pattern would resemble what is called a probability cloud
![Page 37: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/37.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________________
• The electron density diagram represents the probability of finding the electron at a particular point at a given distance r along a line from the nucleus outward
• The probability of the electron being far from the nucleus is very small, but not zero
• An atomic orbital, like a probability cloud, specifies a volume of space where the electron is most likely to be found
![Page 38: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/38.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________________
![Page 39: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/39.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________
S-orbital
(1)
![Page 40: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/40.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________
p-orbital
(3)
![Page 41: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/41.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________
d-orbital
(5)
![Page 42: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/42.jpg)
Lesson 1.5. The Atomic Orbital _______________________________________________________________
f-orbital
(7)
![Page 43: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/43.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
• Each orbital can be described by a set of characteristics called quantum numbers (QN): n – principal QN (characterizes energy
level and size of the orbital) l – azimuthal QN (energy sublevel and
shape)
ml – magnetic QN (orientation in space)
![Page 44: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/44.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
Values Principal QN
n = 1, 2, 3, 4, 5 …The greater the “n” value,
the higher energy level
and the bigger the orbital
12
34
5
![Page 45: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/45.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
Values
Azimuthal QN: “l” = 0, 1, 2, 3, 4…. n-1• “l” represents:
– Energy sublevels: l = 0(s); l = 1(p); l = 2(d); l = 3(f)
– Shape of the orbital: s – sphere; p – double-lobe
d and f – shape varies
Energy levels
pd
f
sublevels
![Page 46: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/46.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
Values
Magnetic QN: “ml” = -l…0…+l
“ml”represents the orientation of the orbital in space:
l = 0 ml = 0 (only 1 orientation)
l = 1 ml = -1, 0, +1 (3 orientations x, y, z)
l = 2 ml = -2, -1, 0, +1, +2 (5 orientations)
l = 3 ml = -3, -2, -1, 0, +1, +2, +3 (7 orientations)
![Page 47: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/47.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
-On a particular energy level, there are:• 1 s-orbital
• 3 p-orbitals
• 5 d-orbitals
• 7 f-orbitals
![Page 48: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/48.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
![Page 49: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/49.jpg)
Lesson 1.5.a. The Atomic Orbital _______________________________________________________________
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
2pxnll
ml
![Page 50: Hollywood High School School for Advanced Studies AP Chemistry Mr. Brombach](https://reader035.vdocuments.us/reader035/viewer/2022062805/5697bff61a28abf838cbdfe0/html5/thumbnails/50.jpg)
Lesson 1.6. Quantum Numbers_________________________________________________________________________________________
• The total number of orbitals on a particular energy level equals: # orbitals = n2
n = 3
n = 2
n = 1
32 = 9 orbitals
22 = 4 orbitals
12 = 1 orbital
n = 4
1s
2s2p
3s
4s
3p
4p
3d
4d 4f
42 = 16 orbitals