1. 10 9 8 7 6 5 4 3 2 1
10/28 Flame Tests
Make a 2 column by 6 row table in your notebook
Label the Columns “Compound” and “Observations”
Light your bunsen burner
Dip the wooden splint in the liquid
Heat it in the flame
Record observations for all 5 compounds Na, Li, K, Sr, Cu
WRITE A HYPOTHESIS OR EXPLANATION.
Why do you think what you are observing is happening?

2. Electromagnetic Spectrum
Long wavelength
Low energy
Low frequency
Short wavelength
High energy
High frequency

3. Bohr’s Model of the Atom
nucleus contains positive protons and neutral (no charge) neutrons
e- circle the nucleus in orbits, like planets around the sun
energy levels are quantized meaning only certain orbits are allowed, the e- can’t be between
every atom has it’s own unique set of energy levels
Bohr
Model

4. The Quantum Model Quantum Model
electrons in orbitals = 3D volume of space where electrons are most likely to be found
electron “cloud” represents a 95% probability that the e- will be inside
Quantum
Model
e- are thought of as both waves and particles (weird right? That’s called wave-particle duality)
which means you can not know the exact position or speed of an e- (that’s called Heisenberg’s Uncertainty Principle)

5. Orbitals

6. Orbitals

7. Spectroscopy Lab Background
Background: The normal electron configuration or arrangement of atoms is known as the ___________ ________. This is the most _________ energy state and all e- are in the __________energy levels possible. When electrons absorb enough energy they can “jump” to higher energy levels and are said to be in the _________ ________. However, the excited state is _______________ and as electrons “relax” back down to lower energy levels the extra energy is ___________ or given back off as ____________ light.
ground
state
stable
lowest
excited
state
unstable
emitted
visible

8. Let’s look at the Hydrogen emission spectrum!
Spectroscopy Lab Background
Each element, depending on its own unique _______________ _________________ (or arrangement), will emit a different _________________ of colored light that our eyes interpret as a ___________ color. In order to actually see the individual colors we need to use a ____________________, which has a _________ that separates the different wavelengths of light.
Let’s look at the Hydrogen emission spectrum!
electron
configuration
combination
single
spectroscope
prism

9. Emission Spectrum of Hydrogen

10. Spectroscopy Lab Background
If we look at the _______________ _____________ of a single element we will see only certain unique bright lines. Looking at this pattern of colored lines is one of many similar analytical techniques chemists use to identify substances called ________________. Each colored line in an emission spectrum represents a specific or ________________ electron transition. electron transition corresponding to a particular energy difference.
emission
spectrum
spectroscopy
quantized

11. Only certain colors are emitted because the transitions are quantized
Electronic Transitions
Heat, electricity, or light provides energy to excite e-
UV, Visible Light, or Infrared emitted as e- drops back to lower energy levels
photon
Unstable excited e-
25
24
23 e- e- e-
n = 5
n = 4 e- e-
n = 3 e-
n = 2
Only certain colors are emitted because the transitions are quantized p+
n = 1

12. Spectroscopy Lab Background
If energy levels were not quantized, then theoretically electrons could make ______ transition. This would result in a full spectrum of visible color in the emission spectrum or in other words we would see __________ light emitted by any excited atom as it relaxes back to the ground state. However, experiments show that only certain colors are emitted. This is direct evidence that ______________ ____________ _________ exist and confirmed __________ model of the atom which has electrons in quantized _____________ around the nucleus.
any
white
quantized
energy
levels
Bohr’s
orbit

13. ESCHS RECYCLES IN THE CLASSROOM
EACH CLASSROOM SHOULD HAVE 3 BINS WITH SIGNS!
WE DEPEND ON YOU TO SORT YOUR RECYCLING

14. ESCHS RECYCLES AND COMPOSTSIN THE CAFETERIA
Metal, Glass, Plastic, Cartons
Landfill
Styrofoam, Plastic bags, Wrappers
Food Scraps & Paper
Milk & Juice container

15. e- e- e- e- n= 1 n=2 n=3 n=4 n= 1 n=2 n=3 n=4 Long wavelength
Low energy
Low frequency
Short wavelength
High energy
High frequency e- e- e- e-
n= 1 n=2 n=3 n=4
n= 1 n=2 n=3 n=4

17. Absorption vs. Emission Spectra

18. Absorption vs. Emission Spectra

19. Absorption vs. Emission Spectra

20. Stellar Spectra

21. Stellar Spectra – Which elements?

23. 700
650
600
550
500
450
400 H
700
650
600
550
500
450
400 He
700
650
600
550
500
450
400 Ne
700
650
600
550
500
450
400 Hg
700
650
600
550
500
450
400
Solar

25. Make three columns in your notebook10 9 8 7 6 5 4 3 2 1
10/31 Spectroscopy Lab Data
Make three columns in your notebook
Mercury Hg
Helium He
Neon Ne

26. accurate / inaccurate / fairly / somewhat / partially / mostly
Science Writing Style: Spectroscopy
matched
… the red line at 650 nm
observed
… the green line (486 nm)
… the 410 nm line (purple)
in a band from ___ to ___
… the 580 nm yellow line
in a pair / group / set of lines
shifted
near
accurate / inaccurate / fairly / somewhat / partially / mostly

27. accurate / inaccurate / fairly / somewhat / partially / mostly
Science Writing Style: Openers
The experimental results for the Helium emission spectrum were ________ compared to the accepted spectrum because ….
Compared to the known spectrum, the experimental results for the Helium emission lines were _________ because…
The experimental Helium spectrum results were ________ in comparison to the accepted emission values because…
accurate / inaccurate / fairly / somewhat / partially / mostly
matched
shifted
… the red line at 650 nm
observed
near
… the green line (486 nm)
… the 410 nm line (purple)
in a band from ___ to ___
… the 580 nm yellow line
in a pair / group / set of lines