Question

1. (7) in your textbook, there is an equation for determining the wavelength or frequency of light. what is that formula, what does each variable stand for, and what unit must they be measured in?
2. (7) in your textbook there is an equation for determining the energy of light. what is that formula, what does each variable stand for, and what unit must they be measured in?

color | red | red orange | orange | orange yellow | yellow | yellow green | green | green blue | blue | blue violet | violet
wavelength (nm) | 701 | 622 | 609 | 597 | 587 | 577 | 535 | 492 | 474 | 455 | 423

1. based on the color observed, use the table above to fill in the wavelength into the data table.
2. (3) using the table above, you must convert the wavelength in nanometers into the same wavelength measured in meters. show one of your conversions in the space to the right, then use the same conversion factor to fill in the column for wavelength in the data table.
3. (3) using the equation for determining the wavelength or frequency of light, show one of your calculations of frequency to the right, then use the same calculation to fill in the column for frequency in the data table.
4. (3) using the equation for determining the energy of light, show one of your calculations of frequency to the right, then use the same calculation to fill in the column for energy in the data table.

data table

	independent variable	dependent variable	wavelength (nm)	wavelength (m)	frequency (hz)	energy (j)
copper (ii) chloride
lithium chloride
potassium chloride
sodium chloride
strontium chloride
unknown

Explanation:

Step1: Recall wavelength - frequency formula

The formula is $c = \lambda
u$, where $c$ is the speed of light ($c = 3\times10^{8}\ m/s$), $\lambda$ is the wavelength (in meters), and $
u$ is the frequency (in hertz, Hz).

Step2: Recall energy - frequency formula

The formula is $E=h
u$, where $E$ is the energy (in joules, J), $h$ is Planck's constant ($h = 6.63\times10^{- 34}\ J\cdot s$), and $
u$ is the frequency (in Hz).

Step3: Convert wavelength from nm to m

For example, if $\lambda = 701\ nm$, since $1\ nm=1\times10^{-9}\ m$, then $\lambda = 701\times10^{-9}\ m = 7.01\times10^{-7}\ m$.

Step4: Calculate frequency

Using $c = \lambda
u$, we can solve for $
u$: $
u=\frac{c}{\lambda}$. For $\lambda = 7.01\times10^{-7}\ m$, $
u=\frac{3\times10^{8}\ m/s}{7.01\times10^{-7}\ m}\approx4.28\times10^{14}\ Hz$.

Step5: Calculate energy

Using $E = h
u$, for $
u = 4.28\times10^{14}\ Hz$, $E=(6.63\times10^{-34}\ J\cdot s)\times(4.28\times10^{14}\ Hz)\approx2.84\times10^{-19}\ J$.

Answer:

For the conversion of wavelength from nm to m, use the conversion factor $1\ nm = 1\times10^{-9}\ m$. For frequency calculation use $
u=\frac{c}{\lambda}$ with $c = 3\times10^{8}\ m/s$. For energy calculation use $E = h
u$ with $h=6.63\times10^{-34}\ J\cdot s$. The values for each compound in the data - table can be filled by repeating these calculations for the given wavelengths.