I must have all parts of the question answered***!!! Question 1 Chemistry Manual

Question

I must have all parts of the question answered***!!!

Question 1 Chemistry Manual:

c ) Why do He and H produce different line spectra? Is the same fundamental process is responsible for emission of photons in both emissions?
d) When observing the various metal salts, you probably noticed that any red bands always appear at approximately the same scale reading. The same is true for other colors too. Why?
e) Can a flame that appears to be a single color be made up of more than one wavelength of emission? Give an example from your experiment

Explanation / Answer

c. Answer-

The energy levels in atoms and ions are the key to the production and detection of light.The kinds of light that interact with atoms indicate the energy differences between shells and energy levels in the quantum theory model of the atom. Typically the valence electrons are the ones involved in these jumps.

Atoms have two kinds of states; a ground state and an excited state. The ground state is the state in which the electrons in the atom are in their lowest energy levels possible (atoms naturally are in the ground state). This means the electrons have the lowest possible values for "n" the principal quantum number.

Specific quantized amounts of energy are needed to excite an electron in an atom and produce an excited state. Energy can be added to atoms many different ways. It can be in the form of light, an electric discharge or heat. This added or extra energy is emitted when the excited electrons in the atoms give off light and fall back to lower shells. The light emitted has wavelengths and colors that depend on the amount of energy originally absorbed by the atoms. Usually each individual excited atom will emit one type of light. Since we have billions and billions of atoms we get billions of excitations and emissions.

Not all atoms in a sample will absorb or be excited exactly the same. For example in hydrogen the ground state has the electron in the n= 1 shell. The electron in some hydrogen atoms may be excited into the n = 2 level. Other hydrogen atoms can have the electron excited into the n = 4 shell.

Different elements emit different emission spectra when they are excited because each type of element has a unique energy shell or energy level system. Each element has a different set of emission colors because they have different energy level spacings. The same fundamental process is responsible for emmision of photon in both the emissions.

d. Answer-

When a metal salt solution is sprayed onto the flame the electrons in the metal are excited and jump from one electron shell level to the next highest shell level. They are said to be excited. They cannot remain there so as they return to the original shell, known as the grounded state the energy gained is lost in the form of light known as emission.

The colour of the light depends upon the metal (lithium(I) gives a magenta red-pink flame, calcium an orange red flame, potassium a lilac flame, strontium a crimson red flame, copper(II) gives a blue or green flame and sodium(I) gives a yellow flame). These colours are also often used in fireworks to give the different colours we see when they burn. Sodium is also used in some street lights and that is why they appear yellow when on.

If the flame is looked at through a spectroscope it will give a characteristic spectrum. This is used in chemistry to analyse a material for type and concentration of atoms.When observing the various metal salts, you probably noticed that any red bands always appear at approximately the same scale reading.The same is true for others too.

e. Answer

A flame appears to be single color can be made up of more than one wavelength of emission.

The energy levels in atoms and ions are the key to the production and detection of light.The kinds of light that interact with atoms indicate the energy differences between shells and energy levels in the quantum theory model of the atom. Typically the valence electrons are the ones involved in these jumps.

Atoms have two kinds of states; a ground state and an excited state. The ground state is the state in which the electrons in the atom are in their lowest energy levels possible (atoms naturally are in the ground state). This means the electrons have the lowest possible values for "n" the principal quantum number.

Specific quantized amounts of energy are needed to excite an electron in an atom and produce an excited state. Energy can be added to atoms many different ways. It can be in the form of light, an electric discharge or heat. This added or extra energy is emitted when the excited electrons in the atoms give off light and fall back to lower shells. The light emitted has wavelengths and colors that depend on the amount of energy originally absorbed by the atoms. Usually each individual excited atom will emit one type of light. Since we have billions and billions of atoms we get billions of excitations and emissions.

Not all atoms in a sample will absorb or be excited exactly the same. For example in hydrogen the ground state has the electron in the n= 1 shell. The electron in some hydrogen atoms may be excited into the n = 2 level. Other hydrogen atoms can have the electron excited into the n = 4 shell.

Different elements emit different emission spectra when they are excited because each type of element has a unique energy shell or energy level system. Each element has a different set of emission colors because they have different energy level spacings. The same fundamental process is responsible for emmision of photon in both the emissions.

d. Answer-

When a metal salt solution is sprayed onto the flame the electrons in the metal are excited and jump from one electron shell level to the next highest shell level. They are said to be excited. They cannot remain there so as they return to the original shell, known as the grounded state the energy gained is lost in the form of light known as emission.

The colour of the light depends upon the metal (lithium(I) gives a magenta red-pink flame, calcium an orange red flame, potassium a lilac flame, strontium a crimson red flame, copper(II) gives a blue or green flame and sodium(I) gives a yellow flame). These colours are also often used in fireworks to give the different colours we see when they burn. Sodium is also used in some street lights and that is why they appear yellow when on.

If the flame is looked at through a spectroscope it will give a characteristic spectrum. This is used in chemistry to analyse a material for type and concentration of atoms.When observing the various metal salts, you probably noticed that any red bands always appear at approximately the same scale reading.The same is true for others too.

e. Answer

A flame appears to be single color can be made up of more than one wavelength of emission.

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