Flame test lab and Part 1 notes chem

List the colors observed in the lab from highest energy to lowest energy

Potassium, copper, sodium, Barium, Calcium, Lithium, Strontium

List the colors observed in the lab from the highest frequency to the lowest frequency

Potassium, copper, sodium, Barium, Calcium, Lithium, Strontium

List the colors observed in this lab from the shortest wavelength to the longest wavelength

Potassium, copper, sodium, Barium, Calcium, Lithium, Strontium

EM waves move at speed of light:

3.00 x 10^8 m/s

Plank's constant

6.626 x 10^-34

What particles are found in chemicals that may be responsible for the production of colored light?

The particles responsible for giving off colored light would be the electrons because the excitement caused by heating makes the electrons jump from ground state into a high energy level.

Why do different chemicals emit different colors of light?

When an electron drops from one level to a lower energy level, it emits a quantum of energy. The wavelength (color) of the light depends on the difference in the two energy levels. Every element has its own characteristic set of energy levels. The specific build of an element causes it to reflect a particular wavelength of light, each element has a "fingerprint" in terms of its line emission spectrum.

calcium color

bright orange

strontium color

bright red/ orange

The speed of light is a _____________. So v and (upside down) y are also constants, therefore they must be ____________ _______________

constant, inversely proportional

Line Spectrums: _____________________________________ the lowest energy state of an atom. _____________________________________ a state in which an atom has a higher potential energy than in its ground state. Think neon lights.

ground state excited state

speed of light equation

C=λv, where λ is the wavelength of a photon, v is the frequency of a photon, and C=3.00*10^8

barium color

light orange

Wavelength (upside down y)

the distance between corresponding points on adjacent waves measured in m/nm

Types of EM Radiation

visible light, x-rays, ultraviolet lights, infrared light, radio waves

Spectroscope

An instrument that separates light into a spectrum.

Unknown 2

Barium

Explain the relationship between energy, frequency, and wavelength using the Electromagnetic Spectrum?

Energy and frequency are directly proportional meaning as energy increases, so does frequency Frequency and wavelength are inversely proportional, meaning as one increases the other decreases and vice versa

Colorful light emissions applicable to everyday life.

Fireworks emit light when a fire, such as the fuse, excites the different electrons in different metals. These light emissions are related because they both have to do with when an element's electrons become excited. Neon lights emit colorful light when gas is touched by the heat and light bulbs, because in the light bulb the wire heats up the gases in the inside, which excites the electrons that produce thelight,

How are electrons "excited" in this part of the experiment? What does it mean when the electrons are excited?

In this part of the experiment, electrons are "excited" by absorbing the heat from the Bunsen burner flame, which allowed them to go to a higher energy level. When electrons are "excited," it means that they have absorbed energy— by being heated to high temperatures— and sometimes absorb enough that it allows them to jump to higher energy levels.

Unknown 1

Sodium

Are these light emission related to the concepts covered in this lab?

The light emissions are related to the concepts covered in this lab by showing how a type ofheat or energy can cause for types of light or colorful light emissions.

Energy of a photon is ____________________________________________________ to the frequency of radiation.

directly proportional

E=hv=hc/λ

energy equation

why do you think the chemicals have to be heated in the flame before the colored light is emitted?

Light carries away energy. At room temperature atoms sit in their lowest-energy state most of the time, so they don't have any energy to give to light. When they're heated, the atoms spend some time in higher energy states, from which they can emit light while falling back down to the low-energy states. The chemicals have to be heated first because the electrons need to obtain the energy given off by the heat.

Incoming EM radiation striking the metal ejects _____________.

electrons

Electrons are ________ from a metal when light shines on the metal

emitted

Energies of atoms are _________________________________________ quantities. Energy transitions occur in jumps of _________________________________________of energy. Electrons only ______________ energy when move to a ________________energy state. Shortcoming of Bohr model is that is does not work for atoms larger than _________________________ and it does not explain chemical behavior.

fixed and definite discrete amounts lose, lower hydrogen

Electromagnetic Radiation

forms of energy which move through space as waves

When a specific or quantized amount of energy is exposed to the atom, the electron jumps from its _____________________ or original state to and _____________________________ state.

ground, excited

Bohr Model - electrons circle around the nucleus on their energy level. Electrons can circle the nucleus only in allowed paths or ______________________. The energy of the electron is ____________________when it is in orbits ________________________ from the nucleus. The atom achieves the ground state when atoms occupy the _____________________ possible positions around the nucleus. _______________________________________ is emitted when electrons move closer to the nucleus.

orbits greater, farther closest EM Radiation

A ______________________________ is a particle of energy having a rest mass of zero and carrying a quantum of energy.

photon

Radiant energy is transferred in units (called quanta) of energy called?

photons

potassium color

pink/purple

A _________________________________ is the minimum of energy that can be lost or gained by an atom.

quantum

Lithium color

red, dark pink

When the excited electron returns to the lower a lower energy levels, it __________________________ energy in the form of ________________________.

releases, light (emission spectrum)

bright line emission spectrum

the light emitted by an element when its electrons return to the lower energy level, light is given off in definite wavelengths

Frequency (V)

the number of complete wavelengths that pass a point in one second measured in s^-1, hertz (Hz), or 1/s

Energy travels through space as ______________________ but can be through of as a stream of particles. Each particle has 1 quantum of energy.

waves

Sodium color

yellow orange