Chapter 5: Lessons 1,2

What is the increasing order of energy based on its colors?

"ROY G. BIV" is an acronym for the colors of the rainbow: red, orange, yellow, green, blue, indigo, and violet.

True or false _________ ________ shows electrons don't move around the nucleus in orbit, but in clouds where their position is uncertain.

True Erwin Schrodinger

True or false ________ _________ Recognized electrons as composed of atom

True J.J. Thompson

True or false ______ _________ recognized atoms of a particular element differ from other element.

True John Dalton

True or false _________ __________ proposed stable electron orbit, explained the emission spectra of some elements

True Niel Bohr

Which of the following is an example when an electron absorbs energy? When an electron releases a photon. When it goes from the second energy level to the fourth. When it goes from the fourth energy level to the first. When it maintains constant energy and doesn't change his energy level.

When it goes from the second energy level to the fourth.

That's what causes different colors of fireworks! For example, when copper is burned, it produces a ______-_______ flame.

bluish-greenish

Each element is going to have its own distinct _____ when its electrons are excited - or its own atomic spectrum.

color

A wavelength is just a numerical way of measuring the _______ of _______. Also, whenever a hydrogen electron dropped only from the third energy level to the second energy level, it gave off a very low-energy _________ light with a wavelength of 656.3 nanometers.

color of light red

The most important feature of this photon is that the ____________ the transition the electron makes to produce it, the __________ the energy the photon will have.

larger higher

The total number of electrons each group can have is determined by the ________

letter

quantum numbers

specify the properties of atomic orbitals and the properties of electrons in orbitals

angular momentum quantum number

symbolized by l, indicates the shape of the orbital

principal quantum number

symbolized by n, indicates the main energy level occupied by the electron

An orbital tells us

the approximate positions in which electrons surround the nucleus.

electron configuration

the arrangement of electrons in an atom

The numbers in superscript represent..... example 1s^2

the number of electrons in each orbital group. 1 is the coefficient s is the variable 2 is the number of electron in the orbital

atomic number

the number of protons in the nucleus of an atom

Atomic Spectrum

the spectrum of frequencies of electromagnetic radiation emitted or absorbed during transitions of electrons between energy levels within an atom.

True or false ________ _________ realized positive charge was localized in the nuclease of an atom

true Ernest rutherford

For example, whenever a hydrogen electron drops from the fifth energy level to the second energy level, it always gives off a ________ light with a wavelength of 434.1 nanometers.

violet

When sodium is burned, it produces a ______-______ flame. When magnesium is burned, it releases photons that are so high in energy that it goes higher than ______ and emits an ________ flame. You wouldn't want to look directly at that one!

yellowish-golden violet ultraviolet

A couple of ways that energy can be added to an electron is in the form of ______, in the case of fireworks, or ______, in the case of neon lights. When these forms of energy are added to ______, their electrons take that energy and use it to move out to _____ _____ _____ farther away from the nucleus.

...heat electricity atoms outer energy levels

As electrons transition from a high-energy orbital to a low-energy orbital, the difference in energy is released from the atom in the form of a ________.

...photon

We can find an orbital's shape if we know the value for l, which always starts at a value of _______ and goes to a maximum of __________.

0 n - 1.

List the oder of the people who created the model of an atom

1 Aristotle 2. Democritus 3. John Dalton 4. JJ. Thompson 5 Ernest Rutherford 6. Neil Bohr 7. Erwin Schrodinger

List the oder of the models of the atom

1 solid Sphere Model 2. Plum Pudding Model 3. Nuclear Model 4. Planetary Model 5. Quantum Model

s can have _____ electrons p can have ______ electrons d can have _____ electrons f can have ______ electrons

2 electrons 6 electrons 10 electrons 14 electrons

So, if this electron is now found in the ground state, can it be found in another state?

Absolutely. If this electron gets excited, it can move up to the second, third or even a higher energy level.

But what causes this electron to get excited?

Adding energy to an electron will cause it to get excited and move out to a higher energy level.

The Greek philosopher ________ believed that matter could be divided infinitely without changing its properties

Aristotle

Why did Democritus disagree with Aristotle? Democritus thought matter could be divided infinitely, but Aristotle thought there were tiny, indivisible particles. Aristotle thought matter could be divided infinitely, but Democritus thought there were tiny, indivisible particles. Aristotle thought all matter was made of atoms, but Democritus thought that only solids were made of atoms. Democritus thought all matter was made of atoms, but Aristotle thought that only solids were made of atoms.

Aristotle thought matter could be divided infinitely, but Democritus thought there were tiny, indivisible particles.

Why should you avoid looking directly at magnesium burning? Because despite the fact that there is no light, it can be damaging to your sight. Because of the high energy released and the ultraviolet flame present. Because there is no energy released, which can deplete the area of oxygen. Because of the low yellow burn that can be annoying to look at.

Because of the high energy released and the ultraviolet flame present.

Which of the following was the instrument used for the discovery of the electron? Cathode ray tube Plum pudding model Alpha particle emitter Oil drop apparatus Gold foil experiment

Cathode ray tube

The really awesome thing about ________ model of the atom is that he came up with it without ever seeing the atom! He had no concept of protons, neutrons or electrons. His model was created solely on experiments that were _______, or seen with the unaided eye.

Dalton's macroscopic

Who first coined the term atom, meaning indivisible? Dalton Rutherford Thomson Aristotle Democritus

Democritus

_____________ disagreed. He thought that matter could only be divided until you got to the smallest particle (which he called the ________, coming from the Greek word atomos, meaning ___________

Democritus atom indivisible

____________ _____________ comes in many forms: heat, light, ultraviolet light and x-rays are just a few.

Electromagnetic radiation

True or false ________ _________ Did not explain why electrons remain in oribit around the nucleus

Ernest Rutherford

_______ ________ , one of Thomson's students, did some tests on Thomson's plum pudding model. The members of his lab fired a beam of positively charged particles called ______ particles at a very thin sheet of _____ _______. (Later on you will learn that alpha particles are really just the nuclei of ________ atoms.)

Ernest Rutherford alpha gold foil helium

__________ ____________ stated that electrons do not move in set paths around the nucleus, but in waves. It is impossible to know the exact location of the electrons, instead, we have " cloud of probability called orbitals, which we are more likely to find an electron.

Erwin Schrodinger

True or false ________ _________ No nucleus, didn't explain later experimental observations

False J.J. Thompson

True or false ______ _______ stated atoms aren't indivisible- they're composed from subatomic particles

False John Dalton

True or false _______ _________ state moving electrons should emit energy and collapse into the nucleus, model did not work well for heaver atoms

False Neil Bohr

The principal quantum number tells us two things. First, it tells us the.... Second, it tells us the .....

First, it tells us the electron's energy level, which we often refer to as its shell. Second, it tells us the orbital's size.

________ atom only has one electron which is located in the 1s orbital.

Hydrogen

Draw the plum pudding model by ______ ________

J.J. Thomson

in the early 1800s, when _______ _______- came along and disproved ____________.

John Dalton Aristotle

_________ also stated that all atoms of the same _________ will be exactly the ______ and that atoms of different elements can combine to form ________.

John Dalton element same compund

Which scientist is credited with discovering the charge of individual electrons? Millikan Rutherford Dalton Democritus

Millikan

________ modified Rutherfords model of the atom by stating that electrons moved around the nucleus in orbit of fixed size and energies.

Neil Bohr

_________ ___________ also stated in his model that Electrons energy in this model was quantized (restrict the number of possible values); electrons could not occupy values of energy between the fixed energy levels.

Neil Bohr

In the early 1900s, a guy named _____ ______ was doing research on the atom and was picturing the Rutherford model of the atom, which - you may recall - depicts the atom as having a small, positively-charged nucleus in the center surrounded by a kind of randomly-situated group of electrons.

Niels Bohr

While ______ ________ was doing research on the structure of the atom, he discovered that as the hydrogen atoms were getting excited and then __________ energy, only three different colors of visible light were being emitted: ________, ________-________ and _______.

Niels Bohr releasing red, bluish-green violet

atomic mass

Number of protons and neutrons

_______ ________ discovers the charge of an electron. He did this using his famous _____ _____ _______,' where he sprayed charged oil drops between two metal plates

Robert Millikan 'oil drop experiment

After this experiment, _________ concluded that these alpha particles must have hit something very small, dense and positively charged in order for them to come straight back.

Rutherford

If the electrons were randomly situated, as he initially believed based upon the experiments of _________, then they would be able to absorb and release energy of random colors of light. His conclusion was that________ are not randomly situated. Instead, they are located in very specific locations that we now call _______ _________.

Rutherford electrons energy levels

_________ claimed that this also shows that the ________ consists mostly of empty ________ and that all the positive charge is not _______ spread throughout the atom but instead squished into a teeny tiny nucleus in the center of the atom.

Rutherford atom space evenly

How does the Bohr Model differ from the Rutherford model? Rutherford believed that each atom consisted only of protons and electrons, while Bohr identified that there were photons present as well. Rutherford assumed that the nucleus was negatively charged, while Bohr correctly identified that it was positively charged. Rutherford assumed that the nucleus did not have any charge at all, while Bohr correctly identified that it was negatively charged. Rutherford assumed that the position of electrons was random, while Bohr identified that they were located in very specific energy levels.

Rutherford assumed that the position of electrons was random, while Bohr identified that they were located in very specific energy levels.

Draw John Dalton's model of the Atom & name it

Solid Sphere Model

What did Rutherford discover in his gold foil experiment? Atoms are small and dense. Electrons are negative. Neutrons are located in the nucleus. The nucleus is positively charged, small, and dense.

The nucleus is positively charged, small, and dense.

_______ used the ______ ______ _____ with a magnet and discovered that the green beam it produced was made up of ________ charged material.

Thomson cathode ray tube negatively

A photon

a particle representing a quantum of light or a weightless particle of electromagnetic radiation.

This led to the Bohr model of the atom, in which ...

a small, positive nucleus is surrounded by electrons located in very specific energy levels.

electron shell

an energy level of electrons at a characteristic average distance from the nucleus of an atom

__________ _________ ___________ ___________ is the sub-shells of the electron energy level shells.

angular momentum quantum number

The more energy that is added to the _______ , the farther out the electron will go. In a later lesson, we'll discuss what happens to the electron if too much energy is added.

atom

From this he decided that these particles must have come from somewhere within the ____ and that _______ was incorrect in stating that _______ cannot be divided into smaller pieces.

atom Dalton atoms

When neon lights are energized with _________, each element will also produce a different color of light.

electricity

Now, let's fast-forward to the late 1800s when J.J. Thomson discovered the __________. Thomson used what was called a _____ ____ ________, or an electron gun.

electron cathode ray tube

These ________ are what let atoms work as building blocks for everything in the universe.

electrons

A neutral atom has the same number of _________ as it does _________.

electrons protons

Atoms are categorized into different types called ________.

elements

The color a substance emits when its electrons get excited can be used to help identify which _______ are present in a given sample. Scientists use these ______ _________ to determine which elements are burning on stars in the distant outer space.

elements atomic spectra

Essentially, each transition that this hydrogen electron makes will correspond to a different amount of ________ and a different_______ that is being released.

energy color

cathode ray tube

evacuated glass tube in which a stream of electrons emitted by a cathode strikes a fluorescent material, causing it to glow

This means hydrogens is in the ______ and ______ energy level, and because it is in an _____ orbital, it will be found in a region that is shaped like a ________ surrounding the nucleus.

first lowest s sphere

When writing electron configurations, electrons are represented in their lowest possible energy state, called their _____. ground state excited state configuration state lowest state

ground state

Here n = 1 is the lowest energy level of an electron, also known as the _______ _______. Then n = 2, n = 3, and so on are ______ _____ with higher energies.

ground state excited states

He performed many experiments and found that the mass of one of these particles was almost 2,000 times lighter than a _______ atom.

hydrogen

Principal quantum numbers are represented as _______ with a smallest possible value of______.

integers 1

Electromagnetic radiation

is the movement of energy- that travel through space and a medium- which is composed of electric and magnetic waves that oscillates @ right angle to each other and in the direction of the wave travel.

Because these alpha particles had so much _____, he fully expected that all of the alpha particles would go right through the gold foil. This is because, if _______ were correct about the _______ _________ model of the atom, the alpha particles would just go through the positively charged matter and hit the detecting screen on the other side.

mass Thomson plum pudding

M A E

mass number/ atomic mass atomic number element

Dalton went on to say that ....

matter is made up of tiny particles, called atoms, that cannot be divided into smaller pieces and cannot be destroyed

ground state

meaning that it has the lowest energy possible.

. Also, as n increases so does the ______ _________.

orbital's size

Thomson went one step further and determined that these negatively charged electrons needed something _______ to balance them out. So, he determined that they were surrounded by positively-charged material. This became known as the______ ______ model of the atom. The negatively charged ______ were surrounded by _____ ________ pudding.

positive 'plum pudding' plums positively charged

J.J. Thomson theorized that electrons were surrounded by a _____ _______ material

positively charged material.

The first quantum number is the _______ _________ ________- (______).

principal quantum number (n).

Each element is defined by the number of ______ in that atom.

protons

High-energy photons are going to look like higher-energy colors:_______, ________, _______ whereas lower-energy photons are going to be seen as lower-energy colors like ______,________,_______.

purple, blue and green, red, orange and yellow.

In fact, the term 'neon' light is just referring to the ______ lights. Blue lights are produced by electrified______, and orange lights are really produced by electrified _______.

red argon helium

When an electron moves from an excited state to a ground state, it will _____. absorb energy release energy maintain a constant energy absorb a photon

release energy

Let's look at the example of n = 3. This means l will consist of integers from 0 to n - 1. n - 1 = 3 -1 = 2 l = 0, 1, 2 Every value of l corresponds to a different orbital shape. Here we have l = 0 which corresponds to the ______ orbital shape, l = 1 corresponds to the______ orbital shape, and l = 2 the ____ orbital shape.

s p d