Bohr discovered that atoms and molecules emit energy only in certain discrete quantities, or quanta.

It can be thought of as a vibrating disturbance by which energy is transmitted.

The speed of a wave only depends in the nature of the medium through which the wave is traveling (for example, air, water, or a vacuum) regarding whatever type of wave it has.

λ (lambda)

ν (nu)

It is the distance between identical points on successive waves.

It is the number of waves that pass through a particular point in one second.

It is the vertical distance from the midline of a wave to the peak or trough.

It is the emission and transmission of energy in the form of electromagnetic waves.

It is a phenomenon in which electrons are ejected from the surface of certain metals exposed to light of at least a certain minimum frequency, called the threshold frequency.

Light is a wave as shown by different experiments like the diffraction of light by a prism to yield the visible spectrum. However, the photoelectric effect experiment showed that light also behaves like a particle.

Neils Bohr, 1913, each line in the spectrum corresponds to a transition between orbits.

This can be used to differentiate one element from another.

Ground state means the lowest energy state. When the electrons absorb energy and jump to outer orbits, this state is called excited state.

No one can predict the exact path an electron will follow as it moves around the nucleus.

The position of a particle and its momentum cannot be simultaneously measure with arbitrarily high precision.

There is a region of space where electrons are most likely to be found.

Quantum Numbers are used to describe the probable location of electrons of atoms.

It is the region of probability where an electron could be found.

It is the distance from nucleus.

Aka shell.

It indicates the relative size and energy of atomic orbitals.

As n increases, orbital becomes larger and energy level increases.

It represents the energy level of the electron.

The smaller the value of n, the further away from the nucleus.

n = 1, 2, 3. . .

It is the shape of orbital.

It can have any value from 0 to n-1.

It contains the orbital and defines the orbital shape (s, p, d, f).

l = 0, 1, 2 . . . (n-1)

It is the orientation in space.

Has a ranged for +l to -l.

This quantum number distinguishes orbitals of given n and l—that is, of given energy and shape but having a different orientation in space.

Determines how many orbitals there are per energy level.

m_l= -l . . . l

It could have a value of anywhere from -l to l-l . . . l

It is the electron spin.

+½ or -½ 

Specifies the orientation of the spin axis of an electron.

An electron can spin in only one of four directions.

It is the representation of the arrangement of electrons distributed among the orbital shells and subshells. 

It is used to describe the orbitals of an atom in its ground state, but it can also be used to represent an atom that has ionized into a cation or anion by compensating with the loss or gain of electrons in their subsequent orbitals.

These, electrons in the outermost shell, are the determining factor for the unique chemistry of the element.

The s-block is the region of the alkali metals including helium (Groups 1 & 2), the d-block are the transition metals (Groups 3 to 12), the p-block (Links to an external site.) are the main group elements from Groups 13 to 18, and the f-block are the lanthanides and actinides series.

It is also known as the building up principle. 

It states that the electrons must first occupy the orbitals with lower energies than those with higher energies. 

The first two orbitals (1s and 2s) are each occupied first with two electrons.

It tells us that when electrons have more than one equivalent orbital available, they will half-fill each of the equivalent orbitals before filling the second half of each.

It states that every orbital in a sublevel is singly occupied before any orbital is doubly occupied. 

It says that all of the electrons in singly occupied orbitals have the same spin (to maximize total spin).

It states that in an atom or molecule, no two electrons can have the same four electronic quantum numbers. 

It states that an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins. This means if one is assigned an up- spin (+1/2), the other must be down spin (-1/2). 

Electrons in the same orbital have the same first three quantum numbers. Only two electrons can have these numbers, so that their spin moments must be either ms= (1/2) or (-1/2). If the 1s orbital contains only one electron, we have one ms value and electron configuration is written as 1s¹.

It refers to the characteristics of an element to be slightly attracted to a magnet. 

Electrons that are alone in an orbital.

If an electron is alone in an orbital, the orbital has a net spin, because the spin of the lone electron does not get canceled out.

Materials are attracted by a strong magnet.

It is characterized by non-attraction, or even a slight repulsion of an element to a magnet. 

Any time two electrons share the same orbital, their spin quantum numbers must be different. 

Materials are repelled by a strong magnet.

Diamagnetic atoms are not attracted to a magnetic field, but rather are slightly repelled.

The radius (size) of an atom.

It is the distance between the nuclei to the boundary of the surrounding cloud of electrons.

It increases to down and left.

The radius of a cation or an anion.

The distance between the nucleus to the farthest electron.

When an electron is removed, it will always be an electron in the innermost shell to be removed first.

The energy needed to remove an electron from an atom.

Adding electrons makes an atom bigger while removing electrons makes an atom smaller.

The trend of ionization energy is the opposite of the atomic radius trend.

The nearer an electron from the nucleus, the easier it is to pull away.

The change in energy that occurs when a neutral atom in gaseous phase gains an electron, releasing energy in the process.

It is how much an atom wants to gain an electron

It is a measure of the ability of an atom in a molecule to draw bonding electrons to itself.

It is the ability of an atom to hold electrons tightly.

Which of the following does not increases to up and right?

Electrons are transferred from an elements to another.

It contains ions.

Metal + Nonmetals

Electrons are shared by two elements.

It shares equal electrons.

It shares unequal electrons.

Nonmetals + Nonmetals

> 1.8

> 0.4 but < or equal to 1.8

> or equal to 0.4

It is the elements in Group 8A such as helium, neon, argon, krypton, xenon, and radon.

They are the most stable elements in the periodic table and are nonreactive under ordinary conditions.

They are also known as inert gas.

Noble gases can form compounds with other elements; examples krypton difluoride, KrF2 and xenon hexafluoride XeF6.

Octet  came from the Latin word "okto" means eight.

This configuration is the most stable arrangement an atom can have. Because of this stability, noble gasses have no tendency to lose, gain or share of electrons, which happens during chemical reactions.

The tendency of atoms to prefer to have eight electrons in the valence shell.

When atoms have fewer than eight electrons, they tend to react and form more stable compounds. This principle is referred to as the octet rule.

It is a system of representing the valence electrons of an atom using diagrams.

It consists of symbol of an element surrounded by one or more dots; each dot corresponds to the number of valence electron of an atom of the element.

They are neutral compounds made up of positively charged ions called cations and negatively charged ions called anions.

It is a chemical compound composed of ions held together by electrostatic forces termed ionic bonding.

Octet rule says that atoms like to have full outer shells of only eight electrons.

In a Lewis structure, the nucleus of the element is represented by its symbol. The valence electrons are represented by dots placed around the symbol in pairs.