states that there are only certain allowed energy states for an electron and that these are quantized. Further, it tells us that no two electrons, in the same system. can occupy the same energy state and that all the energy states are filled from the lowest levels to the highest levels.

quantum theory

A portion of light, which the eyes can detect, is called _____ and occupies a narrow band in the EM spectrum. Visible light consists of different colors (ROYGBIV); each color with distinct characteristics.

visible light

is the distance from the equilibrium point (x-axis) of a propagating wave to the highest (or lowest) point of the waveform.

amplitude

is the distance between identical points in successive cycles in a propagating wave

wavelength

is the number of cycles that a wave makes per unit of time and is usually expressed in units of Hertz (Hz) or 1/s (read as "per second").

frequency

proposed that light, aside from being an electromagnetic wave, also exists as tiny particles, which were later called photons. These two characteristics of light came to be known as the dual nature of light, which is consistent with the quantum theory known today. The photon can be considered as the quantized form of light. The energy of a photon can be measured in quantities of hf.

albert einstein

atoms can only emit certain wavelengths of light as the electrons fall back to its ground state, a process referred to as

electron relaxation

is described as having a small nucleus at the center made of protons and neutrons, and a big space around it where electrons move about in a wavelike manner.

atom

Uncertainty Principle - a German physicist ______(1901-1976) an electron is considered to be traveling at quantum speeds like a wave which then means that it is impossible to simultaneously determine its exact location and momentum at a particular time.

werner heisenberg

describe the distribution or location of electrons in an element

the quantum numbers

- specifies the energy of an electron and the size of the orbital (distance from the nucleus). All orbitals that have the same value of n are said to be on the same level.

principal quantum numbers (n)

- is a wave function for an electron in an atom.

atomic orbital

- specifies the shape of an orbital within a particular principal quantum number.

angular momentum quantum number (l)

- group of orbitals in the same shape

subshells or sublevels

- specifies the orientation in space of an orbital of a given energy (n) and (l). This number divides the subshell into individual orbitals that hold the electrons

magnetic Quantum Number (m)

- describes the spin of an electron in an orbital. An electron can spin in only two directions (clockwise or counterclockwise).

spin quantum number (s)

It states that a lower energy orbital should be filled up first before the next higher energy orbital. The arrangement of orbital energy follows this order: sp df

aufbau principle

refers to the characteristic of an element to be slightly attracted to a magnet. • It results from the presence of unpaired electrons in some of the atomic orbitals of an atom, which creates a net magnetic moment for the atom. These electrons tend to align themselves in the direction of an external magnetic field.

paramagnetism

Elements without unpaired electrons in their orbitals exhibit _____. is characterized by the non-attraction, or even a slight repulsion, of an element to a magnet.

diamagnetism

is a phenomenon that greatly enhances the paramagnetism of a material in such a way that it becomes permanently attracted to a magnet.

ferromagnetism

(from the Greek word "okto," meaning "eight") configuration is the most stable arrangement an atom can have.

octet

American chemist _____ (1875-1946) developed a system of representing the valence electrons of an atom using diagrams called Lewis electron-dot structures or Lewis structures.

gilbert lewis

A ____ consists of a symbol of an element surrounded by one or more dots; each dot corresponds to a valence electron in an atom of the element. Only two dots are placed on each of the four sides.

lewis structure

______ that lose valence electron(s) form cations.

metals

_____ that tend to gain electron(s) become cations.

nonmetals

______ generally exists between a metal and a nonmetal as a result of their high electronegativity difference.

ionic bonding

_____ is a measure of an atom's ability to attract electrons.

electronegativity

is an electrical attraction between the nuclei and valence electrons of an atom and which binds atoms together. Oftentimes, this type of attraction is called an intermolecular force. Three types of chemical bonds may exist in substances: ionic, covalent, and metallic.

chemical bonding

results from the transfer of one or more valence electrons from one atom to another. This bond exists between a metal (lose electrons), and a non-metal (accept electrons). Ionic bonds are formed due to a large difference in electronegativity (is a measure of

ionic bond

mIt states that no two electrons can have exactly the same set of quantum numbers.

pauli exclusion principles

It states that, in filling the orbitals of the same energy level, an orbital must be singly filled up first before pairing the electron.

hund’s rule

it is formed if sharing of an electron pair between atoms exists. This. bond occurs between non-metals.

covalent bond

is a bind in which the electrons are equally shared by the bonded atoms. This indicates a balanced distribution of electrical charge.

nonpolar covalent bond

refers to the bond in which the bonded atoms have an unequal sharing of electrons. This unequal sharing of electrons may be regarded as "partial electron transfer" or a shift in electron density.

polar covalent bond

it happens when two atoms share a pair of electrons.

single covalent bond

we t happens when two atoms share two pairs of electrons. Double bonds are stronger than single bonds.

double covalent bond

it happens when two atoms share six valence electrons, Triple bonds are the strongest bonds

triple covalent bond

Hydrocarbon with only single bonds between carbon atoms.

alkane

Hydrocarbon with at least one double bond.

alkene

Hydrocarbon with at least one triple bond.

alkyne

- A reaction in which atom or group of atoms add to a molecule with multiple bond (double or triple bond) Involve in braking one T1 bond to form two sigma bonds.

addition

A reaction in which an atom or a group of atoms in a molecule is replaced by another atom or group of atoms from the reagent.

substitution

Opposite of addition reaction a single reactant splits into

elimination

- are reactions that involves addition of oxygen to a compound or reaction that increase the oxidation state of a compound and is also terms as an oxidation reaction.

oxidation

- involve reaction that decreased in the oxidation state.

reduction

- of a compound is a type of redox reaction that yields CO, and H20

combustion