2Q_Science_B

Energy Level

The first number and tells us what electron shell can the orbital be located

Orbital

The letter and tells us where an electron would most likely be found

no. of electrons

The superscripted number and they vary depending on the orbital and/or element

S

orbitals can have 2 electrons max

P

orbitals can have 6 electrons max

D

orbitals can have 10 electrons max

F

orbitals can have 14 electrons max

Valence Electrons

are electrons located in the OUTERMOST SHELL/ENERGY LEVEL of the atom

Stability

why do atoms combine because of?

Compound

Two or more elements combined to form stability is called a

He

All noble gases except this has an s2p6 configuration

Octet Rule

Chemical compounds tend to form so that each atom, gain, lose, or share electrons, until they are surrounded by 8 valence electrons (4 electron pairs)

Lewis Dot Structure

is a representation that shows the valence electrons for that atom

Dots

its used to show the valence electrons of atoms.

Gilbert Newton Lewis

devised the structure in 1916

Lewis Dot Structure

Consists of the atomic symbol with dots around it that represent its valence electrons

Electronegativity

It is the measure of atom’s ability to attract electrons.

Ionic Bonding

Chemical bonding resulting from electrical attraction between cations and anions.

Salts

Occurs when elements with low EN (metals) react with elements with high EN (non-metals) to form ionic compounds

Polyatomic Ions

Some compounds can act like positively-charged or negatively-charged ions. They can ionically bond with individual elemental ions.

Covalent Bonding

chemical bonding resulting from the sharing of electron pairs.

Covalent Bonding

Exists when the difference between the EN of the atoms is not enough for an electron transfer

Ionic and Covalent Bonding

2 types of Bonding

Non polar covalent bond-

a covalent bond in which the bonding electrons are shared equally by bonded atoms, resulting in a balanced distribution of electrical charge.

Polar covalent bond

a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons

Single Covalent Bond

sharing of a single pair of electrons between bonded atoms

Double Covalent Bond

share two electron pairs

Triple Covalent Bond

share three electron pairs

Bonding Pairs/Electrons

electrons that are shared between atoms

Lone Pairs

electrons not involved in bonding

Metallic Bond

Attractive force holding pure metals together