Coulomb's law

coulombs law, electrons, atomic radius, ionization, electronegativity, ions,

Columb’s law

The potential energy of two charged particles depends on their charges ( q1 & q2 ) and on the distance between them

Coulmbs law formula

is given by F = k(q1 * q2) / r²

F stands for

force

Ke stands for

coulombs constant 9×10 to the power of 9 NM squared/ C squared

q1 and q2 stands for

formula charges

r squared stands for

distance between the two charges

1) Alike charges

repel ( + and +, -and - )

2) Opposite charges

attract ( + and - )

3) forces of attraction and/ repulsion

-directly proportional to charge difference

-inversely proptinal to distance between

There are two types of electrons

valence electons and core electrons

valence electrons

e-s occupying the outer energy level

core electrons

all e-s not occupying the outer energy level

core electrons repel

valence electrons ( outer electrons)

more core electrons cause

-increase replusive forces on valence e-s

-increase shielding of + charge nucleus

The electron on the outer shell ( valence electrons) wont be as strong because

the first orbital of the electrons would repel the one above it

Atomic Raduis

half the distance between two chemically bonded homonucler atoms ( atoms of the same element)

On the PE the atomic radius

-decrease from left to right across a period

-same number of core electrons ( repulsive force stays constant on valence electrons )

If # of protons increases

atrractive forces increase

in the PE increases from top to bottom down a group

-inc. number of electrons ( repulsive force inc. on valence e-s)

-more energy levels

Ionization Energy

-energy needed to remove e-s

-increas fro left to right across a period

-decreases from top to bottom down a group

Ion

atom ( group of atoms that have gained/ lost e-s

Increas from left to right across a period

• same number of core e-s (repulsive force stays constant on valence e-)

• number of protons increase ( attractive forces increases)

Decreases from top to bottom down a groups

• inc. remember of core e-s ( repulsive force inc. )

• more energy levels

Electron negativity

atrractiveness to an e- in a bond

• increases from left to right across a period

• decrease from top to bottom down a group

Every single element in row

18 has 0 electronegativity

Ions

an atom that has an electric charge

ions can not lose of

gain protons

ions valence e-s can be

lost or gained Ca

Cations ( Cat-ion)

• lost e-

• metals from cations

• postively charged ion

metals tend to lose

e- ( oxidize)

non metals tend

to gain e- ( reduce))

Anions ( an-ion )

• negativly charged ion

• gained electron

  • non-metals from an-ions

metals gain/lose electrons to become a noble gases

in order to gain a valence electron

deterine charge

charge = # protons- # electrons

Atoms want a full valence shell

in other words a noble gas configuration

neon gases do not form ions

because already have a full valence shell

electron configuration can b determined

by the location of an element on the PT

period #

represents highest occupied EL ( for representive element )

block

reprsents last occupied sublevels ( S, p, d, f)

group

reresent number of e in the valence shell