Chem test

Group

Colum

Period

Rows Energy levels

Valence electrons

They are the outermost shell of of an arom. They determine how an atom interacts with other atoms, including how it bonds chemically.

Protons

They determine the number of electrons, theerefire each eelements atomic number is imprtant to grouoing them

Metals

LEFT

lose electrons

Shiny

Maletable

Ductable

High density

High melting and boiling points

Good conductors of heat and electricity

Nonmetal

Right

Gain electrons

Dull brittle

Non ductable

Sometimes low density

Low melting

Bad connections

Effective nucleur charge

The postive attraction that valence electrons fell from yhe nucleus

Usually abbervatied by Z

Shielding

Interior electrons prevent valence electrons from feeling full postive force of the nucleus

First ionization energy

The amount of energy needed to remove the outermost electron

Metals have lowee nucleur charge (z), valence electrons are less attracted so they are easier to remove.

Electronegativity

Ability to attract electrons

Nonmetals have higher nucleur charge Z so they can attract more electrons

Atomic Radius

Distance from nucelus to valence electrons in neutral atom. Metals have lower nucleur charge, cant pull electrons in as close.

Ionic radius

Distance from nucelus to outermost electron in an ion (charged atom)

Metal lose electron gets smaller. Non metal gain electrons, get bigger

Atomic Radius across a period

Decreases

Atomic Radius down a group

Increases

Ionic radius across a period

Decreases

Ionic radius down a grouo

Increases

Ionization energy across a period

Increases

Ionization energy down a group

Decreases

Electronegativity across a period

Increases

Electronegativity down a grouo

Decreases

Metallic character across a period

Decreases

Metallic character down a grouo

Increases

Reactivity metals across a period

Decreases

Reactivity metals down a group

Increases

Reactivity non metals across a period

Increases

Reactivity non metals down a group

Decreases

Shielding effect across a peeiod

Constant

Sheilsing effect down a geoup

Increases

Metallic charcater

How much like a. Eta, an atom behaves like

Metal lose elevtrons, low z= low ionization eneegy= better metal.

Ground state

When an atoms electron are in ten lowest pssible energy levels

ATOMS ARE IN THE GROUND STATE UNLESS ENERGY IS ADDED

Excited state

Is when an atom’s electrons have absorbed energy and moved to a higher energy level.

ENRGY IS ADDED TO LEVEL WHICH CAUSES ELEVYRONS TO JUMP TO HIGHER ENERGY LEVELS

Bright line spectrim

Each elemnets has its won unique bright line spectron that is used to indegy kg. Bright lines are at dofferent wavelengths. Each wavelength is mathematicalaly realated to a definite quantity of energy profuced when an electron moves from one energy level to another. This proves that electrosn exists at specific energy levels in the atom.

Excited state configuration

Elevtrons do not fill shells in order as expected

Lower shell will be left unfilled

They dont match periodic table.

Energy is absorbed when a elevtrons moves from a

Lower to higher energy level

Energy is released when an ekectron moves

from a higee energy level to a lower energy level

Charge is dteemined by

Atomic number , number of protons

Explain how a bright line spectrum is produced, in terms of excited state, energy transtiins, and ground state

an elevyrons absorbs energy and moves to a higher level, as it releases energy it lowers an energy lebel in the form of a bright line spectrum.