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Trends in the Periodic Table of Elements. Atomic Radius. Based on the graph, what do you think Atomic Radius means?. Atomic Radius. Atomic Radius – size of an atom. Atomic Radius. It ________________ as you go down a column because:. increases. Electrons are added to a new energy level.

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atomic radius
Atomic Radius

Based on the graph, what do you think Atomic Radius means?

atomic radius1
Atomic Radius

Atomic Radius – size of an atom

atomic radius2
Atomic Radius

It ________________ as you go down a column because:

increases

Electrons are added to a new energy level

atomic radius3
Atomic Radius

It ________________ as you go across a row because:

decreases

Within an energy level, as you add more protons (and electrons), the heavy protons pull the light electrons in closer

atomic radius4
Atomic Radius

The corner of the Periodic Table with the highest atomic radius is

And the corner with the lowest atomic radius is

Lower left corner

Upper right corner

before we move on
Before we Move on…

Atoms of all elements want to be stable

They will gain or lose electrons until their outer energy level is full (like the noble gases, column 18)

ionization energy
Ionization Energy

Ionization Energy – the amount of energy it takes to remove an electron

ionization energy1
Ionization Energy

It ________________ as you go down a column because:

decreases

The more total electrons an element has, the less it cares about whether or not it loses one electron

ionization energy2
Ionization Energy

It ________________ as you go across a row because:

increases

The more valence electrons an element has, the more it wants to keep its electrons

ionization energy3
Ionization Energy

The corner with the highest ionization energy is

The corner with the lowestionziation energy is

Upper right corner

Lower Left corner

ionization energy4
Ionization Energy

Example) Which of the following elements has the highest ionization energy: sodium, argon, cesium, or radon?

Argon

electronegativity

Atomic Number

Electronegativity

Electronegativity

Electronegativity– how much an atom attracts electrons

electronegativity1
Electronegativity

It ________________ as you go down a column because:

decreases

The more total electrons an element has, the less it cares about whether or not it gets another electron

electronegativity2
Electronegativity

It ________________ as you go across a row because:

increases

The more valence electrons an atom has, the more it really wants another one to get closer to a full shell (column 18)

electronegativity3
Electronegativity

The corner with the highestelectronegativity is

The corner with the lowestelectronegativity is

Upper right (except noble gases)

Lower left

electronegativity4
Electronegativity

Example) Which of the following elements has the highestelectronegativity: sodium, chlorine, rubidium, or iodine?

Chlorine

electronegativity5
Electronegativity

Example) Place the following elements in order in terms of increasing (smallest to largest) electronegativity: silicon, sodium, chlorine.

Sodium, Silicon, Chlorine

electronegativity6
Electronegativity

Example) Place the following elements in order in terms of increasing (smallest to largest) electronegativity: lithium, sodium, cesium.

Cesium, sodium, lithium