Using the Periodic Table to Draw AtomsUsing the Periodic Table to Draw Atoms

Periodic Table & Orbitals/Energy LevelsPeriodic Table & Orbitals/Energy Levels

Each row on the periodic table represents an Each row on the periodic table represents an orbital or orbital or energy levelenergy level that electrons can occupy that electrons can occupy

As you move down the rows on the periodic table, the As you move down the rows on the periodic table, the numbers numbers increaseincrease (beginning at 1 and following all the (beginning at 1 and following all the way to 7)way to 7)

The number on the row is the The number on the row is the amount of orbitalsamount of orbitals available for electrons for available for electrons for EVERY ATOMEVERY ATOM in that row in that row Example: Magnesium (Mg) is in the Example: Magnesium (Mg) is in the 33rdrd row row. This means that it . This means that it

would have would have 3 orbitals3 orbitals for its electrons to occupy. Silicon (Si) is for its electrons to occupy. Silicon (Si) is also in the also in the 33rdrd row. row. So it would also have So it would also have 3 orbitals3 orbitals for its for its electrons to occupyelectrons to occupy

Example: Potassium (K) and Titanium (Ti) are both in the Example: Potassium (K) and Titanium (Ti) are both in the 44thth row. row. This means that both of these atoms would have This means that both of these atoms would have 4 orbitals4 orbitals for for their electrons to occupytheir electrons to occupy

Periodic Table & Orbitals/Energy LevelsPeriodic Table & Orbitals/Energy Levels

Try these examples:Try these examples:

Element Row # of orbitals

Silver(Ag)

Xenon(Xe)

Fluorine(F)

Carbon(C)

What do these orbitals mean?What do these orbitals mean?

Orbitals are energy levels Orbitals are energy levels outside the nucleusoutside the nucleus where the where the electronselectrons are found are found

When you draw atoms, you have to “Fill” the When you draw atoms, you have to “Fill” the orbitals up with orbitals up with electronselectrons

Steps/rules for filling orbitals with electrons:Steps/rules for filling orbitals with electrons: 1) The first orbital can only hold 1) The first orbital can only hold 2 electrons2 electrons 2) The remaining orbitals can only hold 2) The remaining orbitals can only hold 8 electrons8 electrons 3) Each orbital must be completely 3) Each orbital must be completely filledfilled with its with its

maximum amount of electrons before another orbital maximum amount of electrons before another orbital can be drawncan be drawn

Steps for Drawing Atoms – Steps for Drawing Atoms – Example: PhosphorusExample: Phosphorus

1.1. Begin by determining the number of Begin by determining the number of protons, neutrons, protons, neutrons, electrons and orbitalselectrons and orbitals for your atom for your atom

2.2. Draw your nucleusDraw your nucleus- This should look like a - This should look like a circlecircle

3.3. Inside your nucleus write down the number of Inside your nucleus write down the number of protons protons and neutronsand neutrons

- Place a - Place a pp++ by your number of by your number of protonsprotons- Place a - Place a nnoo by your number of by your number of neutronsneutrons

4.4. Draw yourDraw your orbitals orbitals around your nucleus around your nucleus- These should look like - These should look like semicirclessemicircles outside of outside of

the the nucleus nucleus 5.5. Fill the orbitals with Fill the orbitals with electronselectrons

- Remember the steps/rules- Remember the steps/rules