Electron Configuration
Which part of the Periodic Table is the S block?
Columns 1 and 2 (plus He)
How many valence electrons does He have?
2
Which has a larger atomic radius? DRAW A BOHR MODEL TO HELP JUSTIFY YOUR ANSWER
Na VS K
K
valence electrons farther away from the nucleus.
Give an example of a metalloid.
B, Si, Ge, As, Te, Sb
Which element has the LEAST electrons when neutral?
Hydrogen
What is the SHORTHAND electron configuration for Mercury (Hg)? CIRCLE THE VALENCE ELECTRONS
[Xe] 6s² 4f¹⁴ 5d¹⁰
Explain what a valence electron is. Draw a Bohr model of Florine (F) to demonstrate.
The electrons in the outermost shell (farthest from the nucleus).
What is the trend for atomic radius? Explain why (HINT: Draw Bohr models of Li, Na, and F to demonstrate)
Down a Column: Increase going down a column -> add an energy level
Across a Row: Decreases from left to right-> valence electrons added at same proportion as protons. More attraction between valence electrons and protons pulls electrons closer to nucleus.
Is Chlorine a metal or a nonmetal?
nonmetal
Will Beryllium form a cation or an anion? Show the ionic symbol.
Cation
Be+2
What is the electron configuration for Phosphorus (P)?
WRITE THE FULL AND SHORTHAND; CIRCLE VALENCE ELECTRONS
[Ne] 3s²3p³
1s22s22p63s23p3
Write the full and shorthand electron configuration for Chlorine (Cl) and circle the valence electrons.
[Ne] 3s² 3p⁵
1s22s22p63s23p5
Which atom has the higher electronegativity? EXPLAIN
O VS K
O
Increases left to right: Atoms closer to 8 valence electrons want to get to 8 electrons-> more likely to try and hog all of the electrons.
Increases up a column: Electrons are farther away from the nucleus (increase in atomic radius) and electrons are farther away from the nucleus. EASIER TO TAKE AWAY (harder to hog)
List 3 Characteristics of a Metal.
*Malleable
*Conducts heat/electricity
*Shiny
*Strong
*High boiling/melting point
Give an example of an atom with 3 valence electrons.
Anything in column 13
What is the electron configuration for Bromine (Br)? DRAW AN ORBITAL DIAGRAM
[Ar] 4s² 3d¹⁰ 4p⁵
1s22s22p63s23p64s23d104p5 .
How many valence electrons do atoms in group 18 have?
8
Which atom will have the highest ionization energy? EXPLAIN
P VS Ga
P
Down a Column: Decreases-> larger atomic radius means electrons are farther away from the nucleus; easier to take away
Across a Row: Increases from left to right-> Noble gases are the “coolest” atoms and it is hard to take electrons away when they have the desired 8
List 3 characteristics of a non-metal.
*Dull
*Brittle
*Does not conduct heat/electricity
*Low boiling/melting point
What are the 4 orbital types? How many sublevels are there of each and how many total electrons does each hold?
p: 3 sublevels-6
d: 5 sublevels-10
f:7 sublevels-14
DRAW AN ORBITAL DIAGRAM for Potassium (K). What is it's electron configuration?
[Ar] 4s¹
1s22s22p63s23p64s1
How many valence electrons does Nickel (Ni) have?
HINT: You might have to write the electron configuration
2
HINT: Draw Bohr models of Na and H to help.
As atomic radius increases, ionization energy decrease BECAUSE as valence electrons move farther and farther away from the nucleus, the easier they are to lose (ionization energy decreases).
Similarly, as atomic radius decreases, ionization energy INCREASES because valence electrons are closer to the nucleus, making the Coulombic attraction between them stronger (harder to lose).
Atomic Radius: A measure of the size of an atom; the distance from the nucleus to the valence electrons.
Ionization Energy: The amount of energy it takes to remove valence electrons (AKA how easily an atom gives up valence electrons).
Metal: Left of the staircase (minus Hydrogen)
Nonmetal: right of the staircase
Where on the Periodic Table are the atoms with the largest atomic radius?
Bottom left