ELECTRON ARRANGEMENTS
PERIODICITY AND BONDING
GUIDED NOTES
SC3 Students will use the modern atomic theory to explain the characteristics of atoms.
a. Discriminate between the relative size, charge, and position of protons, neutrons, and electrons in
the atom.
b. Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical
properties.
c. Explain the relationship of the proton number to the element’s identity.
d. Explain the relationship of isotopes to the relative abundance of atoms of a particular element.
f. Relate light emission and the movement of electrons to element identification.
SC4. Students will use the organization of the Periodic Table to predict properties of elements.
a. Use the Periodic Table to predict periodic trends including atomic radii, ionic radii, ionization energy,
and electronegativity of various elements.
b. Compare and contrast trends in the chemical and physical properties of elements and their
placement on the Periodic Table.
ESSENTIAL QUESTION: WHAT IS LIGHT AND WHAT CAUSES IT?
LIGHT OR “VISIBLE” LIGHT: The range of wavelengths, or colors, of light that we can see with our human eyes.
ELECTROMAGNETIC SPECTRUM: the entire frequency range of electromagnetic waves.
SPEED: distance travelled per unit time
WAVELENGTH: the distance (measured in the direction of propagation) between two points in the same phase
in consecutive cycles of a wave
FREQUENCY: the number of waves to pass a point in a unit of time.
RELATIONSHIP BETWEEN WAVELENGTH AND FREQUENCY:the shorter the wavelength the higher the
frequency and the longer the wavlength the lower the frequency.
EXAMPLES OF ELECTROMAGNETIC
RADIATION IN ORDER OF
INCREASING FREQUENCY AND
DECREASING WAVELENGTH
Radiowaves
Microwaves
Infrared
Visible
Ultraviolet
Xray
Gamma rays
WAVELENGTH
103-10-1
10-1-10-3
10-3-10-6
10-6-10-7
10-7-10-8
10-8-10-11
10-11-10-15
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VISIBLE LIGHT (WHITE LIGHT) IN ORDER OF INCREASING FREQUENCY: “THE RAINBOW”
Red, orange, yellow, green, blue, indigo, violet
HOW CAN WE USE LIGHT EMISSION AND THE MOVEMENT OF ELECTRONS TO IDENTIFY AN ELEMENT IN A
FLAME TEST? Each element releases an specific color or frequency which is how we identify elements in space.
QUANTUM: quantum jump is a change of an electron from one quantum state to another within an atom.
PHOTON: a photon is an elementary particle, the quantum of the electromagnetic interaction and the basic
"unit" of light and all other forms of electromagnetic radiation.
GROUND STATE: the lowest energy state of an atom or other particle.
EXCITED STATE: particle that has a higher energy than that of its ground state
ESSENTIAL QUESTION: WHAT ARE 3 IMPORTANT MODELS OF THE ATOM?
THE WAVE MECHANICAL MODEL/QUANTUM MODEL OF THE ATOM
4 QUANTUM NUMBERS
PRINCIPAL QUANTUM NUMBER: The number related to the amount of energy an electron has and therefore
describing which shell the electron is in.
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ANGULAR MOMENTUM QUANTUM NUMBER: the total angular momentum of a given particle, by combining
its orbital angular momentum and its intrinsic angular momentum (i.e., its spin).
MAGNETIC QUANTUM NUMBER: which describe the unique quantum state of an electron and is designated by
the letter m. The magnetic quantum number denotes the energy levels available within a subshell.
SPIN QUANTUM NUMBER: describes the spin orientation of an electron relative to an external magnetic field.
** WE WILL USE THIS MODEL OF THE ATOM TO STUDY ELECTRON ARRANGEMENTS AND TO DRAW ORBITAL
NOTATIONS AND
ELECTRON CONFIGURATION NOTATIONS FOR SPECIFIC ATOMS***
ENERGY LEVEL
SUBLEVELS
SPACE ORBITALS
MAX. NUMBER OF
OR SHELL
ELECTRONS
ST
1
1s
1
2
2ND
2s2p
3
8
3RD
3s3p3d
5
18
4TH
4s4p4d4f
7
32
5TH
5s5p5d5f5g
9
50
6TH
6s6p6d6f6g6h
72
7TH
7s7p7d7f
108
ESSENTIAL QUESTION: HOW IS THE ATOM LIKE AN APARTMENT BUILDING?
RULES GOVERNING ELECTRON CONFIGURATIONS
WHAT ARE THE RULES AND HOW ARE WE WILL USE THEM
AUFBAU PRINCIPLE: Electrons occupy the lowest available energy level.
THE DIAGONAL RULE: (insert a picture of the diagonal rule)
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THE FILLING ORDER OF THE ELECTRONS IN THE ENERGY LEVELS
1s
2s 2p
3s 3p
4s 3d 4p
5s 4d 5p
6s 4f 5d 6p
7s 5f 6d 7p
EXCEPTIONS TO THE FILLING ORDER:
PERIOD 4: Cu AND Cr
PERIOD 5: Mo – Ag (ALL)
PERIOD 6: Pt AND Au
WHY ARE THESE EXCEPTIONS TO THE FILLING ORDER? They are multivalent and can have fewer or more
electrons.
PAULI’S EXCLUSION PRINCIPLE: only two electrons with opposite spin can occupy an atomic orbital
HUND’S RULE: electrons fill each and all orbitals in the subshell before they pair up with opposite spins.
THREE WAYS TO SHOW ARRANGEMENTS OF ELECTRONS
ORBITAL CONFIGURATION NOTATION: This uses the arrows and dashes.
MAKE A CHART ON YOUR OWN TO SHOW THE ELECTRON ORBITAL CONFIGURATION NOTATIONS FOR
ELEMENTS 1-36.
ELECTRON CONFIGURATION NOTATION: this uses numbers and letters to represent the energy level, types of
orbital and the number of electrons in the orbital.
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EXAMPLE:
ELECTRON DOT NOTATION: each valence electron is represented by a dot around the symbol of the element.
EXAMPLE:
NOBLE GAS CONFIGURATIONS: MAKE A CHART ON YOUR OWN PAPER AND ATTACH TO THE NOTES.
symbol
electron configuration
helium
He
1s2
neon
Ne
[He]2s22p6
argon
Ar
[Ne]3s23p6
krypton
Kr
[Ar]3d104s24p6
xenon
Xe
[Kr]4d105s25p6
radon
Rn
[Xe]4f145d106s26p6
VALENCE ELECTRONS
VALENCE ELECTRONS: electrons located in the outside energy shell.
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VALENCE NUMBERS/OXIDATION NUMBERS: The charge which an atom of the element has, or appears to
have, in a compound. The number of electrons an atom gains or loses.
GUIDED INSTRUCTION
LIST THE # OF VALENCE ELECTRONS
AND THE VALENCE NUMBER/OXIDATION NUMBER FOR THE FOLLOWING ATOMS
ATOM #VALENCE ELECTRONS
OXYGEN
CHLORINE
SODIUM
POTASSIUM
ALUMINIUM
NITROGEN
HYDROGEN
CALCIUM
LITHIUM
FLUORINE
SULFUR
PHOSPHOROUS
VALENCE #/OXIDATION #
-2
-1
+1
+1
+3
-3
+1
+2
+1
-1
-2
-1
GROUP
VALENCE ELECTRONS
VALENCE # FOR GROUP
1
1
+1
2
2
+2
13
3
+3
14
4
+/-4
15
5
-3
16
6
-2
17
7
-1
18
8
0
OCTET: DEFINE: an atom wants 8 electrons to become stable.
PERIODICITY
STATE THE PERIODIC LAW: states that the repeating chemical and physical properties of elements change
periodically with the elements atomic number.
DRAW A GRAPHIC ORGANIZER TO ILLUSTRATE THE PERIODIC TREND FOR ELECTRONEGATIVY OF THE
ELEMENTS ON THE PERIODIC TABLE
(DESCRIBE THE TREND LEFT TO RIGHT ACROSS A PERIOD AND DOWN IN A GROUP)



Atomic Radius Decreases
Ionization Energy Increases
Electronegativity Increases
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WHICH CATEGORY OF ELEMENTS TENDS TO HAVE THE HIGHEST ELECTRONEGATIVITY AND WHICH GROUP
TENDS TO HAVE THE LOWEST ELECTRONEGATIVITY? WHY?
Group 17 highest: the ionization energy is high and the atomic radius is smaller.
Group 1 lowest: the ionization energy is lower and the atomic radius is larger.
ATOMIC RADIUS: is a measure of the size of its atoms, usually the mean or typical distance from the nucleus to
the boundary of the surrounding cloud of electrons.
DRAW A GRAPHIC ORGANIZER TO ILLUSTRATE THE PERIODIC TREND IN ATOMIC RADIUS OF THE ELEMENTS ON
THE PERIODIC TABLE. LEFT TO RIGHT ACROSS A PERIOD AND DOWN IN A GROUP.
IONIZATION ENERGY: Amount of energy required to remove the highest-energy electron from an isolated
neutral atom in the gaseous state
DRAW/INSERT A PICTURE OR A GRAPHIC ORGANIZER TO ILLUSTRATE THE PERIODIC TREND IN IONIZATION
ENERGY OF THE ELEMENTS ON THE PERIODIC TABLE LEFT TO RIGHT ACROSS A PERIOD AND DOWN IN A
GROUP.
BLOCKS ON THE PERIODIC TABLE
“S” BLOCK: The s orbital is a spherically-shaped region describing where an electron can be found
“P” BLOCK: is a dumbbell-shaped region describing where an electron can be found
“D” BLOCK: there is a set of five d orbitals (with more complex shapes and names) as well as the 3s and 3p
orbitals (3px, 3py, 3pz).
“F” BLOCK: the lanthanide and actinide series…very complex.
USE THE BLOCKS ON THE PERIODIC TABLE, GROUP NUMBERS, PERIODS AND VALENCE ELECTRONS TO QUICKLY
DETERMINE THE “OUTER ENERGY LEVEL CONFIGURAION” OF SPECIFIC ATOMS.
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NAME THE ELEMENT GAME
P BLOCK ELEMENT PERIOD 4 AND GROUP 15: NAME IT___________
S BLOCK ELEMENT PERIOD 2 AND GROUP 1: NAME IT_________
NAME THE “P” BLOCK ELEMENT WITH THE FOLLOWING OUTER ENERGY LEVEL CONFIGURATION:
5S2 5P2 NAME IT _______________
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“D” BLOCK ELEMENTS ( TWO POSSIBLE)
4 S1
NAME THEM _____________________ OR ___________________
“f” BLOCK ELEMENT: PERIOD 6 4 f 5, 6 s2 NAME IT:_______________
“f” BLOCK ELEMENT: PERIOD 7:
“s” BLOCK ELEMENT: 5 S2
6d2, 7s2 NAME IT__________
NAME IT ______________________
“p” BLOCK ELEMENT: 4 S2, 4 P6 NAME IT ______________________
GIVE THE OUTER ENERGY LEVEL CONFIGURATION FOR THE FOLLOWING ELEMENTS USING THE BLOCK, PERIOD
AND GROUP METHOD>
ZINC _______________
OXYGEN_____________
CALCIUM ________________ KRYPTON _______
URANIUM _______________ SILVER _________
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