Limitations of Rutherford's Atomic Model
-Could not explain chemical properties of elements
-Needed a model that better describes behavior of electrons
Neils Bohr
Developed the Bohr Model (Planetary Model)
-Incorporated discoveries about how energy of atom changes when light is absorbed or emitted
-Proposal:electrons travel in specific orbitals
-Electron orbits have a fixed energy
-Amount of energy gained or lost is not the same
-Quantum: Amount of energy required to move an electron from one energy level to another
The Quantum Mechanical Model/Electron Cloud Model
-Erwin Schrondinger- Came up with equation describing behavior of electron; mathematical solutions led to quantum mechanical model
-Determines allowed energies an electron can have and how likely it is to find the electron in various locations
Heisenberg's Uncertainty Principle
Impossible to know the velocity and position of election at the same time
Atomic Orbital
Mathmatical expression describing probability of finding an electron
-Three dimensional region around the nucleus
-Principal quantum number (n)-energy level
-Energy sublevel corresponds to one or more orbitals of different shapes
Electron Configuration
Tells how electrons are arranged in orbitals
Noble Gas Configuration
Shorthand electron configuration
-Portion of electron configuration summarized with noble gas (group 18 element) in brackets
Aufbau's Principle
Electrons occupy the orbitals of lowest energy first
Pauli's Exclusion Principle
Atomic orbitals can hold a maximum of two electrons
-Electrons must have opposite spins (either up, closewise or down, counterclockwise)
Hund's Rule
Electrons of same spin placed in orbital before pairing
Orbital diagrams
A visual representation of electron arrangement in atoms
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p4
Se
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p5
Br
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p6
Kr
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s1
Fr
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s24d10 5p6 6s2 4f14 5d8
Pt
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f10
Dy
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p4
Po
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d5
Mn
The following electron configuration is for a _________________ atom.
1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p2
Sn
The electron configuration for sodium is _________.
1s22s22p63s1
The electron configuration for argon is _____.
1s22s22p63s23p6
The electron configuration for iron is _____.
1s22s22p63s23p64s23d6
The electron configuration for cobalt is _____.
1s22s22p63s23p64s23d7
The electron configuration for Mg+2 is _____.
1s22s22p6
The electron configuration for P-3 is ____
1s22s22p63s23p6
[Kr] 5s2 4d10 5p3
Sb
The following noble gas configuration is for an atom of _____.
[Kr] 5s2 4d10 5p6
Xe
The following noble gas configuration is for an atom of _____.
[Ar] 4s1
K
The following noble gas configuration is for an atom of _____.
[Xe] 6s2 4f9
Tb
The following noble gas configuration is for an atom of _____.
[Xe] 6s2 4f14 5d7
Ir
The following noble gas configuration is for an atom of _____.
[Ne] 3s2 3p1
Al
The noble gas configuration for radium is _____.
[Rn]7s2
The noble gas configuration for gold is _____.
[Xe]6s24f145d9
The noble gas configuration for carbon is _____.
[He]2s22p2
The noble gas configuration for beryllium is _____.
[He]2s2
After drawing the orbital diagram for selenium, how many unpaired electrons remain?
2
After drawing the orbital diagram for carbon, how many unpaired of electrons remain?
2
After drawing the orbital diagram for fluorine, all of the orbitals are filled with paired electrons.
False
What is wrong with the following configuration? Choose all that apply.
1s22s33s22p63p5
violates Pauli's exclusion principle and violates Aufbau's principle
Use the following electron configuration to answer the question.
1s2 2s2 2p6 3s2 3p6 4s2
How many shells (energy levels) does this atom have?
4
s
sphere, 1 orbital, maximum 2 electrons
p
dumbbell, 3 orbitals, ,maximum 6 electrons
d
double dumbbell, 5 orbitals, maximum 10 electrons
f
complex, 10 orbitals, maximum 14 electrons
sublevel 1
1s maximum 2 electrons
sublevel 2
2s, 2p maximum 8 electrons
sublevel 3
3s, 3p, 3d maximum 18 electrons
sublevel 4
4s, 4p, 4d, 4f maximum 32 electrons
After drawing the orbital diagram for oxygen, _______ electrons remain unpaired.
2
The electron configuration for potassium is ___________________. (
1s22s22p63s23p64s1
[Kr]5s2 is the noble gas configuration for ________.
Sr
Aufbau Principle
Electrons are added one at a time to the lowest energy levels first
Hund's Rule
Electrons occupy equal-energy orbitals so that a maximum number of unpaired electrons results
Pauli Exclusion Principle
An orbital can hold a maximum of 2 electrons
arrows
electrons
lines/boxes
orbitals
The maximum number of electrons that can occupy the 2nd energy level, n=2, is
8
The following electron configuration shows the distribution of electrons in an atom of ____________.
1s22s22p63s23p64s23d6
Fe
Which of the following statements are true regarding electron arrangement in atoms?
- Electrons enter the lowest energy levels first
- An “s” orbital is spherically shaped
Is calcium a metal, nonmetal, or metalloid?
Metal
What is the name of the element located in Group 17, Period 3?
Chlorine
What is the symbol of the element that has an atomic mass of 200.59?
Hg
What period and group do you find silver? (Enter it in like this: period number, group number)
5, 11
How many protons does iron have?
26
What is the name of the element that has a mass number of 35?
Chlorine
What is the atomic number for gold?
76
What is the symbol of the element found in Group 15, Period 5?
Sb
What is the mass number of cobalt?
59
Is sulfur a metal, nonmetal, or metalloid?
nonmetal
How many electrons does a neutral atom of Sr have?
38
What is the symbol of the element that has an atomic mass of 237.048 amu?
Np
Write the symbol for bohrium.
Bh
What period and group would you find osmium?
6, 8
What is the symbol of the element found in Group 6, Period 4?
Cr
What is the number of neutrons in Kr?
48
Which series (s, p, d, or f) is uranium located?
f
What is the name of the group barium is located in?
Alkaline Earth Metals
What is the name of the group iodine is located in?
Halogens
What series (s, p, d, or f) is hassium located?
d
Alkali Metals
Group 1 excluding Hydrogen s block 1 valence electron
Alkaline Earth Metals
Group 2 s block 2 valence electron
Transition Metals
Groups 3-12 d block n-1
Metalloids
B, Si, Ge, As, Sb, Te, Po p block 3-6 valence electron
Halogens
Group 17 p block 7 valence electrons
Noble Gases
Group 18 p block 8 valence electrons
Diatomic Molecules
Cannot stand alone in nature, 2 of same atom bonded
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine
Inner Transition Elements
F block n-2
Atomic Radius and Shielding Effect
Right-Small Bottom-Large
Ionization Energy and Electronegativity
Right-high Bottom-Lower
Ionization Energy
energy to remove e
Electronegativity
ability to attract e
Shielding Effect
inner e shield outer e
Which of the following trends increase across a period?
electronegativity ionization energy
Elements in group 1 will typically (gain/lose) 1 electron.
lose because cations lose electrons
Noble gases, with the exception of helium, have _____ electrons in their outermost shell (valence electrons).
8
The most electronegative atom is ________
Fluorine
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
Dmitri Mendeleev
Which of the following decreases with increasing atomic number in Group 2?
ionization energy
After drawing the orbital diagram for a sodium atom, how many unpaired electrons are there?
1
Which group contains the alkaline earth metal family of elements?
2
Atoms will gain, lose, or share electrons in order to achieve an electron configuration of what type of elements?
noble gases
What charge will halogens more than likely form?
-1
Transition metals have electron configurations that end in the _________ sublevel.
d
Look at your periodic table. Which atom has the largest atomic radius?
Radium
The element with the following electron configuration, 1s22s22p63s23p64s23d104p1 , has electrons in what highest energy level?
4
How many periods are on the periodic table?
7
The Periodic Law states that when elements are arranged in order of increasing _____, their chemical and physical properties show a periodic pattern.
atomic number
The alkali metals belong to group _____.
1
What is the electron configuration for Oxygen?
1s2, 2s2, 2p4
Many of the groups on the periodic table have names you should know. The halogen s belong to group _____.
17
The periodic table we use today reflects the arrangement of elements as done by _____.
Henry Moseley
How many valence electrons does Nitrogen have?
5
Which of the following elements would most likely gain electrons in order to achieve stability?
N
The following information is true for carbon
The highest energy level containing electrons in a carbon atom is the 2nd energy level.
Carbon has 4 valence electrons.
C-12 and C-14 are isotopes of carbon.
Of the periodic trends, which of the following decrease within a group from top to bottom?
Electronegativity
Ionization Energy
Because these elements have achieved octet (a full valence shell), they do not have an attraction for electrons
Rn
Ne
What happens to the shielding effect when you move from left to right on the periodic table?
there is no change
J.J. Thomson
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