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 2^nd 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?

1. Electrons enter the lowest energy levels first
2. 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