10. Periodic Properties of the Elements

The Electron Configuration

Electron Configurations for Multielectron Atoms

Draw orbital-filling diagrams for atoms with the follow-ing atomic numbers. Show each electron as an up or down arrow, and use the abbreviation of the preceding noble gas to represent inner-shell electrons. 
(b) Z = 56

Two possible electron configurations for an Li atom are shown here. (c) In the absence of an external magnetic
field, can we say that one electron configuration has a lower energy than the other? If so, which one has the lowest energy?

The two most common isotopes of uranium are 235U and 
238U. (d) 238U undergoes radioactive decay to 234Th. How many 
protons, electrons, and neutrons are gained or lost by the 
238U atom during this process? (e) Examine the electron 
configuration for Th in Figure 6.31. Are you surprised by 
what you find? Explain.

Write the full orbital diagram for each element. 
a. S

Which outer electron configurations would you expect to
belong to a noble gas?
a. ns2 b. ns2np6 c. ns2np5 d. ns2np2

Name an element in the fourth period (row) of the periodic 
table with the following: 
c. three 3d electrons

According to Auf Bau Principle, starting from 1s, electrons fill lower energy orbitals before filling higher energy orbitals.

Electron Configurations Using the Periodic Table

Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. 
(e) Contains the outermost electrons in a beryllium atom

According to Hund's Rule, degenerate orbitals are first half filled before being totally filled.

Electron Configurations

Write the full orbital diagram for each element. 
c. Ne

The Electron Configuration Example 1

The two most common isotopes of uranium are 235U and 
238U. (b) Using the periodic table in the frontinside 
cover, write the electron configuration for a U atom.

The periodic table is divisible into four blocks corresponding to the fillings of the four quantum sublevels (s, p, d, and f).

The group number of a main-group element is equal to the number of valence electrons for that element.

The row number of a main-group element is equal to the highest principal quantum number of that element.

Correct, all of these statements characterize the periodic table.

All of these statements characterize the periodic table.

 Review the organization of the periodic table in terms of the relation of row numbers to the principle quantum number and group numbers to valence electrons.   

Which of the following statements is/are true?

(b) If we add one electron to form the He atom, would your answer to
part (a) change?

Four possible electron configurations for a nitrogen atom are 
shown below, but only one schematic represents the correct 
configuration for a nitrogen atom in its ground state. 
Which configurations violate the Pauli exclusion principle?

Write the full electron configuration for each element.
a. Si
b. O
c. K
d. Ne

Electron Configurations Part 1- Electrons and Sublevels

Electron Configuration Diagrams | Properties of Matter | Chemistry | FuseSchool

What is the expected ground-state electron configuration of the recently discovered element with Z = 116?

Identify the element with the given electron orbital diagram.&nbsp;<img src="https://cdn.clutchprep.com/problem_images/147457-2fe64be237b63f0f.png" alt="" />

Which electron configuration represents a violation of the Auf Bau Principle?&nbsp;

Give examples of transition metal ions with +3 charge that
have an electron configuration of nd5 (n = 3, 4, 5...).

(b) Hafnium, Hf, is also found in group 4. Write
the electron configuration for Hf.

Electron configuration of Boron (Z= 5) is 1s2 2s2&nbsp;2p1.

Name an element in the fourth period (row) of the periodic 
table with the following: 
b. four 4p electrons

What atom has the following orbital-filling diagram? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/6d951fcde8e8e9c2-1669938256678.jpg" alt="" />

Write the full orbital diagram for each element.
a. N
b. F
c. Mg
d. Al

Write the symbol, give the ground-state electron configuration, and draw an orbital-filling diagram for each of the following atoms. Use the abbreviation of the preceding noble gas to represent the inner-shell electrons.
(a) The heaviest alkaline earth metal

According to the aufbau principle, which orbital is filled immediately after each of the following in a multielectron atom?
(a) 4s 
(b) 3d
(c) 5f
(d) 5p

The Electron Configuration Example 2

Name an element in the third period (row) of the periodic table 
with the following: 
c. six 3p electrons

Practice Problem: Electron Configuration and Quantum Numbers

Which electron configuration represents a violation of Hund’s Rule?&nbsp;

Write the electron configuration and electron orbital diagram for the following element:&nbsp;Mn (Z = 25)&nbsp;

Four possible electron configurations for a nitrogen atom are
shown below, but only one schematic represents the correct
configuration for a nitrogen atom in its ground state.
Which one is the correct electron configuration? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/5def54002cba295b-1664386363473.jpg" alt="" />

SPDF Electronic Configuration Trick | Super trick

(c) What does each box in an orbital diagram represent?

Assuming that g orbitals fill according to Hund’s rule, what is the atomic number of the first element to have a filled g orbital?

The sublevels of each principal level are not degenerate for multielectron atoms.

This is true due to electron-electron repulsions.

In a hydrogen atom, the sublevels of each principal level are degenerate.

This is true since there are no electron-electron repulsions.

Due to shielding, the 3d orbitals lie lower in energy than the 4s orbital.

Some atoms have anomalies in their electron configurations due to the fact that energy separations of the orbitals become smaller as the principal quantum number increases.

This is true as evidenced by the electron configurations of some of the transition metals.

 Electron-electron repulsions in many electron atoms affect the energy of atomic orbitals. 

Which of the following statements is false?

Name an element in the fourth period (row) of the periodic
table with the following:
d. full s and p sublevels

What is the atomic number and expected ground-state electron configuration of the yet undiscovered element directly below Fr in the periodic table?

Periodic Law:&nbsp;elements in same group arranged by increasing atomic weight, share chemical properties, which influence electron arrangements, trends and atomic structure.

Write the full orbital diagram for each element. 
b. Ca

Which outer electron configuration would you expect to belong to a reactive nonmetal?
a. ns2 b. ns2np6 c. ns2np5 d. ns2np2

How to Find the Charge of an Ion! (The Octet Rule)

Which outer electron configurations would you expect to
belong to a metalloid?
a. ns2 b. ns2np6 c. ns2np5 d. ns2np2

Write the ground-state electron configuration for the following element:&nbsp;Lead (Z = 82) &nbsp;

How to Draw Orbital Diagrams

No two electrons in an atom can have the same four quantum numbers.

Each electron has a unique set of quantum numbers.

Electron spin is a fundamental property of electrons.

Spin is the fundamental property that affects how many electrons are allowed in one orbital.

All electrons have the same amount of spin.

This is a basic property of all electrons.

The orientation of an electron&#8217;s spin is quantized.

Spin is quantized with only two possibilities called spin up and spin down.

The possible values of spin are +1 and &#x2212;1.

Correct, the possible values are +1/2 and &#x2212;1/2.

 Review the Pauli exclusion principle and its implications. 

Which outer electron configuration would you expect to belong
to a reactive metal?
a. ns2 b. ns2np6 c. ns2np5 d. ns2np2

Shown below is a qualitative diagram of the atomic orbital 
energies for an Na atom. The number of orbitals in each subshell 
is not shown. 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/d574596b99f97902-1660909304577.jpg" alt="" /> 
(d) A sodium vapor lamp (Figure 7.23) operates by using 
electricity to excite the highest-energy electron to the 
next highest-energy level. Light is produced when the 
excited electron drops back to the lower level. Which 
two energy levels are involved in this process for the Na 
atom?

(d) For the hydrogen atom, list the following orbitals
in order of increasing energy: 3s, 2s, 2p, 5s, 4d.

Name an element in the third period (row) of the periodic table 
with the following: 
b. four 3p electrons

Name an element in the third period (row) of the periodic table 
with the following: 
d. two 3s electrons and no 3p electrons

At what atomic number is the filling of a g orbital likely to begin?

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Periodic Trend: Cumulative

Periodic Trends are patterns present in the periodic table based on an element's size and electron distribution.&nbsp;

Periodic Trend: Ionic Radius

Ionic Radius is the distance between an ion's nucleus and its most outer occupied electron shell.&nbsp;

The electron configuration of an element is the distribution of its electrons within atomic orbitals.&nbsp;

The Electron Configuration: Ions

The Electron Configuration of Ions involves either adding or removing electrons from a given orbital of an element.

Periodic Trend: Successive Ionization Energies

Successive Ionization Energies deals with the removal of multiple electrons from a gaseous atom or ion through multiple steps.

Periodic Trend: Atomic Radius

The atomic radius of an element is the distance from its nucleus to its outer electron shell.

Valence Electrons of Elements

The Valence Electrons represent the outer shell electrons of an element or ion.&nbsp;

Periodic Trend: Effective Nuclear Charge

Effective Nuclear Charge (Zeff) measures the force exerted onto an electron by the nucleus.&nbsp;

Periodic Trend: Ionization Energy

Ionization Energy is the energy absorbed&nbsp;in order to remove an electron from a gaseous atom or ion.&nbsp;

Periodic Trend: Metallic Character

Metallic Character&nbsp;deals with how easily an electron can be removed from an element.&nbsp;

Paramagnetism and Diamagnetism

Paramagnetism&nbsp;and&nbsp;Diamagnetism deal with the presence of electrons that are either unpaired or paired in an orbital.

Periodic Trend: Electron Affinity

Electron Affinity is the energy released from the addition of an electron to a gaseous atom or ion.&nbsp;

The Electron Configuration: Quantum Numbers

The Quantum Numbers ultimately can be used to determine the precise location of an electron.&nbsp;

Periodic Trend: Electronegativity

Electronegativity is an element's ability to attract electrons.

The Electron Configurations: Exceptions

Most Electron Configuration Exceptions are the result of elements drive to obtain half filled or totally filled d orbitals.&nbsp;

The Electron Configuration: Condensed

Condensed Electron Configurations are a faster method in determining the configuration of elements and ions.&nbsp;