10. Periodic Properties of the Elements

Periodic Trend: Cumulative

Periodic Trends & Properties Tutorial: Periodicity & the Periodic Table of Elements; Crash Chemistry

The highest principal quantum number of the valence orbitals increases.

Both effective nuclear charge and the principal quantum number of valence orbitals increases.

For main-group elements, the atomic radius increases going down a group because:&nbsp;

Trends in the Periodic Table — Part 2: Halogens!

Trends in the Periodic Table - A level Chemistry

Many early chemists noted a diagonal relationship among ele-ments in the periodic table, whereby a given element is some-times more similar to the element below and to the right than it is to the element directly below. Lithium is more similar to magnesium than to sodium, for example, and boron is more similar to silicon than to aluminum. Use your knowledge about the periodic trends of such properties as atomic radii and Zeff to explain the existence of diagonal relationships.

What Are Periods & Groups In The Periodic Table? | Properties of Matter | Chemistry | FuseSchool

Trends on the Periodic Table | Patterns on the Periodic Table

(a) What is the general relationship between the size of an
atom and its first ionization energy?

Valence electrons are more difficult to remove than inner core electrons.

Argon and bromide are isoelectronic species.

Francium possesses the greatest electronegativity.

The second ionization energy of an atom is always larger than its first ionization energy.

The aluminum atom will experience a larger jump in its third ionization energy than its fourth.

Which of the following statements is true?&nbsp;

Which of these spheres represents F, which represents Br,
and which represents Br-?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/fc473fc1ddd73a97-1660838390400.jpg" alt="" />

Trends in the Periodic Table — Reactivity!

Cesium has the smallest ionization energy of all elements (376 kJ/mol), and chlorine has the most negative electron affinity 1-349 kJ/mol2. Will a cesium atom transfer an electron to a chlorine atom to form isolated Cs+1g2 and Cl-1g2 ions? Explain.

Life on Earth evolved based on the element carbon. Based on 
periodic properties, what two or three elements would you expect 
to be most like carbon?

What is the relationship between the electron affinity of a singly charged cation such as Na+ and the ionization energy of the neutral atom?

Potassium and hydrogen react to form the ionic compound 
potassium hydride. (b) Use data in Figures 7.10 and 7.12 to determine 
the energy change in kJ/mol for the following two reactions: 
K1g2 + H1g2 ¡ K+1g2 + H-1g2 
K1g2 + H1g2 ¡ K-1g2 + H+1g2

Elements that have large negative electron affinities generally have (LO 6.10) 
(a) high values for Zeff and a vacancy in a valence orbital. 
(b) low values for Zeff and a vacancy in a valence orbital. 
(c) high values for Zeff and filled valence orbitals. 
(d) low values for Zeff and filled valence orbitals.

The first ionization energy of chlorine is larger than magnesium.

Anions are larger than their parent atoms.

The removal of the first electron from boron is highly exothermic.

The oxygen atom is smaller than the barium atom.

Which of the following statements is false?&nbsp;

Periodic Trend: Cumulative Example 1

Which of the following statements is false?&nbsp;a) The electron affinity of phosphorus is less exothermic than those of both silicon and sulfur.&nbsp;b) The second ionization energy of oxygen is less than the first ionization of fluorine.c) As the principal quantum number of an atom increases the effective nuclear charge will increase.&nbsp;d) Cations are smaller than their parent atoms.&nbsp;e) The second electron affinity of an atom will be more exothermic than the first electron affinity.&nbsp;

Consider the following equation:
Al3+1g2 + e-¡Al2+1g2
Which of the following statements are true? (i) The energy
change for this process is the second electron affinity of Al
atom since Al2+1g2 is formed. (ii) The energy change for this
process is the negative of the third ionization energy of the Al
atom. (iii) The energy change for this process is the electron
affinity of the Al2+ ion.

Consider the isoelectronic ions F- and Na+. (d) For isoelectronic ions, 
how are effective nuclear charge and ionic radius related?

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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 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

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;

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