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

10. Periodic Properties of the Elements

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: Ionic Radius

Ionic Size - Which ion is bigger?

The following ions all have the same number of electrons: Ti4+, Sc3+, Ca2+, S2-. Order them according to their expected sizes, and explain your answer.

3.2 Trends in ionic radii (SL)

Which ion has a larger atomic radius, Cu+ or Cu2+? Explain your reasoning.

Which isoelectronic series is correctly arranged in order of increasing radius?

Periodic Trend: Ionic Radius Example 2

Which is the larger species in each pair?
a. Li o r Li+
b. Cs- o r Cs+ 
c. Cr- or Cr3+
d. O or O2-

Isoelectronic Series Atomic Radius

Which atom or ion in the following pairs would you expect to be larger?
(c) Cr3+ or Cr6+

Ionic Radius

For an isoelectronic series of ions, the ion that is the smallest is always

Kr < Br- < Sr2+ < Rb+

Kr < Sr2+ < Rb+ < Br-

Sr2+ < Rb+ < Kr < Br-

Rb+ < Sr2+ < Kr < Br-

Br- < Kr < Rb+ < Sr2+

Arrange the following atoms and/or ions in the order of increasing size:Br&nbsp;–, Kr, Rb+, Sr2+.

Periodic Trend: Ionic Radius Example 1

Order the following ions from smallest to largest: Sr2+, Se2-, Br-, Rb+.

Arrange this isoelectronic series in order of increasing atomic
radius: Se2 - , Sr2 + , Rb+ , Br - .

The following ions contain the same number of electrons. rank them in order of decreasing ionic radii.

Identify each statement as true or false: (b) Li+ is smaller 
than Li.

Which is the larger species in each pair?
a. Sr or Sr2+ b. N or N3- 
c. Ni or Ni2+ d. S2-or Ca2+

Place the following ions in order of increasing radius. ca2+ s2- cl-

Consider the Mg2+, Cl-, K+, and Se2- ions. The four spheres 
below represent these four ions, scaled according to ionic size. 
(b) In terms of size, between which of the spheres 
would you find the (i) Ca2 + and (ii) S2 - ions? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b35dee250c65e14b-1672947683444.jpg" alt="" />

Consider S, Cl, and K and their most common ions.(c) Explain any differences in the orders of the atomic and ionic sizes.

Identify each statement as true or false: (a) Cations are larger
than their corresponding neutral atoms.

For an isoelectronic series of ions, the ion that is the smallest is always&nbsp;

Periodic Trend: Ionic Radius increases as the number of electrons increases.

Consider the ionic compounds KF, NaCl, NaBr, and LiCl. 
(a) Use ionic radii (Figure 7.8) to estimate the cation–anion 
distance for each compound.

Correct, this ion has the largest electron to proton ratio.

There is a species listed in this isoelectronic series that has fewer protons.

 Cations are generally smaller than their parent atoms; anions are generally larger than their parent atoms. 

Which of the following atoms or ions is the largest?

In the ionic compounds LiF, NaCl, KBr, and RbI, the measured 
cation–anion distances are 201 pm (Li–F), 282 pm 
(Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (b) Calculate the difference between 
the experimentally measured ion–ion distances and the ones 
predicted from Figure 7.8. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/843748a19af42bfb-1664465393863.jpg" alt="" />

Order the following ions from smallest to largest: Mg2+, O2-, F-, Na+.

Which of the following spheres is likely to represent a metal atom and which a nonmetal atom? Which sphere in the products represents a cation and which an anion? <img src="https://lightcat-files.s3.amazonaws.com/problem_images/7b8baca55abe85ad-1669931107791.jpg" alt="" />

The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity

Which atom or ion in the following pairs would you expect to be larger? 
(c) O-or O2-

Atomic and Ionic Radius

In the ionic compounds LiF, NaCl, KBr, and RbI, the measured 
cation–anion distances are 201 pm (Li–F), 282 pm 
(Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (c) What estimates of the cation– 
anion distance would you obtain for these four compounds 
using neutral atom bonding atomic radii? Are these estimates 
as accurate as the estimates using ionic radii?

Provide a brief explanation for each of the following.K+ is larger than Na+.

Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius, and Electron Affinity

Arrange each of the following sets of atoms and ions, in order
of increasing size: (a) Pb, Pb2+, Pb4+

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Periodic Trend: Cumulative

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

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;