Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
The Electron Configuration
The Electron Configuration: Condensed
The Electron Configurations: Exceptions
The Electron Configuration: Ions
Paramagnetism and Diamagnetism
The Electron Configuration: Quantum Numbers
Valence Electrons of Elements
Periodic Trend: Metallic Character
Periodic Trend: Atomic Radius
Periodic Trend: Ionic Radius
Periodic Trend: Ionization Energy
Periodic Trend: Successive Ionization Energies
Periodic Trend: Electron Affinity
Periodic Trend: Electronegativity
Periodic Trend: Effective Nuclear Charge
Periodic Trend: Cumulative
Additional Guides
Atomic Radius
Ionization Energy
Jules Bruno

Atomic radius represents the distance from the nucleus of an atom to its outer shell. 

Understanding Atomic Radius

As a result of electrons not being confined in truly organized orbitals, the radial size of the elements can vary greatly. By comparing identical atoms bonded together we get a more accurate description of atomic radius. 

Atomic-Radii-Diatomic-MoleculesAtomic Radii (Diatomic Molecules)

Atomic radius is defined as half the distance between the nuclei in a molecule of two identical elements.

Trends in Atomic Radius 

The general trend is that as we move from left to right across a period and as we move up any group the atomic radius decreases. 

Atomic Radius Trend

PRACTICE: Which of the following correctly lists the five atoms in order of decreasing size (largest to smallest)?

Ca,       K,       Ne,         O,         P

a) P > Ne > Ca > K >O

b) O > Ca > K > P > Ne

c) F > O > P > Ca > K

d) K > Ca > P > O > Ne

e) Ca > P > O > Ne > K

STEP 1: Locate each of the elements given within the question. 

Atomic-radius-of-oxygen-of-carbon-of-sodium-covalent-radius-isolated-atoms-outermost-orbitalAtomic Radii (Ca, K, Ne, O, P)

STEP 2: Since we are going from the largest to smallest atomic radius start on the left side where elements are larger and move to the right. 

STEP 3: Going from left to right across the period and up any groups gives the answer from largest to smallest as: 

K > Ca > P > O > Ne

This gives Choice D as the correct answer. 

Exceptions to Atomic Radius (Transition Metals)

Exceptions to atomic radii occur when examining the transition metals of the periodic table. 

Lanthanide-ContractionLanthanide Contraction

Under the lanthanide contraction we have a decrease in the atomic radii as we transition from the 3d to 4d transition metals. Conversely, a transition from 4d to 5d transition metals sees the atomic radii held relatively constant. 

Exceptions to Atomic Radius (Main Group Elements)

There are also a few exceptions to atomic radii when examining some of the main group elements. 

Atomic-Radii-Main-Group-same-size-unitsVan der Waals Radius (in picometers)

When comparing oxygen to nitrogen, tellurium to antimony or polonium to bismuth we see an unexpected increase in atomic radii. This can be attributed to an increase in electron-electron repulsions, which causes a slight increase in the atomic radius. 

The Other Periodic Trends

The number of electrons and size of ions and atoms have a big impact on their chemical properties. These chemical properties can be explained through other periodic trends such as ionic radius, electronegativity, ionization energy, effective nuclear charge and metallic character. 

Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.